We provide electrochemistry practice exercises, instructions, and a learning material that allows learners to study outside of the classroom. We focus on electrochemistry skills mastery so, below you will get all questions that are also asking in the competition exam beside that classroom.

#### List of electrochemistry Questions

Question No | Questions | Class |
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1 | Find the over voltage if electrolysis of brine solution requires ( 2.19 mathrm{V} ) to produce ( mathrm{H}_{2} ) and ( mathrm{Cl}_{2} . ) (Write your answer upto two decimal places) Given: ( boldsymbol{E}_{boldsymbol{H}^{+} / boldsymbol{H}}^{boldsymbol{o}}=mathbf{0} ) and ( boldsymbol{E}_{C l^{-} / C l_{2}}^{o}= ) ( -1.36 V ) | 12 |

2 | When a corroded metal object is rubbed by a sand paper then: A. outer metal surface is removed B. metal becomes thin c. outer corroded layer will be removed D. all of the above | 12 |

3 | The life span of a Daniel cell may increased by: A. large Cu electrode B. lowering of CuSO ( _{4} ) concentration C. lowering of ZnSO ( _{4} ) concentration D. large zinc electrode | 12 |

4 | Resistance of a cconductivity cell filled with a solution of an electrolyte of concentration ( 0.1 M ) is ( 100 Omega ). The conductivity of this solution is ( 1.29 S m^{-1} . ) Resistance of the same cell when filled with ( 0.02 ~ M ) of the same solution is ( 520 Omega ). The molar conductivity of ( 0.02 M ) solution of the electrolyte will be: A ( cdot 124 times 10^{-4} mathrm{Sm}^{2} mathrm{mol}^{-1} ) В. ( 1240 times 10^{-4} mathrm{Sm}^{2} mathrm{mol}^{-1} ) c. ( 1.24 times 10^{-4} mathrm{Sm}^{2} mathrm{mol}^{-1} ) D. ( 12.4 times 10^{-4} mathrm{Sm}^{2} mathrm{mol}^{-1} ) | 12 |

5 | The ( mathrm{E}^{o} ) for reduction of ( mathrm{HNO}_{2} ) to ( mathrm{NO} ) is ( 0.99 mathrm{V} ) and ( mathrm{E}^{circ} ) for reduction of ( mathrm{NO}_{3}^{-} ) to ( mathrm{HNO}_{2} ) is ( 0.94 mathrm{V} . ) The equilibrium constant at ( 25^{circ} mathrm{C} ) for the disproportionation of 3 mole of aqueous ( mathrm{HNO}_{2} ) to yield ( mathrm{NO} ) and ( mathrm{N} mathrm{O}_{3}^{-} ) ions is: A. ( K_{c}=344.64 ) В. ( K_{c}=336.97 ) c. ( K_{c}=639.73 ) D. None of these | 12 |

6 | When the terminals of a cell of e.m.f. ( 1.5 v ) are connected to an ammeter of resistance ( 4 Omega, ) the ammeter read 0.30 amp. which of the following statements is/are correct? This question has multiple correct options A. The cell is non-ideal B. If a ( 4 Omega ) resistor is also connected across terminals of the cell, the ammeter will read 0.50 amp. c. If a ( 4 Omega ) resistor is also connected across terminals of the cell, one-third of the electrical power generated will dissipate as heat within the cell D. If a voltmeter of resistance ( 4 Omega ) is used to measure potential difference between terminals of the cell, it will read ( 1.2 mathrm{v} ) | 12 |

7 | After electrolysis of NaCl solution with inert electrodes for a certain period of time, ( 600 mathrm{mL} ) of the solution was left. Which was found to be ( 1 mathrm{N} ) in ( mathrm{NaOH} ) During the same time, 31.75 g ( mathrm{Cu} ) deposited in the copper voltameter in series with the electrolytic cell. Calculate the percentage yield of NaOH obtained. A. ( n=60 % ) a B . ( n=50 % ) c. ( n=70 % ) D. None of these | 12 |

8 | Observe the given diagram and fill in the blanks by choosing the correct option. ( mathbf{A} cdot mathbf{x}-H_{2(g)} ) at 1 atm ( , y-10^{-2} M H^{+}, z^{-} ) Finely divided ( P t ) B . ( x-H_{2(g)} ) at 1 bar, ( y-1.00 M H^{+}, z ) – Finely divided Pt C. ( x-1.00 M H^{+}, y-H_{2(g)} ) at 1 bar, ( z ) – Finely divided ( N ) i D. ( x-H_{2}(g) ) at 1 bar, ( y-1.00 M H^{+}, z ) – Pt granules | 12 |

9 | State True or False. The ratio of gases liberated at cathode and anode during electrolysis of ( mathrm{CH}_{3} ) COONa(aq) is 1: 3 A. True B. False | 12 |

10 | Which of the following complexes has lowest molar conductance? A. ( operatorname{CoCl}_{3} .3 mathrm{NH}_{3} ) в. ( operatorname{CoCl}_{3} .4 mathrm{NH}_{3} ) c. ( operatorname{CoCl}_{3} .5 mathrm{NH}_{3} ) D. ( operatorname{CoCl}_{3} .6 mathrm{NH}_{3} ) | 12 |

11 | The specific conductivity of ( N / 10 K C l ) solution at ( 20^{circ} mathrm{C} ) is 0.0212 ohm ( ^{-1} ) ( c m^{-1} ) and the resistance of the cell containing this solution at ( 20^{circ} mathrm{C} ) is 55 ohm. The cell constant is: A ( cdot 3.324 mathrm{cm}^{-1} ) B. ( 1.166 mathrm{cm}^{-1} ) ( mathbf{c} cdot 2.372 mathrm{cm}^{-1} ) D. ( 3.682 mathrm{cm}^{-1} ) | 12 |

12 | The equivalent conductance of NaCl at concentration ( C ) and at infinite dilution ( operatorname{are} lambda_{C} ) and ( lambda_{infty} ) respectively. The correct relationship between ( lambda_{C} ) and ( lambda_{infty} ) is given as: (Where the constant B is positive) A ( cdot lambda_{C}=lambda_{infty}-(B) sqrt{C} ) в. ( lambda_{C}=lambda_{infty}+(B) sqrt{C} ) c. ( lambda_{C}=lambda_{infty}+(B) C ) D. ( lambda_{C}=lambda_{infty}-(B) C ) | 12 |

13 | (a) Following reactions occur at cathode during the electrolysis of aqueous sodium chloride solution: ( N a^{+}(a q)+e^{-} longrightarrow N a(s) E^{0}= ) ( -2.71 V ) ( boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q})+boldsymbol{e}^{-} longrightarrow frac{mathbf{1}}{mathbf{2}} boldsymbol{H}_{2}(boldsymbol{g}) boldsymbol{E}^{0}= ) ( 0.00 V ) On the basis of their standard reduction electrode potential ( left(boldsymbol{E}^{0}right) ) values which reaction is feasible at the cathode and why? (b) Why does the cell potential of mercury cell remain constant throughout its life? | 12 |

14 | A current of 5 amperes is passed through ( mathrm{AlCl}_{3} ) solution for 15 minutes using Pt electrodes, when 0.504 g of ( A l ) is produced. What is the molar mass of Al? | 12 |

15 | Given ( boldsymbol{E}_{boldsymbol{C r}^{3+} / boldsymbol{C r}}^{circ}=-boldsymbol{0 . 7 4} boldsymbol{V} ; boldsymbol{E}_{M n O_{4}^{-} / M n^{2+}}^{circ}= ) ( +1.51 V ) ( boldsymbol{E}_{C r_{2} O_{7}^{2-} / C r^{3+}}^{circ}=+mathbf{1 . 3 3} boldsymbol{V} ; boldsymbol{E}_{C l / C l^{-}}^{circ}= ) ( +1.36 V ) based on the data given above, strongest oxidizing agent will be A. ( M n^{2+} ) в. ( M n O_{4}^{-} ) c. ( C l ) D. ( C r^{3} ) | 12 |

16 | In the hydrogen atom, the energy difference between the states ( n=2 ) and ( n=3 ) is ( mathrm{E} ) eV. The ionisation potential of ( mathrm{H} ) atom is: A. 3.2 в. 5.6 Е ( c cdot 7.2 E ) D. 13.2 E | 12 |

17 | Assertion We apply paint on iron articles. Reason Iron is a metal, metals rust when they come in contact of direct air so to prevent rusting. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

18 | Assertion Li electrode always acts as anode in voltaic cell. Reason Li electrode has lowest SRP among all the electrodes. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct. | 12 |

19 | The weight in grams of ( O_{2} ) formed at ( P t ) anode during the electrolysis of aq. ( K_{2} S O_{4} ) solution during the passage of one coulomb of electricity is: A ( cdot frac{16}{96800} ) в. ( frac{8}{96500} ) c. ( frac{32}{96500} ) D. ( frac{64}{96500} ) | 12 |

20 | Pure water consists entirely of (ions / molecules) | 12 |

21 | In a galvanic cell, electrons flow through connecting wires from: A. anode to cathode B. cathode to anode c. top to bottom D. anode | 12 |

22 | Which of the following is/are nondisposable batteries? This question has multiple correct options A. Dry cell B. Mercury cell c. Lead acid battery D. ( N i-C d ) battery | 12 |

23 | According to Kohlrausch law, the limiting value of molar conductivity of an electrolyte ( A_{2} B ) is: ( mathbf{A} cdot Lambda_{A}^{infty}+Lambda_{B}^{infty} ) B ( cdot Lambda_{A}^{infty}-Lambda_{B}^{infty} ) ( mathbf{C} cdot Lambda_{A}^{infty}+frac{1}{2} Lambda_{B}^{infty} ) ( mathbf{D} cdot 2 Lambda_{A}^{infty}+Lambda_{B}^{infty} ) | 12 |

24 | Pick out the pair in which the energy change of one is reverse of the energy change in the other : (1) radio (2) fluorescent lamp (3) toaster (4) photoelectric cell A . 1 and 2 B. 2 and 3 ( c cdot 2 ) and 4 D. 3 and 4 | 12 |

25 | What is the charge of 96 amu of ( S^{2-} ? ) A ( .2 C ) B . ( 3.2 times 10^{-19} C ) c. ( 9.6 times 10^{-19} C ) D. ( 6 C ) | 12 |

26 | The equivalent conductance of ( B a^{2+} ) and ( C l^{-} ) are respectively 127 and 76 ( operatorname{oh} m^{-1} c m^{2} e q^{-1} ) at infinite dilution. What will be the equivalent conductance of ( B a C l_{2} ) at infinite dilution? A . 139.5 ohm ( ^{-1} mathrm{cm}^{2} ) eq ( ^{-1} ) B . 203 ohm ( ^{-1} mathrm{cm}^{2} ) eq( ^{-1} ) c. 279 ohm ( ^{-1} mathrm{cm}^{2} ) eq ( ^{-1} ) D. 101.5 ohm ( ^{-1} mathrm{cm}^{2} ) eq ( ^{-1} ) | 12 |

27 | If Molar conductivity of ( C a^{2+}=119 & ) Molar conductivity of ( C l^{=} 71 ) then find the molar conductivity of ( C a C l_{2} ) A .341 в. 261 ( c cdot 126 ) D. 431 | 12 |

28 | Match List I with List II. | 12 |

29 | Assertion: The more negative the standard reduction potential, the more is its ability to displace hydrogen from acids. Reason: Ability to displace hydrogen from acids translates to the strength of the reductant. | 12 |

30 | The specific conductivity of ( N / 10 K C l ) solution at ( 20^{circ} mathrm{C} ) is 0.0212 oh ( m^{-1} mathrm{cm}^{-1} ) and the resistance of the cell containing this solution at ( 20^{circ} C ) is 55 ohm. The cell constant is: A ( cdot 4616 mathrm{cm}^{-1} ) B. ( 1.166 mathrm{cm}^{-1} ) c. ( 2.173 mathrm{cm}^{-1} ) D. ( 3.324 mathrm{cm}^{-1} ) | 12 |

31 | Calculate ( Delta G ) for the following cell reaction. ( boldsymbol{Z} boldsymbol{n}_{(s)}+boldsymbol{A} boldsymbol{g}_{2} boldsymbol{O}_{(s)}+boldsymbol{H}_{2} boldsymbol{O}_{(l)} rightarrow boldsymbol{Z} boldsymbol{n}_{(a q)}^{2+}+ ) ( mathbf{2} boldsymbol{A} boldsymbol{g}_{(s)}+mathbf{2} boldsymbol{O} boldsymbol{H}^{-}(boldsymbol{a} boldsymbol{q}) ) ( boldsymbol{E}_{A boldsymbol{g}^{+} / boldsymbol{A} boldsymbol{g}}^{0}=+mathbf{0 . 8 0} boldsymbol{V} ) and ( boldsymbol{E}_{boldsymbol{Z n}^{+2} / Z boldsymbol{n}}^{0}= ) ( -0.76 V ) A . -305 k ( J / operatorname{mol} ) в. ( -301 k J / ) mol c. ( 305 k J / ) mol D. 301 kJ/mol | 12 |

32 | Characteristics & Relation | 12 |

33 | faraday ( = ) A ( .10000 C ) B. ( 95000 C ) c. ( 96.5 C ) D. 96500 ( C ) | 12 |

34 | An electrochemical cell stops working after some time because: A. electrode potential of both the electrodes becomes zero B. electrode potential of both the electrodes become equal C . one of the electrode is eaten away. D. the reaction starts proceeding in opposite direction | 12 |

35 | Why zinc metal is used for galvanisation? A. zinc get corroded easily than iron B. zinc does not corrode c. corrosion constant of iron increase D. All of the above | 12 |

36 | Why does the bulb glow, when the electric current passes through it? A. Due to the lighting effect of electric current B. Due to the magnetic effect of electric current. c. Due to the chemical effect of electric current D. Due to the heating effect of electric current | 12 |

37 | The potential of a hydrogen electrode at ( boldsymbol{p} boldsymbol{H}=mathbf{1} ) is A. 0.059 volt B. 0 volt c. -0.059 volt D. 0.59 volt | 12 |

38 | Acetic acid is titrated with ( N a O H ) solution. Which of the following statement is correct for this titration? A. Conductane increases upto equivalence point, then it it decreases B. Conductance decreases upto equivalence point, then it increases c. First conductance increases slowly upto equivalence point and then increases rapidly D. First conductance increases slowly upto equivalence point and then drops rapidly | 12 |

39 | Voltaic cell is same as: A. galvanic cell B. electrolytic cell C. fuel cell D. lead cell | 12 |

40 | ( ln ) a daniel cell, if ( boldsymbol{A}left(boldsymbol{E}^{o}=-mathbf{0 . 7 6} boldsymbol{C}right) ) and ( Bleft(E^{o}=-2.36 Vright) ) half cells are taken then: ( A cdot B ) acts as anode B. ( A ) acts as anode c. ( B ) acts as cathode D. cannot be predicted | 12 |

41 | 0.68 What is the relationship between Gibbs free energy of the cell reaction in a galvanic cell and the emf of the cell? When will the maximum work be obtained from a galvanic cell? | 12 |

42 | Q2. What is standard hydrogen electrode? For what purpose it is used? What are signs of oxidation potential and reduction potential decided by using SHE (Standard hydrogen electrode)? | 12 |

43 | Which of the following is one of the most common application of chemical effects of electric current? A. Electrophoresis B. Electroplating c. Galvanization D. Mineralization | 12 |

44 | the blanks by choosing an appropriate option. In the given cell, hydrogen and oxygen | 12 |

45 | Number of Faradays (F) required to reduce 3 mol of ( M n O_{4}^{ominus} ) to ( M n^{2+} ) is: | 12 |

46 | ( lambda^{infty} ) of ( N H_{4} O H ) at infinite dilution is ( boldsymbol{S} boldsymbol{c m}^{2} boldsymbol{m o l}^{-1} operatorname{given} boldsymbol{lambda}^{infty} boldsymbol{o f} ) ( O H^{-}=174, lambda^{infty} ) if ( C l^{-}=66 ) and ( lambda^{infty} ) of ( N H_{4} C l=130 S c m^{2} m o l^{-1} ) A . 140 в. 218 c. 238 D. 198 | 12 |

47 | What is the potential of a half cell consisting of zinc electrode in ( 0.01 mathrm{M} ) ( Z n S O_{4} ) solution of ( mathbf{2 5}^{circ} boldsymbol{C} ?left[boldsymbol{E}^{boldsymbol{o}}=mathbf{0 . 7 6 3} boldsymbol{V}right] ) | 12 |

48 | What are fuel cells? How are they different from Galvanic cells? Give the construction of hydrogen-oxygen fuel cells. | 12 |

49 | The resistance of solution decreases with increase in temperature. A. True B. False | 12 |

50 | ( C H_{3} C O O H ) is titrated with ( N a O H ) solution. Which of the following statement is true? A. Conductance decreases upto equivalence point, after which it increases. B. conductance increases upto equivalence point, after which it decreases. c. conductance first increases (but not rapidly) upto equivalence point and then increases rapidly after equivalence point. D. None of the above | 12 |

51 | How many coulombs of electricity are required for the oxidation of one mole of water to dioxygen? A ( .9 .65 times 10^{4} C ) в. ( 1.93 times 10^{4} C ) c. ( 1.93 times 10^{5} mathrm{C} ) D. ( 19.3 times 10^{5} C ) | 12 |

52 | Answer the following, in short, using a maximum 30 words. Explain Faraday’s first law of electrolysis | 12 |

53 | In electrochemical corrosion. the metal undergoing corrosion: A. acts as anode B. acts as cathode c. undergoes reduction D. liquifies | 12 |

54 | The resistance of ( 0.5 mathrm{M} ) solution of an electrolyte in a cell was found to be 50 Omega. If the electrodes in the cell are ( 2.2 mathrm{cm} ) a part and have an area of ( 4.4 mathrm{cm}^{2} ) than the molar conductivity ( left(operatorname{in} S m^{2} m o l^{-1}right) ) of the solution is: A . 0.2 B. 0.02 c. 0.002 D. None of these | 12 |

55 | When lead storage battery is charged: A. lead dioxide dissolves B. sulphuric acid is regenerated C. the lead electrode becomes coated with lead sulphate D. the amount of sulphuric acid decreases | 12 |

56 | Q1. Define electrochemical cell. | 12 |

57 | Which one is not correct for e.m.f. of a galvanic cell? This question has multiple correct options ( mathbf{A} cdot E_{c e l l}=E_{O P_{a n o d e}}+E_{R P_{c a t h a d e}} ) B. ( E_{text {cell}}=E_{O P_{L H S}}+E_{R P_{text {RHS}}} ) C ( . E_{text {cell}}= ) higher oxidation potential – lower oxidation potential D. ( E_{text {cell}}= ) lower oxidation potential – higher oxidation potential | 12 |

58 | Calculate the molarity of a solution containing ( 5 g ) of NaOH dissolved in the product of a ( boldsymbol{H}_{2}-boldsymbol{O}_{2} ) fuel cell operated at ( 1 A ) current for 595.1 hours. (Assume ( 1 F=96500 mathrm{C} / mathrm{mol} ) of electrons and molecular weight of NaOH as ( 40 mathrm{g} ) mol ( ^{-1} ) ) A . 0.05 M B. 0.025 м ( c .0 .1 mathrm{m} ) D. 0.075 м E. 1 M | 12 |

59 | Which of the following reaction occurs at the cathode during the charging of lead storage battery? ( mathbf{A} cdot P b rightarrow P b^{2+}+2 e^{-} ) B ( cdot P b^{2+}+2 e^{-} rightarrow P b ) ( mathbf{c} cdot P b O_{2}+S O_{4}^{2-} rightarrow P b S O_{4} ) D ( cdot P b S O_{4}(s)+2 H_{2} O rightarrow P b O_{2}(s)+4 H^{+}+S O_{4}^{2-}+2 e^{-} ) | 12 |

60 | The potential of a hydrogen electrode in a solution with ( mathrm{pH}=5 ) at ( 25^{circ} mathrm{C} ) is: A ( .+0.059 ) B. 0.59 c. -0.295 D. 0.295 | 12 |

61 | Assertion Standard hydrogen electrode is a half cell having ( 1 M H^{+} ) concentration bubbled with hydrogen at any pressure Reason A hydrogen electrode will always show ( boldsymbol{E}_{c e l l}=mathbf{0 . 0 0} boldsymbol{V} ) | 12 |

62 | Consider the cell: ( boldsymbol{Z} boldsymbol{n} mid boldsymbol{Z} boldsymbol{n}^{2+}(boldsymbol{a q})(boldsymbol{1} . boldsymbol{0} boldsymbol{M}) | boldsymbol{C u}^{2+}(boldsymbol{a q}) ) The standard reduction potential are ( 0.350 mathrm{V} ) for ( boldsymbol{C u}^{2+}(boldsymbol{a q})+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{C u} ) and ( -0.763 mathrm{V} ) for ( mathrm{Zn}^{2+}(a q)+2 e^{-} rightarrow ) ( Z n ) The EMF (in V) of the cell is (write your answer as nearest integer): | 12 |

63 | Question 16. Three electrolytic cells A, B, C containing solutions of ZnSO4, AgNO3 and CuSO4 respectively are connected in series. A steady current of 1.5 amperes was passed through them until 1.45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited? [Atomic masses; Cu=63.5, Zn= 65.3 ; Ag = 108] | 12 |

64 | At ( 298 mathrm{K} ) temperature, ( A ) hydrogen gas electrode is made by dipping platinum wire in a solution of HCl of ( mathrm{pH}=10 ) and by passing hydrogen gas around the platinum were at one atm pressure. The potential of electrode would be? ( mathbf{A} cdot 0.59 mathrm{V} ) B. ( 0.118 v ) c. ( 1.18 v ) D. ( 0.059 mathrm{V} ) | 12 |

65 | The products formed when an aqueous solution of ( N a B r ) is electrolysed in a cell having inert electrodes are : A. ( N a ) and ( B r_{2} ) B. ( N a ) and ( O_{2} ) ( mathrm{c} cdot mathrm{H}_{2}, mathrm{Br}_{2} ) and ( mathrm{NaOH} ) D. ( H_{2} ) and ( O_{2} ) | 12 |

66 | The amount of ( N a ) produced by the passage of 2 moles of electrons through the fused ( N a C l ) is ( _{-}—–8 ) A . 23 B. 46 c. 11.5 D. 34.5 | 12 |

67 | Amount of ( C u ) deposited from ( boldsymbol{C u} boldsymbol{S O}_{4}(boldsymbol{a q}) ) when 5 amp current is passed for 965 seconds through it, is ( boldsymbol{C u}=mathbf{6 3 . 5 g m o l}^{-1} mathbf{)} ) A . ( 1.6 g ) B. ( 3.2 g ) c. ( 1.45 g ) D. ( 2.9 g ) | 12 |

68 | Question 5. Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 min in separate electrolytic cell. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer. | 12 |

69 | 0.5 Which of the following statement is not correct about an inert electrode in a cell? (a) It does not participate in the cell reaction (b) It provides surface either for oxidation or for reduction reaction (c) It provides surface for conduction of electrons (d) It provides surface for redox reaction | 12 |

70 | Which of the following reactions occurs at cathode during charging of storage battery? ( mathbf{A} cdot P b^{2+}+2 e^{-} rightarrow P b ) B ( cdot P b rightarrow P b^{2+}+2 e^{-} ) ( mathbf{c} cdot P b^{2+}+S O_{4}^{2-} rightarrow P b S O_{4} ) D ( cdot P b S O_{4}+2 H_{2} O rightarrow P b O_{2}+4 H^{+}+S O_{2}^{2-}+2 e^{-} ) | 12 |

71 | State Faraday’s first law of electrolysis. Write any ‘two’ uses of each of the following (a) ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) (b) Chlorine Distinguish between crystalline solids and amorphous solids. A solution of a substance having mass ( 1.8 times 10^{-3} k g ) has the osmotic pressure of 0.52 atm at ( 280 mathrm{K} ). Calculate the molar mass of the substance used. [Volume ( =1 d m^{3}, R= ) ( left.8.314 J K^{-1} m o l^{-1}right] ) | 12 |

72 | Calculate ( boldsymbol{E}^{circ} ) of the following half-cell reaction at ( 298 K ) ( boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g}+boldsymbol{2} boldsymbol{N} boldsymbol{H}_{3} ) ( boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g} ; boldsymbol{E}_{A boldsymbol{g}^{+} / A boldsymbol{g}}^{circ}=mathbf{0 . 8 0} boldsymbol{V} ) ( boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}^{+} rightleftharpoons boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{2} boldsymbol{N} boldsymbol{H}_{3} ; boldsymbol{K}=boldsymbol{6} times ) ( 10^{-8} ) | 12 |

73 | Define molar conductivity. How it is related with conductivity. | 12 |

74 | . 21 Conductivity of an electrolytic solution depends on (a) nature of electrolyte (b) concentration of electrolyte (c) power of AC source (d) distance between the electrodes | 12 |

75 | What is the voltage of the voltaic cell ( Z nleft|Z n^{2+}right|left|C u^{2+}right| C u ) at ( 298 K ) if ( left[Z n^{2+}right]=0.2 M ) and ( left[C u^{2+}right]=4.0 M ? ) ( boldsymbol{C u}^{2+}+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{C u} boldsymbol{E}^{circ}=+mathbf{0 . 3 4} boldsymbol{V} ) ( Z n^{2+}+2 e^{-} rightarrow Z n E^{circ}=-0.76 V ) ( left[text { Note }: boldsymbol{E}=boldsymbol{E}^{circ}-(mathbf{0 . 0 5 9 1} / boldsymbol{n})(log boldsymbol{Q})right. ) A. ( +1.10 V ) в. ( -1.10 mathrm{V} ) c. ( +1.07 V ) D. ( +1.14 V ) E . ( -1.07 mathrm{V} ) | 12 |

76 | What current strength in amperes will be required to liberate 10 gm of iodine from potassium iodide solution in one hour? (Equivalent mass of lodine is 127 ). | 12 |

77 | The solution of a salt of a metal of atomic mass 112 was electrolysed for 15 minutes with a current of 1.5 ampere. The mass of the metal deposited was ( 0.788 g ). Find the valency of the metal. ( A cdot 1 ) B. 2 ( c cdot 3 ) ( D ) | 12 |

78 | Question 1. Can absolute electrode potential of an electrode be measured? Colin N anl+he diff | 12 |

79 | The ( E_{text {cell}} ) for a given cell is 1.2346 and ( 1.2340 V ) at ( 300 mathrm{K} ) and ( 310 mathrm{K} ) respectively. Calculate the change in entropy during the cell reaction if the redox change involves three electrons. A. ( -17.37 mathrm{JK}^{-1} ) B. ( +17.37 J K^{-1} ) c. ( 173.7 J K^{-1} ) D. ( 5.79 J K^{-1} ) | 12 |

80 | A voltaic cell is represented as ( boldsymbol{A}_{(s)}left|boldsymbol{A}_{(a q)}^{+2}right|left|boldsymbol{B}_{(a q)}^{+2}right| boldsymbol{B}_{(s)} . ) Which of the following statements of false regarding the above cell? A. The double vertical line indicates salt bridge B. ( A ) is called the anode and ( B ) is called the cathode C. The cell reactions are represented as ( A^{2+}+2 e^{-} rightarrow A ) and ( B rightarrow B^{2+}+2 e^{-} ) D. None of the above | 12 |

81 | A tester is used to check the conduction of electricity through two liquids, labelled ( A ) and ( B ). It is found that the bulb of the tester glows brightly for liquid A while it glows very dim for liquid B. You would conclude that: A. liquid ( A ) is a better conductor than liquid ( B ) B. liquid ( B ) is a better conductor than liquid ( A ) c. both liquids are equally conducting D. conducting properties of liquid cannot be compared in this manner. | 12 |

82 | If the ( H^{+} ) concentration decreased from ( 1 mathrm{M} ) to ( 10^{-4} mathrm{M} ) at ( 25^{circ} mathrm{C} ) for the couple ( M n O_{4}^{-} / M n^{2+}, ) then the oxidising power of the ( M n O_{4}^{-} / M n^{2+} ) couple decreases by A . -0.18v B. 0.18V c. ( 0.38 v ) D. -0.38V | 12 |

83 | The electrolysis of aqueous solution of ( boldsymbol{C u B r _ { 2 }} ) using platinum electrode would leads to: This question has multiple correct options A. ( B r_{2} ) gas at anode B. ( B r_{2} ) gas at anode and ( O_{2} ) gas at cathode c. copper(s) at cathode D. ( H_{2} ) gas at cathode | 12 |

84 | If the lead-acid battery is discharged too far or left in a discharged condition, it cannot be recharged any more because: A. terminal voltage becomes too low B. hard lead sulphate forms on its electrodes c. internal resistance of the cell becomes very high D. internal resistance of the cell becomes too low | 12 |

85 | The conductivity of ( 0.20 mathrm{M} ) solution of ( K C l ) at ( 298 mathrm{K} ) is ( 0.0248 S c m^{-1} ) Calculate its molar conductivity. A ( cdot 112 operatorname{Scm}^{2} m o l^{-1} ) B. ( 124 S c m^{2} m o l^{-1} ) ( mathbf{c} cdot 136 S c m^{2} m o l^{-1} ) D. 148 Scm ( ^{2} ) mol ( ^{-1} ) | 12 |

86 | Assertion Anode is the electrode at which oxidation occurs and cathode is the electrode at which reduction occurs. Reason Anode and cathode in electrochemical | 12 |

87 | Which of the following condition is correct for operation of electrolytic cell? A. ( triangle G=0, E=0 ) в. ( triangle G0 ) c. ( triangle G>0, E0, E>0 ) | 12 |

88 | When a steady current of ( 2 A ) was passed through two electrolytic cells ( boldsymbol{A} ) and ( B ) containing electrolytes ( Z n S O_{4} ) and ( C u S O_{4} ) connected in series, ( 2 g ) of ( C u ) were deposited at the cathode of cell ( B ) How long did the current flow? What mass of ( Z n ) was deposited at cathode of cell ( boldsymbol{A} ) ? [Atomic mass: ( C u= ) ( mathbf{6 3 . 5 g} mathbf{m o l}^{-mathbf{1}}, mathbf{Z n}=mathbf{6 5 g} mathbf{m o l}^{-mathbf{1}} ; mathbf{1} mathbf{F}= ) ( left.96500 C m o l^{-1}right] ) | 12 |

89 | Why is anode in galvanic cell considered to be -ve and cathode to be +ve electrode? | 12 |

90 | If four moles of electrons are transferred from anode to cathode in a experiment on electrolysis of water, then total volume of the two gases produced at STP will be: ( mathbf{A} cdot 224 L ) B. ( 72.6 L ) c. ( 67.2 L ) D. ( 89.4 L ) | 12 |

91 | The correct order of equivalent conductance at infinite dilution of ( L i C l, N a C l ) and ( K C l ) is : A. ( L i C l>N a C l>K C l ) в. ( K C l>N a C l>L i C l ) c. ( N a C l>K C l>L i C l ) D. ( L i C l>K C l>N a C l ) | 12 |

92 | An element ( A ) combines with oxygen to form an oxide ( A O . ) This oxide is electrically conducting. Find (A) the number of valence electrons in ( A ) (B) the group to which the element ( boldsymbol{A} ) belongs (C) the formula of the compound when ( A ) reacts with chlorine | 12 |

93 | For a reaction, ( boldsymbol{A}(s)+mathbf{2} boldsymbol{B}^{+} leftrightharpoons boldsymbol{A}^{2+}+ ) ( 2 B, K_{c} ) has been found to be ( 10^{12} ). The ( boldsymbol{E}_{c e l l}^{o} ) is: A . ( 0.354 V ) в. ( 0.708 V ) c. ( 0.0098 V ) D. ( 1.36 V ) | 12 |

94 | The resistance of a conductivity cell containing ( 0.001 M K C l ) solution at ( 298 K ) is ( 1500 Omega . ) What is the cell constant (in ( mathrm{mm}^{-1} ) ) if the conductivity of ( 0.001 M K C l ) solution is ( 2 times 10^{-3} mathrm{s} ) ( mathrm{mm}^{-1} ? ) | 12 |

95 | Assertion: Input of energy is required by electrolytic cells. Reason: Electrolytic cells have just one container, while voltaic cells have two A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

96 | Which one is/ are correct among the following? Given, the half cell emf’s ( E_{C u^{+2} / C u}^{0}= ) | 12 |

97 | Nickel and cadmium are used in combination. A. As a catalyst B. In alloys that can resisthigh pressure c. In electric batteries having a very long life D. In cooking utensils | 12 |

98 | The EMF (in Volts) for the following electrodes are ( boldsymbol{P t}, boldsymbol{H}_{2} mid boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}(boldsymbol{p} boldsymbol{H}=mathbf{2 . 0}) ) | 12 |

99 | State Kohlrausch Law, and write mathematical expression of molar conductivity of the given solution at infinite dilution. | 12 |

100 | A device that converts energy of combustion of fuels like hydrogen and methane, directly into electrical energy is known as: A. dynamo B. Ni-Cd cell c. fuel cell D. electrolytic cell | 12 |

101 | Normal calomel electrode has e.m.f. of ( 0.67 mathrm{V} ) at ( 25^{circ} mathrm{C} ). Calculate pH of solution. The oxidation potential of calomel electrode on ( H ) scale is ( 0.28 V ) (nearest integer). | 12 |

102 | The weight of gold formed when 1 faraday of electricity is passed through water solution of gold (III) chloride is : A. One gram atom of Au B. 2 gram atom of Au c. 3 gram atom of Au D. ( 1 / 3 ) gram atom of Au | 12 |

103 | Consider the cell; ( boldsymbol{V}^{2+}+boldsymbol{V} boldsymbol{O}^{2+}+boldsymbol{2} boldsymbol{H}^{+} rightarrow boldsymbol{2} boldsymbol{V}^{3+}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ; boldsymbol{E}^{o}=mathbf{0 . 6 1 6} boldsymbol{V} ) ( boldsymbol{V}^{3+}+boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{V} boldsymbol{O}^{2+}+ ) ( mathbf{2} boldsymbol{H}^{+}+boldsymbol{A} boldsymbol{g} ; boldsymbol{E}^{o}=mathbf{0 . 4 3 9} boldsymbol{V} ) Potential of ( boldsymbol{E}_{boldsymbol{V}^{3+} / boldsymbol{V}^{2+}}^{boldsymbol{o}} ) is : (Given that ( left.boldsymbol{E}_{A g^{+} / A g}^{o}=mathbf{0 . 7 9 9} boldsymbol{V}right) ) A. ( -0.256 V ) ( v ) B. ( 0.256 mathrm{V} ) c. ( 1.055 V ) D. ( 0.177 V ) | 12 |

104 | A quantity of electrical charge that brings about the deposition of ( 4.5 g A l ) from ( A l^{3+} ) at the cathode will also produce the following volume at ( (boldsymbol{S T P}) ) of ( boldsymbol{H}_{2}(boldsymbol{g}) ) from ( boldsymbol{H}^{+} ) at the cathode A . ( 44.8 L ) B. 22.4 L c. ( 11.2 L ) D. ( 5.6 L ) | 12 |

105 | The standard reduction potentials of ( C u^{2+} mid C u ) and ( C u^{2+} mid C u^{oplus} ) are 0.337 V and ( 0.153 mathrm{V} ), respectively. The standard electrode potential of ( C u oplus mid C u ) half cell is: A . ( 0.184 mathrm{v} ) в. 0.827 c. ( 0.521 mathrm{v} ) D. 0.490 | 12 |

106 | A ( 0.5 ~ M ) Na ( O H ) solution offers a resistance of 31.6 ohm in a conductivity cell at room temperature. What shall be the approximate molar conductance of this ( N a O H ) solution if cell constant of the cell is ( 0.367 mathrm{cm}^{-1} ? ) A ( cdot 234 S mathrm{cm}^{2} ) mole ( ^{-1} ) B. ( 23.2 mathrm{S} mathrm{cm}^{2} ) mole ( ^{-1} ) c. ( 4645 S mathrm{cm}^{2} ) mole ( ^{-1} ) D. ( 5464 S mathrm{cm}^{2} ) mole ( ^{-1} ) | 12 |

107 | A solution of ( 9.65 A ) flowing for 10 min deposits ( 3.0 g ) of the metal which is monovalent. The atomic mass of the metal is : A . 10 B. 50 c. 30 D. 96.5 | 12 |

108 | toppr Q Type your question Fill in the blanks by choosing an appropriate option. At a particular spot of an object made of iron, ( (i) ) of iron to ferrous ion takes place and that spot behaves as ( (i i) ) Electrons released at ( (i) ) spot move through the metal and ( $ 0 ) to another spot on the metal and reduce oxygen in presence of ( boldsymbol{H}^{+} . ) This spot behave as (iiii). The ferrous ions are further oxidised by atmospheric oxygen to ferric ions which come out as rust, ( (i v) ) and with further production of ( (v) ) ions. ( A cdot(i)- ) Oxidation (ii)- Anode, (iii)-Cathode, (iv)( F e_{2} O_{3} cdot x H_{2} O,(v)-H y d r o g e n ) B. (i)- Reduction, (ii)-Cathode, (iii)-Anode, (iv)- ( F e_{3} O_{4},(v) ) Hydrogen C . (i)-Oxidation, (ii)-Cathode, (iii)-Anode, (iv)( F e_{2} O_{3} x H_{2} O,(v)-H y d r o g e n ) D. (i)-Oxidation, (ii)-Anode, (iii)-Cathode, (iv)- ( F e_{2} O_{3} ) ( H_{2} O,(v) ) -Ferrous | 12 |

109 | The reduction potential at ( mathrm{pH}=14 ) for the ( boldsymbol{C u}^{2+} / boldsymbol{C u} ) couples is: ( left[mathrm{Given}, boldsymbol{E}_{boldsymbol{C u}^{2+} / boldsymbol{C u}}^{boldsymbol{o}}=right. ) ( left.mathbf{0 . 3 4} boldsymbol{V} ; quad boldsymbol{K}_{s p} boldsymbol{C u}(boldsymbol{O H})_{2}=mathbf{1} times mathbf{1 0}^{-mathbf{1 9}}right] ) A . ( 0.34 mathrm{V} ) в. ( -0.34 mathrm{V} ) c. ( 0.22 V ) D. ( -0.22 V ) | 12 |

110 | Sea water is a good conductor of electricity but distilled water is not because: A. sea water contains mineral salts B. distilled water contains mineral. c. both A and B D. none of the above | 12 |

111 | Calculate the cell EMF in mV for: ( boldsymbol{P t}left|boldsymbol{H}_{2}(boldsymbol{1} boldsymbol{a} boldsymbol{t m})right| boldsymbol{H} boldsymbol{C l}(boldsymbol{0} . boldsymbol{0} boldsymbol{1} boldsymbol{M})|boldsymbol{A} boldsymbol{g} C l(s)| boldsymbol{A} ) if ( Delta G_{t}^{o} ) values are at ( 25^{circ} mathrm{C} ) ( -109.56 frac{k J}{m o l} ) for ( A g C l(s) ) and ( -130.79 frac{k J}{m o l} ) for ( left(H^{+}+C l^{-}right)(a q) ) A ( .456 m V ) в. ( 654 m V ) c. ( 546 m V ) D. None of these | 12 |

112 | How much electricity in terms of Faraday is required to produce 40.0 g of ( A l ) from molten ( A l_{2} O_{3} ? ) A. 1 Faraday B. 2 Faraday c. 3.2 Faraday D. 4.44 Faraday | 12 |

113 | The EMF of a cell corresponding to the reaction: ( boldsymbol{Z} boldsymbol{n}(boldsymbol{s})+boldsymbol{2} boldsymbol{H}^{oplus}(boldsymbol{a} boldsymbol{q}) rightarrow ) ( Z n^{2+}(0.1 M)+H_{2}(g, 1 a t m) ) is ( 0.82 V ) ( operatorname{at} 25^{circ} C ) The pH of the solution at the hydrogen electrode is: ( boldsymbol{E}_{Z n^{2+} mid boldsymbol{Z n}}^{ominus}=-mathbf{0 . 7 6} boldsymbol{V} ) ( boldsymbol{E}_{boldsymbol{H}^{ominus} mid boldsymbol{H}_{2}}^{Theta}=mathbf{0} ) If the value is ( 63 times 10-x ), then what is the value of ( x ? ) | 12 |

114 | The passage of electricity in the Daniell cell when ( mathrm{Zn} ) and ( mathrm{Cu} ) electrodes are connected: A. from Cu to Zn inside the cell B. from Cu to Zn outiside the cell c. from zn to Cu outside the cell D. none of the above | 12 |

115 | The chemical effect produced by an electric current depends on: A. the nature of electrode B. the tester c. the conducting solution D. none of the above | 12 |

116 | In a Daniel cell when ( C u ) and ( Z n ) electrodes are connected current flows from: A. ( C u ) to ( Z n ) within the cell B. ( C u ) to ( Z n ) outside the cell c. ( Z n ) to ( C u ) outside the cell D. all of the above | 12 |

117 | Alloy formation gives rise to: A. decrease in corrosion B. increase in hardness C . decrease in conductivity D. All are correct | 12 |

118 | State True or False. It is not necessary that both oxidation and reduction should takes place in the same redox reaction. A. True B. False | 12 |

119 | When electricity is passed through molten ( A l C l_{3}, 13.5 g ) of ( A l ) is deposited. The number of Faraday’s must be: A . 0.5 в. 1.0 c. 1.5 D. 2.0 | 12 |

120 | ( boldsymbol{C u}left|boldsymbol{C u}^{+2}(mathbf{1} boldsymbol{M})right|left|boldsymbol{Z} boldsymbol{n}^{+2}(mathbf{1} boldsymbol{M})right| boldsymbol{Z} boldsymbol{n} ) A cell represented above should have emf: A. positive B. negative c. zero D. cannot be predicted | 12 |

121 | Which are true for a standard hydrogen electrode? This question has multiple correct options A. The hydrogen ion concentration is 1 m B. Temperature is ( 25^{circ} mathrm{C} ) c. Pressure of hydrogen is 1 bar D. It contains a metallic conductor which does not absorb hydrogen | 12 |

122 | Question 11. How will the pH of brine (aq. NaCl solution) be affected when it is electrolysed? | 12 |

123 | Selenium has the unusual property of being a good conductor in light but a poor conductor in the dark. It was, therefore, used in making. A. Shaded glass B. Photo-electric cells c. Photo chemical celles D. Chromatic lenses | 12 |

124 | The standard reduction potential for ( C u^{2+} / C u ) is +0.34 V. What will be the reduction potential at ( mathrm{pH}=14 ?[ ) Given: ( left.boldsymbol{K}_{s p} text { of } boldsymbol{C u}(boldsymbol{O H})_{2} text { is } mathbf{1 . 0} times mathbf{1 0}^{-mathbf{1 9}}right] ) A . ( 2.2 v ) в. 3.4v c. ( -0.22 v ) D . ( -2.2 v ) | 12 |

125 | From the standard potential in acidic medium as shown in the following la- timer diagram, the value of ( left(boldsymbol{E}_{1}^{mathbf{0}}+boldsymbol{E}_{2}^{0}right) ) in volts is: | 12 |

126 | ( boldsymbol{P t}left|boldsymbol{O}_{2}(boldsymbol{g}, boldsymbol{1} boldsymbol{a} boldsymbol{t m})right| boldsymbol{O} boldsymbol{H}^{-}(boldsymbol{1} boldsymbol{M}) | boldsymbol{C l}^{-}(boldsymbol{1} boldsymbol{M}) mid ) For the given cell, the cell reaction is: | 12 |

127 | During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to ( 1.139 g m L^{-1} . H_{2} S O_{4} ) of density ( 1.294 g m L^{-1} ) is ( 39 % ) and that of density ( 1.139 g m L^{-1} ) is ( 20 % ) by weight.The battery holds 3.5 L of acid and the volume practically remains constant during discharge. The number of ampere hours for which the battery must have been used are.. The discharging and charging reactions | 12 |

128 | toppr ( t ) Q Type your question ( A ) ( B ) ( c ) ( D ) | 12 |

129 | 0.3 Which of the following statement is correct? (a) Ecell and A, G of cell reaction both are extensive properties (b) Ecell and A, G of cell reaction both are intensive properties (c) Ecell is an intensive property while A.G of cell reaction is an extensive property (d) Ecell is an extensive property while A,G of cell reaction is an intensive property Thinking Process This problem is based on thermodynamical concept of intensive and extensive property During answering this question must keep in mind that intensive property is independent on number of particles and extensive property is dependent on number of particles. | 12 |

130 | Consider the cell: ( boldsymbol{A} boldsymbol{g}(boldsymbol{s}), boldsymbol{A} boldsymbol{g} boldsymbol{C l}(boldsymbol{s})|boldsymbol{K} boldsymbol{C l}(boldsymbol{0} cdot mathbf{1} boldsymbol{M})| boldsymbol{H} boldsymbol{g}_{2} boldsymbol{C l}_{2}(boldsymbol{s}) ) The cell potential This question has multiple correct options A . increases on increasing concentration of ( C l^{-} ) ions B. decreases on decreasing concentration of ( C l^{-} ) ions c. is independent of concentration of ( C l^{-} ) ions. D. is independent of amounts of ( A g C l ) and ( H g_{2} C l ) | 12 |

131 | At ( 25^{circ} mathrm{C} ), the molar conductances at infinite dilution for the strong electrolytes ( N a O H, N a C l ) and ( B a C l_{2} ) ( operatorname{are} 248 times 10^{-4}, 126 times 10^{-4} ) and ( 280 times ) ( 10^{-4} S m^{2} m o l^{-1} ) respectively. ( wedge_{m}^{circ} B a(O H)_{2} ) in ( S m^{2} m o l^{-1} ) is : A. ( 52.4 times 10^{-4} ) В. ( 524 times 10^{-4} ) c. ( 402 times 10^{-4} ) ( mathbf{D} cdot 262 times 10^{-4} ) | 12 |

132 | Question 3. Depict the galvanic cell in which the reaction, Zn(s) + 2Ag* (aq) → Zn2+ (aq) + 2Ag(s) takes place. Further show: i) Which of the electrode is negatively charged? (ü) The carriers of the current in the cell. (iii) Individual reaction at each electrode. Anode is negative electrode and cathode is positive electrode. Anode is always the site of oxidation and cathode is the site of reduction. In a galvanic cell. anode half-cell is written on the left and cathode half-cell on right. Salt bridge is represented as (parallel lines). | 12 |

133 | Among ( N a, H g, S, P t ) and graphite, which can be used as electrodes in electrolytic cells having aqueous solutions? A. ( H g ) and ( P t ) в. ( H g, P t ) and graphite c. ( N a ) and ( S ) D. ( N a, H g ) and ( S ) | 12 |

134 | The reaction, [ begin{array}{c} (mathbf{1} / mathbf{2}) boldsymbol{H}_{mathbf{2}}(boldsymbol{g})+boldsymbol{A} boldsymbol{g} boldsymbol{C} boldsymbol{l}(boldsymbol{s})= \ boldsymbol{H}+(boldsymbol{a} boldsymbol{q})+boldsymbol{C} boldsymbol{l}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{A} boldsymbol{g}(boldsymbol{s}) text { occurs in } end{array} ] the galvanic cell The correct cell representation is given by ( mathbf{A} cdot A g|A g C l(s)| K C l(s o l n .)left|A g N O_{3}(s o l n .)right| A g ) B ( cdot P tleft|H_{2}(g)right| H C l(text {soln.}) mid A g N O_{3}(text {soln.}) mid A g ) ( mathbf{c} cdot P tleft|H_{2}(g)right| H C l(s o l n .)|A g C l(s)| A g(s) ) D ( cdot P tleft|H_{2}(g)right| K C l(s o l n .)|A g C l(s)| A g ) | 12 |

135 | The amount of ion discharged during electrolysis is not directly proportional to A . resistance B. time c. current D. chemical equivalent of ion | 12 |

136 | A cell contains two hydrogen electrodes. The negative electrode is in contact with a solution of ( 10^{-6} mathrm{M} ) hydrogen ions. The ( E M F ) of the cell is ( 0.118 V ) at ( 25^{circ} C . ) The concentration of hydrogen ions at the positive electrode is: A ( cdot 10^{-4} M ) В. ( 10^{-3} M ) ( mathrm{c} cdot 10^{-1} M ) D. None of these | 12 |

137 | Which of the following is free of salts? A. Distilled water B. Sea water c. tap water D. All of the above | 12 |

138 | The efficiency of fuel cell is given by the expression, ( eta ) is: A ( quad eta=-frac{n F E_{c l l}}{Delta H} times 100 ) B. ( eta=-frac{n F E_{c l l l}}{Delta S} times 100 ) c. ( _{eta}=-frac{n F E_{c l l}}{Delta A} times 100 ) D. None of the above | 12 |

139 | 0.30 Under what condition is E cell = 0 or A, G = 0 ? | 12 |

140 | For how long current of ( 3 mathrm{A} ) has to passed through ( A g N O_{3} ) solution to coat a metal surface of ( 80 mathrm{cm}^{2} ) area and thickness of ( 5 times 10^{-4} c m . ) The density of silver is ( 10.5 mathrm{gm} / mathrm{cm}^{3} ) | 12 |

141 | When electric current passes through the filaments of a bulb, it starts emitting light due to : A. heating effect of electric current. B. magnetic effect of electric current. c. chemical effect of electric current D. lighting effect of electric current. | 12 |

142 | In the electrochemical cell shown above, which of the following half-reactions occurs at the anode? ( mathbf{A} cdot C u^{2+}+e rightarrow C u^{-} ) B ( cdot Z n(s) rightarrow Z n^{2+}+2 e ) ( mathbf{c} cdot Z n^{2+}+2 e rightarrow Z n(s) ) ( mathbf{D} cdot C u(s) rightarrow C u^{2+}+2 e ) E ( cdot C u^{2+}+2 e rightarrow C u(s) ) | 12 |

143 | The e.m.f. of the cell begin{tabular}{l|c||c|c} ( boldsymbol{P t} boldsymbol{H}_{2} ) & ( boldsymbol{H O C N} ) & ( boldsymbol{A} boldsymbol{g}^{+} ) \ ( boldsymbol{1} boldsymbol{a} boldsymbol{t m} ) & ( boldsymbol{1} . boldsymbol{3} times mathbf{1 0}^{-boldsymbol{3}} boldsymbol{M} ) & ( boldsymbol{0 . 8} boldsymbol{M} ) end{tabular} mid ( boldsymbol{A} boldsymbol{g}(s) ) is ( 0.982 mathrm{V} . ) The ( mathrm{K}_{a} ) for HOCN is : ( boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{e} rightarrow boldsymbol{A} boldsymbol{g}(boldsymbol{s}) ; boldsymbol{E}^{o}=mathbf{0 . 8 0} boldsymbol{V} ) A. ( 3.33 times 10^{-4} ) B . ( 2.22 times 10^{-4} ) c. ( 4.44 times 10^{-4} ) D. ( 1.6 times 10^{-3} ) | 12 |

144 | Question 13. Write the chemistry of recharging the lead storage battery, highlighting all the materials that are involved during recharging. Recall the reactions during use of battery and reverse them. | 12 |

145 | 5th Question 23. Consider the following diagram and answer the questions Pe 6) to (vi) given below. (1) Redraw the diagram to show the direction of electron flow. Salt bridge Zinc plate Silver plate Ag+ (aq) Zn2+ (aq) 1 (ii) Is silver plate the anode or cathode? (iii) What will happen if salt bridge is removed (iv) When will the cell stop functioning (v) How will concentration of Znions and Agt ions be affected when the cell functions? (vi) How will the concentration of Zn²+ ions and Agions be affected after the cell becomes ‘dead’? | 12 |

146 | Q15. Define EMF of cell. | 12 |

147 | Construct the cells in which the following reactions are taking place. Which of the electrodes shall act as anode (negative electrode) and which one as cathode (positive electrode)? (a) ( Z n+C u S O_{4}=Z n S O_{4}+C u ) (b) ( boldsymbol{C u}+mathbf{2 A g} boldsymbol{N O}_{3}=boldsymbol{C u}left(boldsymbol{N O}_{3}right)_{2}+ ) ( mathbf{2} boldsymbol{A} boldsymbol{g} ) ( (c) Z n+H_{2} S O_{4}=Z n S O_{4}+H_{2} ) (d) ( boldsymbol{F} boldsymbol{e}+boldsymbol{S} boldsymbol{n} boldsymbol{C l}_{2}=boldsymbol{F} boldsymbol{e} boldsymbol{C l}_{2}+boldsymbol{S} boldsymbol{n} ) | 12 |

148 | Which of the following solution will not make the bulb glow? A. Copper sulphate B. Sodium chromate c. Potassium dichromate D. Sugar | 12 |

149 | The conductivity of N/10 KCl solution at ( 20^{circ} mathrm{C} ) is ( 0.0212 mathrm{Scm}^{-1} ) and the resistance of cell containing this solution at ( 20^{circ} C ) is 55 ohm. The cell constant is: A ( .2 .173 mathrm{cm}^{-1} ) B. ( 1.166 mathrm{cm}^{-1} ) c. ( 4.616 mathrm{cm}^{-1} ) D. ( 3.324 c m^{-1} ) | 12 |

150 | On passing one faraday of electricity through a dilute solution of an acid, the volume of hydrogen obtained at NTP is A. ( 22400 m L ) B. ( 1120 m L ) c. ( 2240 m L ) D. ( 11200 m L ) | 12 |

151 | What is the chemical formula of rust? | 12 |

152 | 44 which reference electrode is used to measure the electrode potential of other electrodes? | 12 |

153 | If ( boldsymbol{E}^{o}_{boldsymbol{F} e^{2+} / boldsymbol{F} e}=boldsymbol{x}_{1} boldsymbol{V} ) and ( boldsymbol{E}^{o}_{boldsymbol{F} e^{3+} / boldsymbol{F} e^{2+}}= ) ( boldsymbol{x}_{2} boldsymbol{V}, ) then ( boldsymbol{E}^{o} boldsymbol{F e}^{3+} / boldsymbol{F} e ) will be : A ( cdotleft(2 x_{1}+x_{2}right) V ) В . ( left(3 x_{2}-x_{1}right) V ) ( mathbf{c} cdotleft(2 x_{1}+x_{2}right) / 3 V ) ( mathbf{D} cdotleft(x_{1}+2 x_{2}right) / 3 V ) | 12 |

154 | The electrochemical cell stops working after some time because: A. electrode potentials of both electrodes becomes zero B. electrode potentials of both electrodes becomes equal C. temperature of the cell increases D. the reaction starts proceeding in opposite direction | 12 |

155 | What is the electric current required to deposit 0.972 g of chromium in three hours? (E.C.E. of chromium is 0.00018 g/c) A . ( 0.50 A ) B. 1A c. zero D. 2.5A | 12 |

156 | Most liquids that conduct electricity are solutions of : A . acids B. bases c. salts D. all of the above | 12 |

157 | The Kohlrausch law is realted to: A. Conductance of ions at infinite dilution B. Independent migration of ions C. Both (a) and (b) D. neither (a) and (b) | 12 |

158 | Iron rod is immersed in ( K C l K C l ) solution such that half its length is exposed to air and the other half immersed in ( K C l K C l ) solution. The part corroded faster is | 12 |

159 | The capacity of cell is measured in: A. amperes B. ampere-hour c. watts D. watt-hours | 12 |

160 | Calculate the e.m.f of the following cell reaction at ( 298 K: ) ( boldsymbol{M} boldsymbol{g}_{(s)}+boldsymbol{C u}^{2+}(mathbf{0 . 0 0 0 1 M}) rightarrow ) ( M g^{2+}(0.001 M)+C u_{(s)} ) The standard potential ( left(boldsymbol{E}^{o}right) ) of teh cell is ( 2.71 V ) | 12 |

161 | EMF of the cell ( Z nleft|Z n S O_{4}(a=0.2)right|left|Z n S O_{4}left(a_{2}right)right| Z n ) is ( -0.0088 mathrm{V} ) at ( 25^{circ} mathrm{C} ). Calculate the value of ( a_{2} ) A ( cdot a_{2}=0.1006 mathrm{M} ) В . ( a_{2}=0.2012 M ) ( mathbf{c} cdot a_{2}=0.3018 M ) D. None of these | 12 |

162 | ( M g^{2+}+2 e^{-} rightarrow M g ; E_{c e l l}^{circ}(V)=-2.37 ) ( boldsymbol{C u}^{2+}+mathbf{2} e^{-} rightarrow boldsymbol{C u} ; boldsymbol{E}_{c e l l}^{circ}=mathbf{0 . 3 4} ) Analyze the data above. Which substance should be used for electrode B in this galvanic cell? A ( cdot M g^{2} ) в. ( M g ) ( c cdot C u^{2} ) D. ( C_{7} ) | 12 |

163 | Chemical compounds which conduct electricity in the fused or in aqueous solution state and undergo chemical decomposition due to the flow of current through it are known as: A. electrolytes B. non-electrolytes c. weak electrolytes D. all of the above | 12 |

164 | The fraction of the total current carried by an ion is known as: A. transport number of that ion B. conductance of that ion c. both (A) and (B) D. none of the above | 12 |

165 | Which of the following reactions occur at the cathode during the charging of lead storage battery? ( mathbf{A} cdot P b^{2+}+2 e^{-} rightarrow P b ) B ( cdot P b^{2+}+S O_{4}^{2-} rightarrow P b S O_{4} ) ( mathbf{c} cdot P b rightarrow P b^{2+}+2 e^{-} ) D ( cdot P b S O_{4}+2 H_{2} O rightarrow P b O_{2}+4 H^{+}+S O_{4}^{2-}+2 e^{-} ) | 12 |

166 | The density and eq. wt. of a metal are ( 10.5 g c m^{-3} ) and ( 100, ) respectively. The time required for a current of 3 amp to deposit a 0.005 mm thick layer of the same metal on an area of ( 80 mathrm{cm}^{2} ) is closest to: ( mathbf{A} cdot 120 s ) B. 135 s c. ( 67.5 s ) D. 270 ( s ) | 12 |

167 | At ( 25^{circ} C lambda_{infty}left(H^{+}right)=3.4982 times ) ( 10^{-2} S m^{2-1} lambda_{infty}left(O H^{-}right)=1.98 times ) ( 10^{-2} mathrm{Sm}^{2-1} ) Given: Sp. conductance ( =mathbf{5 . 1} times ) ( 10^{-6} S m^{-1} ) for ( H_{2} O, ) determine ( p H ) and ( boldsymbol{K}_{boldsymbol{w}} ) | 12 |

168 | The value of equilibrium constant for a feasible cell reaction is: ( mathbf{A} cdot1 ) D. zero | 12 |

169 | Iron nails rust fast when used for fixing plates or strips of aluminium on a building. Similarly, a water pipe made of iron corrodes faster when connected to a pipe of copper. This happens because of the? A. Greater wetting of iron B. Easier flow of electrons to iron c. Higher rusting power of iron D. Chemical reduction of iron | 12 |

170 | In following cell reaction ( M g(s)+2 A g^{+}(0.001 M) rightarrow ) ( M g^{2+}(0.20 M)+2 A g(s) ) Calculate ( E_{text {cell}} ) for the reaction ( left[E^{o}=right. ) ( left.mathbf{3 . 1 7} boldsymbol{V}, frac{mathbf{2 . 3 0} boldsymbol{R} boldsymbol{T}}{boldsymbol{F}}=mathbf{0 . 0 5 4}right] ) ( A cdot 2.63 V ) B. 3.01V c. ( 3.33 v ) D. 3.51V | 12 |

171 | Why does anode material have good hydrogen storage capacity for a Nickelmetal hydride battery? | 12 |

172 | 0.39 How will the pH of brine (aq NaCl solution) be affected when it is electrolysed? | 12 |

173 | ( C u^{2+}+2 e^{-} rightarrow C u ) ( boldsymbol{E}_{text {red}} boldsymbol{v s} cdot log left[boldsymbol{C u}^{2+}right] ) graph is of the type as shown in figure where ( O A=0.34 V ) then electrode potential of the half cell of ( C u mid C u^{2+}(0.1 M) ) will be : A. ( _{-0.34}+frac{0.0591}{2} mathrm{V} ) В. ( 0.34+0.0591 V ) ( c .0 .34 V ) D. none of thes | 12 |

174 | ( boldsymbol{N} boldsymbol{i}left|boldsymbol{N} boldsymbol{i}^{2+}(boldsymbol{1} . boldsymbol{0} boldsymbol{M}) | boldsymbol{A} boldsymbol{u}^{3+}(mathbf{1} . boldsymbol{0} boldsymbol{M})right| boldsymbol{A} boldsymbol{u} ) (where ( boldsymbol{E}^{o} ) for ( boldsymbol{N} boldsymbol{i}^{2+} / boldsymbol{N} boldsymbol{i} ) is ( -mathbf{0 . 2 5} ) and ( boldsymbol{V} ) and ( E^{o} ) for ( A u^{3+} / A u ) is ( 0.150 V ) ). What is the emf of the cell? A ( .+0.4 V ) в. ( -1.75 V ) ( mathrm{c} .+1.25 mathrm{V} ) D. ( +1.75 V ) | 12 |

175 | The reaction ( mathbf{1} / mathbf{2} boldsymbol{H}_{mathbf{2}}(boldsymbol{g})+boldsymbol{A} boldsymbol{g} boldsymbol{C l}(boldsymbol{s}) rightarrow boldsymbol{H}^{oplus}(boldsymbol{a} boldsymbol{q})+ ) ( boldsymbol{C l}^{ominus}(boldsymbol{a q})+boldsymbol{A} boldsymbol{g}(boldsymbol{s}) ) occurs in the galvanic cell: A ( cdot A g|A g C l(s)| K C l(s o l)left|A g N O_{3}right| A g ) B . ( P tleft|H_{2}(g)right| H C l(s o l)left|A g N O_{3}(s o l)right| A g ) c. ( P tleft|H_{2}(g)right| H C l(s o l)|A g C l(s)| A g ) D. ( P tleft|H_{2}(g)right| K C l(s o l)|A g C l(s)| A g ) | 12 |

176 | The standard reduction potential values, ( boldsymbol{E}^{circ}left(boldsymbol{B} boldsymbol{i}^{3+} / boldsymbol{B} boldsymbol{i}right) ) and ( E^{circ}left(C u^{2+} / C uright) ) are ( 0.226 mathrm{V} ) and ( 0.344 mathrm{V} ) respectively. A mixture of salts of bismuth and copper at unit concentration each is electrolysed at ( 25^{circ} mathrm{C} . ) To what value ( operatorname{can}left[C u^{2+}right] ) be brought down before bismuth starts to deposit, in electrolysis. ( mathbf{A} cdotleft[C u^{2+}right]=10^{-8} M ) B. ( left[C u^{2+}right]=10^{-4} M ) ( mathbf{C} cdotleft[C u^{2+}right]=10^{-3} M ) D. ( left[C u^{2+}right]=10^{-6} M ) | 12 |

177 | For a cell reaction involving a two-electron change, the standard emf of the cell is found to be ( 0.295 mathrm{V} ) at ( 25^{circ} mathrm{C} ). The equilibrium constant of the reaction at ( 25^{circ} mathrm{C} ) will be : A ( cdot 1 times 10^{-10} ) B . ( 29.5 times 10^{-2} ) c. 10 D. ( 1 times 10^{10} ) | 12 |

178 | The potential of hydrogen electrode having a solution of ( mathrm{pH}=4 ) at ( 298 mathrm{K} ) is: A. ( -0.177 V ) B. ( -0.236 V ) c. ( 0.177 V ) D. ( 0.236 V ) | 12 |

179 | The cell constant of a given cell is ( 0.47 mathrm{cm}^{-1} . ) The resistance of a solution placed in this cell is measured to be 31.6 ohm. The conductivity of the solution ( left(text { in } S c m^{-1} text {where } S ) has usual right. meaning) is : A . 0.15 в. 1.5 c. 0.015 D. 150 | 12 |

180 | What will be the reduction potential for the following half-cell reaction at ( 298 mathrm{K} ? ) (Given: ( left[boldsymbol{A} boldsymbol{g}^{+}right]=mathbf{0 . 1} mathbf{M} ) and ( boldsymbol{E}_{c e l l}^{o}=+mathbf{0 . 8 0} ) ( mathbf{V}) ) A . ( 0.741 mathrm{v} ) B. ( 0.80 v ) c. ( -0.80 v ) D. ( -0.741 mathrm{V} ) | 12 |

181 | Assertion When an electric current is passed through an aqueous solution of sodium chloride, sodium ions move towards cathode and chloride ions move towards anode. Reason Cathode is a negatively charged electrode and therefore attracts ( mathrm{Na}^{+} ) ions. Anode is a positively charged electrode and therefore attracts ( mathrm{Cl}^{-} ) ions. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

182 | An electrolysis of a oxytungsten complex ion using ( 1.10 A ) for 40 min produces ( 0.838 g ) of tungsten. What is the charge of tungsten in the material? (Atomic weight: ( boldsymbol{W}=mathbf{1 8 4} ) ) A . 6 B. 3 ( c .5 ) D. | 12 |

183 | Which of the following reaction is used to make a fuel cell? ( mathbf{A} cdot C d(s)+2 N i(O H)_{3}(s)+H_{2} O(l) longrightarrow C d O(s)+ ) [ 2 N i(O H)_{3}(s)+H_{2}(g) ] B ( .2 mathrm{Fe}(s)+mathrm{O}_{2}(g)+4 H^{+}(a q) longrightarrow 2 mathrm{Fe}^{2+}(a q)+2 mathrm{H}_{2} mathrm{O}(l) ) ( mathbf{c} cdot P b(s)+P b O_{2}(g)+2 H_{2} S O_{4}(a q) longrightarrow 2 P b S O_{4}(s)+ ) ( 2 H_{2} O(l) ) D. ( 2 H_{2}(g)+O_{2}(g) longrightarrow 2 H_{2} O(l) ) | 12 |

184 | Water obtained from which of the following sources is a good conductor of electricity? A . Tap B. Ponds c. wells D. All of the above | 12 |

185 | In voltaic cell, oxidation takes place at: A . positive electrode B. negative electrode c. cathode D. none of the above | 12 |

186 | Observe the following picture and answer the following question: What is corrosion? | 12 |

187 | Which of the following is used to detect the current? A . Tester B. LED c. compass needle D. All of the above | 12 |

188 | Some oils and fats give a bad smell and taste because of A. rancidity B. decomposition reaction c. hydrogenation reaction D. double displacement reaction | 12 |

189 | A standard hydrogen electrode has zero electrode potential because: A. hydrogen is easiest to oxidise B. this electrode potential is assumed to be zero c. hydrogen atom has only one electron D. hydrogen is the lightest element | 12 |

190 | What is a cathode? A. Electrode where reduction takes place and electrons are gained. B. Electrode where oxidation takes place and electrons are lost. C. Electrode where reduction takes place and electrons are lost. D. A fluid that conducts electricity. E. Electrode where oxidation takes place and electrons a re gained. | 12 |

191 | The products obtained at cathode and anode on electrolysis of aqueous sodium succinate are : A. anode: ethene ( +C O_{2} ), cathode : ( H_{2} ) B. anode: ethyne ( +C O_{2} ), cathode : ( H_{2} ) c. anode : ethyne + ( H_{2} ), cathode : Na D. anode: ethyne ( +C O_{2} ), cathode : Na | 12 |

192 | What weight of zinc will get deposited? A . 65.3 g B. 0.33 mg c. 0.438 g D. 42.3 ( g ) | 12 |

193 | Which of the following is true for electrolytic refining? A. Pure metal is used at anode and impure metal at cathode B. Pure metal is used at cathode and impure metal at anode c. Both can be possible A and B D. None of these | 12 |

194 | State True or False. The redox reaction involved in galvanic cell is a non-spontaneous process. A. True B. False | 12 |

195 | If the molar conductivities (in ( mathrm{S} mathrm{cm}^{2} ) ( mathrm{mol}^{-1} ) ) of ( mathrm{NaCl} ), ( mathrm{KCl} ) and ( mathrm{NaOH} ) at infinite dilution are 126,150 and 250 respectively, the molar conductivity of KOH is: ( left[operatorname{in} mathrm{S} mathrm{cm}^{2} mathrm{mol}^{-1}right] ) A .526 в. 226 c. 26 D. 274 | 12 |

196 | Assertion: In a Daniell cell, electrons flow from zinc electrode to copper electrode outside the cell. Reason: In Daniell cell, Zn electrode is anode and Cu is cathode. A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

197 | Pieces of copper, silver and gold are dropped into a solution of iron sulphate. The piece that will get a coating of copper is: ( A ). iron B. silver c. gold D. None of them | 12 |

198 | How many grams of copper will be deposited from a solution of ( C u S O_{4} ) bypassing 0.5 faradays of electricity? [Atomic weight of ( boldsymbol{C u}=mathbf{6 3 . 5} text { g/mole }] ) A. ( 31.75 mathrm{g} ) B. 63.6 g c. ( 15.875 mathrm{g} ) D. 127 g | 12 |

199 | Electricity can be obtained by oxidation-reduction reaction in voltaic cell. A. True B. False | 12 |

200 | . 36 Consider the following diagram in which an electrochemical cell is coupled to an electrolytic cell. What will be the polarity of electrodes A and ‘B’ in the electrolytic cell? Salt bridge 6) Tlr Zince Copper plate plate Solution Znso. -Cuso. (B) Electrode (A) Electrode Electrolytic cell | 12 |

201 | For a given reaction: ( boldsymbol{F} boldsymbol{e}+boldsymbol{2} boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+} rightarrow boldsymbol{3} boldsymbol{F} boldsymbol{e}^{boldsymbol{2}+} ) | 12 |

202 | ( E^{o} ) of an electrode half reaction is related to ( Delta G^{o} ) by the equation, ( E^{o}= ) ( -Delta G^{o} / n F . ) If the amount of ( A g^{+} ) in the half reaction ( boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g} ) is tripled then: A . n is tripled B. ( Delta G^{o} ) increases to three times c. ( E^{o} ) reduces to one third D. All the above | 12 |

203 | Calculate the number of coulombs required to deposit 6.75 g of ( A l ) when the electrode reaction is: ( boldsymbol{A l}^{3+}+mathbf{3} e^{-} rightarrow boldsymbol{A l} ) | 12 |

204 | How many moles of ( boldsymbol{P t} ) may be deposited on the cathode when ( 0.80 mathrm{F} ) of electricity is passed through a ( 1.0 mathrm{M} ) solution of ( boldsymbol{P} boldsymbol{t}^{4+} ) ? A. 0.1 mol B. 0.2 mol ( c .0 .4 mathrm{mol} ) D. 0.6 mo | 12 |

205 | 18. Standard electrode potential data are useful for understanding the stability of an oxidant in redox titration. Some half-cell reactions and their standard potentials are given below: MnO2 (aq) +8H+ (aq) +5e- Mn2+ (aq) + 4H20 (0) Eº=1.51 V Cryo- (aq) +14H+ (aq) + 6e — 2Cr3+ (aq) +7H2O(C) E° =1.38 V Fe3+ (aq) +é – Fe2+ (aq) E° = + 0.77 V Cl2(g) + 2e 2014 (aq) E° =1.40 V Identify the only incorrect statement regarding the quantitative estimation of aqueous Fe(NO2), (a) MnO2 can be used in aqueous HCI (b) Cr2O3 can be used in aqueous HCI (c) MnOcan be used in aqueous H2SO4 (d) Cr2O2 can be used in aqueous H,SO | 12 |

206 | Assertion: Dry cell is a primary cell and lead storage cell is a secondary cell Reason: A primary cell can only be used once while secondary cells are rechargeable. A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

207 | The conductivity of an electrolytic solution decreases on dilution due to: A. decrease in number of ions per unit volume B. increase in ionic mobility of ions C. increase in percentage ionisation D. increase in number of ions per unit volume | 12 |

208 | Aluminium is more reactive than iron. But aluminium is less easily corroded than iron because: A. aluminium is a noble metal B. oxygen forms a protective oxide layer on aluminium surface C. iron unergoes reaction easily with water D. iron forms both mono and divalent ions | 12 |

209 | Given : Oxidation: ( H_{2} O_{2} rightarrow O_{2}+2 H^{oplus}+2 e^{-} ) ( E^{ominus}=-0.69 V ) ( 2 F^{ominus} rightarrow F_{2}+2 e^{-} ) ( E^{ominus}=-2.87 V ) Reduction: ( H_{2} O_{2}+2 H^{oplus}+2 e^{-} rightarrow 2 H_{2} O ) ( E^{ominus}=-1.77 V ) ( 2 I^{ominus} rightarrow I_{2}+2 e^{-} E^{ominus}=-0.54 V ) Which of the following statements is/are correct? This question has multiple correct options A ( cdot H_{2} O_{2} ) behaves as an oxidant for ( I^{ominus} ) B. ( H_{2} O_{2} ) behaves as a reductant for ( I_{2} ) C. ( H_{2} O_{2} ) behaves as an oxidant for ( F^{ominus} ) D. ( H_{2} O_{2} ) behaves as a reductant for ( F_{2} ). | 12 |

210 | Assertion ( mathrm{E}^{0} ) value of single electrode is determined experimentally by combining the electrode with SHE Reason SHE is taken as a reference electrode A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

211 | The emf ( left(E^{circ}right) ) of the following cells are: ( boldsymbol{A} boldsymbol{g} / boldsymbol{A} boldsymbol{g}^{+}(mathbf{1} boldsymbol{M}) | ) ( boldsymbol{C u}^{2+}(mathbf{1} boldsymbol{M}) mid boldsymbol{C u} ; boldsymbol{E}^{circ}=-mathbf{0 . 4 6} boldsymbol{v o l t} ) ( boldsymbol{Z} boldsymbol{n} / boldsymbol{Z} boldsymbol{n}^{boldsymbol{2}+}(boldsymbol{1} boldsymbol{M}) | ) ( boldsymbol{C u}^{2+}(mathbf{1} boldsymbol{M}) mid boldsymbol{C u} ; boldsymbol{E}^{circ}=+mathbf{1 . 1 0} boldsymbol{v o l t} ) Calculate the emf of the cell: ( boldsymbol{Z} boldsymbol{n}left|boldsymbol{Z} boldsymbol{n}^{2+}(boldsymbol{1} boldsymbol{M}) | boldsymbol{A} boldsymbol{g}^{+}(boldsymbol{1} boldsymbol{M})right| boldsymbol{A} boldsymbol{g} ) | 12 |

212 | A conductivity cell has been calibrated with a ( 0.01 M 1: 1 ) electrolyte solution (specific conductance ( kappa=1.25 times ) ( 10^{-3} mathrm{Scm}^{-1} ) ) in the cell and the measure resistance was ( 800 Omega ) at ( 25^{circ} C ) The cell constant will be: A ( cdot 1.02 mathrm{cm}^{-1} ) В. ( 0.102 c m^{-1} ) c. ( 1.00 mathrm{cm}^{-1} ) D. ( 0.5 mathrm{cm}^{-1} ) | 12 |

213 | If the pressure of ( H_{2} ) gas is increased from 1atm to 100atm keeping ( boldsymbol{H}^{+} ) concentration constant at ( 1 M, ) the change in reduction potential of hydrogen half cell at ( 25^{circ} C ) will be: A. ( 0.059 V ) ( V ) B . ( 0.59 V ) c. ( 0.0295 V ) D. ( 0.118 V ) | 12 |

214 | How many spoons can be electroplated by silver when 7 ampere current is passed through electrolyte cell of ( A g N O_{3} ) for 1.93 hours? ( 0.01 g m A g ) layer is deposited on each spoon. ( left(A g=108 g cdot m o l^{-1}right) ) | 12 |

215 | Select the correct statement(s) about NHE. This question has multiple correct options ( mathbf{A} cdot E^{ominus} ) of ( mathrm{NHE} ) is arbitrarilly assumed to be zero. B. ( E^{ominus} ) of NHE is equal to zero. ( mathbf{C} cdot ) NHE refers as ( P t, H_{2}(g) mid H_{a=1}^{oplus}(a q) ) at ( 25^{circ} C ) D. NHE is very susceptible to dissolved ( O_{2}, H_{2} S ), and all other reducing agents. | 12 |

216 | Which of the following is correct statement? A. Conductivity & molar conductivity of solution increase on dilution B. Voltage of button cell remain unchanged through out its life time C. On electrolysis of aqueous ( C u S O_{4} ) using platinum electrode its concentration ( left[C u^{2+}right] ) remain constant D. On electrolysis of aqueous ( N a C l ), solution becomes acidic | 12 |

217 | Which of the following is incorrect in a galvanic cell? A. Oxidation occurs at anode B. Reduction occurs at cathode c. The electrode at which electrons are gained is called cathode D. The electrode at which electrons are lost is called cathode | 12 |

218 | How will you show that air and moisture both are required for rusting of iron? | 12 |

219 | For mercury at ( 0^{circ} mathrm{C} ) specific conductance, ( boldsymbol{K}=mathbf{1 . 0 6 2 9 6 3} times mathbf{1 0}^{mathbf{6}} boldsymbol{S} / boldsymbol{m} ) (a) If the resistance of a cell containing mercury is 0.243166 ohm, What is the cell constant of the cell? (b) If the same cell is fixed with ( K C l ) solution at ( 0^{circ}, ) the resistance of the cell is ( 3.966 times 10^{4} ) ohm. What is the conductivity of ( K C l ) solution? (c) If the average cross-sectional area of the cell is ( 0.9643 m m^{2}, ) what is the effective distance between the electrodes? | 12 |

220 | (a) What type of battery is the lead storage battery? Write the anode and the cathode reactions and the overal reaction occurring in a lead storage battery when current is drawn from it. (b) In the button cell, widely used in watches, the following reaction taken place. ( Z n(s)+A g_{2} O(s)+H_{2} O(l) rightarrow ) ( Z N^{2+}(a q)+2left(A g(s)+2 O H^{-}(a q)right. ) Determine ( E^{o} ) and ( Delta G^{o} ) for the reaction (given: ( boldsymbol{E}_{boldsymbol{beta} boldsymbol{g}^{+} / boldsymbol{A} boldsymbol{g}}=+boldsymbol{0 . 8 0} boldsymbol{V}, boldsymbol{E}_{Z n^{2+} / Z n}^{o}= ) ( -0.76 V) ) | 12 |

221 | State True or False. Corrosion of motor cars is the major problem in the winter, when salt is spread on road to melt ice and snow A. True B. False | 12 |

222 | Two Faraday of electricity is passed through a solution of ( C u S O_{4} . ) The mass of copper deposited at the cathode is at. mass of ( mathrm{Cu}=63.5 text { amu }) ) ( A cdot O g ) в. ( 63.5 mathrm{g} ) ( c cdot 2 g ) D. 127 g | 12 |

223 | Which of the following changes will cause the free energy of the cell reaction to decrease: ( boldsymbol{Z} boldsymbol{n}left|boldsymbol{Z n} boldsymbol{S} boldsymbol{O}_{4(boldsymbol{a q})}(boldsymbol{x}, boldsymbol{M}) | boldsymbol{H} boldsymbol{C l}_{(boldsymbol{a q})}left(boldsymbol{x}_{boldsymbol{2}} boldsymbol{M}right)right| boldsymbol{H} ) This question has multiple correct options ( 200 mathrm{m} ) B. Increase in pressure of hydrogen from 1 atm to 2 atm c. Increase in molarity ( x_{2} ) from 0.1 to 1 M D. Decrease in molarity ( x_{1} ) from 1 M to 0.1 M | 12 |

224 | How much ( O_{2} ) gas will be collected at the anode at ( 300 K ) temperature and 1 bas pressure if 2.5 ampere electric current is passed for one hour in electrolysis of aqueous solution of ( N a_{2} S O_{4} .(F=96500 text { Coulomb) }[1text { mole } ) gas volume is 22.4 litre at STP]. | 12 |

225 | Assertion The mobility of ( N a^{oplus} ) is lower than that of ( boldsymbol{K}^{oplus} ) ion Reason The ionic mobility depends upon the effective radius of the ion. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

226 | A piece granulated zinc was dropped into copper sulphate solution. After sometime the colour of the solution changed from blue to colourless. Why? | 12 |

227 | When the electric current is passed through a cell having an electrolyte, the positive ions move towards cathode and negative ions towards the anode. If the cathode is pulled out of the solution then A. the positive and negative ions will be move towards anode B. the positive ions will start moving towards the anode and while negative ions will stop moving c. the negative ions will continue to move towards and while positive ions will stop moving D. the positive and negative ions will start moving random | 12 |

228 | Assertion Lead storage battery is galvanic cell without salt bridge. Reason A secondary cell is rechargeable cell. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

229 | Electric circuit provides a complete path for: A. solution to flow B. metal to flow c. neutron to flow D. current to flow | 12 |

230 | Which of the following is anodic reaction: ( mathbf{A} cdot S O_{4}^{2-}+H_{2} O rightarrow H_{2} S O_{4}+1 / 2 O_{2}+2 e^{-} ) ( mathbf{B} cdot H^{oplus}+e^{-} rightarrow 1 / 2 H_{2} ) ( mathbf{C} cdot A g^{oplus}+e^{-} rightarrow A g ) D. None of above | 12 |

231 | State True or False. The electrical energy released from an electrochemical cell can do useful work. A. True B. False | 12 |

232 | A current of 2 ampere passing for 5 hours deposits ( 22.2 mathrm{g} ) of tin, the oxidation state of tin is: [At. wt. ( =119] ) A. 0 B. 3 ( c cdot 2 ) D. 4 | 12 |

233 | At ( p H=2, E_{Q u i n h y d r o n e} ) will be: ( left(E_{Q u i h y d r o n e}^{o}=1.30 Vright) ) A . ( 1.36 V ) B . ( 1.30 V ) c. ( 1.42 v ) D. ( 1.20 V ) | 12 |

234 | The equilibrium constant for the following reaction at ( 25^{circ} mathrm{C} ) is ( 2.9 times 10^{9} ) Calculate standard voltage of the cell. ( boldsymbol{C l}_{2(boldsymbol{g})}+boldsymbol{B r}_{(boldsymbol{a q})}^{-} rightleftharpoons boldsymbol{2} boldsymbol{C l}_{(boldsymbol{a q})}^{-} ) ( mathbf{A} cdot 0.18 mathbf{V} ) B. ( 0.22 v ) c. ( 0.26 v ) D. ( 0.28 mathrm{v} ) | 12 |

235 | Water is broken down into its constituent elements …………. and | 12 |

236 | A method of protecting steel and iron from rusting is: A. rusting B. corrosion. c. galvanisation. D. sublimation | 12 |

237 | For the cell reaction ( : C u^{2+}(a q)left(C_{1}right)+ ) ( Z n(s) rightarrow Z n^{2+}(a q)left(C_{2}right)+C u(s) ) the change in free energy ( Delta G ) at a given temperature is a function of ( A cdot ln C_{1} ) в. ( ln left(frac{C_{2}}{C_{1}}right) ) ( mathrm{c} cdot ln left(C_{2}+C_{2}right) ) D. ( ln left(C_{2}right) ) | 12 |

238 | If ( x ) is the ratio of currents it takes to produce 4.5 g of platinum from molten ( P t C l_{3} ) and ( P t C l_{5}, ) then ( 10 x ) is Electrolysis in each case is carried out for ( 1 mathrm{min} 40 ) s. (Atomic Mass of ( mathrm{Pt}= ) 195.0) | 12 |

239 | Passage of a current for 548 seconds through a silver coulometer results in the deposition of ( 0.746 mathrm{g} ) of silver. What is the current (in A)? A . 1.22 в. 1.16 c. 1.07 D. 1.00 | 12 |

240 | ( boldsymbol{S}_{1} rightarrow ) Conductivity increases on decreasing concentration of electroyte ( boldsymbol{S}_{1} rightarrow ) Molar Conductivity increases on decreasing concentration of electroyte ( A cdot S_{1} ) is true, ( S_{2} ) is False B. Both ( S_{1} & S_{2} ) are true c. Both ( S_{1} & S_{2} ) are false D. ( S_{1} ) is false, ( S_{2} ) is true | 12 |

241 | Calculate the dissociation constant of water at ( 25^{circ} mathrm{C} ) from the following data. Specific conductance of ( boldsymbol{H}_{2} boldsymbol{O}=mathbf{5} . boldsymbol{8} times ) ( 10^{-8} m h o c m^{-1},: lambda_{H^{+}}^{infty}=350.0 ) and ( lambda_{O H^{-}}^{infty}=198.0 m h o c m^{2} ) The ans is ( k times 10^{-16} ) mole/litre. find ( k ) A . 1.8 в. 100 ( c . ) D. 0.01 | 12 |

242 | During discharge of a lead storage cell, the density of sulphuric acid in the cell: A. increases B. decreases c. remains unchanged D. initially increases but decreases subsequently | 12 |

243 | If one mole electrons is passed through the solutions of ( A l C l_{3}, A g N O_{3} ) and ( M g S O_{4}, ) in what ratio ( A l, A g ) and ( M g ) will be deposited at the electrodes? A .3: 6: 2 B . 2: 6: 3 ( mathrm{c} cdot 1: 2: 3 ) D. 3: 2: 1 | 12 |

244 | In which of the following electrolysis, electrodes act as active electrodes. Electrolysis of: A. fused NaCl between graphite electrodes B. fused AgNO between platinum electrodes C . aqueous AgNO solution between Ag electrodes D. aqueous AgNO solution between pt electrodes | 12 |

245 | Calculate the potential of a half cell having reaction: ( quad A g_{2} S(s)+2 e^{-} rightleftharpoons ) ( 2 A g(s)+S^{2-}(a q) ) in a solution buffered at ( p H=3 ) and which is also saturated with ( 0.1 M H_{2} S(a q) ) ( left[text { Given: } boldsymbol{K}_{s p}left(boldsymbol{A} boldsymbol{g}_{2} boldsymbol{S}right)=right. ) ( mathbf{1 0}^{-49}, boldsymbol{K}_{boldsymbol{a}_{1}} cdot boldsymbol{K}_{boldsymbol{a}_{2}}=mathbf{1 0}^{-mathbf{2 1}} ) A . 1.18 B. 0.19 c. ( -0.19 V ) D. None of these | 12 |

246 | Iron and rust are the same things. A. True B. False | 12 |

247 | Explain two ways by which food industries prevent rancidity. Discuss the importance of decomposition reaction in metal industry with three points. | 12 |

248 | The process of lead action in a simple voltaic cell A. Catalyses the process of electrolysis B. Increases the efficiency of the cell c. Decreases the efficiency of the cell D. Increases the charge carriers | 12 |

249 | Assertion: In the calomel half-cell, the reduction reaction to be considered is ( mathrm{Hg}_{2} mathrm{Cl}_{2}(mathrm{s})+2 mathrm{e}^{-} rightarrow 2 mathrm{Hg}(mathrm{I})+2 mathrm{Cl}^{-}(mathrm{aq}) ) Reason: The Saturated calomel electrode (SCE) is a reference electrode based on the reaction between elemental mercury and mercury(l) chloride A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion C. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

250 | For the following reactions: ( Z n rightarrow Z n^{2+}+2 e^{-} ; E=+0.76 V ) ( boldsymbol{A u} rightarrow boldsymbol{A u}^{3+}+mathbf{3} e^{-} ; boldsymbol{E}=-mathbf{1 . 4 2} boldsymbol{V} ) If gold foil is placed in a solution containing ( Z n^{2+}, ) the reaction potential would be: A . ( -1.34 V ) в. ( -2.18 V ) c. ( -0.66 V ) D. ( +2.18 V ) E . ( +1.34 V ) | 12 |

251 | ( Delta G_{f}^{o} ) (standard free energy of formation) of ( Z n O ) and ( C O ) are ( -318.2 mathrm{kJ} ) ( mathrm{mol}^{-1} ) and ( -137.3 mathrm{kJ} mathrm{mol}^{-1} ) respectively. ( Z n O+C longrightarrow Z n+C O ) The approximate value of ( Delta G_{f}^{o} ) in kJmol -1 for the above reaction is ( mathrm{kJ} mathrm{mol}^{-1} ) [Write your answer in form of inearest integer] | 12 |

252 | A sample of water from a large swimming pool has a resistance of ( 9200 Omega ) at 25 of NaCl wear dissolved in the pool, which was throughly stirred. A sample of this solution gave a resistance at ( 7600 Omega ). calculate the volume of water in the pool Given: Molar conductor of NaCl at that concentration is ( 126.5 Omega^{-1} c m^{2} m o l^{-1} ) and molar conductivity of KCl at ( 0.02 mathrm{M} ) is ( 138 Omega^{-1} c m^{2} ) mol ( ^{-1} ) and resist is 85 ( Omega^{-1} ) | 12 |

253 | During electrolysis of an aqueous solution of sodium sulphate, 2.4 L of oxygen at STP was liberated at anode. The volume of hydrogen at STP, liberated at cathode would be: A . 1.2 B. 2.4 L c. 2.6 D. 4.8 L | 12 |

254 | Effect of temperature on internal resistance of a battery is: A. directly proportional B. inversely proportional c. no effect D. none of these | 12 |

255 | Which is correct about the reaction between ( H_{2} O ) and ( O_{2} ? ) ( mathbf{A} cdot ) It is a case of mutual reduction B. ( O_{3} ) will oxidize ( H_{2} O_{2} ) into ( O_{2} ) C. It is not a redox reaction D. ( H_{2} O_{2} ) being a stronger oxidizing agent will decompose ozone into oxygen | 12 |

256 | ( boldsymbol{E}^{0}left(boldsymbol{N} boldsymbol{i}^{2+} / boldsymbol{N} boldsymbol{i}right)= ) ( -0.25 v o l t, E^{0}left(A u^{3+} / A uright)=1.50 v o l t ) The standard emf of the voltaic cell. ( boldsymbol{N} boldsymbol{i}_{(s)}left|boldsymbol{N} boldsymbol{i}_{(a q)}^{2+}(mathbf{1} . boldsymbol{0} boldsymbol{M}) | boldsymbol{A} boldsymbol{u}_{(a q)}^{3+}(mathbf{1} . boldsymbol{0} boldsymbol{M})right| boldsymbol{A} boldsymbol{u}_{(s)} ) is: A. 1.25 volt B . – 1.75 volt c. 1.75 volt D. 4.0 volt | 12 |

257 | Which of these metals do not corrode? A. Lead B. copper C. Platinum D. Silver | 12 |

258 | acts as the cathode. ( mathbf{A} cdot Z n(s) ) B. ( C u^{2+}(a q) ) ( mathbf{c} cdot Z n^{2+}(a q) ) ( mathbf{D} cdot C u(s) ) E ( . H_{2} O ) | 12 |

259 | How much electricity in terms of Faraday is required to produce: (i) ( 20 g ) of ( C a ) from molten ( C a C l_{2} ) (ii) ( 40 g ) of ( A l ) from molten ( A l_{2} O_{3} ) [Given : Molar mass of calcium & Aluminium are 40 g ( m o l^{-1} & 27 g ) mol ( left.^{-1} text {respectively }right] ) | 12 |

260 | Which Nernst equation is true to find out the potential of non-standard electrochemical cell from the following? ( boldsymbol{F} boldsymbol{e}(boldsymbol{s})left|boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{x} boldsymbol{M}) | boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q} cdot)right| boldsymbol{I}_{2}(boldsymbol{s})(boldsymbol{P} boldsymbol{t}) ) ( mathbf{A} cdot_{E e l l}=E_{c e l l}^{circ}-frac{0.592}{n} log _{10}left[F e^{2+}right]left[I^{-}right]^{2} ) B. ( quad E_{text {cell }}=E_{text {cell }}^{circ}-frac{0.0592}{n} log _{10}left[mathrm{Fe}^{2+}right]left[I^{-}right]^{2} ) ( ^{mathbf{C}} E_{text {cell }}=E_{text {cell }}^{circ}-frac{0.0592}{n} log _{10}left[F e^{2+}right]left[I^{-}right] ) D ( quad E_{text {cell }}=E_{text {cell }}^{circ}-frac{0.0592}{n} log _{10} frac{left[F e^{2+}right]left[I^{-}right]^{2}}{[F e]left[I_{2}right]} ) | 12 |

261 | Q. 4 The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called. (a) cell potential (b) cell emf (c) potential difference (d) cell voltage de botential of the lectrodes when no | 12 |

262 | The cell constant of a conductivity cell: A. changes with change of electrolyte B. changed with change of concentration of electrolyte C. changes with temperature of electrolyte D. remains constant for a cell | 12 |

263 | Specific conductance of a decinormal solution of ( K C l ) is 0.0112 ohm ( ^{-1} c m^{-1} ) The resistance of a cell containing the solution was found to be ( 56 . ) Waht is the cell constant? | 12 |

264 | Conductivity of ( 0.00241 mathrm{M} ) acetic acid is ( mathbf{7} . mathbf{8} 9 mathbf{6} times mathbf{1 0}^{-5} mathbf{S} mathbf{c m}^{-1} . ) Calculate its molar conductivity. If ( lambda_{m}^{o} ) for acetic acid is ( 390.5 S c m^{2} ) mol ( ^{-1} . ) what is its degree of dissociation? | 12 |

265 | Q Type your question Determine the time it would take to plate ( 10.0 g A g ) with a current of ( 0.452 A ) A ( .2 .5 h r ) B. ( 3.5 h r ) c. ( 4.5 h r ) ( 0.5 .5 h ) | 12 |

266 | The first electro-chemical was invented by: A. Luigí Galvani B. Alessandro Volta c. Deniel. D. Lechanche | 12 |

267 | The ions associated with salt bridge are A. sodium B. potassium c. calsium D. magnesium | 12 |

268 | A compound which liberates reddish brown gas around the anode during electrolysis in its molten state is A. Sodium chloride B. Copper (II) oxide c. copper (II) sulphate D. Lead (II) bromide | 12 |

269 | Question 14. Suggest two materials other than hydrogen that can be used as fuels in fuel cells. TOLD | 12 |

270 | Which of the following statements is/are incorrect? This question has multiple correct options A. Rust is ( F e_{2} O_{3} ) B. zn-Cu cell is called Daniell cell. c. Saline water slows down rusting. D. Pure metals undergo corrosion faster than impure metals. | 12 |

271 | we have taken a saturated solution of AgBr. Ksp of AgBr is ( 12 times 10^{-4} ) if ( 10^{-7} ) mole of ( A g N O_{3} ) are added to 1 litre of this solution then the conductivity of solution in terms of ( 10^{-7} S m^{-1} ) units will be ( ? mathrm{GIVEN} boldsymbol{lambda} boldsymbol{A} boldsymbol{g}+=mathbf{4} times mathbf{1 0}^{-mathbf{3}} ; boldsymbol{lambda} ) ( mathrm{Br}_{-}=6 times 10^{-3} mathrm{Sm}^{2} boldsymbol{m} ) | 12 |

272 | According to Faraday’s first law, the amount of substance deposited at electrode when an electric current is passed through electrolyte depends upon: This question has multiple correct options A. amount of current passed B. dissociation of electrolyte c. time till which current is passed D. nature of electrode materia | 12 |

273 | For the given cell ( boldsymbol{P t}_{D_{2} mid D^{+}} | boldsymbol{H}^{+}|boldsymbol{P t}| boldsymbol{H}_{2} ) if ( boldsymbol{E}_{D_{2} mid D^{oplus}=0.003 V}^{ominus}, ) what will be the ratio of ( D^{oplus} ) and ( H^{oplus} ) at ( 25^{circ} C ) when he reaction: ( D_{2}+2 H^{oplus} rightarrow 2 D^{oplus}+H_{2} ) attains equilibrium: A .1 .34 B . 1.24 c. 1.124 D. 1.45 | 12 |

274 | Which of the following solutions of Na ( C l ) will have the highest specific conductance? B. ( 0.1 N ) c. ( 0.01 N ) D. ( 1.0 N ) | 12 |

275 | Assertion The Daniell cell becomes dead after sometimes. Reason The oxidation potential of Zn anode decreases and that of Cu increases. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

276 | State True or False. The mass of a substance deposited on the cathode or anode during electrolysis is given by ( mathbf{w}=frac{boldsymbol{E} boldsymbol{i} boldsymbol{t}}{boldsymbol{F}} ) A. True B. False | 12 |

277 | Given standard electrode potentials: ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{3} boldsymbol{e}^{-} longrightarrow boldsymbol{F} boldsymbol{e} ; boldsymbol{E}^{boldsymbol{o}}=-mathbf{0 . 0 3 6} boldsymbol{v o l} boldsymbol{t} ) ( boldsymbol{F} boldsymbol{e}^{2+}+boldsymbol{2} boldsymbol{e}^{-} longrightarrow boldsymbol{F} boldsymbol{e} ; boldsymbol{E}^{o}=-mathbf{0 . 4 4 0} boldsymbol{v o l t} ) The standard electrode potential ( E^{o} ) for ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{e}^{-} longrightarrow boldsymbol{F} boldsymbol{e}^{boldsymbol{2}+} ) is: A. 0.476 volt B. 0.404 volt c. 0.440 volt D. 0.772 volt | 12 |

278 | ( boldsymbol{K}, boldsymbol{C} boldsymbol{a} ) and ( boldsymbol{L} boldsymbol{i} ) metals may be arranged in the decreasing order of their standard electrode potentials as A. ( K, C a ) and ( L i ) в. ( L i, K ) and ( C a ) c. ( L i, ) Ca and ( K ) D. ( C a, L i ) and ( K ) | 12 |

279 | Two students use same stock solution of ( Z n S O_{4} ) and a solution of ( C u S O_{4} ). The emf of one cell is ( 0.03 V ) higher than that of other. The concentration of ( C u S O_{4} ) in the cell with higher emf value is ( 0.5 M . ) Find out the concentration of ( C u S O_{4} ) in the other cell. ( left(frac{2.303 R T}{F}=0.06right) ) | 12 |

280 | Assertion For the Daniel cell, ( Z nleft|Z n^{2+}right|left|C u^{2+}right| C u ) with ( E_{c e l l}=1.1 V, ) the application of opposite potential greater than ( 1.1 mathrm{V} ) results into flow of electron from cathode to anode. Reason ( Z n ) is deposited at anode, and ( C u ) is deposited at cathode. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

281 | The electric batteries used in small calculators are? A. weston cell B. Leclanche cell c. Nickel-cadmium batteries D. Lead acid batteries | 12 |

282 | Represent the cell in which the following reaction takes place ( M g(s)+ ) ( mathbf{2} boldsymbol{A} boldsymbol{g}^{+}(mathbf{0 . 0 0 0 1} boldsymbol{M}) rightarrow ) ( M g^{2+}(0.130 M)+2 A g(s) ) Calculate its ( E_{(c e l l)} ) if ( E_{(c e l l)}^{o}=3.17 V ) | 12 |

283 | The purpose of a salt bridge in a galvanic cell is to: A. prevent accumulation of charges around the electrodes B. facilitate continuity of the cell reaction c. to produce current at a constant strength D. all of the above | 12 |

284 | The efficiency of an hypothetical cell is about ( 84 % ) which involves the following reaction: ( boldsymbol{A}(s)+boldsymbol{B}^{2+}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{A}^{2+}(boldsymbol{a} boldsymbol{q})+ ) ( B(s): Delta H=-285 k J ) Then, the standard electrode potential of the cell will be: (Assume as ( Delta S=0 ) ) A . 1.20 B. 2.40 c. ( 1.10 v ) D. 1.24 | 12 |

285 | ( boldsymbol{C u}^{+}+boldsymbol{e}^{-} longrightarrow boldsymbol{C u}, quad boldsymbol{E}^{o}=boldsymbol{x}_{1} ) volt ( boldsymbol{C u}^{2+}+mathbf{2} e^{-} longrightarrow boldsymbol{C u}, quad boldsymbol{E}^{o}=boldsymbol{x}_{2} ) volt then for ( boldsymbol{C u}^{+}+boldsymbol{e}^{-} longrightarrow boldsymbol{C u}^{+}, quad boldsymbol{E}^{o}(text { volt }) ) will be A. ( x_{1}-2 x_{2} ) В. ( x_{1}+2 x_{2} ) c. ( x_{1}-x_{2} ) D. ( 2 x_{2}-x_{1} ) | 12 |

286 | Molar conductance of a ( 0.2 mathrm{M} ) solution of a weak acid, ( boldsymbol{H} boldsymbol{A} ) is ( 2.8 times 10^{-2} boldsymbol{S m}^{2} ) mol ( ^{-1} ). If the limiting molar conductance of ( boldsymbol{H} boldsymbol{A} ) is ( mathbf{5 6 0} mathbf{~} mathbf{S} boldsymbol{m}^{2} boldsymbol{m o l}^{-1} ) the dissociation constant of the acid is: ( mathbf{A} cdot 5 times 10^{-10} ) B . ( 10^{-10} ) C ( .5 times 10^{-5} ) D. ( 2 times 10^{-15} ) | 12 |

287 | The units of conductivity are: A. siemens ( ^{-1} mathrm{cm}^{-1} ) B. siemens cm c. siemens ( c m^{-1} ) D. siemens ( c m^{-1} m o l^{-1} ) | 12 |

288 | An iron wire is immersed in a solution containing ( Z n S O_{4} ) and ( N i S O_{4} . ) Predict giving reasons which of the following reactions is likely to proceed? (i) Iron reduces ( Z n^{2+} ) ions (ii) Iron reduces ( N i^{2+} ) ions. Given: ( boldsymbol{E}_{boldsymbol{Z} n^{2+} / boldsymbol{Z} boldsymbol{n}}= ) -0.76 volt; ( E_{F e^{2+} / F e}^{circ}=-0.44 ) volt and ( boldsymbol{E}_{N i^{2+} / N i}^{circ}=-mathbf{0 . 2 5} ) volt. | 12 |

289 | When 9.65 coulomb of electricity is passed through a solution of silver nitrate, the amount of silver deposited is: A. ( 16.2 mathrm{mg} ) B. ( 21.2 mathrm{mg} ) c. ( 10.8 mathrm{mg} ) D. ( 6.4 mathrm{mg} ) | 12 |

290 | An excess of liquid Hg was added to ( 10^{-3} mathrm{M} ) acidified solution of ( F e^{3+} ) ions. was found that only ( 4.6 % ) of the ions remained as ( F e^{3+} ) at equilibrium at ( 25^{circ} ) C. Calculate ( boldsymbol{E}^{o} ) for ( mathbf{2} boldsymbol{H} boldsymbol{g} / boldsymbol{H} boldsymbol{g}_{2}^{2+} ) at ( boldsymbol{2} mathbf{5}^{boldsymbol{o}} mathbf{C} ) for, ( 2 H g+2 F e^{3+} rightleftharpoons H g_{2}^{2+}+2 F e^{2+} ) and ( boldsymbol{E}_{boldsymbol{F e}^{2+} / boldsymbol{F e}^{3+}}^{o}=-mathbf{0 . 7 7 1 2} boldsymbol{V} ) A. – -0.7912 V в. – 0.7721 V c. ( -0.9922 mathrm{v} ) D. None of these | 12 |

291 | Which is not true for a standard hydrogen electrode? A. It can act both as cathode and anode B. Temperature is ( 273 mathrm{K} ) C. Pressure is 0 atm. D. It contains a metallic conductor which does not absorb hydrogen | 12 |

292 | Given below are the half-cell reactions: ( M n^{2+}+2 e^{-} rightarrow M n ; E^{o}=-1.18 V ) ( mathbf{2}left(boldsymbol{M} boldsymbol{n}^{+mathbf{3}}+boldsymbol{e}^{-} rightarrow boldsymbol{M} boldsymbol{n}^{2+}right) ; boldsymbol{E}^{boldsymbol{o}}= ) ( +1.51 V ) The ( boldsymbol{E}^{o} ) for ( boldsymbol{3} boldsymbol{M} boldsymbol{n}^{2+} rightarrow boldsymbol{M} boldsymbol{n}+boldsymbol{2} boldsymbol{M} boldsymbol{n}^{3+} ) will be: A. ( +0.33 V ; ) the reaction will occur B. ( -2.69 V ); the reaction will not occur c. ( +2.69 V ; ) the reaction will occur D. ( -0.33 V ); the reaction will not occur | 12 |

293 | Calculate the molar conductivity of water at infinite dilution (in ( mathrm{Sm}^{2} mathrm{mol}^{-1} ) ). ( molar conductivity of hydrogen ions and the molar conductivity of hydroxide ions at infinite dilution are ( 349.6 times 10^{-4} mathrm{Sm}^{2} ) ( left.mathrm{mol}^{-1} text {and } 198.3 times 10^{-4} mathrm{Sm}^{2} mathrm{mol}^{-1}right) ) A . 547.9 B. 647.9 c. ( 647.9 times 10^{-4} ) D. ( 547.9 times 10^{-4} ) | 12 |

294 | The following electrochemical cell has been set-up: ( boldsymbol{P t}(1) mid boldsymbol{F} e^{3+}, boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{a}= ) ( mathbf{1})left|boldsymbol{C} boldsymbol{e}^{boldsymbol{4}+}, boldsymbol{C} boldsymbol{e}^{boldsymbol{3}+}(boldsymbol{a}=mathbf{1})right| boldsymbol{P} boldsymbol{t}(boldsymbol{2}) ) ( E^{0}left(F e^{2+}, F e^{2+}right)=0.77 mathrm{V} ) and ( boldsymbol{E}^{0}left(boldsymbol{C} boldsymbol{e}^{boldsymbol{4}+}, boldsymbol{C} boldsymbol{e}^{boldsymbol{3}+}right)=1.61 mathrm{V} ) If an ammeter is connected between the two platinum electrodes, predict the direction of flow of current, will the current increases or decreases with time? | 12 |

295 | In ( _{-1}-ldots_{text {eactants are }} ) continuously supplied energy which can be withdrawn indefinately until outside supply of reactant is maintained. These cells are more efficient than conventional batteries and moreover, these are eco-friendly. A . fuel B. galvanic C. primary D. secondary | 12 |

296 | In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode? | 12 |

297 | Spacecraft like the satellites that circle the earth and are used in television transmission have electric batteries that supply power for various purposes These batteries contain ion-exchange resins instead of a liquid electrolyte solution because: A. of extreme cold conditions B. of lack of oxygen c. a high electric voltage is required D. of zero gravity | 12 |

298 | What happens when a copper rod is placed in ( F e S O_{4} ) solution? | 12 |

299 | During electroplating by electrolysis, the article to be electroplated is: A. Kept immersed in the electrolyte at the bottom. B. Made the cathode of an electrolytic cell. C. Made the anode of an electrolytic cell. D. Made the electrolyte of the electrolytic cell. | 12 |

300 | We have taken a saturated solution of ( A g B r . K_{s p} ) of ( A g B r ) is ( 12 times 10^{-14} .1 f ) ( 10^{-7} ) mole of ( A g N O_{3} ) are added to 1 litre of this solution find conductivity (specific conductance) of this solution in terms of ( 10^{-7} mathrm{Sm}^{-1} ) Given: ( lambda_{A g^{+}}^{0}=6 times 10^{-3} mathrm{Sm}^{2} mathrm{mol}^{-1} ) ( lambda_{B r^{-}}^{0}=8 times 10^{-3} mathrm{Sm}^{2} mathrm{mol}^{-1} ) and ( lambda_{N O_{3}^{-}}^{0}=7 times 10^{-3} mathrm{Sm}^{2} mathrm{mol}^{-1}[ ) If answe is ( X ) then give answer in form of ( frac{X}{11} ) | 12 |

301 | By passing electric current, ( N a C l O_{3} ) is converted into ( N a C l O_{4} ) according to the following equation ( N a C l O_{3}+ ) ( boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{N} boldsymbol{a} boldsymbol{C l} boldsymbol{O}_{4}+boldsymbol{H}_{2} ) How many moles of ( N a C l O_{4} ) will be formed when three Faradays of charge is passed through ( N a C l O_{3} ? ) A . 1.5 в. 1.0 ( c .3 .0 ) D. 0.75 | 12 |

302 | The standard reduction potential of ( E_{B i^{3+} / B i}^{o} ) and ( E_{C u^{2+} / C u}^{o} ) are ( 0.226 mathrm{V} ) and ( 0.344 mathrm{V} ) respectively. A mixture of salts of Bi and Cu at unit concentration each is electrolysed at ( 25^{circ} mathrm{C} ). To what value ( operatorname{can}left[C u^{2+}right] ) be brought down before bismuth starts to deposit during electrolysis? В. ( 10^{-3} M ) ( mathbf{c} cdot 10^{-5} M ) D. ( 10^{-6} M ) | 12 |

303 | The indication of the state of charge of a battery is best given by: A. specific gravity of electrolyte B. temperature of electrolyte c. colour of electrolyte. D. level of electrolyte | 12 |

304 | The number of faradays of electricity required to decompose ( 100 mathrm{ml} ) water (density ( =0.99 mathrm{gm} / mathrm{ml} ) ) is: A .2 B. 11 ( c .100 ) D. 5.5 | 12 |

305 | For the cell ( boldsymbol{P t}, boldsymbol{H}_{2}(boldsymbol{g}) mid boldsymbol{2} boldsymbol{M} boldsymbol{C} boldsymbol{H}_{3} boldsymbol{C O O N} boldsymbol{H}_{4} | mathbf{2} M boldsymbol{n} ) 20 ( operatorname{atm} quad 0.2 operatorname{atm} ) Given ( : boldsymbol{p} boldsymbol{K}_{boldsymbol{a}}left(boldsymbol{C H}_{3} boldsymbol{C O O H}right)=mathbf{4 . 7 4} ) and ( boldsymbol{p} boldsymbol{K}_{boldsymbol{b}}left(boldsymbol{N} boldsymbol{H}_{4} boldsymbol{O} boldsymbol{H}right)=mathbf{4 . 7 4} ) EMF of the cell in millivolt is: (Given ( left.frac{2.303 R T}{F}=0.059right) ) | 12 |

306 | What is the amount of Al deposited on the electrolysis of molten ( A l_{2} O_{3} ) when a current of ( 9.65 mathrm{A} ) is passed for ( 10.0 mathrm{s} ) | 12 |

307 | In electrolyte concentration cell: This question has multiple correct options A. the electrode material and the solution in both halfcells are composed of the same substances B. only the concentrations of solutions of the same substances is different ( mathbf{c} cdot E_{c e l l}^{circ}=0 ) D. the Nernst equation reduces to ( E_{text {cell}}= ) ( -left(frac{0.0591}{n}right) log Q ) at ( 25^{circ} mathrm{C} ) | 12 |

308 | A conductance cell was filled with a 0.02 M KCl solution which has a specific conductance of ( 2.768 times ) ( 10^{-3} ) oh ( m^{-1} c m^{-1} . ) If its resistance is 82.4 ohm at ( 25^{circ} mathrm{C}, ) then the cell constant is: A. ( 0.2182 mathrm{cm}^{-1} ) В. ( 0.2281 mathrm{cm}^{-1} ) c. ( 0.2821 mathrm{cm}^{-1} ) D. 0.2381 ( c m^{-1} ) | 12 |

309 | Q. 15 While charging the lead storage battery …….. (a) PbSO4 anode is reduced to Pb (b) Pbso, cathode is reaus (c) PbSO4 cathode is oxidised to Pb (d) Pbso, anode is oxidise ollie reversed and bSO4 cathode is reduced to Pb | 12 |

310 | Which of the following gas is formed at the electrode connected to the negative terminal of the battery? A. Nitrogen gas B. Hydrogengas c. oxygen gas D. carbon dioxide gas | 12 |

311 | Why metal gets deposited at the negative pole when electric current is passed through a metal salt?? A. Metal is negatively charged. B. Metal is positively charged. c. Metal does not have any charges. D. Both a and c. | 12 |

312 | A current of 1.5 ampere is passed through a solution of a salt of a bivalent metal for 30 minutes. Increase in mass of cathode is ( 0.8898 g . ) Find the atomic mass of the metal. ( A cdot 63 g ) B. 63.6 g c. ( 73.6 g ) D. 70g | 12 |

313 | Indicate the correct statements. This question has multiple correct options A. Conductivity cells have cell constant values independent of the solution filled into the cell B. DC (direct current) is not used for measuring the resistance of a solution C. Kohlrausch law is valid both for strong and weak electrolytes D. The k decreases but ( lambda_{M} ) and ( lambda_{E} ) increase on dilution | 12 |

314 | Q. 56 Assertion (A) Cu is less reactive than hydrogen. Reason (R) E is negative. 2+ I OAN | 12 |

315 | If ( E_{C H_{3} C O O O H mid C_{2} H_{5} O H}^{ominus}=0.06 V, ) Then ( E_{c e l l}^{ominus} ) of the reaction taking place in alcohol meter is : ( mathbf{A} cdot 1.39 V ) B. ( 1.27 V ) c. ( 1.60 V ) D. ( 1.51 V ) | 12 |

316 | In the galvanic cell : ( Z n / Z n^{2+}left(C_{1}right) | C u^{2+}left(C_{2}right) / C u ) ( boldsymbol{E}_{c e l l}-boldsymbol{E}_{c e l l}^{o}=+mathbf{0 . 0 5 9 1} boldsymbol{V} . ) The value of ( frac{C_{1}}{C_{2}} ) at ( 298 K ) is: A ( cdot 10^{-1} ) B. ( 10^{2} ) ( c cdot 10^{-2} ) D. 10 | 12 |

317 | Lead storage battery contains: A. ( P b ) rod as anode B. ( P b ) plates coated with ( P b O_{2} ) act as cathode C . electrolyte is ( H_{2} S O_{4} ) D. all are currect | 12 |

318 | Hydrogen – Oxygen fuel cells are used in space craft to supply: A. power for heat and light B. electrical power c. oxygen D. water | 12 |

319 | What is the correct formula for determining the voltage of an electrochemical cell? A ( cdot E_{text {cell }}^{0}=E_{text {cathode }}^{0}-E_{text {anode }}^{0} ) added C ( cdot E_{text {constant }}^{0}=E_{text {cathode }}^{0}-E_{text {ande }}^{0} ) D. ( E_{text {constant}}^{0}=E_{text {cathode}}^{0}+E_{text {anode}}^{0} ) E . ( E_{c e l l}^{0}=-E_{text {cathode }}^{0}+E_{text {ande }}^{0} ) | 12 |

320 | Assertion Silver metal does not show any change when it is placed in HCl solution. Reason Silver metal does not react with dilute HCI A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

321 | How many faradays of electricity will be required by ( 3 times 10^{12} ) electrons? | 12 |

322 | An acid is a substance that produces ions in a water solution A. oxygen B. nitrogen c. carbon D. hydrogen | 12 |

323 | The EMFs of the following cells are ( boldsymbol{C u}left|boldsymbol{C u}^{2+}(mathbf{1} boldsymbol{M}) | boldsymbol{A} boldsymbol{g}^{+}(mathbf{1} boldsymbol{M})right| boldsymbol{A} boldsymbol{g}, boldsymbol{E}^{o}= ) ( 0.46 V ) ( Z nleft|Z n^{2+}(1 M) | C u^{2+}(1 M)right| C u, E^{o}= ) ( 1.10 V ) The EMF of the cell ( Z nleft|Z n^{2+}right|left|A g^{+}(1 M)right| A g ) will be: A . ( 1.56 V ) B . ( -1.56 V ) c. ( 0.64 V ) D. ( 2.02 V ) | 12 |

324 | can be obtained from bauxite by A. Aluminium, Electrolysis B. Copper, Electroplating c. Aluminium, Electroplating D. Copper, Electrolysis | 12 |

325 | The standard reduction potential data at ( 25^{circ} mathrm{C} ) is given below: ( mathbf{E}^{mathrm{o}}left(mathbf{F e}^{mathbf{3}+}, mathbf{F e}^{mathbf{2}+}right)=+mathbf{0 . 7 7} mathbf{V} ) ( mathbf{E}^{mathbf{o}}left(mathbf{F e}^{mathbf{2}+}, mathbf{F e}right)=-mathbf{0 . 4 4} mathbf{V} ) ( mathbf{E}^{mathrm{o}}left(mathbf{C u}^{2+}, mathbf{C u}right)=+mathbf{0 . 3 4} mathbf{V} ) ( mathbf{E}^{circ}left(mathbf{C u}^{+}, mathbf{C u}right)=+mathbf{0 . 5 2 V} ) ( mathbf{E}^{mathrm{o}}left[mathbf{O}_{2}(mathbf{g})+mathbf{4 H}^{+}+mathbf{4 e}^{-} rightarrow mathbf{2} mathbf{H}_{mathbf{2}} mathbf{0}right]= ) ( +1.23 V ) ( mathbf{E}^{circ}left[mathbf{O}_{2}(mathbf{g})+mathbf{2} mathbf{H}_{2} mathbf{O}+mathbf{4} mathbf{e}^{-} rightarrow mathbf{4 0} mathbf{H}^{-}right]= ) ( +0.40 mathrm{V} ) ( mathbf{E}^{circ}left(mathbf{C r}^{3+}, mathbf{C r}right)=-mathbf{0 . 7 4 V} ) ( mathbf{E}^{mathbf{o}}left(mathbf{C r}^{2+}, mathbf{C r}right)=-mathbf{0 . 9 1} mathbf{V} ) Match ( mathrm{E}^{0} ) of the redox pair in List 1 with the values given in List 2 and select the correct answer using the code given below the lists. | 12 |

326 | If ( E_{F e^{2+} / F e}^{0}=-0.441 mathrm{V} ) and ( E_{F e^{3+} / F e^{2+}}^{0}= ) ( 0.771 mathrm{V}, ) the standard ( boldsymbol{E} boldsymbol{M} boldsymbol{F} ) of the reaction, ( boldsymbol{F} boldsymbol{E}+mathbf{2} boldsymbol{F} boldsymbol{E}^{3+} rightarrow mathbf{3} boldsymbol{F} boldsymbol{E}^{2+} ) will be: A ( .0 .330 V ) ( V ) B. ( 1.653 V ) c. ( 1.212 V ) D. ( 0.111 V ) | 12 |

327 | ionizes in a fused or in aqueous solution state and furnish positive ions other than ( boldsymbol{H}^{+} ) and negative ions other than ( boldsymbol{O} boldsymbol{H}^{-} ) A. Mineral acids B. Bases c. lonic salts D. compounds | 12 |

328 | The metal which cannot liberate ( H_{2} ) gas from hydrochloric acid is: ( A cdot Z n ) B. cu ( mathrm{c} . ) мв D. Al | 12 |

329 | What will be the emf for the given cell : ( P tleft|H_{2}left(P_{1}right)right| H^{+}(a q)left|H_{2}left(P_{2}right)right| P t ) ( ^{text {A } cdot} frac{R T}{F} log frac{P_{1}}{P_{2}} ) в. ( frac{R T}{2 F} log frac{P_{1}}{P_{2}} ) c. ( frac{R T}{F} log frac{P_{2}}{P_{1}} ) D. noneofthese | 12 |

330 | ( C u(S)+2 A g^{+}(a q) rightarrow C u^{2+}(a q)+2 A g(S) ) In the given reaction, the reduction half cell reaction is: A ( cdot mathrm{Cu}^{2+}+2 mathrm{e}^{-} rightarrow mathrm{cu} ) B. ( operatorname{cu} 2 e^{-} rightarrow c u^{2} ) ( mathrm{c} cdot mathrm{Ag}^{+}+mathrm{e}^{-} rightarrow mathrm{Ag} ) D. ( A g e^{-} rightarrow A g^{+} ) | 12 |

331 | Identify the reaction taking place at cathode in fuel cell. A. ( O_{2}+2 H_{2} O+4 e^{-} rightarrow 4 O H^{-} ) B ( cdot 2 H_{2}+4 O H^{-} rightarrow 4 H_{2} O+4 e^{-} ) c. ( O_{2}+2 H_{2} O+4 e^{-} rightarrow 4 O H^{-}+H^{+} ) D. ( 4 H_{2} O+4 e^{-} rightarrow 2 H^{2}+4 O H^{-} ) | 12 |

332 | ( ln H_{2}-O_{2} ) fuel cell a reaction occuring at cathode is: A. ( 2 H_{2} O+O_{2}+4 e^{-} rightarrow 4 O H^{-} ) В. ( 2 H_{2}+O_{2} rightarrow 2 H_{2} O(l) ) ( mathrm{c} cdot H^{+}+O H^{-} rightarrow H_{2} mathrm{O} ) D. ( H^{+}+e^{-} rightarrow frac{1}{2} H_{2} ) | 12 |

333 | The storage battery generally used in electric power station is: A. Nickel-Cadmium battery B. zinc-Carbon battery c. Lead-Acid battery D. None of the above | 12 |

334 | At equimolar concentrations of ( boldsymbol{F} boldsymbol{e}^{2+} ) and ( F e^{3+}, ) what must ( left[A g^{+}right] ) be so that the voltage of the galvanic cell made from the ( left(A g^{+} mid A gright) ) and ( left(F e^{3+} mid F e^{2+}right) ) electrodes equals zero? ( boldsymbol{F} boldsymbol{e}^{2+}+boldsymbol{A} boldsymbol{g}^{+} rightleftharpoons boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{A} boldsymbol{g} ) ( boldsymbol{E}_{A boldsymbol{g}^{o} mid boldsymbol{A} boldsymbol{g}}^{o}=boldsymbol{0 . 7 9 9 1} ; boldsymbol{E}_{boldsymbol{F e}^{3+} mid boldsymbol{F} e^{2-}}=mathbf{0 . 7 7 1} ) A .0 .34 B. 0.44 c. 0.47 D. 0.61 | 12 |

335 | Q. 32 Aqueous copper sulphate solution and aqueous silve are electrolysed by 1 ampere current for 10 minu electrolytic cells. Will the mass of copper and silver depo. cathode be same or different? Explain your answer. thoda According to Faraday’s on and aqueous silver nitrate solution current for 10 minutes in separate of copper and silver deposited on the A nrding Dufor | 12 |

336 | A photo-cell employs photoelectric effect to convert: A. change in the frequency of light into a change in electric voltage. B. change in the intensity of illumination into a change in photoelectric current. C. change in the intensity of illumination into a change in the work function of the photocathode. D. change in the frequency of light into a change in the electric current. | 12 |

337 | ( operatorname{acts} ) as the anode. ( mathbf{A} cdot Z n(s) ) B. ( C u^{2+}(a q) ) ( mathbf{c} cdot Z n^{2+}(a q) ) ( mathbf{D} cdot C u(s) ) E ( . H_{2} O ) | 12 |

338 | The standard electrode potential ( boldsymbol{E}_{l_{2} / r}^{o}, quad boldsymbol{E}_{B r^{-} / B r_{2}}^{0} quad ) and ( quad boldsymbol{E}_{boldsymbol{F} e / F e^{2+}}^{0} ) are respectively ( +0.54 mathrm{V},-1.09 mathrm{V} ) and ( 0.44 mathrm{V} . ) On the basis of above data which of the following process is non spontaneous? ( mathbf{A} cdot B r_{2}+2 I^{1} rightarrow 2 B r+I_{2} ) B. ( F e+B r_{2} longrightarrow F e^{2+}+2 B r ) C. ( F e+I_{2} longrightarrow F e^{2+}+2 I^{-} ) D. ( I_{2}+B r longrightarrow 2 I^{-}+B r_{2} ) | 12 |

339 | The resistance of ( 0.01 mathrm{N} ) solution of an electrolyte ( A B ) at ( 328 mathrm{K} ) is 100 ohm. The specific conductance of solution is : ( left[text { cell constant }=1 mathrm{cm}^{-1}right] ) A. 100 ohm B. ( 10^{-2} ) ohm ( ^{-1} ) ( mathbf{c} cdot 10^{-2} operatorname{ohm}^{-1} c m^{-1} ) D. ( 10^{2} ) ohm ( -c m ) | 12 |

340 | The charge required to reduce 1 mole ( mathrm{Cr}_{2} mathrm{O}_{7}^{2-} ) to ( mathrm{Cr}^{3+} ) ions is: ( mathbf{A} cdot 3 F ) B. ( 3 C ) ( mathbf{c} cdot 6 F ) D . ( 2 times 6.023 times 10^{23} e^{-} ) | 12 |

341 | Corrosion can not be prevented by which of the following method? A. Use of an anode connected to a direct current power B. Create a barrier between the object being corroded and oxygen c. Painting D. Exposing it to sunlight | 12 |

342 | The e.m.f. of the cell ( boldsymbol{A} boldsymbol{g}|boldsymbol{A} boldsymbol{g} boldsymbol{C l} | boldsymbol{K} boldsymbol{C l}(boldsymbol{a q} .)| boldsymbol{H}_{2} boldsymbol{C l}_{2} mid boldsymbol{H} boldsymbol{g} ) is ( 0.0455 mathrm{K} ) at ( 298 mathrm{K} ) and the temperature coefficient is ( 3.38 times 10^{-4} V K^{-1} . ) The reaction is taking place is: A. ( H g_{2} C l_{2}(s)+2 A g(s) rightarrow 2 A g C l(s)+2 H g(l) ) B. ( H g_{2} C l_{2}(s)+3 A g(s) rightarrow 3 A g C l(s)+4 H g(l) ) C. ( H g_{2} C l_{2}(s)+A g(s) rightarrow 2 A g C l(s)+4 H g(l) ) D. none of these | 12 |

343 | The value of cell constant ( left(text { in } m^{-1} ) ) is: right. write your answer to nearest integer) | 12 |

344 | The equilibrium constant of the reaction ( boldsymbol{C}_{boldsymbol{u}}(boldsymbol{s})+boldsymbol{2} boldsymbol{A} boldsymbol{g}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{C} boldsymbol{u}^{2+}(boldsymbol{a} boldsymbol{q})+ ) ( mathbf{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s}) ; boldsymbol{E}^{0}=mathbf{0 . 4 6} boldsymbol{V} boldsymbol{a} boldsymbol{t} mathbf{2} boldsymbol{9} boldsymbol{8} boldsymbol{K} ) is: ( mathbf{A} cdot 4.0 times 10^{15} ) B . ( 2.4 times 10^{10} ) c. ( 2.0 times 10^{10} ) D. ( 4.0 times 10^{10} ) | 12 |

345 | Three faradays of electricity are passed through molten ( A l_{2} O_{3}, ) aqueous solution of ( C u S O_{4} ) and molten ( N a C l ) taken in three different electrolytic cells. The amount of ( A l, C u ) and ( N a ) deposited at the cathodes will be in the ratio of A. 1 mole : 1 mole : 1 mole B. 1 mole : 1.5 mole: 3 mole c. 3 mole : 2 mole : 1 mole D. 1 mole : 1.5 mole: 2 mole | 12 |

346 | The standard emf for the cell reaction, ( Z n+C u^{2+} rightarrow Z n^{2+}+C u ) is 1.10 volt at ( 25^{circ} mathrm{C} ). The emf for the cell reaction when ( 0.1 M C u^{2+} ) and ( 0.1 M Z n^{2+} ) solutions are used at ( 25^{circ} mathrm{C} ) is: A. 1.10 volt B. 0.110 volt c. -1.10 volt D. -0.110 volt | 12 |

347 | What is the density of solution of sulphuric acid used as an electrolyte in lead accumulator? ( mathbf{A} cdot 1.5 mathrm{gm} L^{-1} ) B. ( 1.2 mathrm{gm} L^{-1} ) c. ( 1.8 mathrm{gm} L^{-1} ) D. ( 2.0 mathrm{gm} L^{-1} ) | 12 |

348 | A weak electrolyte having the limiting equivalent conductance of ( 400 S mathrm{cm}^{2} g ) equiv ( ^{-1} ) at ( 298 K ) is ( 2 % ) ionized in its ( 0.1 N ) solution. The resistance of this solution (in ohm) in an electrolytic cell of cell constant ( 0.4 mathrm{cm}^{-1} ) at this temperature is: A . 200 в. 300 c. 400 D. 500 E. 600 | 12 |

349 | Which of the following gas is formed at the electrode, connected to the positive terminal of the battery? A. Nitrogen gas B. Hydrogengas c. oxygen gas D. carbon dioxide gas | 12 |

350 | During discharging of a lead storage battery, which of the following is/are true? This question has multiple correct options ( mathbf{A} cdot H_{2} S O_{4} ) is produced B. ( H_{2} O ) is consumed ( mathrm{C} cdot P b S O_{4} ) is formed at both electrodes D. Density of electrolytic solution decreases | 12 |

351 | Consider the following concentration cell ( Z n(s)left|Z n^{2+}(0.024 M) | Z n^{2+}(0.480 M)right| Z ) which of the following statements is/are correct? This question has multiple correct options | 12 |

352 | The volume of gases evolved at ( S T P ) by passing ( 0.1 A ) of current for ( 965 g ) through an aqueous solution of potassium acetate: A . ( 22.4 m L ) в. ( 11.2 m L ) ( c .89 .6 m L ) D. ( 44.8 mathrm{mL} ) | 12 |

353 | The standard e.m.f. of the cell involving the reaction, ( 2 A g^{+}(a q)+H_{2}(g) rightarrow ) ( 2 A g(s)+2 H^{+}(a q), ) is ( 0.80 mathrm{V} . ) The standard oxidation potential of ( mathrm{Ag} ) electrode is: A . ( 0.80 V ) в. ( -0.80 V ) c. ( 0.40 V ) D. ( 0.20 V ) | 12 |

354 | If ( E^{o} ) denotes reduction potential, then which is true? ( mathbf{A} cdot E_{c e l l}^{0}=E_{r i g h t}^{o}-E_{l e f t}^{o} ) B ( cdot E_{text {cell }}^{0}=E_{text {left }}^{o}+E_{text {right }}^{o} ) ( mathbf{c} cdot E_{c e l l}^{0}=E_{l e f t}^{o}-E_{r i g h t}^{o} ) D. ( E_{c e l l}^{0}=-left(E_{l e f t}^{o}+E_{r i g h t}^{o}right) ) | 12 |

355 | One ampere hour charge is equivalent to : A. 36 coulombs B. 360 coulombs c. 3600 coulombs D. 36000 coulombs | 12 |

356 | When the free ends of a tester are dipped into a solution, the magnetic needle shows deflection due to: A . electrical effect B. mechanical effect c. magnetic effect D. lighting effect | 12 |

357 | A shiny brown-coloured element ‘X’ on heating in air becomes black in colour Name the element ‘X’? A. Sodium B. Calcium c. copper D. Aluminium | 12 |

358 | Why distilled water does not conduct electricity? | 12 |

359 | What is the potential of the cell containing two hydrogen electrodes as represented below? ( boldsymbol{p t} ; frac{1}{2} boldsymbol{H}_{2}(boldsymbol{g})left|boldsymbol{H}_{2} boldsymbol{O}right|left|boldsymbol{H}^{oplus}(mathbf{0 . 0 0 1} boldsymbol{M})right| mathbf{1} / mathbf{2} boldsymbol{H} ) A. ( -0.236 V ) В. ( -0.0591 V ) c. ( 0.236 V ) D. ( 0.0591 V ) | 12 |

360 | A) Electrolysis of NaCl solution gives chlorine at anode Q. 61 Assertion (A) Electrolysis of NaCl solution instead of 02. Reason (R) Formation of oxygen at anode requires over voltage. Jonation of | 12 |

361 | Electrolysis of water is carried out in hoffman voltameter. Litmus is added to both cathodic and anodic compartments.What changes do you observe in the above process at the end of electrolysis? Justify. | 12 |

362 | Aluminum displaces hydrogen in dil. HCl whereas silver does not. The e.m.f of a cell prepared by combination ( A l / A l^{3+} ) and ( A g / A g^{+} ) is 2.46 V. The reduction potential reduction potential of aluminum electrodes is: A ( .+1.66 v ) B. – -3.26 V ( c .+3.26 v ) D. -1.66 V | 12 |

363 | A current of 9.95 amperes flowing for 10 minutes, deposits ( 3 g ) of metal. An equivalent weight of the metal is: A . 12.5 B. 18.5 c. 21.5 D. 48.5 | 12 |

364 | The quantity of charge (in Faraday) required to electrolyse ( 54 mathrm{g} mathrm{H}_{2} mathrm{O} ) is : | 12 |

365 | 0.46 Write the Nernst equation for the cell reaction in the Daniel cell. How will the Ecell be affected when concentration of Zn2+ ions is increased? | 12 |

366 | In a copper wire, current is the flow of : A. positive charge B. negative charge c. both a and b D. none of above | 12 |

367 | The solubility product of a saturated solution of ( A g_{2} C r O_{4} ) in water at ( 298 mathrm{K} ) will be……………., if the EMF of the cell: ( boldsymbol{A} boldsymbol{g} mid boldsymbol{A} boldsymbol{g}^{oplus}left(boldsymbol{s} boldsymbol{a} boldsymbol{t} boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C r} boldsymbol{O}_{4} boldsymbol{s o l}right) | boldsymbol{A} boldsymbol{g}(boldsymbol{0} . boldsymbol{1} boldsymbol{M} ) is ( 0.164 V ) at ( 298 mathrm{K} ) A. ( 2.287 times 10^{-12} M^{3} ) B . ( 2.659 times 10^{-12} M^{3} ) c. ( 1.965 times 10^{-12} M^{3} ) D. None of these | 12 |

368 | The conductivity at infinite dilution of ( N H_{4} C l, N a O H ) and ( N a C l ) are ( 130,218,120 o h m^{-1} c m^{2} e q^{-1} . ) If equivalent conductance of ( frac{N}{100} ) solution of ( N H_{4} O H ) IS ( 10, ) then degree of dissociation of ( N H_{4} O H ) at this dilution is: A. 0.005 B. 0.043 c. 0.015 D. 0.025 | 12 |

369 | Corrosion is the process of rusting of any kind of metal or alloy due to the presence of moisture and air in it’s surrounding. As it comes in contact with air and water it reacts with it and a layer is formed above it’s surface. Type 1 for true and 0 for False. | 12 |

370 | Match the following. | 12 |

371 | Which of the following is a chemical effect of electric current? A. Formation of gas bubbles on the electrodes B. Change of color of solution c. Deposition of metals on the electrodes D. All of the above | 12 |

372 | Question 24. What is the relationship between Gibbs free cell reaction in a galvanic cell and the emf of the cell? When will the maximum work be obtained from a galvanic cell? | 12 |

373 | The emf of the cells obtained by combining zinc and copper electrodes of the Daniell cell with calomel electrodes are 1.083 volt and -0.018 volt respectively at ( 25^{circ} mathrm{C} . ) If the reduction potential of normal calome electrode is +0.28 volt, find he emf of the Daniell cell. | 12 |

374 | The standard e.m.f. of a cell involving one electron change is found to ( 0.591 mathrm{V} ) at ( 25^{circ} mathrm{C} ). The equilibrium constant of the reaction is: A ( cdot 10^{30} ) B . ( 10^{5} ) ( c cdot 10^{10} ) D. ( 10^{text { }} ) | 12 |

375 | Amount of zinc deposited when ( 3.01 times ) ( 10^{20} ) electrons pass through ( Z n S O_{4} ) solution is: A . ( 16.35 g ) B . ( 16.375 times 10^{-3} g ) c. ( 32.7 times 10^{-3} g ) D. 32.7g | 12 |

376 | During electrolysis of fused calcium hydride, the hydrogen is produced at: A. cathode B. anode c. hydrogen is not liberated at all D. ( H_{2} ) produced reacts with oxygen to form water | 12 |

377 | Which one of the following scientists showed that if electrodes are immersed in water and a current was passed, bubbles of oxygen and hydrogen were produced? A. William Thomson B. William Nicholson c. william watson D. William Harvey | 12 |

378 | A conductivity cell filled with ( 0.01 M ) KCl gives at ( 25^{circ} mathrm{C} ) the resistance of 604 ohms. The conductivity of ( K C l ) at ( 25^{circ} C ) is ( 0.00141 Omega^{-1} c m^{-1} . ) The same cell filled with ( 0.001 M A g N O_{3} ) gives a resistance of 6529 ohms. Calculate the molar conductivity of ( 0.001 M A g N O_{3} ) solution at ( 25^{circ} mathrm{C} ) | 12 |

379 | 0.53 Match the items of Column I and Column II. Column 1 Column II Α. κ 1. Ixt В. 2. Amlan ca 3. D. O | 12 |

380 | The ( boldsymbol{E}^{ominus} ) for ( boldsymbol{C u}^{2+} / boldsymbol{C u}^{oplus}, boldsymbol{C u}^{oplus} / boldsymbol{C u}, boldsymbol{C u}^{2+} / boldsymbol{C} ) are ( 0.15 vee, 0.50 mathrm{V}, ) and ( 0.325 mathrm{V} ) respectively. The redox cell showing redox reaction ( 2 C u^{+}, rightarrow C u^{2+}+C u ) is made. ( E^{ominus} ) of this cell reaction and ( Delta G^{ominus} ) may be : A ( cdot E^{ominus}=0.175 V ) or ( E^{ominus}=0.350 V ) B. ( n=1 ) or 2 c. ( Delta G^{ominus}=-33.775 k J ) D. All of these | 12 |

381 | State True or False. The effect of a change in the concentration of a reactant or product on the cell voltage can be predicted by applying Le-chateliers principle. A. True B. False | 12 |

382 | Entropy change in ( mathrm{JK}^{-1} ) is (Give answer to the nearest integer) | 12 |

383 | Calculate ( boldsymbol{K}_{c} ) for ( boldsymbol{H} boldsymbol{g}^{2+}+boldsymbol{H} boldsymbol{g} rightleftharpoons boldsymbol{H} boldsymbol{g}_{2}^{2+} ) Give that ( E_{2 H g / H g^{2+}}^{o}=-0.788 V ) and ( boldsymbol{E}_{boldsymbol{H} boldsymbol{g}_{2}^{2+} / mathbf{2 H g}^{2+}}^{boldsymbol{o}}=-mathbf{0 . 9 2 0} boldsymbol{V} ) Write answer as nearest integer after dividing by 100 | 12 |

384 | is defined as a process where materials, usually metals, deteriorate as a result of a chemical reaction with air, moisture, chemical etc. For example, iron, in the presence of moisture, reacts with oxygen to form hydrated iron oxide. | 12 |

385 | Assertion ( H_{2} S ) reacts with oxygen under standard conditions in acid medium to give ( boldsymbol{H}_{2} boldsymbol{O} ) and sulphur. Reason ( boldsymbol{E}_{boldsymbol{H}^{+} / boldsymbol{O}_{2} / boldsymbol{P t}}>boldsymbol{E}_{boldsymbol{H}^{+} / boldsymbol{H}_{2} boldsymbol{S} / boldsymbol{S}}^{boldsymbol{o}} ) A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

386 | Glucose solution is an electrolyte and hence conducts electricity. A. True B. False | 12 |

387 | Conductivity of ( C a C l_{2} ) solution is: A ( cdot 4.87 times 10^{-4} mathrm{Scm}^{1} ) B. ( 7.84 times 10^{-4} mathrm{Scm}^{1} ) c. ( 8.47 times 10^{-4} mathrm{Scm}^{1} ) D. None of these | 12 |

388 | Calculate the amount of charge required to deposit 1.0 g of sodium metal(molar mass 23.0 g ( m o l^{-1} ) ) from sodium ion. A . 2098 B. 96500 c. 193000 D. 4196 | 12 |

389 | Two half-cells have potentials -0.44 and 0.799 volt respectively. These two are coupled to make a galvanic cell. Which of the following will be true? A. Electrode of half-cell potential ( -0.44 mathrm{V} ) V will act as anode B. Electrode of half-cell potential -0.44 V will act as cathode c. Electrode of half-cell potential ( 0.799 mathrm{V} ) will act as anode D. Electrode of half-cell potential ( -0.44 mathrm{V} ) will act as a positive terminal | 12 |

390 | A Science teacher wrote 3 statements about rancidity: (i) When fats and oils are reduced, they become rancid (ii) In chips packet, rancidity is prevented by oxygen (iii) Rancidity is prevented by adding antioxidants. Selects the correct option. A. (i) B. (ii) and (iii) c. (iii) D. (i), (ii) and (iii) | 12 |

391 | An example of secondary battery cell is: A. Edison Alkaline cell B. Daniel cell. c. Lachanche cell. D. Bunsen cell. | 12 |

392 | The molar conductivities of ( wedge_{N a O A C}^{0} ) and ( wedge_{H C l}^{0} ) at infinite dilution in water at ( 25^{0} C ) and 91.0 and ( 426.2 mathrm{Scm}^{2} / mathrm{mol} ) respectively. To calculate ( wedge_{H O A c}^{0} ), the additional value required is: ( mathbf{A} cdot wedge_{N a C l}^{0} ) B. ( wedge_{H_{2} O}^{0} ) c. ( wedge_{K C l}^{0} ) D. ( wedge_{N a O H}^{0} ) | 12 |

393 | The molar conductance at infinite dilution of ( A g N O_{3}, A g C l ) and ( N a C l ) are 116.5,121.6 and 110.3 respectively. The molar conductance of ( N a N O_{3} ) is: ( mathbf{A} cdot 111.4 ) B. 105.2 c. 130.6 D. 150.2 | 12 |

394 | ( ln ) a ( H_{2}-O_{2} ) fuel cell, combustion of hydrogen occurs to: A. remove adsorbed oxygen from electrode surface B. create potential difference between the two electrodes c. produce high purity water D. generate heat | 12 |

395 | For the cell (at ( 298 mathrm{K} ) ), which of the following is correct? ( boldsymbol{A} boldsymbol{g}(boldsymbol{s})|boldsymbol{A} boldsymbol{g} boldsymbol{C l}(boldsymbol{s})| boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q}) | boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3}(boldsymbol{a} boldsymbol{q}) mid boldsymbol{A} ) A. The cell emf will be zero when ( ( left.left[mathrm{Ag}^{+}right]right) ) in anodic compartment ( =left[mathrm{Ag}^{+}right] ) in cathodic compartment B. The amount of AgCl(s) precipitate in anodic compartment will decrease will the working of the cell C. The concentration of ( left[mathrm{Ag}^{+}right]= ) constant, in anodic compartment during working of cell D. ( E_{text {cell}}=E_{A g^{+} mid A g}^{0}-E_{C l^{-}|A g C l| A g}^{0}-frac{0.059}{1} log frac{1}{left[C l^{-}right]_{a}} ) | 12 |

396 | The potential of hydrogen electrode at ( 25^{circ} C ) will be: ( left(P_{H_{2}}=1 text { atm, concentration of } boldsymbol{H}^{+}=right. ) ( mathbf{0 . 1} boldsymbol{M} ) ( mathbf{A} cdot 0.00 V ) В. ( -0.059 V ) c. ( 0.118 V ) D. ( 0.059 V ) | 12 |

397 | When an aqueous solution of ( boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3} ) is electrolysed between platinum electrodes, the substances liberated at anode and cathode are: A. silver is deposited at cathode and ( O_{2} ) is liberated at anode B. Silver is deposited at cathode and ( H_{2} ) is liberated at anode C. Hydrogen is liberated at cathode and ( O_{2} ) is liberated at anode D. Silver is deposited at cathode and Pt is dissolved in electrolyte | 12 |

398 | ( boldsymbol{Z} boldsymbol{n}left|begin{array}{c}boldsymbol{Z} boldsymbol{n}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}(boldsymbol{a} boldsymbol{q}) \ boldsymbol{1} mathbf{0} boldsymbol{0} boldsymbol{m} boldsymbol{L}, boldsymbol{1} boldsymbol{M}end{array}right|left|begin{array}{c}boldsymbol{C u}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}(boldsymbol{a} boldsymbol{q}) \ boldsymbol{1} mathbf{0} boldsymbol{0} boldsymbol{m} boldsymbol{L}, mathbf{1} boldsymbol{M}end{array}right| ) The following galvanic cell was operated as an electrolytic cell using Cu as anode and ( mathrm{Zn} ) as cathode. A current of 0.48 ampere was passed for 10 hour and then the cell was allowed to function as galvanic cell. The e.m.f. of the cell at ( 25^{circ} ) ( mathrm{C} ) is (write the nearest integer value): Assume that the only electrode reactions occurring were those involving ( boldsymbol{C} boldsymbol{u} / boldsymbol{c u}^{2+} ) and ( boldsymbol{Z} boldsymbol{n} / boldsymbol{Z} boldsymbol{n}^{2+} ) Given ( E_{C u^{2+}, C u}^{o}=0.34 V ) and ( E_{Z n, Z n^{2+}}^{o}= ) ( -0.76 V ) | 12 |

399 | ( boldsymbol{A} boldsymbol{g} mid boldsymbol{A} boldsymbol{g}^{oplus}(boldsymbol{1} boldsymbol{M})left|boldsymbol{A} boldsymbol{g}^{oplus}right| boldsymbol{A} boldsymbol{g} ) ( 0.5 mathrm{F} ) electricity is first passed in this LHS (anode) and 1 F of electricity is passed in the RHS (cathode) making them independent electrolytic cells at 298 K. EMF of the cell after electrolysis will: A. increase B. decrease c. not change D. none of the above | 12 |

400 | Balanced equation of the reaction of formation of ( P b O_{2} ) at the anode is ( P b^{2+}(a q)+x H_{2} O rightleftharpoons P b O_{2} downarrow ) ( +boldsymbol{y} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q})+boldsymbol{z} boldsymbol{e}^{-} ) What will be value of y? | 12 |

401 | Assertion If ( boldsymbol{lambda}_{N a^{+}}^{circ} ) and ( boldsymbol{lambda}_{C l^{-}}^{circ} ) are molar limiting conductivity of sodium and chloride ions respectively, then the limiting molar conductivity for sodium chloride is given by the equation: ( wedge_{N a C l}^{circ}= ) ( boldsymbol{lambda}_{N a^{+}}^{circ}+boldsymbol{lambda}_{C l^{-}}^{circ} ) Reason This is according to Kohlrausch law of independent migration of ions. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

402 | Given the following molar conductivity at infinite dilution and ( 25^{circ} mathrm{C} ) ( mathrm{HCl}: wedge_{m}^{infty}=426.2 mathrm{S} mathrm{cm}^{2} mathrm{mol}^{-1} mathrm{KCl}: wedge_{m}^{infty}= ) ( 114.42 mathrm{S} mathrm{cm}^{2} mathrm{mol}^{-1} mathrm{CH}_{3} mathrm{COOK}: wedge_{m}^{infty}= ) ( 149.86 mathrm{s} mathrm{cm}^{2} mathrm{mol}^{-1} ) The molar conductance at infinite dilution and ( 25^{circ} mathrm{C}, ) for acetic acid solution is: A. ( 390.76 mathrm{Scm}^{2} mathrm{mol}^{-1} ) B . ( 461.86 mathrm{Scm}^{2} mathrm{mol}^{-1} ) c. ( 289.63 mathrm{Scm}^{2} mathrm{mol}^{-1} ) D. ( 172.94 mathrm{Scm}^{2} mathrm{mol}^{-1} ) | 12 |

403 | Electrolysis involves conversion of chemical energy to electrical energy. A. True B. False | 12 |

404 | Consider the table of standard reduction potentials shown below. Half-reaction [ begin{array}{ll} C l_{2}+2 e^{-} rightarrow 2 C l^{-} & 1.36 V \ O_{2}+4 H^{+}+4 e^{-} rightarrow 2 H_{2} O & 1.23 V \ 2 H_{2} O+2 e^{-} rightarrow H_{2}+2 O H^{-} & -0.83 V \ R b^{+}+e^{-} rightarrow R b & -2.93 V end{array} ] Use the information from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when an aqueous solution of rubidium chloride undergoes electrolysis. ( mathbf{A} cdot 2 R b^{+}+2 C l^{-} rightarrow 2 R b+C l_{2} ) B ( cdot 2 H_{2} O rightarrow 2 H_{2}+O_{2} ) ( mathbf{c} cdot H_{2}+2 O H^{-}+2 R b^{+} rightarrow 2 R b+2 H_{2} O ) ( mathbf{D} cdot 4 C l^{-}+O_{2}+4 H^{+} rightarrow 2 H_{2} O+2 C l_{2} ) | 12 |

405 | Calculate the electrode potential at a copper electrode dipped in a ( 0.1 M ) solution of copper sulphate at ( 25^{circ} mathrm{C} ). The standard electrode potential of ( C u^{2+} / C u ) system is 0.34 volt at ( 298 K ) | 12 |

406 | Chromium plating can involve the electrolysis of an electrolyte of an acidified mixture of chromic acid and chromium sulphate. If during electrolysis the article being plated increases in mass by ( 2.6 mathrm{g} ) and ( 0.6 mathrm{dm}^{3} ) of oxygen are evolved at an inert anode, the oxidation state of chromiumions being discharged must be : (assuming atomic weight of ( mathrm{Cr}=52 ) and 1 mole of gas at room temperature and pressure occupies a volume of ( left.24 d m^{3}right) ) A . -1 в. Zero ( c cdot+1 ) D. +2 | 12 |

407 | Which of the following oxide(s) of iron would be obtained on prolonged reaction of iron with steam? A. FeO в. ( F e_{2} O_{3} ) ( mathbf{c} cdot F e_{3} O_{4} ) D. ( F e_{2} O_{3} ) and ( F e_{3} O_{4} ) | 12 |

408 | Copper sulphate solution ( (250 mathrm{ml}) ) was electrolysed using a platinum anode and a copper cathode. A constant current of ( 2 mathrm{mA} ) was passed for 16 minutes. It was found that after electrolysis, the absorbance of the solution was reduced to ( 50 % ) of its original value. Calculate the concentration of copper sulphate in the solution to begin with. A ( .0 .22 M ) в. 2 М c. ( 0.04 M ) D. ( 0.13 M ) | 12 |

409 | The standard ( E_{r e d}^{o} ) values of ( A, B ) and ( C ) ( operatorname{are}+mathbf{0 . 6 8} boldsymbol{V},-mathbf{2 . 5 4} boldsymbol{V},-mathbf{0 . 5 0} boldsymbol{V} ) respectively. The order of their reducing power is: A. ( A>B>C ) в. ( A>C>B ) c. ( C>B>A ) D. ( B>C>A ) | 12 |

410 | If a current of 1.5 ampere flows through a metallic wire for 3 hours, then how many electrons would flow through the wire? A ( cdot 2.25 times 10^{22} ) electrons B. ( 1.13 times 10^{23} ) electrons C ( cdot 1.01 times 10^{23} ) electrons D. ( 4.5 times 10^{23} ) electrons | 12 |

411 | Which one of the following conditions will increase the voltage of the cell represented by the equation? ( boldsymbol{C u}(s)+mathbf{2 A g}^{+}(boldsymbol{a q} .) rightleftharpoons boldsymbol{C u}^{2+}(boldsymbol{a q} .)+ ) ( mathbf{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s}) ) A. Increase in the dimension of ( C u ) electrode B. Increase in the dimension of ( A g ) electrode C. Increase in the concentration of ( C u^{2+} ) ion D. Increase in the concentration of ( A g^{+} ) ion | 12 |

412 | The electrode potentials for ( boldsymbol{C u}^{2+}(boldsymbol{a q})+boldsymbol{e}^{-} rightarrow ) ( boldsymbol{C u}^{+}(boldsymbol{a q}) ) and ( boldsymbol{C u}^{+}(boldsymbol{a q})+boldsymbol{e}^{-} rightarrow boldsymbol{C u}(boldsymbol{s}) ) are ( +0.15 mathrm{V} ) and +0.50 respectively. The value of ( boldsymbol{E}^{0} boldsymbol{C u}^{2+} mid boldsymbol{C u} ) will be : A . ( 0.500 mathrm{v} ) B. 0.325 ( c .0 .650 v ) D. 0.150 | 12 |

413 | If a half cell ( boldsymbol{X} mid boldsymbol{X}^{2+}(mathbf{0 . 1} boldsymbol{M}) ) is connected to another half cell ( boldsymbol{Y} mid boldsymbol{Y}^{2+}(mathbf{1} . mathbf{0} boldsymbol{M}) ) by means of ( mathbf{a} ) salt bridge and an external circuit at ( 25^{circ} C, ) the cell voltage would be: ( mathbf{A} cdot 0.06 V ) B. ( 0.12 V ) c. ( 0.62 V ) D. ( 0.72 V ) | 12 |

414 | Electrolyte ( quad wedge^{infty}left(S c m^{2} m o l^{-1}right) ) ( K C l quad 149.9 ) ( K N O_{3} ) 145.0 ( H C l quad 426.2 ) ( N a O A c quad 91.0 ) ( N a C l quad 126.5 ) Calculate ( Lambda^{infty}_{H O A c} ) using appropriate molar conductances of the electrolytes listed above at infinite dilution with ( H_{2} O ) at ( 25^{circ} mathrm{C} ? ) A. 217. 5 ( operatorname{Scm}^{2} ) mol ( ^{-1} ) В. 390.7 ( S c m^{2} ) mol ( ^{-1} ) c. ( 552.7 mathrm{Scm}^{2} mathrm{mol}^{-1} ) D. 517.2 ( S c m^{2} m o l^{-1} ) | 12 |

415 | Q. 42 When acidulated water (dil. H.SO, solution) is electrolyse the solution be affected ? Justify your answer. olutions, pH of the 250, solution) is electrolysed, with pH of | 12 |

416 | If ( E_{1}^{o}, E_{2}^{o} ) and ( E_{3}^{o} ) are standard oxidation potentials for ( boldsymbol{F e}left|boldsymbol{F} boldsymbol{e}^{2+}, boldsymbol{F} boldsymbol{e}^{2+}right| boldsymbol{F} boldsymbol{e}^{3+} ) and ( boldsymbol{F} e mid boldsymbol{F} e^{3+}, ) then ( boldsymbol{E}_{3}^{o}=frac{boldsymbol{E}_{2}^{o}+boldsymbol{2} boldsymbol{E}_{1}^{o}}{boldsymbol{n}} . ) The value of ( n ) is: | 12 |

417 | The efficiency of a fuel cell is ( 80 % ) and the standard heat of reaction is ( -300 k J . ) The reaction involves two electrons in redox change. ( boldsymbol{E}^{ominus} ) for the cell is: A . ( 1.24 V ) B . ( 2.48 V ) c. ( 0 V ) D. ( 0.62 V ) | 12 |

418 | If the solution of the ( C u S O_{4} ) in which copper rod is immersed in diluted to 10 times, the oxidation electrode potential: A. increase by 0.030 volt B. decrease by 0.30 volt c. increase by 0.059 volt D. decrease by 0.0059 volt | 12 |

419 | State True or False. In an electrode concentration cell, the cell reaction ( mathrm{Zn}left(mathrm{C}_{1}right) rightarrow mathrm{Zn}left(mathrm{C}_{2}right) ) will be spontaneous if ( mathbf{c}_{1}>mathbf{c}_{2} ) A. True B. False | 12 |

420 | The U shaped vessel used in Nelson cell is lined inside with asbestos which: A. helps in the separation of cathode and anode compartments B. acts as an insulator. C. helps ( H^{+} ) ions to reduced to ( H_{2} ) gas D. allows the dissociation of steam. | 12 |

421 | A dilute aqueous solution of sodium fluoride is electrolyzed, the products at the anode and cathode are: A. ( O_{2}, H_{2} ) в. ( F_{2}, ) Na ( c cdot O_{2}, N a ) D. ( F_{2}, H_{2} ) | 12 |

422 | ( boldsymbol{C d}(s)left|boldsymbol{C d C l}_{2}(mathbf{0 . 1 0} boldsymbol{M})right| boldsymbol{A} boldsymbol{g} boldsymbol{C l}(boldsymbol{s}) mid boldsymbol{A} boldsymbol{g}(s ) The EMF of the above cell is 0.6315 V at ( 0^{circ} mathrm{C} ) and ( 0.6753 mathrm{V} ) at ( 25^{circ} mathrm{C} ). The ( Delta H ) of reaction in ( mathrm{kJ} ) at ( 25^{circ} mathrm{C} ) is: A . – 176 B. – 234.7 c. 123.5 D . – 167.6 | 12 |

423 | Explain refining of nicket by mond process. State kohlarausch’s law | 12 |

424 | Assertion: Electrode potential for the electrode ( M^{n+} mid M ) with concentration is given by the expression under STP conditions; ( boldsymbol{E}=boldsymbol{E}^{ominus}+frac{mathbf{0 . 0 5 9}}{boldsymbol{n}} log left[boldsymbol{M}^{boldsymbol{n}+}right] ) Reason: STP conditions require the temperature to be ( 273 mathrm{K} ) A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

425 | The cell EMF is independent of the concentration of the species of the cell in: A ( cdot operatorname{Fe}^{ominus}|operatorname{KOH}(a q)| N i O(s)left|N i_{2} O_{3}(s)right| N i ) B ( cdot P tleft|left(H_{2}right)right| H C l midleft(C l_{2}right) P t ) ( mathbf{c} cdot Z nleft|Z n^{2+} | C u^{2+}right| C u ) D. ( H g, H g_{2} C l_{2}left|K C l | A g N O_{3}right| A g ) | 12 |

426 | Which of the following metal do no evolve ( boldsymbol{H}_{2} ) gas from dil. acid? A ( cdot Aleft(E_{A^{+} / A}^{o}=0.25 Vright) ) B ( cdot Bleft(E_{B / B^{+}}^{0}=+0.22 Vright) ) c. ( Cleft(E_{C^{+} / C}^{0}=0.30 Vright) ) D・ ( Dleft(E_{D / D^{+}}^{0}=+0.44 Vright) ) | 12 |

427 | Solid calcium oxide reacts vigorously with water to form calcium hydroxide accompanied by liberation of heat. This process is called slaking of lime. Which among the following is (are) true about slaking of lime? (i) It is an endothermic reaction (ii) It is an exothermic reaction (iii) The pH of the resulting solution will be more than seven (iv) The pH of the resulting solution will be less than seven A ( cdot ) (i) and (ii) B. (ii) and (iii) c. (i) and (iv) D. (iii) and (iv) | 12 |

428 | Given, Question 9. The molar conductivity of 0.025 mol L methanoic acid is 46.1 S cm’ mol-. Calculate its degree of dissociation and dissociation constant. 2°(H+)= 349.6 S cmmol-1 and 2°(HC00 ) = 54.6 S cm mol-. (1) Degree of dissociation, a is related to conductivity as a u m Am is given. Calculate an by using Kohlrausch’s law. (ii) Calculate K, as Kara and we know Cand a both. of COOH | 12 |

429 | A button cell used in watches functions as following: ( Z n(s)+A g_{2} O(s)+H_{2} O(l) rightleftharpoons ) ( 2 A g(s)+Z n^{2+}(a q)+2 O H^{-}(a q) ) If half cell potentials are: ( Z n^{2+}(a q)+2 e^{-} rightarrow Z n(s) ; E^{circ}= ) ( -0.76 V ) ( boldsymbol{A} boldsymbol{g}_{2} boldsymbol{O}(boldsymbol{s})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l})+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s})+ ) ( mathbf{2 O H}^{-}(boldsymbol{a q}), boldsymbol{E}^{circ}=mathbf{0 . 3 4} boldsymbol{V} ) The cell potential will be: A. ( 1.10 v ) B. 0.42 c. ( 0.84 mathrm{v} ) D. 1.34 | 12 |

430 | Energy efficiency during electroplating is usually in the range: ( A cdot 50 ) to ( 70 % ) B. 80 to 85 % c. 85 to ( 90 % ) D. 90 to 99 % | 12 |

431 | A depolarizer used in dry cell is: A. ammonium chloride B. manganese dioxide C . potassium oxide D. sodium phosphate | 12 |

432 | Q. 16 A, (NH, OH) is equal to ………. (a) Am (NH4OH) + Am (NH, CI – A (HC) (b) Am (NH, C + Am (NaOH) – NaCl (c) AM (NH4C) + Am (NaCl) – (NaOH | (d) Am (NaOH + Am (NaCl) – A (NH, CI) Thinking Process This question is based on the concept of Kohlrausch law and can be solved by using the concept involved in calculation of limiting molar conductivity of any salt. According to Kohlrausch law limiting molar conductivity of any salt is equal to sum of limiting molar conductivity of individual molar conductivity of cations and anions of electrolyte. | 12 |

433 | The standard reduction potential of ( A g^{+} mid A g ) electrode is 0.80 volt. Calculate the standard electrode potential of ( boldsymbol{C l}^{-}|boldsymbol{A} boldsymbol{g} boldsymbol{C l}| boldsymbol{A} boldsymbol{g} ) at ( boldsymbol{2} boldsymbol{5}^{circ} boldsymbol{C} ) Given solubility product, ( boldsymbol{K}_{s p}(boldsymbol{A} boldsymbol{g} boldsymbol{C l})= ) ( 1.8 times 10^{-10} ) | 12 |

434 | Which of the following metals has been used for building boats because it has resistance to corrosion by sea water? A. copper B. Nickel c. Fungsten D. Titanium | 12 |

435 | A decinormal solution of ( A g N O_{3} ) was electrolysed between Pt electrodes. After passing a small current for two hours, a fall of concentration of 0.0005124 equivalent occurred in anodic solution. The mass of copper deposited in copper coulometer placed in series was found to be 0.03879 g. Find the transport number of ( N O_{3}^{-} ) in ( A g N O_{3} . ) Write answer to the nearest integer after multiplying transport number calculated with 10. | 12 |

436 | When an aqueous solution of sodium fluoride is electrolysed, the gas liberated at anode is ( O_{2} ) If true enter 1 , else enter 0 . | 12 |

437 | Formulate a cell from the following electrode reactions: (a) ( C I_{2(g)}+2 e^{-} longrightarrow 2 C I_{(a q)}^{-} ) ( (b) 2 I_{(a q)} longrightarrow I_{2(s)}+2 e^{-} ) | 12 |

438 | Calculate the solubility product constant of ( A g I ) from the following values of standard electrode potentials. ( E_{A g^{+} / A g}^{circ}=0.80 ) volt and ( E_{I / A g I / A g}^{circ}= ) -0.15 volt at ( 25^{circ} C ) | 12 |

439 | In the refining of silver by electrolytic method what will be the weight of 100 g Ag anode if 5 ampere current is passed for 2 hours? Purity of silver is ( 95 % ) by weight. in gram is: A . 57 B. 32 c. 60 D. 13 | 12 |

440 | How long (approximate) should water be electrolysed by passing through 100 amperes current so that the oxygen released can completely burn ( 27.66 g ) of diborane? (Atomic weight of ( boldsymbol{B}=mathbf{1 0 . 8 u} ) ) A. 3.2 hours B. 1.6 hours c. 6.4 hours D. 0.8 hours | 12 |

441 | Kunal took few iron turnings and mixed them well with Sulphur powder. He could separate the iron turnings with the help of a magnet. He heated the mixture for some time and tried to separate the iron turnings with the magnet but he could not. Why? A. on heating, a chemical change takes place and a new compound is formed. B. on heating, iron becomes non-magnetic hence, it is not attracted by magnettet c. on heating, a physical change takes place hence iron and Sulphur gets mixed up D. on heating, iron evaporates and only sulphur is left behind | 12 |

442 | Assertion: Rusting of Fe is quicker in saline water than in ordinary water. Reason: Presence of ( N a^{+} ) and ( C l^{-} ) ions increase the conductance of the saline water A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

443 | ( A g N O_{3}(a q .) ) was added to an aqueous ( K C l ) solution gradually and the conductivity of the solution was measured. The plot of conductance ( (wedge) ) versus the volume of ( boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3} ) is ( (mathbf{R}) ) ( (mathbf{S}) ) A ( cdot(P) ) B. ( (Q) ) c. ( (R) ) D. ( (S) ) | 12 |

444 | Saturated solution of ( K N O_{3} ) is used to make salt bridge because: A. velocity of ( K^{+} ) ion is greater than that of ( N O_{3}^{-} ) ion B. velocity of ( N O_{3}^{-} ) ion is greater than that of ( K^{+} ) ion C. velocities of both ( K^{+} ) and ( N O_{3}^{-} ) ions are nearly the same D. ( K N O_{3} ) is highly soluble in water | 12 |

445 | How is rust formed? | 12 |

446 | Which expression gives the correct value for the standard potential for a gold-rhodium voltaic cell? Half-reaction ( mathbb{E}^{circ}(mathbf{V}) ) ( R h_{(q q)}^{+3}+3 e^{-} rightarrow R h_{(s)} ) ( A u_{(q q)}^{+}+e^{-} rightarrow A u_{(s)} ) A . ( 1.69 V+0.76 V ) B . ( 1.69 V-0.76 V ) c. ( 3(1.69) V+0.76 V ) D. ( 3(1.69) V-0.76 V ) | 12 |

447 | The specific conductance of a saturated solution of AgCl in water is ( 1.826 times ) ( 10^{-6} Omega^{-1} mathrm{cm}^{-1} ) at ( 25^{circ} mathrm{C} ) calculate its solubility in water at ( 25^{circ} mathrm{C} ) Given that ( :-lambda^{circ}left(A g^{+}right)=61.92 ) [ boldsymbol{lambda}^{circ}left(mathbf{C l}^{-}right)=mathbf{7 6 . 3 4} ] | 12 |

448 | For cell reaction ( : Z n+C u^{2+} rightarrow Z n^{2}+ ) ( C u ) cell representation is: A ( cdot Z nleft|Z n^{2+} | C u^{2+}right| C u ) в. ( C uleft|C u^{2+} | Z n^{2+}right| Z n ) c. ( C uleft|Z n^{2+}right||Z n| C u^{2+} ) D. ( C u^{2+}left|Z n | Z n^{2+}right| C u ) | 12 |

449 | 0.59 Assertion (A) A, for weak electrolytes shows a sharp increase when the electrolytic solution is diluted. Reason (R) For weak electrolytes degree of dissociation increases with dilution of solution. | 12 |

450 | The concentration of ( K^{+} ) in interior and exterior of a Nerve cell are ( 500 mathrm{mM} ) and ( 25 mathrm{mM} ) respectively. The electrical potential (in volt) that exists across the membrane is : ( left[log _{10} 2=right. ) ( mathbf{0 . 3}, mathbf{2 . 3 0 3} boldsymbol{R} boldsymbol{T} / boldsymbol{F}=mathbf{0 . 0 6}] ) (Given answer be multiplying with 1000) | 12 |

451 | When the power delivered by a 100 volt battery is 40 watts, the equivalent resistance of the circuit is: A. 100 ohms B. 250 ohms c. 300 ohms D. 350 ohms | 12 |

452 | When lead storage battery is charged: A. lead dioxide dissolves B. sulphuric acid is regenerated C. lead electrode becomes coated with lead sulphate D. the concentration of sulphuric acid decreases | 12 |

453 | Question 15. A solution of Ni(NO3)2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 min. What mass of Ni is deposited at the cathode? (Atomic mass of Ni= 58.7) W (0) Find the quantity of electricity used by the formula, Q = i xt. Feb (1) Write the balance equation for the electrolysis of Ni(NO3), to find the quantity of electricity used to deposit 1 mole (58.7 g mol-‘) Ni. (iii) Apply the mole concept for calculating the mass of Ni. . | 12 |

454 | When 4.0 A of current is passed through a ( 1.0 mathrm{L}, 0.10 mathrm{M} F e^{3+}(a q) ) solution for 1.0 hour, it is partly reduced to ( mathrm{Fe}(mathrm{s}) ) and partly of ( boldsymbol{F e}^{2+}(boldsymbol{a q}) ). The correct statements(s) is/are: This question has multiple correct options A. 0.10 mol of electrons are required to convert all ( F e^{3} ) to ( F e^{2+} ) B. 0.025 mol of Fe(s) will be deposited. c. 0.075 mol of iron remains as ( F e^{2+} ) D. 0.050 mol of iron remains as ( F e^{2+} ) | 12 |

455 | The two aqueous solutions; ( boldsymbol{A}left(boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3}right) ) and ( boldsymbol{B}(boldsymbol{L} boldsymbol{i} boldsymbol{C l}) ) were electrolysed using Pt electrodes. The pH of the resulting solutions will : A. increase in A and decrease in B B. decrease in both c. increase in both D. decrease in A and increase in B | 12 |

456 | For a reaction, ( boldsymbol{A}(boldsymbol{s})+mathbf{2} boldsymbol{B}^{+} rightarrow boldsymbol{A}^{2+}+ ) ( 2 B, K_{c} ) has been found to be ( 10^{12} ). The ( boldsymbol{E}_{c e l l}^{o} ) is: A. ( 0.138 V ) ( V ) в. ( 0.235 mathrm{V} ) c. ( 0.354 V ) D. none of these | 12 |

457 | Electrolysis of sea-water produces ( C l_{2}(g) ) at the anode by the oxidation of Cl (aq) ions. What volume of the gas will be produced at STP by current of ( 1.50 mathrm{A} ) applied for 90.0 minutes? B. 0.548 L c. ( 0.94 mathrm{L} ) D. 0.470 L | 12 |

458 | A hydrogen electrode placed in a buffer solution of ( mathrm{CH}_{3} mathrm{COONa} ) and acetic acid in the ratio’s ( x: y ) and ( y: x ) has reduction electrode potential values ( mathrm{E}_{1} ) volt and ( mathrm{E}_{2} ) volt respectively at ( 25^{circ} mathrm{C} ). The ( mathrm{pK}_{a} ) values of acetic acid is ( left(mathrm{E}_{1} text { and } mathrm{E}_{2} ) are oxidation right. potential): A. ( frac{E_{1}+E_{2}}{0.118} ) в. ( frac{E_{2}-E_{1}}{0.118} ) c. ( -frac{E_{1}+E_{2}}{0.118} ) D. ( -frac{E_{2}-E_{1}}{0.118} ) | 12 |

459 | The term used to indicate the development of unpleasant smell and taste in fat and oil-containing foods due to aerial oxidation is: A . acidity B. radioactivity c. rabidity D. rancidity | 12 |

460 | The specmc conductances in oh ( m^{-1} c m^{-1} ) of four electrolytes ( P, Q, R ) and ( S ) are given in brackets: ( Pleft(5.0 times 10^{-5}right) ) ( Qleft(7.0 times 10^{-8}right) ) ( boldsymbol{R}left(mathbf{1} . mathbf{0} times mathbf{1 0}^{-mathbf{1 0}}right) ) ( boldsymbol{S}left(boldsymbol{9} cdot boldsymbol{2} times mathbf{1} boldsymbol{0}^{boldsymbol{3}}right) ) The one that offers highest resistance to the passage of electric current is: A . ( P ) в. ( Q ) ( c . s ) D. ( R ) | 12 |

461 | At infinite dilution stage, the solution of ( C H_{3} C O O H ) in water does not contain : A. ( H^{+} ) ion в. ( C H_{3} C O O^{-} ) ion c. ( C H_{3} C O O H ) molecule D. all of these | 12 |

462 | (A) Define the following terms: (i) Limiting molar conductivity (ii) Fuel cell (B) Resistance of a conductivity cell filled with 0.1 mol ( L^{-1} ) KCl solution is 100Omega. If the resistance of the same cell when filled with 0.02 mol ( L^{-1} ) KCl solution is ( 540 Omega ), calculate the conductivity and molar conductivity of 0.02 mol ( L^{-1} K C l ) solution. The conductivity of 0.1 mol ( L^{-1} ) KCl solution is ( 1.29 times 10^{-2} Omega^{-1} mathrm{cm}^{-1} ) | 12 |

463 | Select the correct statements about galvanic cells. This question has multiple correct options A. Electrons are fed into anode by the oxidation reaction that takes place at the electrode. B. The anode pushes these electrons into the external circuit and thus, acts as a source of negative charge. C. The cathode acts as an electron sink and thus, called positive electrode. D. The algebraic sum of E ( _{O P} ) of anode and E ( _{O P} ) of cathode gives the +ve value for spontaneous process. | 12 |

464 | The maximum work that can be obtained from the cell ( boldsymbol{A l}left|boldsymbol{A l}^{3+}(mathbf{0 . 1} boldsymbol{M}) | boldsymbol{F} boldsymbol{e}^{boldsymbol{2}+}(boldsymbol{0 . 2} boldsymbol{M})right| boldsymbol{F e} ) is: ( left[text { Given }: boldsymbol{E}_{A l^{3+} / A l}^{o}=-mathbf{1 . 6 6} mathbf{V} ) and right. ( left.boldsymbol{E}_{boldsymbol{F} e^{2+} / boldsymbol{F} e}^{boldsymbol{o}}=-mathbf{0 . 4 4} boldsymbol{V}right] ) A. ( 605.8 mathrm{kJ} ) B. 505.8 kJ c. 705.8 kJ D. 905.8 kJ | 12 |

465 | Given ( : boldsymbol{H}_{2} boldsymbol{O}_{2} rightarrow boldsymbol{O}_{2}+boldsymbol{2} boldsymbol{H}^{oplus}+boldsymbol{2} boldsymbol{e}^{-} ) ( boldsymbol{E}^{ominus}=-mathbf{0 . 6 9} boldsymbol{V} ) ( boldsymbol{H}_{2} boldsymbol{O}_{2}+boldsymbol{2} boldsymbol{H}^{oplus}+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O} ) ( boldsymbol{E}^{ominus}=mathbf{1 . 7 7} boldsymbol{V} ) ( boldsymbol{I}^{ominus} rightarrow+mathbf{2} e^{-} ) ( boldsymbol{E}^{ominus}=-mathbf{0 . 5 3 5} boldsymbol{V} ) Which of the following statements is / (are) correct? This question has multiple correct options ( mathbf{A} cdot H_{2} O_{2} ) behaves as an oxidant for ( I_{2} / I^{ominus} ) B. ( H_{2} O_{2} ) behaves as an reductant for ( I_{2} / I^{ominus} ) C ( cdot I^{ominus} / I_{2} ) behaves as an reductant for ( H_{2} O_{2} ) D. None of these is correct. | 12 |

466 | Assertion: It is safe to stir ( 1 mathrm{M} A g N O_{3} ) solution with a copper spoon. [ begin{aligned} text { Reason: } boldsymbol{E}_{boldsymbol{A} boldsymbol{g} oplus mid boldsymbol{A} boldsymbol{g}}^{ominus} &=mathbf{0 . 8 0} boldsymbol{V} \ boldsymbol{E}_{boldsymbol{C u}^{2+} mid boldsymbol{C u}}^{ominus} &=mathbf{0 . 3 4} boldsymbol{V} end{aligned} ] A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

467 | In a dry cell containing a moist paste of plaster of Paris, ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{C l} ) and ( Z n C l ) acts as A. copper vessel, Cathode B. zinc vessel, Cathode c. zinc vessel, Anode D. copper vessel, Anode | 12 |

468 | The apparatus in which electrical energy is converted into chemical energy is known as: A. voltameter B. coulometer ( c cdot operatorname{both}(A) ) and ( (B) ) D. none of these | 12 |

469 | Resistance of ( 0.2 M ) solution of an electrolyte is ( 50 Omega ). The specific conductance of the solution is ( 1.4 S ) ( m^{-1} . ) The resistance of ( 0.5 M ) solution of the same electrolyte is ( 280 Omega ). The molar conductivity of ( 0.5 ~ M ) solution of the electrolyte in ( S m^{2} m o l^{-1} ) is: A ( .5 times 10^{3} ) В . ( 5 times 10^{2} ) c. ( 5 times 10^{-4} ) D. ( 5 times 10^{-3} ) | 12 |

470 | In an experiment set up for the measurement of EMF of a half cell using reference electrode and a salt bridge, when the salt bridge is removed, the voltage: A. Does not change B. Increase to maximum c. Decreases to half the value D. Drops to zero | 12 |

471 | In corrosion of iron, A. electrons flow from anode to cathode through the metal, while ions flow through the water droplets B. an electrochemical (galvanic) cell is formed in which ( F e ) acts as anode and ( O_{2} ) is reduced at cathode C ( . ) dissolved ( O_{2} ) oxidizes ( F e^{2+} ) to ( F e^{3+} ) before it is deposited as rust ( left(F e_{2} O_{3} cdot x H_{2} Oright) ) D. All of the above takes place | 12 |

472 | Among ( N a, H g, S, P t, ) and graphite which can be used as electrodes in electrolytic cell having aqueous solutions ? A. ( N ) aand ( S ) в. ( H g, P t ), and ( S ) c. ( N a, H g ), and ( S ) D. ( H g, P t ), and graphite | 12 |

473 | For an electrochemical reaction occuring in a galvanic cell. ( mathbf{2} boldsymbol{F} boldsymbol{e}_{(boldsymbol{a q})}^{+mathbf{3}}+boldsymbol{Z} boldsymbol{n}_{(s)} rightarrow boldsymbol{Z} boldsymbol{n}_{(a q)}^{+2}+mathbf{2} boldsymbol{F} boldsymbol{e}_{(a q)}^{+mathbf{2}} ) if concentration of ( F e^{+2} ) is increased. A. ( E_{text {cll}} ) will remain unchanged B. ( E_{text {cll}} ) will decrease c. ( p H ) of the solution will change D. less non P-V work will be obtained | 12 |

474 | On passing a current through molten KCI ( 19.5 mathrm{g} ) of ( mathrm{K} ) is deposited. The amount of ( mathrm{Al} ) deposited by the same quantity of electricity if passed through molten AlCl is : A. ( 4.5 mathrm{g} ) B. ( 9.0 mathrm{g} ) c. ( 13.5 mathrm{g} ) D. 27 g | 12 |

475 | Acidified water is electrolysed by using carbon electrodes.What is produced at negative carbon electrode? | 12 |

476 | An alloy weighing 1.05 g of ( P b-A g ) was dissolved in desired amount of ( H N O_{3} ) and the volume was made 350 ( mathrm{mL} . ) An ( mathrm{Ag} ) electrode was dipped in solution and ( E_{text {cell}} ) of the cell K. The percentage of lead in alloy is (divide answer by 25 ) : Given: ( boldsymbol{E}_{A boldsymbol{g}^{+} / boldsymbol{A} boldsymbol{g}}^{o}=mathbf{0 . 8 0} boldsymbol{V} ) | 12 |

477 | In passing ( 3 mathrm{F} ) of electricity through three electrolytic cells connected in series containing ( boldsymbol{A} boldsymbol{g}^{oplus}, boldsymbol{C} boldsymbol{a}^{2+}, boldsymbol{a} boldsymbol{n} boldsymbol{d} boldsymbol{A} boldsymbol{l}^{3} ) ions, respectively. The molar ratio in which the three metal ions are liberated at the electrode is: A. 1: 2: 3 B . 2: 3: 1 c. 6: 3: 2 D. 3: 4: 2 | 12 |

478 | During the electrolysis of the aqueous solution of copper sulphate using Pt electrodes, the reaction taking place at anode electrode is: A ( cdot C u^{2+}+2 e^{-} rightarrow C u ) в. ( C u rightarrow C u^{2+}+2 e^{-} ) ( mathbf{c} cdot 2 H_{2} O rightarrow 4 H^{+}+O_{2}+4 e^{-} ) ” ( quad H_{2} O+e^{-} rightarrow O H^{-}+frac{1}{2} H_{2} ) | 12 |

479 | Write Nernst equation for Daniel cell at equilibrium condition and derive relationship between ( E_{(text {cell})}^{o} ) and equilibrium constant ( left(boldsymbol{K}_{c}right) ) | 12 |

480 | Which of the following electrolytic solutions has the least specific conductance? A. ( 0.002 mathrm{N} ) N ( mathrm{N} ) N ( . .0000 ) B. ( 0.1 N ) c. ( 0.2 N ) D. ( 2 N ) | 12 |

481 | Using Pt electrodes same quantity of electricity is passed in ( mathbf{0 . 0 3} M A I C I_{3}, 0.01 M A I C I_{3}, 0.01 M A g ) solutions. If 0.36 g silver is deposited what is the mass of Al deposited in two ( A I C I_{3} ) solutions and volume of ( O_{2} ) evolved at STP in NaOH solution? | 12 |

482 | The technique of protecting a metal from corrosion by connecting it to a second metal (that is more easily oxidized) is called: A. galvanization B. anodic protection C . cathodic protection D. sacrificial protection | 12 |

483 | Give equations for the racharging of a lead storage battery. | 12 |

484 | What is molar conductivity? How is it related to the concentration of electrolyte? | 12 |

485 | Peroxodisulphate salts (e.g., ( N a_{2} S_{2} O_{8} ) ) are strong oxidizing agents used as bleaching agents for fats, oils, etc. Given : ( O_{2}(g)+4 H^{oplus}(a q)+4 e^{-} rightarrow 2 H_{2} O(l) ) ( E^{ominus}=1.23 V ) ( S_{2} O_{8}^{2-}(a q)+2 e^{-} rightarrow S O_{4}^{2-}(a q) ) ( E^{ominus}=2.01 V ) Which of the following statements is (are) correct? This question has multiple correct options A. Oxygen gas can oxidize sulphate ion to per-oxo disulphate ion ( left(S_{2} O_{8}^{2-}right) ) in acidic solution в. ( O_{2}(g) ) is reduced to water c. water is oxidized to ( O_{2} ) D. ( S_{2} O_{8}^{2-} ) ions are reduced to ( S O_{4}^{2-} ) ions | 12 |

486 | The amount of chlorine evolved by passing 2 A of current in an aqueous solution of ( N a C l ) for 30 minutes is: A. 2.648 в. ( 1.32 mathrm{g} ) c. ( 3.62 g ) D. ( 4.22 mathrm{g} ) | 12 |

487 | The bulb does not glow in the set up shown in the figure. List the possible reasons. Explain your answer. | 12 |

488 | Equivalent conductance and molar conductance of ( boldsymbol{F e}_{2}left(boldsymbol{S} boldsymbol{O}_{4}right)_{3} ) are related by relation: ( mathbf{A} cdot wedge_{e}=Lambda_{m} ) B ( cdot wedge_{e q}=frac{Lambda_{m}}{3} ) ( mathbf{C} cdot wedge_{e q}=3 wedge_{m} ) D ( cdot wedge_{e q}=frac{Lambda_{m}}{6} ) | 12 |

489 | os 0.27 For the given cell, Mg Mg2+ || Cu2+ Cu (a) Mg is cathode (b) Cu is cathode (c) The cell reaction is Mg + Cu2+ Mg2+ + Cu (d) Cu is the oxidising agent | 12 |

490 | While charging the lead storage battery, This question has multiple correct options ( mathbf{A} cdot P b S O_{4} ) on anode is reduced to ( P b ) B. ( P b S O_{4} ) on cathode is reduced to ( P b ) ( mathrm{C} cdot P b S O_{4} ) on cathode is oxidised to ( P b ) D. ( P b S O_{4} ) on anode is oxidised to ( P b O_{2} ) | 12 |

491 | In cell representation, oxidation half cell is represented on the: A. Ieft hand side B. right hand side c. salt bridge D. none of the above | 12 |

492 | At ( p H=3 ) and rest all reductant and oxidant in change (I) being in standard state, ( M n O_{4}^{-} ) can oxidise: A ( cdot I^{-} ) and ( B r^{-} ) both B. ( I^{-} ) and ( C l^{-} ) both c. ( I^{-}, B r^{-} ) and ( C l^{-} ) all D. ( B r^{-} ) and ( C l^{-} ) both | 12 |

493 | Which statements about conductivity of distilled water are correct? This question has multiple correct options A. It possesses almost non-conducting nature B. It is obtained by distillation of water several times C. It is contaminated with little acid D. None of the above | 12 |

494 | Question 14. When acidulated water (dil. H2SO4 solution) is electrolysed, will the pH of the solution be affected? Justify your answer. | 12 |

495 | Assertion In a Daniell cell, if the concentration of ( C u^{2+} ) and ( Z n^{2+} ) ions are doubled, the EMF of the cell will be doubled. Reason f the concentration of ions in contact with metals is doubled, the electrode potential is doubled. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

496 | (a) Write Faraday’s second law of electrolysis (b) Draw labelled diagram of standard Hydrogen electrode | 12 |

497 | Give reasons. ( boldsymbol{E}^{o} ) value for ( boldsymbol{M} boldsymbol{n}^{3+} / boldsymbol{M} boldsymbol{n}^{2+} ) couple is much more positive than that for ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+} / boldsymbol{F} boldsymbol{e}^{boldsymbol{2}+} ) | 12 |

498 | Time required to deposit one millimole of aluminium metal by the passage of 9.65 amperes through aqueous solution of aluminium ion is : A . ( 30 s ) в. ( 10 s ) c. ( 30,000 s ) D. ( 10,000 s ) | 12 |

499 | Find the mass of silver deposited when a current of 1.5 ampere is passed through silver nitrate solution for 5 min. (Atomic mass of ( A g ) is 108 g) | 12 |

500 | A hydrogen gas. electron is made by dipping platinum wire in a solution of ( H C I ) of ( p H=10 ) and by passing hydrogen gas around the platinum wire at one atm pressure.The oxidation potential of electrode would be? A . ( 1.18 V ) в. ( 0.059 V ) c. ( -0.59 V ) D. ( 0.118 mathrm{V} ) | 12 |

501 | Through a solution of ( C u S O_{4}, ) a current of 3 amperes was passed for 2 hours. At cathode, ( 3 g ) of ( C u^{2+} ) ions were discharged. The current efficiency is : [At. wt. of ( boldsymbol{C u}=mathbf{6 3 . 5} ) ] A . ( 33.3 % ) B . ( 42.2 % ) % c. ( 48.7 % ) D . 54.4 % | 12 |

502 | Q Type your question “I 11 ( left.sqrt{boldsymbol{c}}(text {in } boldsymbol{m o l} / boldsymbol{L})^{1 / 2}right) ) for ( boldsymbol{K} boldsymbol{C l} ) solution? ( left(boldsymbol{y}=wedge_{m} ; boldsymbol{x}=sqrt{boldsymbol{c}}right) ) ( A ) B. ( c ) ( D ) | 12 |

503 | Theoretical efficiency of fuel cell is: A. nearly ( 60 % ) B. 50% c. ( 33 % ) D. nearly 100% | 12 |

504 | Resistance of a conductivity cell filled with 0.15 mol ( L^{-1} ) NaCl solution is ( 50 Omega ) If resistance of the same cell when filled with 0.02 mol ( L^{-1} ) NaCl solution is 500 ( Omega, ) calculate the conductivity of 0.02 mol ( L^{-1} ) NaCl solution. (The conductivity of 0.15 mol ( L^{-1} ) NaCl solution is ( 1.5 mathrm{s} / mathrm{m} ) ). | 12 |

505 | Consider the reaction, ( mathbf{2} boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{C} boldsymbol{d} rightarrow boldsymbol{2} boldsymbol{A} boldsymbol{g}+boldsymbol{C} boldsymbol{d}^{2} ) The standard electrode potentials for ( A g^{+} rightarrow A g ) and ( C d^{2+} rightarrow C d ) couples are 0.80 volt and -0.40 volt respectively. (i) What is the standard potential ( E^{circ} ) for this reaction? (ii) For the electrochemical cell, in which this reaction takes place which electrode is negative electrode? | 12 |

506 | Which of the following has the highest molar conductivity under similar conditions? A. Diamminedichloroplatinum (II) B. Tetraamminedichlorocobalt (III) Chloride c. Potassium hexacyanoferrate (II) D. Hexaaquachromium (III) chloride | 12 |

507 | Q. 25 Conductivity k, is equal to……… (6) (c) Am RA (a) 1 1 | 12 |

508 | Assertion The electrolysis of potassium iodide, ( mathrm{K} ) I produces electrical energy. Reason Electrolytic cells convert chemical energy into electrical energy A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

509 | At ( 25^{circ} C, ) the standard oxidation potential of ( Z n ) and ( A g ) in water are: ( Z n(s) rightarrow Z n^{+2}(a q)+2 e^{-}, E^{0}= ) ( 0.76 V ) and ( A g(s) rightarrow A g^{+}(a q)+e^{-}, E^{0}= ) ( -0.80 V ) Which of the following reaction actually takes place? A ( cdot Z n^{2+}(a q)+2 A g(s) rightarrow 2 A g^{+}(a q)+Z n(s) ) B. ( Z n(s)+2 A g^{+}(a q) rightarrow Z n^{2+}(a q)+2 A g(s) ) C. ( Z n^{2+}(a q)+2 A g^{+}(a q) rightarrow Z n(s)+2 A g(s) ) D. ( Z n(s)+A g(s) rightarrow Z n^{2+}(a q)+A g^{+}(a q) ) | 12 |

510 | An electric charge of 5 Faraday’s is passed through three electrolytes ( A g N O_{3}, C u S O_{4} ) and ( F e C l_{3} ) solution The grams of each metal liberated at cathode will be: A. ( A g=10.8 g, C u=12.7 g, F e=1.11 g ) в. ( A g=540 g, C u=367.5 g, F e=325 g ) c. ( A g=108 g, C u=63.5 g, F e=56 g ) D. ( A g=540 g, C u=158.8 g, F e=93.3 g ) | 12 |

511 | In a galvanic cell, the salt bridge (i) does not participate chemically in the cell reaction (ii) stops the diffusion of ions from one electrode to another (iii) is necessary for the occurrence of the cell reaction (iv) ensures mixing of the two electrolytic solutions. A. (i) and (iii) only B. (i) and (ii) only c. (iii) and (iv) only D. All of these | 12 |

512 | An acidic solution of ( C u^{2+} ) salts containing ( 0.4 mathrm{g} ) of ( C u^{2+} ) is electrolyzed until all the copper is deposited. The electrolysis is continued for seven more minutes with the volume of solution kept at ( 100 mathrm{mL} ) and the current at ( 1.2 mathrm{A} ) The volume (in ( mathrm{mL} ) ) of gases evolved at STP during the entire electrolysis is : (write your answer to nearest integer) | 12 |

513 | The conductivity ( left(operatorname{in} Omega^{-1} m^{-1}right) ) of ( K_{2} S O_{4} ) solution is: ( ( ) write your answer to nearest integer) | 12 |

514 | Define : Standard electrode potential. | 12 |

515 | Calculate the ( p H ) at which the potential of hydrogen electrode will be ( 0.059 V ) | 12 |

516 | (A) 1 faraday ( =96,500 ) coulomb. It is a charge of 1 mole electrons. (R) 1 faraday charge liberates one gram equivalent of substance at an electrode. A. Both (R) and (A) are true and reason is the. correct explanation of assertion B. Both (R) and (A) are true but reason is not correct explanation of assertion c. Assertion (A) is true but reason (R) is false D. Assertion (A) and reason (R) both are false E. Assertion (A) is false but reason (R) is true | 12 |

517 | A half cell reaction is one which: A. involves only half a mole of electrolyte B. goes only half way to completion C. takes place at one electrode D. consumes half a unit of electricity | 12 |

518 | (a) What do you understand by corrosion? (b) Write electro-chemical theory of corrosion (Rust). (c) Write prevention (two) of corrosion. | 12 |

519 | Q. 66 Consider the figure and answer the following questions. Salt bridge Zinc plate & Zn² (aq) Copper plate & Cu²+ (aq) Cell A lectrode (A) Electrode Electrolytic cell Cell B (i) Cell A has Ecell = 2V and Cell ‘B’ has E cell = 1.1V which of the two cells A’ or ‘B’ will act as an electrolytic cell. Which electrode reactions will occur in this cell? (ii) If cell A has E cell = 0.5V and cell ‘B’ has E cell = 1.1V then what will be the reactions at anode and cathode? Thinking Process This problem includes concept of electrochemical cell, electrolytic cell and charge on electrode. To solve this problem identify the charge on each electrode first | 12 |

520 | The potential across the metal and the aqueous solution of its ions of unit activity at ( 298 mathrm{K} ) is known as: A . electrode potential B. standard electrode potential c. formal electrode potential D. oxidation potential | 12 |

521 | Iron is not protected from rusting by: A. galvanization B. electroplating with ( N i ) or ( C r ) C. heating the iron to redness in steam D. treating it with ( H_{3} P O_{4} ) | 12 |

522 | The specific conductance of a ( 0.1 mathrm{N} mathrm{KC} ) solution is 0.012 ohm ( ^{-1} c m^{-1} ). The resistance of the cell containing the same solution is 55 ohms. Then the cell constant is : ( begin{array}{lll}text { A } cdot 0.918 & c m^{-1}end{array} ) B. ( 0.66 mathrm{cm}^{-1} ) ( begin{array}{lll}text { C } cdot & 1.142 & c m^{-1}end{array} ) D. 1.12 cm ( ^{-1} ) | 12 |

523 | The reduction potential of hydrogen half-cell will be negative if: ( mathbf{A} cdot mathrm{p}left(mathrm{H}_{2}right)=1 ) atom and ( left[mathrm{H}^{+}right]=2.0 mathrm{M} ) ( mathbf{B} cdot mathbf{p}left(mathbf{H}_{2}right)=1 ) atm and ( left[mathrm{H}^{+}right]=1.0 mathrm{M} ) ( mathbf{C} cdot mathrm{p}left(mathrm{H}_{2}right)=2 mathrm{atm} ) and ( left[mathrm{H}^{+}right]=1.0 mathrm{M} ) ( mathbf{D} cdot mathrm{p}left(mathrm{H}_{2}right)=2 mathrm{atm} ) and ( left[mathrm{H}^{+}right]=2.0 mathrm{M} ) | 12 |

524 | Typical battery used is the mercury cell, which is used in? A . Electric watches B. Television sets c. Radio transistors D. Electric torches | 12 |

525 | Cell constant of a conductivity cell is: A. specific conductance / resistance B. specific conductance ( times frac{1000}{text { Normality }} ) c. specific conductance / conductance D. conductance / specific conductance | 12 |

526 | 0.58 Assertion (A) Conductivity of all electrolytes decreases on dilution. Reason (R) On dilution number of ions per unit volume decreases. | 12 |

527 | toppr ( = ) Q Type your question ( A ) B. ( c ) ( D ) | 12 |

528 | Assertion Molar conductivity increases with decrease in concentration. Reason Conductivity always decreases with decrease in concentration. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

529 | Molar conductivity ( left(lambda_{M}right) ) and equivalent conductivity ( left(lambda_{e q}right) ) for an electrolyte ( A_{x} B_{y} ) at any dilution are related as: A ( . lambda_{M}=lambda_{e q} . times(x+y) ) B . ( lambda_{M}=lambda_{e q} ). ( times x times y ) c. ( lambda_{M}=frac{lambda_{e q}}{x+y} ) D. ( lambda_{M}=frac{lambda_{e q}}{x times y} ) | 12 |

530 | The ( E_{M^{3+} / M^{2+}}^{0} ) values of ( mathrm{Cr}, mathrm{Mn}, mathrm{Fe} ) and Co are ( -mathbf{0 . 4 1},+mathbf{1 . 5 7},+mathbf{0 . 7 7} ) and ( +1.97 mathrm{V} ) respectively. For which one of these metals the change in oxidation state from +2 to +3 is easiest? A ( . C r ) в. ( M n ) c. ( F e ) D. ( C o ) | 12 |

531 | What will be the volume of ( O_{2} ) at N.T.P liberated by 5 A current flowing for 193 s through acidulated water? ( mathbf{A} cdot 56 mathrm{m} ) B. ( 112 mathrm{ml} ) c. ( 158 mathrm{ml} ) D. 965 ml | 12 |

532 | During the working of the cell: ( boldsymbol{P b}- ) ( boldsymbol{H} boldsymbol{g}(mathbf{1} . boldsymbol{0} boldsymbol{M})left|boldsymbol{P} boldsymbol{b}^{2+}(boldsymbol{a} boldsymbol{q})(boldsymbol{1} boldsymbol{M})right| boldsymbol{P} boldsymbol{b}^{2+}(boldsymbol{a} boldsymbol{q})(mathbf{1} ) ( boldsymbol{H} boldsymbol{g}(mathbf{0 . 5} boldsymbol{M}) ) This question has multiple correct options ( mathbf{A} cdotleft[P b^{2+}right] ) in right half cell decreases B ( cdotleft[P b^{2+}right] ) in left half cell decreases c. ( left[P b^{2+}right] ) does not change in either of the half cells D. molarity of lead amalgam in right half cell increases while that of left half cell decreases | 12 |

533 | The standard reduction potential of metals ( X, Y ) and ( Z ) are ( -0.403 vee, 0.337 V ) and ( 0.79 mathrm{V} ) respectively. Which of the following reaction is not possible? A ( cdot X+H_{2} S O_{4} rightarrow X S O_{4}+H_{2} ) в. ( 2 Z+2 H N O_{3} rightarrow 2 Z N O_{3}+H_{2} ) c. ( Y+Z_{S} O_{4} rightarrow Y S O_{4}+2 Z ) D. ( X+2 Z N O_{3} rightarrow Xleft(N O_{3}right)_{2}+2 Z ) | 12 |

534 | How many faradays are required to reduce one mole of ( M n O_{4}^{ominus} ) to ( M n^{2+} ? ) ( mathbf{A} cdot mathbf{1} ) B. 2 ( c .3 ) D. | 12 |

535 | Among the four successive members of the first series of the transition metals listed below in the options, which one has a positive standard potential ( left(boldsymbol{E}_{M^{2+} / M}^{0}right) ) value? A. ( N i(Z=28) ) в. ( C u(Z=29) ) c. ( F e(Z=26) ) D. ( operatorname{Co}(Z=27) ) | 12 |

536 | What is the value of ( Delta S^{ominus} ) for the fuel cell at ( 25^{circ} C ) ? В. ( -160 J K^{-1} ) c. ( 160 J K^{-1} ) D. ( 1600 J K^{-1} ) | 12 |

537 | The molar conductivities of ( wedge_{N a O A c}^{circ} ) and ( wedge_{H C l}^{circ} ) at infinite dilution in water at ( 25^{circ} mathrm{C} ) are 91 and ( 426.2 S mathrm{cm}^{2} mathrm{mol}^{-1} ) respectively. To calculate, ( wedge_{H O A c}^{circ}, ) the additional value required is ( mathbf{A} cdot wedge_{H_{2} O}^{circ} ) в. ( wedge_{K C l}^{circ} ) c. ( wedge_{N a O H}^{circ} ) ( mathbf{D} cdot wedge_{N a C l}^{circ} ) | 12 |

538 | Which of the following is always true regarding the spontaneity of reaction occuring in a galvanic cell? A ( cdot E^{0}_{c e l l}>0, Delta G^{0}K_{c} ) B . ( E^{0}_{c e l l}>0, Delta G^{0}<0 ) and ( Q0, Delta G^{0}>0 ) and ( Q>K_{c} ) D . ( E^{0}_{c e l l}>0, Delta G^{0}>0 ) and ( Q<K_{c} ) | 12 |

539 | Metals react differently with water. The more vigorous is the reaction, the more is the bubble formation. The following diagram illustrates the reaction of sodium, magnesium and copper with water. What can be concluded from this diagram? A. Magnesium reacts more vigorously with water than sodium and copper B. Sodium reacts more vigorously with water than magnesium and copper. c. Sodium reacts more vigorously than copper but less vigorously than magnesium. D. copper reacts more vigorously with water than sodium and magnesium. | 12 |

540 | In a galvanic cell electrical energy is generated at the expense of chemical energy. If true enter 1 , else enter 0 | 12 |

541 | To liberate ( 5.4 mathrm{g} ) of silver (atomic mass 108 amu) from an aqueous solution of sliver nitrate, it is required to pass: A. 965C of electricity B. 4825C of electricity c. ( 9650 mathrm{c} ) of electricity D. ( 48250 mathrm{c} ) of electricity | 12 |

542 | An oxide of iron from the following is: A. mud B. dust c. rust D. none of these | 12 |

543 | ( Z n(s) / Z n^{2+}(a q) | C u^{2+}(a q) / C u(s) ) ( boldsymbol{E}^{0} z n^{2+} / Z n=-0.76 mathrm{V} ) ( boldsymbol{E}^{0}_{C u^{2+} / C u}=+0.34 mathrm{V} ) Calculate ( boldsymbol{E}_{c e l l}^{0} ) and equilibrium constant ( boldsymbol{K} ) | 12 |

544 | The molar conductivity of a ( 0.5 m o l / d m^{3} ) solution of ( A g N O_{3} ) with electrolytic conductivity of ( 5.76 times ) ( 10^{-3} operatorname{Scm}^{-1} ) at ( 298 K ) is: A ( .2 .88 S mathrm{cm}^{2} / mathrm{mol} ) B . ( 11.52 mathrm{S} mathrm{cm}^{2} / mathrm{mol} ) c. ( 0.086 S mathrm{cm}^{2} / mathrm{mol} ) D. ( 28.8 S mathrm{cm}^{2} / mathrm{mol} ) | 12 |

545 | Two weak acid solutions ( H A_{1} ) and ( H A_{2} ) each with the same concentration and having pKa values 3 and 5 are placed in contact with hydrogen electrode ( (1 mathrm{atm} ) ( 25^{0} C ) ) and are interconnected through a salt bridge. Find emf of the cell. A ( .+0.059 mathrm{V} ) B. 0.059 c. ( 0.0295 mathrm{v} ) D. 0.118 V | 12 |

546 | Solution ( A, B ) and ( C ) of the same strong electrolyte offered resistances of ( 50 Omega, 100 Omega, ) and ( 150 Omega ) in a given conductivity cell. The resistance observed if they are mixed in a volume proportion which is reciprocal of their resistances and tested in the same conductivity cell would be: A . ( 67.3 Omega ) B. ( 81.8 Omega ) c. ( 100 Omega ) D. ( 300 Omega ) | 12 |

547 | Question 4. Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10. (i) Since, pH is given, calculate Ht from the relation [H* ] = 1×107 (ii) Then, calculate Et by using Nernst equation as EiH+ /V2H) IS taken as 0.00 V. | 12 |

548 | The highest electrical conductivity of the following aqueous solutions is of A. ( 0.1 M ) acetic acid B. ( 0.1 M ) chloroacetic acid c. ( 0.1 M ) fluoroacetic acid D. ( 0.1 M ) difluoroacetic acid | 12 |

549 | Find the equilibrium constant for the reaction, ( boldsymbol{F e}^{2+}+boldsymbol{C e}^{4+} rightleftharpoons boldsymbol{F e}^{3+}+boldsymbol{C e}^{3+} ) ( left[text { Given: } boldsymbol{E}_{C e^{4+} / C e^{3+}}^{o}=right. ) ( left.mathbf{1} . mathbf{4 4} boldsymbol{V} ; boldsymbol{E}_{boldsymbol{F e}^{3+} / mathbf{F e}^{mathbf{2 +}}}^{boldsymbol{o}}=mathbf{0 . 6 8} boldsymbol{V}right] ) A . ( 7.6 times 10^{12} ) B . ( 5.4 times 10^{12} ) c. ( 3.3 times 10^{12} ) D. None of the above | 12 |

550 | Determine the standard reduction potential for the half reaction: ( boldsymbol{C l}_{2}+boldsymbol{2} boldsymbol{e}^{-} longrightarrow boldsymbol{2} boldsymbol{C l}^{-} ) Given: ( boldsymbol{P} boldsymbol{t}^{2}+boldsymbol{2} boldsymbol{C l} longrightarrow boldsymbol{P} boldsymbol{t}+ ) ( boldsymbol{C l}_{2}, boldsymbol{E}_{c e l l}^{0}=-mathbf{0 . 1 5} boldsymbol{V} ) ( boldsymbol{P t}^{2}+boldsymbol{2} boldsymbol{e}^{-} longrightarrow boldsymbol{P t}, boldsymbol{E}^{0}=mathbf{1 . 2 0} boldsymbol{V} ) | 12 |

551 | The standard electrode potentials ( left(boldsymbol{E}_{boldsymbol{M}^{+} / M}^{o}right) ) of four metals ( mathbf{A}, mathbf{B}, mathbf{C} ) and ( mathbf{D} ) are ( -1.2 vee, 0.6 vee, 0.85 mathrm{V} ) and ( -0.76 mathrm{V} ) respectively. The increasing sequence of deposition of metals on applying potential is : ( A cdot A, C, B, D ) B. B, D, C, A c. ( c, B, D, A ) D. D, A, B, C | 12 |

552 | A solution of metal salt was electrolyzed with a current of 0.1 A for 160 minutes. Ni deposited at cathode was found 0.2950 g. What is the charge on metal ion? (Atomic mass of metal is 58.71 ) | 12 |

553 | Assertion The electrical resistance of any object decreases with increase in its length. Reason Electrical resistance of any object increases with increase in its area of cross-section. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

554 | Question 3. Consult the table on standard electrode potentials and suggest three substances that can oxidise ferrous ions under suitable condition. | 12 |

555 | At ( 298 K, ) given that: [ begin{array}{c} boldsymbol{C u}(boldsymbol{s})left|boldsymbol{C} boldsymbol{u}^{2+}(mathbf{1} . boldsymbol{0} boldsymbol{M}) | boldsymbol{A} boldsymbol{g}^{+}(mathbf{1} . boldsymbol{0} boldsymbol{M})right| boldsymbol{A} boldsymbol{g}(boldsymbol{s}) \ boldsymbol{E}_{c e l l}^{o}=mathbf{0 . 4 6} boldsymbol{V} \ boldsymbol{Z} boldsymbol{n}(boldsymbol{s})left|boldsymbol{Z} boldsymbol{n}^{2+}(mathbf{1} cdot mathbf{0} boldsymbol{M}) | boldsymbol{C} boldsymbol{u}^{2+}(mathbf{1} . boldsymbol{0} boldsymbol{M})right| boldsymbol{C} boldsymbol{u} \ boldsymbol{E}_{text {cell }}^{o}=mathbf{1 . 1 0} boldsymbol{V} end{array} ] Then, the ( E_{text {cell}} ) for the following reaction at ( 298 K ) will be: [ boldsymbol{Z} boldsymbol{n}(boldsymbol{s})left|boldsymbol{Z} boldsymbol{n}^{2+}(boldsymbol{0} cdot boldsymbol{1} boldsymbol{M}) | boldsymbol{A} boldsymbol{g}^{+}(mathbf{1} cdot boldsymbol{0} boldsymbol{M})right| boldsymbol{A} boldsymbol{g}(s ] A . ( 1.56 V ) в. ( 1.53 V ) ( mathbf{c} .2 .53 V ) D. cannot be calculated due to insufficient data | 12 |

556 | ( C H_{3} C O O H ) is titrated with NaOH solution. Which of the following statement is true? A. conductance increases upto equivalence point, after which it decreases. B. Conductance decreases upto equivalence point, after which it increases. c. conductance first increases (but not rapidly) upto equivalence point and then increases rapidly after equivalence point. D. none | 12 |

557 | Na is used in reduction of ( Z n ) salt because: A ( cdot E Z n(o x i)>E N a(o x i) ) B . ( E Z n(r e d)<E N a(r e d) ) C. ( E Z n(o x i)<E N a(o x i) ) D. Both (A) and (B) | 12 |

558 | Resistance and conductivity of a cell containing ( 0.001 mathrm{M} ) KCl solution at 298 ( mathrm{K} ) are ( 1500 Omega ) and ( 1.46 times 10^{-4} mathrm{S.cm}^{-1} ) respectively. What is the cell constant? ( mathbf{A} cdot 0.219 mathrm{cm}^{-1} ) B. ( 0.319 mathrm{cm}^{-1} ) c. ( 0.419 c m^{-1} ) D. None of these | 12 |

559 | • 2 Electrode potential for Mg electrode varies according to the equation Ema 2+ Mg = 5Mg 2+/Mg 0.059 log 1. The graph of EMg2+ /Mg 2 9[Mg2+] vs log [Mg2+ ] is Emg2*/Mg EMg? Mg EMg2+/Mg EMq2*/Mg log[Mg2+1 log[Mg2+) → log[Mg2+1 log[Mg2+1 Thinking Process This problem includes concept of Nernst equation and its transformation to equation of straight line | 12 |

560 | Which of the following statement is correct? A. Cathode is negative terminal both in galvanic and electrolytic cells B. Anode is positive terminal both in galvaniv and electrolytic cells C. Cathode is negative terminal in an electrolytic cell whereas anode is negative terminal in a galvanic cell D. Anode is negative terminal in an electrolytic cell whereas cathode is positive terminal in galvanic cell | 12 |

561 | What are ‘fuel cells’? Write cathode and anode reaction in a fuel cell. | 12 |

562 | Any article of iron if left in open for some time, acquires a film of brownish substance (rust) having chemical formula: ( mathbf{A} cdot F e_{3} O_{4} ) в. ( F e_{2} O_{3} ) c. Feo D. ( operatorname{Fe}(O H)_{2} ) | 12 |

563 | The following two redox reactions are given: ¡) ( M n O_{4}^{-}+8 H^{+}+5 e^{-} rightarrow M n^{2+}+ ) ( mathbf{4} boldsymbol{H}_{2} boldsymbol{O} ; boldsymbol{E}^{boldsymbol{o}}=boldsymbol{X}_{mathbf{1}} boldsymbol{V} ) ii) ( boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2}+boldsymbol{4} boldsymbol{H}^{+}+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{M} boldsymbol{n}^{2+}+ ) ( mathbf{2} boldsymbol{H}_{2} boldsymbol{O} ; boldsymbol{E}^{o}=boldsymbol{X}_{2} boldsymbol{V} ) Find ( E^{o} ) for the following reaction. ( M n O_{4}^{-}+4 H^{+}+3 e^{-} rightarrow M n O_{2}+ ) ( 2 H_{2} O ) A. ( X_{2}-X_{1} ) В. ( X_{1}-X_{2} ) c. ( frac{5 X_{1}-2 X_{2}}{3} ) D. ( frac{2 X_{1}-5 X_{2}}{3} ) | 12 |

564 | For the reaction ( boldsymbol{A}+mathbf{2} boldsymbol{B}^{+} rightleftharpoons boldsymbol{A}^{2+}+ ) ( 2 B ; K_{c} ) has been found to be ( 10^{12} ). The ( boldsymbol{E}_{c e l l}^{o} ) is: A . 0.354 в. 0.708 c. ( 0.0098 mathrm{v} ) D. 1.36 ( v ) | 12 |

565 | The quantity of electricity required to reduce 12.3 g of nitro benzene to aniline assuming 50% current efficiency is: ( A cdot 115800 C ) B. 57900 C c. 231600 ( c ) D. 28950 C | 12 |

566 | During electrolysis of ( 1 mathrm{L}, 1 mathrm{M} ) AgNO ( _{3} ) using silver electrodes, 9.65 A current is used for one hour. Assuming the volume to remain unchanged, the molarity of ( A g N O_{3} ) at the end of the electrolytic process is : A. 1 м B. 0.36 м c. 0.64 М D. None of these | 12 |

567 | Aluminium oxide may be electrolysed at ( 1000^{circ} mathrm{C} ) to furnish aluminium metal. The cathode reaction is ( A l^{3+}+3 e^{-} rightarrow ) Al. To prepare ( 5.12 mathrm{kg} ) of aluminium metal by this method would require: A ( cdot 5.49 times 10^{1} C ) of electricity B . ( 5.49 times 10^{4} C ) of electricity c. ( 1.83 times 10^{7} C ) of electricity D. ( 5.49 times 10^{7} C ) of electricity | 12 |

568 | Which of the following statement is correct? ( mathbf{A} cdot E_{text {cell}} ) and ( triangle_{r} G ) of cell reaction both are extensive properties B. ( E_{text {cell}} ) and ( triangle_{r} G ) of cell reaction both are intensive properties C. ( E_{text {cell}} ) in the intensive property while ( triangle_{r} G ) of cell reaction is an extensive property. D. ( E_{text {cell}} ) in the intensive property while ( triangle_{r} G ) of cell reaction is an intensive property. | 12 |

569 | Which of the following represents increasing order of ionic conductance? ( mathbf{A} cdot F^{-}<C l^{-}<B r<I^{-} ) B ( cdot I^{-}<B r^{-}<F^{-}<C l^{-} ) ( mathbf{c} cdot F^{-}<C l^{-}<I^{-}<B r^{-} ) D ( cdot F^{-}<I^{-}<C l^{-}<B r^{-} ) | 12 |

570 | An examples of a simple fuel cell is: A. lead storage battery в. ( H_{2}-O_{2} ) cell c. daniell cell D. lechlanche cell | 12 |

571 | To carry out the so-called electrolysis of water, sulphuric acid is added to water. How does the addition of sulphuric acid produce a conducting solution? | 12 |

572 | ( H C l ) can be used to remove rust from iron. A. True B. False | 12 |

573 | The STP volume of oxygen liberated by 2 ampere of current when passed through acidulated water for 3 minutes and 13 seconds, is: A . 120 ( c c ) B. 22.4 cc c. ( 11.2 mathrm{c} ) D. 44.8 сс | 12 |

574 | ( ln H_{2}-O_{2} ) fuel cell, the reaction occurring at cathode is : ( mathbf{A} cdot 2 H_{2(g)}+O_{2(g)} rightarrow 2 H_{2} O_{(l)} ) B. ( O_{2(g)}+2 H_{2} O_{(l)}+4 e^{-} longrightarrow 4 O H_{(a q)}^{-} ) ( ^{mathrm{c}} cdot H^{+}+e^{-} rightarrow frac{1}{2}^{H}_{2} ) ( mathbf{D} cdot H_{(a q)}^{+}+O H_{(a q)}^{-} longrightarrow H_{2} O_{(l)} ) | 12 |

575 | Assertion Galvanic cell convert chemical energy into electrical energy. Reason Redox reactions are those in which oxidation takes place at anode and reduction at cathode. A. If both Assertion and Reason are correct and Reason is the correct explanation of assertion B. If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion C. If Assertion is correct but Reason is incorrect D. If Assertion is incorrect but Reason is correct | 12 |

576 | At ( 298 K, ) the equilibrium constant for the reaction ( Z n^{2+}+4 N H_{3} rightleftharpoonsleft[Z nleft(N H_{3}right)_{4}right]^{2} ) is ( 10^{circ} ) If ( boldsymbol{E}_{left[Z nleft(N H_{3}right)^{4}right]^{2} /left[Z n, 4 N H_{3}right]}=-1.03 V ) then the value of ( E_{Z n / Z n^{2+}}^{o} ) will be: A. ( -0.7654 V ) в. ( -1.1 V ) c. ( +1.1 V ) D. none of these | 12 |

577 | The ionic conductances of ( A l^{3+} ) and ( boldsymbol{S} boldsymbol{O}_{3}^{2-} ) ions at infinite dilution are ( boldsymbol{x} ) and ( y ) oh ( m^{-1} c m^{2} m o l^{-1} ) respectively. If Kohlrausch’s law is valid, then molar conductance of aluminium sulphate at infinite dilution will be A ( .3 x+2 y ) в. ( 3 y+2 x ) ( c cdot 2 x+2 y ) D. ( 3 x+3 y ) | 12 |

578 | If a monovalent metal ion carries ( 1.6 times ) ( 10^{-19} ) coulomb of electricity, what is the amount of electricity carried by one gram molecular mass of the metal ions? ( mathbf{A} cdot 9.6336 times 10^{4} )coulomb B. ( 10.6336 times 10^{4} ) coulomb c. ( 95.336 times 10^{4} ) coulomb D. ( 96.336 times 10^{4} ) coulomb | 12 |

579 | For a cell reaction involving two electron changes, ( boldsymbol{E}_{c e l l}^{0}=mathbf{0 . 3} boldsymbol{V} ) at ( mathbf{2 5}^{circ} boldsymbol{C} ). The equilibrium constant of the reaction is: ( mathbf{A} cdot 10^{-10} ) В. ( 3 times 10^{-2} ) c. 10 D. ( 10^{10} ) | 12 |

580 | The main factors which affect corrosion are : A. Position of metal in electrochemical series B. Presence of ( C O_{2} ) in water c. Presence of impurities coating D. All are correct | 12 |

581 | Write the complete chemical reaction of rusting of iron. | 12 |

582 | What is a secondary cell? | 12 |

583 | The cathode in the central compartment of Castner Kellner cell used for the manufacture of ( N a O H ) is: A. Iron B. Carbon C. Mercury D. Steel | 12 |

584 | Standard free energies of formation(in ( k J / m o l ) ) at ( 298 mathrm{K} ) are -237.2,-394.4 and -8.2 for ( H_{2} O(I), C O_{2}(g) ) and pentane(g) respectively. The value of ( E_{c e l l}^{o} ) for the pentane-oxygen fuel cell is: A . ( 1.968 mathrm{v} ) в. 2.0968 V c. ( 1.0968 mathrm{v} ) D. ( 0.0968 mathrm{V} ) | 12 |

585 | Write the cell reaction and calculate ( boldsymbol{E}^{o} ) cell of the following electrochemical cell: ( boldsymbol{A} boldsymbol{l}left|boldsymbol{A} boldsymbol{l}^{3+} | boldsymbol{Z} boldsymbol{n}^{2+}right| boldsymbol{Z} boldsymbol{n} ) ( (boldsymbol{s})(boldsymbol{a q} cdot) ) [ begin{array}{c} (mathbf{1} boldsymbol{M})(mathbf{1} boldsymbol{M}) \ boldsymbol{E}_{boldsymbol{A} l}^{o}=-mathbf{1 . 6 6 V} \ boldsymbol{E}_{Z n}^{o}=-mathbf{0 . 7 6 V} end{array} ] | 12 |

586 | Identify the electrolyte which deposits maximum amount of cathodic product for the passage of 1 faraday of electricity. A. ( F e C l_{2} ) B. FeBr ( _{3} ) c. ( A g N O_{3} ) D. ( C u S O_{4} ) | 12 |

587 | The standard reduction potential of ( boldsymbol{C u}^{2+} / boldsymbol{C u} ) couple is ( mathbf{0 . 3 4} mathrm{V} ) at ( mathbf{2 5}^{mathbf{0}} mathrm{C} ) Calculate the reduction potential at ( boldsymbol{p} boldsymbol{H}=mathbf{1 4} ) for this couple. ( operatorname{Given} boldsymbol{K}_{s p} ) of ( boldsymbol{C u}(boldsymbol{O H})_{2}=mathbf{1 . 0} times mathbf{1 0}^{-mathbf{1 8}} mathbf{)} ) | 12 |

588 | Assertion faraday is the charge that liberates 1 eq. of metal at cathode. Reason Passsage of 1 faraday charge through aq. ( mathrm{MgCl}_{2} ) liberates 12 g Mg at cathode. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

589 | What is anodising? Give its applications. | 12 |

590 | A button cell used in watches functions as following: ( boldsymbol{Z n}(s)+boldsymbol{A g}_{2} boldsymbol{O}(s)+boldsymbol{H}_{2} boldsymbol{O}(l) rightleftharpoons ) ( 2 A g(s)+Z n^{2+}(a q)+2 O H^{-}(a q) ) f half cell potentials are: ( Z n^{2+}(a q)+ ) ( 2 e rightarrow Z n(s) ; E^{0}=-0.76 V ) ( A g_{2} O(s)+H_{2} O(l) 2 e rightarrow 2 A g(s)+ ) ( mathbf{2} boldsymbol{O} boldsymbol{H}^{-}(boldsymbol{a} boldsymbol{q}), boldsymbol{E}^{0}=mathbf{0} . boldsymbol{3} mathbf{4} boldsymbol{V} ) The cell potential will be: A . ( 1.10 V ) B. ( 0.42 V ) c. ( 0.84 V ) D. ( 1.34 V ) | 12 |

591 | Write the equations for the reactions taking place at anode and cathode in lead storage cell. | 12 |

592 | How many electrons flow through a metallic wire if a current of ( 0.5 A ) is passed for 2 hours? (Given : ( 1 F= ) ( left.mathbf{9 6}, mathbf{5 0 0} boldsymbol{C} boldsymbol{m o l}^{-mathbf{1}}right) ) | 12 |

593 | Assertion Statement-I: If an aqueous solution of NaCl is electrolysed, the product obtained at the cathode is ( H_{2} ) gas and not Na. Reason Statement-II : Gases are liberated faster than the metals. A. Statement-l is true, Statement-II is true; Statement-II is correct explanation for Statement-I B. Statement-lis true, Statement-II is true; Statement-II is NOT a correct explanation for statement- c. Statement-I is true, Statement-II is false D. Statement-I is false, Statement-II is true | 12 |

594 | When the liquid between two ends allow electric current, then : A. bulb of tester glows B. only heating of the tester takes place c. bulb of the tester does notglow D. none of the above | 12 |

595 | Presence of ( mathrm{CO}_{2} ) in natural water facilitate rusting of iron. If true enter 1 , else enter 0 | 12 |

596 | A reversible galvanic cell is connected to an external battery. If the EMF of the battery is less than the EMF of the galvanic cell, then the current: A. will not pass through the circuit B. will flow from the battery to the galvanic cell c. will flow from the galvanic cell to the battery D. can flow in any direction | 12 |

597 | Question 12. How much charge is required for the following reductions: (i) 1 mole of A13+ to AIP (ii) 1 mole of Cu4+ to Cup (iii) 1 mole of MnO4 to Mn2+? Write electrode reaction (balanced), to find the number of electron taking part in the reaction and then calculate Q by using, Q = n <96500 C. | 12 |

598 | When one faraday of electric current is passed, the mass deposited is equal to: A. one gram equivalent B. one gram mole c. electrochemical equivalent D. half gram equivalent | 12 |

599 | Which among the following equations represents the reduction reaction taking place in lead accumulator at positive electrode, while it is being used as a source of electrical energy? ( mathbf{A} cdot P b rightarrow P b^{2} ) B. ( P b^{4+} rightarrow P b ) ( mathbf{c} cdot P b^{2+} rightarrow P b ) D. ( P b^{4+} rightarrow P b^{2} ) | 12 |

600 | For ( boldsymbol{Z} boldsymbol{n}^{2+} / boldsymbol{Z} boldsymbol{n}, boldsymbol{E}^{boldsymbol{o}}= ) ( -0.76 V, ) for ( A g^{+} / A g, E^{o}=0.799 V ) The correct statement is : A. the reaction ( Z n ) getting reduced ( A g ) getting oxidized is spontaneous B. ( Z n ) undergoes reduction and ( A g ) is oxidized C. ( Z n ) undergoes oxidation and ( A g^{+} ) gets reduced D. no suitable answer | 12 |

601 | Does pure water conduct electricity? A. Yes B. No c. Sometimes D. None of above | 12 |

602 | LED stands for: A. light emitting diode B. loose emitting diode C . light emission device D. light emitting device | 12 |

603 | Which of the following reactions is correct for a given electrochemical cell ( operatorname{at} 25^{circ} C ? ) ( boldsymbol{P t}left|boldsymbol{B r}_{2}(boldsymbol{g})right| boldsymbol{B r}^{-}(boldsymbol{a q}) | boldsymbol{C l}^{-}(boldsymbol{a q}) mid boldsymbol{C l}_{2}(boldsymbol{g}) ) A ( cdot 2 B r^{-}(a q)+C l_{2}(g) rightarrow 2 C l^{-}(a q)+B r_{2}(g) ) B . ( B r_{2}(g)+2 C l^{-}(a q) rightarrow 2 B r^{-}(a q)+C l_{2}(g) ) C. ( B r_{2}(g)+C l_{2}(g) rightarrow 2 B r^{-}(a q)+2 C l^{-}(a q) ) D ( cdot 2 B r^{-}(a q)+2 C l^{-}(a q) rightarrow B r_{2}(g)+C l_{2}(g) ) | 12 |

604 | Question 2. Can Ecell or A,G°for cell reaction ever be equal to zero? | 12 |

605 | Which of the following is disposable battery? A. Lead acid battery B. Mercury cell c. ( N i-C d ) battery D. None of these | 12 |

606 | I. Conductance of electrolyte solution increases with temperature. II. Resistivity is reciprocal of molar conductivity of electrolyte. III. Cell constant has unit ( c m^{-1} ) Which of the above statements are correct? A. All the statements are correct B. II and III are correct c. I and III are correct D. Only II is correct | 12 |

607 | A current of ( 19.3 mathrm{mA} ) is passed for 9375 seconds through ( 500 mathrm{ml} ) of ( 2 mathrm{mM} ) ( Z n S O_{4} ) solution. If the final molarity of ( Z n^{2+} ) is ( 0.5 mathrm{mM} ), then the current efficiency of the source is (assume volume remains constant during this process): A . 80% B. 75% c. 72% D. 65% | 12 |

608 | A battery of e.m.f. E and internal resistance ( r ) is connected to an external resistance ( R ) the condition for maximum power transfer is A. $$ldisplaystyler в. ( r>R ) c. ( r=1 / R ) ( mathbf{D} cdot r=R ) | 12 |

609 | Electrolyte ( quad K C l quad K N O_{3} ) ( boldsymbol{H} C l ) [ begin{array}{ll} Lambda_{left(S c m^{2}right.}^{Lambda infty}_{left.m o l^{-1}right)}^{infty} & 149.9 end{array} ] ( 426 . ) Calculate ( Lambda^{infty}_{H O A c} ) using appropriate molar conductances of the electrolytes listed above at infinite dilution in ( boldsymbol{H}_{2} boldsymbol{O} ) ( operatorname{at} 25^{circ} C ) ( mathbf{A} cdot 517.2 ) B. 552.7 c. 390.7 D. 217.5 | 12 |

610 | During charging of lead accumulator? A. concentration of ( H_{2} S O_{4} ) decreases B. specific gravity of ( H_{2} S O_{4} ) increases ( mathrm{C} cdot P b mathrm{O}_{2} ) dissolves in electrolyte D. lead is deposited at positive terminal | 12 |

611 | In the electrochemical cell ( H_{2}(g), 1 a t mleft|H^{+}(1 M)right|left|C u^{2+}(1 M)right| C u(s) ) which one of the following is the correct value of reduction potential? A . ( 1.10 mathrm{V} ) B. 0.110 c. ( 1.50 mathrm{v} ) D. 0.220 | 12 |

612 | The conductivity of 0.001028 mol ( L^{-1} ) acetic acid is ( 4.95 times 10^{-5} mathrm{Scm}^{-1} ) Calculate its dissociation constant if ( boldsymbol{Lambda}_{mathbf{m}}^{mathbf{o}} ) for ( mathbf{3} mathbf{9 0 . 5} mathbf{S} mathbf{c m}^{2} mathbf{m o l}^{-mathbf{1}} ) | 12 |

613 | Solutions which are decomposed due to the current passed through them are called | 12 |

614 | Define corrosion. What is meant by rust? Write the chemical formula of rust. | 12 |

615 | The equivalent conductance at infinite dilution of ( B a C l_{2}, H_{2} S O_{4} ) and ( H C l ) aqueous solutions are ( x_{1}, x_{2} ) and ( x_{3} ) respectively. The equivalent conductance of ( B a S O_{4} ) solution is: A. ( x_{1}+x_{2}-x_{3} ) В. ( x_{1}-x_{2}-x_{3} ) c. ( x_{1}+x_{2}-2 x_{3} ) D. ( x_{1}-2 x_{2}-x_{3} ) | 12 |

616 | Which one is correct about a hypothetical electrochemical cell shown below? ( underset{A}{Theta}left|boldsymbol{A}^{+}(boldsymbol{X} boldsymbol{M}) | boldsymbol{B}^{+}(boldsymbol{Y} boldsymbol{M})right| underset{boldsymbol{B}}{oplus} boldsymbol{E}_{c e l l}= ) ( +0.20 V ) A. The cell reaction cannot be predicted B . ( A+B^{+} rightarrow A^{+}+B ) ( mathbf{c} cdot A^{+}+B rightarrow A+B^{+} ) D. ( A^{+}+e rightarrow A ; B^{+}+e rightarrow B ) | 12 |

617 | The emf of the cell involving the following reaction, ( 2 A g^{+}+H_{2} longrightarrow ) ( 2 A g+2 H^{+} ) is 0.80 volt. The standard oxidation potential of silver electrode is: B. ( 0.50 mathrm{v} ) c. ( -0.30 v ) D. ( 0.40 mathrm{v} ) | 12 |

618 | ( boldsymbol{E}_{c e l l}^{o}=boldsymbol{E}_{O boldsymbol{P}}^{o}+boldsymbol{E}_{R P}^{o} ) if two electrodes are connected. If true enter 1 , else enter 0 . | 12 |

619 | The specific conductivity of a saturated solution of silver chloride is ( 2.30 times ) ( 10^{-6} ) mho ( c m^{-1} ) at ( 25^{circ} C . ) Calculate the solubility of silver chloride at ( 25^{circ} mathrm{C} ) if ( lambda_{A g^{+}}=61.9 m h o c m^{2} m o l^{-1} ) and ( boldsymbol{lambda}_{C l^{-}}=mathbf{7 6 . 3} boldsymbol{m h o c m}^{2} boldsymbol{m o l}^{-1} ) | 12 |

620 | Which of the following represents the oxidation half-reaction for the unbalanced redox equation? ( boldsymbol{C u}+boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} rightarrow boldsymbol{C u}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}+boldsymbol{N} boldsymbol{O}_{2} ) A ( cdot C u^{2+}+2 e^{-} rightarrow C u ) в. ( C u rightarrow C u^{2+}+2 e^{-} ) c. ( N O_{3}^{-} rightarrow N O_{2}+1 e ) D. ( 2 H^{+}+N O_{2}^{-}+1 e^{-} rightarrow N O_{2}+H_{2} O ) | 12 |

621 | Calculate the mass and volume at NTP of hydrogen and chlorine that will be formed by passing 10,000 coulomb of charge through an aqueous solution of potassium chloride. The cell reaction is: ( 2 K C l+2 H O H rightarrow 2 K O H+C l_{2}+ ) ( boldsymbol{H}_{2} ) | 12 |

622 | Write the cell reaction and calculate the emf of the cell ( boldsymbol{P t}left|boldsymbol{H}_{2}(boldsymbol{g}, mathbf{1} boldsymbol{a} boldsymbol{t m})right| boldsymbol{H}^{+}(mathbf{0 . 5} boldsymbol{M}) | boldsymbol{K} boldsymbol{C l}(mathbf{1} boldsymbol{M}) ) ( operatorname{at} 25^{circ} C, E=0.28 V ) | 12 |

623 | ( boldsymbol{A} boldsymbol{g} mid boldsymbol{A} boldsymbol{g}^{oplus}(boldsymbol{1} boldsymbol{M})left|boldsymbol{A} boldsymbol{g}^{oplus}right| boldsymbol{A} boldsymbol{g} ) ( 0.5 F ) electricity in this LHS (anode) and 1 F of electricity in the RHS (cathode) is first passed making them independent electrolytic cells at ( 298 mathrm{K} ). EMF of the cell after electrolysis will be: A. increased B. remain same c. decreased D. None of these | 12 |

624 | 0.52 Match the items of Column I and Column II. Column Column II A. Lead storage battery 1. Maximum efficiency B. Mercury cell 2. Prevented by galvanisation C Fuel cell 3. Gives steady potential D. Rusting 4. Pb is anode, Pbo, is cathode | 12 |

625 | ( boldsymbol{N} boldsymbol{i}left|boldsymbol{N} boldsymbol{i}^{2+} | boldsymbol{C} boldsymbol{u}^{2+}right| boldsymbol{C} boldsymbol{u} ) The standard EMF of the above cell is ( 0.59 mathrm{V} . ) The standard electrode potential (reduction potential) of the copper electrode is 0.34 V. Calculate the standard electrode potential of nicke electrode. A . ( -0.5 V ) B. ( 0.25 V ) c. ( 0.93 V ) D. – ( 0.25 V ) | 12 |

626 | On passing 0.01 Faraday of elctricity through a solution of aluminum chloride, the weight of Aluminium metal (at.wt. ( =mathbf{2 7} ) ) deposited on cathode is: ( mathbf{A} cdot 0.9 g m ) В. ( 0.09 g m ) c. ( 2.7 g m ) D. ( 0.27 g m ) | 12 |

627 | Is the reaction, ( 2 A l+3 F e^{2+} rightleftharpoons ) ( 2 A l^{3+}+2 F e ) possible? A. No, because standard oxidation potential of ( A lF e ) c. cannot be predicted D. Yes, because aluminium is a strong oxidising agent | 12 |

628 | Electrochemical cells are also called: This question has multiple correct options A. electrolytic cells B. galvanic cells c. fuel cells D. voltaic cells | 12 |

629 | Which of the following shows maximum molar conductance? A ( cdotleft[operatorname{Co}left(N H_{3}right)_{6}right] C l_{3} ) В ( cdotleft[operatorname{Co}left(N H_{3}right)_{3} C l_{3}right] ) c. ( left[operatorname{Co}left(N H_{3}right)_{4} C l_{2}right] C l ) D ( cdotleft[operatorname{Co}left(N H_{3}right)_{5} C lright] C l_{2} ) | 12 |

630 | Calomel is: A ( . H g_{2} C l_{2} ) в. ( mathrm{HgCl}_{2} ) ( mathrm{c} . H g_{2} C l_{2}+H g ) D. ( H g+H g C l_{2} ) | 12 |

631 | What will be the molar conductivity of ( A l^{3+} ) ions at infinite dilution if molar conductivity of ( A l_{2}left(S O_{4}right)_{3} ) is ( 858 S c m^{2} ) ( m o l^{-1} ) and ionic conductance of ( S O_{4}^{2-} ) is 160 S ( c m^{2} ) mol ( ^{-1} ) at infinite dilution? A ( cdot 189 mathrm{S} mathrm{cm}^{2} mathrm{mol}^{-1} ) B. ( 698 mathrm{S} mathrm{cm}^{2} mathrm{mol}^{-1} ) c. ( 1018 mathrm{s} mathrm{cm}^{2} mathrm{mol}^{-1} ) D. ( 429 mathrm{S} mathrm{cm}^{2} mathrm{mol}^{-1} ) | 12 |

632 | Which of the following is/are correct about 1 mole electrons? This question has multiple correct options A . ( 6.023 times 10^{23} ) electrons В . ( 5.48 times 10^{-7} mathrm{kg} ) c. 96500 coulomb charge D. None of these | 12 |

633 | According to Kohlrausch law, the limiting value of molar conductivity of an electrolyte ( boldsymbol{A}_{2} boldsymbol{B} ) ( mathbf{A} cdot lambda_{A^{+}}+lambda_{B^{2}} ) в. ( frac{1}{2} lambda_{A+}+lambda_{B^{2}} ) c. ( _{2 lambda_{A^{+}}+frac{1}{2} lambda_{B^{2}}} ) D. ( 2 lambda_{A^{+}}+lambda_{B^{2}} ) | 12 |

634 | Electrolytic reduction of alumina to aluminium by Hall-Heroult process is carried out: A. in the presence of Nacı B. in the presence of fluoride c. in the presence of cryolite which forms a melt with lower melting temperature. D. in the presence of cryolite which forms a melt with higher melting temperature | 12 |

635 | Two platinum electrodes were immersed in a solution of ( C u S O_{4} ) and electric current was passed through the solution. After some time, it was found that colour of ( C u S O_{4} ) disappeared with evolution of gas at the electrode. The colorless solution contains: A. Platinum sulphate B. Copper hydroxide c. copper sulphate D. Sulphuric acid | 12 |

636 | Question 9. The resistance of a conductivity cell containing 0.001 M KCI solution at 298 K is 1500S2. What is the cell constant if conductivity of 0.001 M KCl solution at 298 K is 0.146 x 10-3 S cm-1. Cell constant = Conductivity < Resistance | 12 |

637 | Which of the following has the highest molar conductivity in solution? ( mathbf{A} cdotleft[P tleft(N H_{3}right)_{6}right] C l_{4} ) в. ( left[P tleft(N H_{3}right)_{5} C lright] C l_{3} ) ( mathbf{c} cdotleft[operatorname{Pt}left(N H_{3}right)_{4} C l_{2}right] C l_{2} ) D ( cdotleft[operatorname{Pt}left(N H_{3}right)_{3} C l_{3}right] C l ) | 12 |

638 | Whats the potential of the reaction below given the half-reaction potentials: ( 2 F e_{2}++C l_{2} rightarrow 2 F e^{3+}+2 C l^{-} ) ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{e}^{-} rightarrow boldsymbol{F} boldsymbol{e}^{2+} ; boldsymbol{E}=mathbf{0 . 7 7} boldsymbol{V} ) ( boldsymbol{C l}_{2}+mathbf{2} boldsymbol{e}^{-} rightarrow mathbf{2} boldsymbol{C l}^{-} ; boldsymbol{E}=mathbf{1 . 3 6} boldsymbol{V} ) A . ( 0.18 V ) B . ( 0.59 V ) c. ( 1.05 V ) D. ( 2.13 V ) E ( .2 .90 V ) | 12 |

639 | If a piece of iron gains ( 10 % ) of its weight due to partial rushing into ( F e_{2} O_{3} ) the percentage of total iron that has rusted is: A . 23 B. 13 c. 23.3 D. 90 | 12 |

640 | Number of coulombs required to deposit ( 90 g ) of ( A l ) when the electrode reaction ( A l^{3+}+3 e rightarrow A l ) is A ( cdot 9.65 times 10^{6} ) B. ( 8.685 times 10^{4} ) c. ( 9.65 times 10^{4} ) D. 6.955 | 12 |

641 | What is the amount of chlorine evolved when 2 ampere of current is passed for 30 minutes in an aqueous solution of NaCl? A ( .66 g ) в. ( 1.32 g ) ( mathrm{c} cdot 33 mathrm{g} ) D. ( 99 g ) | 12 |

642 | Units of the properties measured are given. Which of the properties has not been matched correctly? A. Molar conductance ( =mathrm{S} m^{2} m o l^{-1} ) B. Cell constant ( =m^{-1} ) C. Specific conductance ( =mathrm{S} m^{2} ) D. Equivalent conductance ( =operatorname{Sm}^{2}(g e q)^{-1} ) | 12 |

643 | Calculate the cell potential (in V) if ( triangle G=-96.5 k J / m o l ) and ( n=1 ) | 12 |

644 | Given below are the half-cell reactions: ( M n^{2+}+2 e^{-} rightarrow M n ; E^{0}=-1.18 V ) ( mathbf{2}left(boldsymbol{M} boldsymbol{n}^{3+}+boldsymbol{e}^{-} rightarrow boldsymbol{M} boldsymbol{n}^{2+}right) ; boldsymbol{E}^{0}= ) ( +1.51 V ) The ( boldsymbol{E}^{0} ) for ( boldsymbol{3} boldsymbol{M} boldsymbol{n}^{2+} rightarrow boldsymbol{M} boldsymbol{n}+boldsymbol{2} boldsymbol{M} boldsymbol{n}^{3+} ) will be: A. ( -0.33 V ); the reaction will not occur B. ( -0.33 V ; ) the reaction will occur c. ( -2.69 V ); the reaction will not occur D. ( -2.69 V ); the reaction will occur | 12 |

645 | Suppose the concentration of hydroxide ion in the cell is doubled, then the cell voltage will be: A. Reduced by half B. Increased by a factor of 2 c. Increased by a factor of 4 D. Unchanged | 12 |

646 | The EMF of the cell ( Z nleft|Z n^{2+}(0.01 M) | F e^{2+}(0.001 M)right| F e ) at ( 298 K ) is 0.2905 then the value of equilibrium constant for the cell reaction is : B. ( 10^{frac{1.33}{35}} ) ( mathbf{c} cdot 10 frac{0.25}{15} ) D. ( 10^{frac{0.32}{0.539}} ) | 12 |

647 | Which of the following reactions is used to make a fuel cell? ( mathbf{A} cdot 2 H_{2}(g)+O_{2}(g) rightarrow 2 H_{2} O(l) ) B. ( 2 F e(s)+O_{2}(g)+4 H^{+}(a q) rightarrow 2 F e^{2+}(a q)+2 H_{2} O(l) ) ( mathbf{c} cdot P b(s)+P b O_{2}(s)+2 H_{2} S O_{4}(a q) rightarrow 2 P b S O_{4}(s)+ ) ( H_{2} O(l) ) D. ( C d(s)+2 N i(O H)_{3}(s) rightarrow C d O(s)+2 N i(O H)_{2}+ ) ( 2 H_{2} O(l) ) | 12 |

648 | Cells are connected in series in order to: A. increase the voltage rating B. increase the electric current rating. c. increase the life of cells. D. none of above. | 12 |

649 | Which of the following statements is correct about ( lambda_{a}^{infty} ) or ( lambda_{c}^{infty} ) (i.e., ionic conductivities)? A. Increases with temperature due to increase in viscosity of medium. B. Increases with pressure due to decrease in viscosity of medium. c. Decreases with pressure due to increase in viscosity of medium. D. Decreases with pressure due to decrease in viscosity of medium | 12 |

650 | Select the correct statements about SHE: This question has multiple correct options ( mathbf{A} cdot ) The ( E_{O P}^{o} / R_{R P}^{o} ) for SHE has been arbitrarily assigned to be zero at all temperatures. B. SHE refers for ( P t, H_{2}(g) mid H^{+}(a q) ) C. SHE is very susceptible to electrode poisoning. D. SHE is very susceptible to dissolved oxygen, ( mathrm{H}_{2} mathrm{S} ) and all other reducing species. | 12 |

651 | The compounds which decompose on passage of an electric current through them are known as: A. electrolytes B. non-electrolytes c. electrolytically compounds D. non-electrolytically compounds | 12 |

652 | Zinc is used to protect iron from corrosion because: ( mathbf{A} cdot E_{r e d} ) of ( Z n<E_{r e d} ) of iron B. ( E_{text {oxidation}} ) of ( Z n<E_{text {oxidation}} ) of iron C . ( E_{text {oxidation}} ) of ( Z n=E_{text {oxidation}} ) of iron D. zinc is cheaper than iron | 12 |

653 | A cell ( boldsymbol{C u}left|boldsymbol{C u}^{2+} | boldsymbol{A} boldsymbol{g}^{oplus}right| boldsymbol{A} boldsymbol{g} ) initially contains ( 2 mathrm{M} A g^{oplus} ) and ( 2 mathrm{M} C u^{2+} ) ions in 1 L solution each. The change in cell potential after it has supplied 1 1 current for 96500 s is : ( mathbf{A} cdot-0.003 V ) в. ( -0.02 V ) c. ( -0.04 V ) D. None of these | 12 |

654 | Q. 40 Unlike dry cell, the mercury cell has a constant celu its useful life. Why? cury cell has a constant cell potential throughout o not involved in the overall | 12 |

655 | For a number of years, it was not clear whether mercury (I) ion existed in solution as ( H g^{oplus} ) or as ( H g_{2}^{2+} . ) To distinguish between these two possibilities, the following set up was made: Hg(I) I Solution A II Solution B I Hg(I) where solution A contained 0.263 g mercury | 12 |

656 | Determine the equilibrium constant of the following reaction at ( 298 K: ) ( 2 F e^{3+}+S n^{2+} rightarrow 2 F e^{2+}+S n^{4+} ) (Given: ( boldsymbol{E}_{boldsymbol{S n}^{4+} / boldsymbol{S n}^{2+}}^{circ}= ) ( mathbf{0 . 1 5} )volt; ( boldsymbol{E}_{boldsymbol{F} e^{3+} / mathbf{F e}^{2+}}^{circ}=mathbf{0 . 7 7 1} mathbf{v o l t} mathbf{t} ) | 12 |

657 | Which one of the following processes involve chemical reactions? A. Storing of oxygen gas under pressure in a gas cylinder B. Liquefaction of air C. Keeping petrol in a china dish openly D. Heating copper wire in presence of air at high temperature | 12 |

658 | Conductance of ( boldsymbol{A l}^{+mathbf{3}} ) is ( boldsymbol{x} boldsymbol{S} boldsymbol{m}^{2} boldsymbol{g} boldsymbol{e q}^{-1} ) and that of ( S O_{4}^{-2} ) is ( y S m^{2} g e q^{-1} . ) Molar conductance of Aliminium sulphate is ( boldsymbol{S m}^{2} boldsymbol{m} boldsymbol{o l} boldsymbol{e}^{-1} ) A. ( frac{x+y}{6} ) B. ( x+y ) c. ( 6(x+y) ) D. ( 2 x+3 y ) | 12 |

659 | Glucose saline is used as: A. salt drink B. health drink c. soft drink D. re-hydrating solution | 12 |

660 | Column 1 A) ( wedge^{0}_{m}left(N a N O_{3}right) ) (P) Can be obtained by Kohlraush law B) ( wedge^{0}_{m} ) (Q) Can be obtained by ( left(boldsymbol{C}_{2} boldsymbol{H}_{5} boldsymbol{C O O H}right) quad ) extrapolating ( wedge^{0} m ) vs ( (text {Molarity})^{1 / 2} ) graph to zero molarity. C) Ilonic conductance (R) Contribution by the ion to ( wedge^{0}_{m} ) D) ( wedge^{0}_{m} ) of ( C H_{3} C O O H ) (S) increases on dilution A. A-P,R: B-Q,S:C-S:D-S B. A-P,Q: B-P,S:C-S:D-P,S c. A-R: B-Q:C-R,S:D-P,Q D a c. B-Q.R:C-P:D-Q | 12 |

661 | Name the substance dissolved in pure water to make it a conductor of electricity. | 12 |

662 | To prevent a piece of iron from rusting which one of the following metals will provide the best coating? A. zinc B. copper c. Aluminium D. Leadd | 12 |

663 | Calculate the volume of gas liberated at the anode at STP during the electrolysis of a ( C u S O_{4} ) solution by a current of ( 1 A ) passed for 16 minutes and 5 seconds. A . ( 224 mathrm{mL} ) в. ( 56 mathrm{mL} ) ( c cdot 112 m L ) D. ( 448 mathrm{mL} ) | 12 |

664 | Consider the cell: ( boldsymbol{C d}(boldsymbol{s})left|boldsymbol{C} boldsymbol{d}^{2+}(mathbf{1} . boldsymbol{0} boldsymbol{M}) | boldsymbol{C} boldsymbol{u}^{2+}(mathbf{0 . 1} boldsymbol{M})right| boldsymbol{C} ) If we wish to make a cell with a more positive voltage using the same substance, we should: This question has multiple correct options | 12 |

665 | Write the cathodic and anodic cell reactions of a Hydrogen-Oxygen fuel cell. | 12 |

666 | The electrolyte in lead storage battery is dilute sulphuric acid. The concentration of sulphuric acid in a lead-storage battery must be between ( 4.8 mathrm{M} ) and 5.3 M for most efficient functioning: A 5 mL sulphuric acid sample of a particular battery requires ( 50 mathrm{mL} ) of ( 1.0 mathrm{M} ) NaOH for complete neutralization. Which of the following statements about the functioning of battery is the, most appropriate? A. The acid concentration in the battery is not in the mos effective range B. The acid concentration in the battery is in the most effective range c. The add concentration in the battery is hardly in the most effective range D. only a good mechanic can tell whether or not the acid concentration in the battery is in the most effective range | 12 |

667 | Calculate ( boldsymbol{E}_{text {cell}} ) ( boldsymbol{P t}(boldsymbol{s})left|boldsymbol{H}_{2}(boldsymbol{g})_{1 a t m}right| boldsymbol{H} boldsymbol{A}_{left(boldsymbol{K}_{a}=10^{-7}right)} mathbf{1} boldsymbol{M} | boldsymbol{H} boldsymbol{B}_{(boldsymbol{k}} ) A .0 .06 B. 0.03 V c. ( 0.04 v ) D. ( 0.05 mathrm{v} ) | 12 |

668 | For car battery which one is correct statement? A. Cathode is lead dioxide ( left(P b O_{2}right) ) and anode is copper ( (C u) ) B. Cathode is copper ( (C u) ) and anode is lead dioxide ( left(P b O_{2}right) ) C. Cathode is copper ( (C u) ) and anode is lead ( (P b) ) D. cathode is lead dioxide ( left(P b O_{2}right) ) and anode is lead ( (P b) ) | 12 |

669 | Q Type your question- Given ( : boldsymbol{E}_{boldsymbol{L i} oplus mid boldsymbol{L} i}^{ominus}=-mathbf{3 . 0 5} boldsymbol{V} ) [ begin{array}{l} boldsymbol{E}_{N a oplus mid N a}^{ominus}=-2.71 V \ boldsymbol{E}_{boldsymbol{K}^{oplus} mid boldsymbol{K}}^{ominus}=-mathbf{2 . 9 3} boldsymbol{V} end{array} ] Alkali metals react with water according to the following reaction ( (mathrm{M}= ) Alkali metals): [ mathbf{2} boldsymbol{M}+boldsymbol{H}_{2} boldsymbol{O} rightarrow mathbf{2} boldsymbol{M} boldsymbol{O} boldsymbol{H}+boldsymbol{H}_{2} ] It is found that Li reacts gently with water, whereas K reacts violenly with water. Statements ( Delta G ) values have nothing to do with kinetics of the reaction. The metal having large standard oxidation potential will have lesseer reactivity Potassium (K) has low melting point and heat of reaction which is sufficient to make it melt or even vapourize. This leads to expotential increase in its surface area. | 12 |

670 | In the atmosphere of industrial smog, copper corrodes to form: A. basic copper carbonate and sulphate B. copper oxide c. copper sulphide D. copper nitrate | 12 |

671 | Consider the following cell reaction: [ begin{array}{c} 2 F e(s)+O_{2}(g)+4 H^{+}(a q) rightarrow \ 2 F e^{2+}(a q)+2 H_{2} O(l) ; E^{o}=1.67 V end{array} ] ( mathbf{A t}left[boldsymbol{F} boldsymbol{e}^{2+}right]=mathbf{1 0}^{-mathbf{3}} boldsymbol{M}, boldsymbol{P}_{O_{2}}=mathbf{0 . 1} ) atm and ( p H=3, ) the cell potential at ( 25^{circ} C ) is: A . 1.47 B. 1.77 V c. ( 1.87 mathrm{v} ) D. 1.57 V | 12 |

672 | Calomel electrode is reversible with respect to: ( A cdot H^{+} ) ions B. ( mathrm{Hg}_{2}^{2+} ) ions c. ( mathrm{cl}^{-} ) ions D. None of these | 12 |

673 | Which one of the following could not be liberated from a suitable electrolyte by the passage of 0.25 faraday of electricity through that electrolyte A. 0.25 mole of ( mathrm{Ag} ) B. ( 16 g ) m of ( mathrm{Cu} ) ( c cdot 2 g m ) of ( 0_{2}(g) ) D. 2.8ltrs of H at stp | 12 |

674 | ( boldsymbol{Z} boldsymbol{n}(boldsymbol{s})left|boldsymbol{Z} boldsymbol{n} boldsymbol{C l}_{2}(boldsymbol{a} boldsymbol{q}) | boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q})right| boldsymbol{C l}_{2}(boldsymbol{g}) mid boldsymbol{C} ) In the electrochemical cell described by the cell diagram above, what reaction occurs at the anode? A. ( Z n rightarrow Z n^{2+}+2 e ) B. ( Z n^{2+}+2 e rightarrow Z n ) c. ( C l_{2}+2 e rightarrow 2 C l ) D. ( 2 C^{-} rightarrow C l_{2}+2 e ) E ( . Z n+C l_{2} rightarrow Z n C l_{2} ) | 12 |

675 | The conductivity of a saturated solution of ( B a S O_{4} ) is ( 3.06 times 10^{-6} ) ohm ( ^{-1} c m^{-1} ) and its molar conductance is ( 1.53 o h m^{-1} c m^{-1} m o l^{-1} ) the ( K_{s p} ) of ( B a S O_{4} ) will be ? A ( cdot 4 times 10^{-12} ) В. ( 2.5 times 10^{-9} ) c. ( 2.5 times 10^{-13} ) D. ( 4 times 10^{-6} ) | 12 |

676 | When a conductance cell was filled with ( 0.0025 mathrm{M} ) solution of ( mathrm{K}_{2} mathrm{SO}_{4} ), its resistance was 326 ohm. Length of cell ( =100 mathrm{cm} ) and cross-sectional area ( 2.14 times ) ( 10^{-4} mathrm{cm}^{2} . ) The specific resistance of ( mathrm{K}_{2} mathrm{SO}_{4} ) is: ( mathbf{A} cdot 4.994 times 10^{-4} ) B . ( 5.997 times 10^{-4} ) ( mathbf{c} cdot 6.997 times 10^{-4} ) D. ( 7.997 times 10^{-4} ) | 12 |

677 | Who invented the first true battery? A. Faraday B. onm c. volta D. Alva Edison | 12 |

678 | If the ( Delta G ) of a cell reaction, ( A g C l+ ) ( e^{-} rightarrow A g+C l^{-} ) is ( -21.20 mathrm{kJ}, ) the standard emf of cell is A . ( 0.239 mathrm{v} ) B. ( 0.220 v ) c. ( -0.320 v ) D. – 0.110v | 12 |

679 | The dissociation constant on n-butyric acid is ( 1.6 times 10^{-5} ) and the molar conductivity at infinite dilution is ( 380 times 10^{-4} S m^{2} m o l^{-1} . ) The specific conductance of the ( 0.01 mathrm{M} ) acid solution is: A ( cdot 1.52 times 10^{-5} mathrm{Sm}^{-1} ) В. ( 1.52 times 10^{-2} mathrm{Sm}^{-1} ) C. ( 1.52 times 10^{-3} mathrm{Sm}^{-1} ) D. None | 12 |

680 | A current is passed through 500 mLof an aqueous solution of ( boldsymbol{C a} boldsymbol{I}_{2} ). After sometime, it is observed that 50 millimoles of ( I_{2} ) have been formed. Which of the following statements is(are) correct? This question has multiple correct options A. The number of faradays of charge passed through the solution is ( 0.10 F ) B. The volume of dry ( H_{2} ) at ( S T P ) that has been formed during electrolysis is ( 1120 mathrm{mL} ). c. The ( p H ) of the solution is nearly 0.7 D. The mass of calcium produced is ( 2.0 g ). | 12 |

681 | The electric charge for electrode deposition of 1 g equivalent of a substance is: A. 1 ampere per second B. 96500 Coulombs per second c. 1 ampere for one hour D. The charge on one mole of electrons | 12 |

682 | lumn I with the units given in Column II. Column 11 . 50 Match the terms given in Column I with the units Column! 1. Sem 2 mt CK 3. Sem? mol D G 4 V | 12 |

683 | An electric current is passed through silver voltameter connected to a water voltameter. The cathode of the silver voltameter weighed ( 0.108 g ) more at the end of the electrolysis. The volume of oxygen evolved at STP is: ( mathbf{A} cdot 56 mathrm{cm}^{3} ) В. ( 550 mathrm{cm}^{3} ) ( c cdot 5.6 mathrm{cm}^{3} ) D. ( 11.2 mathrm{cm}^{3} ) E . ( 22.4 mathrm{cm}^{3} ) | 12 |

684 | Molar conductivities of oxalate, ( boldsymbol{K}^{+} ) and ( N a^{+} ) ions at infinite dilution are 148.2 ( mathbf{5 0 . 1 , 7 3 . 5} S mathrm{cm}^{2} ) mol ( ^{-1} ) respectively. Then, equivalent conductivity at infinite dilution for sodium-potassium oxalate ( left[left(boldsymbol{C O O}^{-}right)_{2} boldsymbol{N} boldsymbol{a}^{+} boldsymbol{K}^{+}right] ) will be: A. ( 271.8 mathrm{S} mathrm{cm}^{2} ) eq ( ^{-1} ) В. ( 67.95 mathrm{S} mathrm{cm}^{2} mathrm{eq}^{-1} ) c. ( 543.6 S mathrm{cm}^{2} e q^{-1} ) D. ( 135.9 S mathrm{cm}^{2} e q^{-1} ) | 12 |

685 | toppr ) Q Type your question_ watches, etc. (ii) It consists of zinc-mercury amalgam as anode and a paste of HgO and carbon as the cathode. (iii) The electrolyte is a paste of ( Z n(O H)_{2} ) and ( K O_{2} ) (iv) The electrode reactions for the cell are At anode: ( Z n(H g)+H_{2} O rightarrow Z n O_{(s)}+ ) ( 2 O H^{-}+2 e^{-} ) At cathode: ( boldsymbol{H} boldsymbol{g} boldsymbol{O}+boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{2} boldsymbol{e}^{-} rightarrow ) ( boldsymbol{H} boldsymbol{g}_{(l)}+2 boldsymbol{O} boldsymbol{H} ) A. (ii) and (iii) only B. (i) ad (ii) only C. (i), (iii) and (iv) only D. (iii) and (iv) only | 12 |

686 | ( 100 mathrm{ml} mathrm{CuSO}_{4} ) (aq) was electrolyzed using inert electrodes by passing 0.965 A till the ( p H ) of the resulting solution was ( 1 . ) The solution after electrolysis was neutralized, treated with excess ( K I ) and titrated with ( 0.04 mathrm{M} N a_{2} S_{2} O_{3} ) Volume of ( N a_{2} S_{2} O_{3} ) required was 35 ml. Assume no volume change during electrolysis. If the initial concentration ( (mathrm{M}) ) of ( mathrm{CuSO}_{4} ) was ( 64 times ) ( 10^{-x}, ) then what is the value of ( x ? ) | 12 |

687 | The resistance of a conductivity cell containing ( 0.001 mathrm{M} ) KCl solution at ( 298 mathrm{K} ) is ( 1500 Omega . ) What is the cell constant if conductivity of ( 0.001 mathrm{M} ) KCl solution at ( 298 K ) is 0.146 times ( 10^{-3} S c m^{-1} ? ) | 12 |

688 | Q1. What is meant by electrochemical series? What are characteristics of electrochemical series? | 12 |

689 | An electrochemical cell is constructed with an open swtich as shown below: When the switch is closed, mass of tin- electrode increases. If ( boldsymbol{E}^{circ}left(boldsymbol{S} boldsymbol{n}^{2+} / boldsymbol{S} boldsymbol{n}right)= ) ( -0.14 V ) and for ( E^{circ}left(X^{n+} / Xright)= ) ( -0.78 V ) and initial emf of the cell is ( 0.65 mathrm{V}, ) determine ( n ) ( A cdot 3 ) в. ( c .5 ) ( D ) | 12 |

690 | State True or False. Pure water can be used as an electrolyte in the process of electrolysis. A. True B. False | 12 |

691 | If copper is kept open in air, it slowly loses its shining brown surface and gains a green coating. It is due to the formation of: A ( cdot C u C O_{3} ) в. ( C u S O_{4} ) c. ( C u C O_{3} cdot C u(O H)_{2} ) D. ( C u O ) | 12 |

692 | Which of the following will increase the voltage of the cell? ( boldsymbol{S} boldsymbol{n}(boldsymbol{s})+boldsymbol{2} mathbf{A} mathbf{g}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s})+boldsymbol{S} boldsymbol{n}^{2+} ) A. Increase in the concentration of ( operatorname{Sn}^{2+} ) ions B. Increase in the concentration of ( A g^{+} ) ions c. Increase in the size of silver rod D. Removal of salt bridge | 12 |

693 | The tarnishing of silver ornaments in atmosphere is due to: This question has multiple correct options A. ( A g_{2} O ) в. ( A g_{2} S ) c. ( A g_{2} C O_{3} ) D. ( A g_{2} S O_{4} ) | 12 |

694 | Question 10. The conductivity of sodium chloride at 298 K has been determined at different concentrations and the results are given below: Concentration/M 0.001 0.010 0.0200.050 0.100 10-2 x k/Sm-? 1.237 11.85 23.15 55.53 106.74 12 Calculate 4 for all concentrations and draw a plot between Am. and C . Find the value of me In order to plot a graph between Am and JC first find the values of C2 and am and plot the graph. After that find am from the graph, as it is equal to the intercept on the maxis. | 12 |

695 | Give reasons: On the basis of ( E^{circ} ) values, ( O_{2} ) gas should be liberated at anode but it is ( C l_{2} ) gas which is liberated in the electrolysis of aqueous NaCl. | 12 |

696 | The electrolytic process by which an oxide of metal is coated over metal surface is called: A. electrolysis B. electroplating c. anodising D. electrorefining | 12 |

697 | Assertion In an electrochemical cell, the electrode that is the site of reduction is called the anode. Reason Oxidation always occurs at the cathode. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

698 | A silver article generally turns black when kept in the open for a few days. The article when rubbed with toothpaste again starts shining. Name the black substance formed and give its chemical formula: A . silver oxide, ( left(A g_{2} text { , } ) ) right. B. Silver chloride, ( (A g C l) ) C. Silver sulphide, ( left(A g_{2} Sright) ) D. silver iodide,( ( (A g I) ) | 12 |

699 | What is the standard reduction potential ( left(boldsymbol{E}^{o}right) ) for ( boldsymbol{F} boldsymbol{e}^{mathbf{3}+} rightarrow boldsymbol{F} boldsymbol{e} ) Given that: ( boldsymbol{F} boldsymbol{e}^{2+}+boldsymbol{2} boldsymbol{e} boldsymbol{6}-rightarrow boldsymbol{F} boldsymbol{e} ; boldsymbol{E}_{boldsymbol{F}}^{o} boldsymbol{e}_{boldsymbol{F} e^{2+} / boldsymbol{F} e}= ) ( -0.47 V ) ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{e}^{-} rightarrow boldsymbol{F} boldsymbol{e}^{2+} ; boldsymbol{E}_{boldsymbol{F} e^{3+} / boldsymbol{F} e^{2+}}^{o}= ) ( +0.77 V ) A ( .+0.057 V ) в. ( +0.30 V ) c. ( -0.30 V ) D. ( -0.057 V ) | 12 |

700 | Match the List I with the List II. | 12 |

701 | The standard electrode potential ( left(E^{circ}right) ) for Daniel cell is ( +1.1 mathrm{V} ). Calculate ( Delta G^{circ} ) for the reaction. ( boldsymbol{Z} boldsymbol{n}(boldsymbol{s})+boldsymbol{C} boldsymbol{u}_{(a q)}^{2+} rightarrow boldsymbol{Z} boldsymbol{n}_{(a q)}^{2+}+boldsymbol{C u}(boldsymbol{s}) ) ( (1 F=96500 C / m o l) ) | 12 |

702 | The chemical reaction, ( 2 A g C l_{(s)}+ ) ( boldsymbol{H}_{2(g)} rightarrow 2 boldsymbol{H} boldsymbol{C l}_{(a q)}+boldsymbol{2} boldsymbol{A} boldsymbol{g}_{(s)} ) taking place in a galvanic cell is represented by the notation: A ( cdot P t_{(s)} mid H_{2(g)}, 1 ) bar ( left|1 M K C l_{(a)}right| A g C l_{(s)} mid A g_{(s)} ) B . ( P t_{(s)} mid H_{2(g)}, 1 ) bar ( mid 1 ) M ( H C l_{(a q)}left|1 M A g_{(a q)}^{+}right| A g_{(s)} ) C. ( P t_{(s)} mid H_{2(g)}, 1 ) bar ( mid 1 ) M ( H C l_{left(a_{9}right)}left|A g C l_{(s)}right| A g_{(s)} ) D. ( P t_{s} mid H_{2(g)}, 1 ) bar ( left|1 M H C l_{(a q)}right| A g_{(s)} mid A g C l_{s} ) | 12 |

703 | Question 11. Conductivity of 0.00241M acetic acid is 7.896 x 10-5 S cm-1 Calculate its molar conductivity. If for acetic acid is 390.5 S cmmol-, what is its dissociation constant? Use the formula 1m = to find molar conductivity; Ca² so calculate Ka (dissociation constant) as you know Cand a. | 12 |

704 | A magnet is pulled away from a conducting coil in a circuit. The direction of the induced emf in the coil can be found from………………… A. Faraday’s law of electromagnetic induction B. Joule’s law c. Lenz’s law D. Fleming’s left hand rule | 12 |

705 | Define the terms conductivity and molar conductivity for the solution of an electrolyte. Comment on their variation with temperature. | 12 |

706 | The EMF of an ( boldsymbol{H}_{2}-boldsymbol{O}_{2} ) fuel cell: ( A cdot ) is independent of partial pressures of ( H_{2} ) and ( O_{2} ) B. decreases on increasing ( P_{H_{2}} ) and ( P_{O_{2}} ) C. increases on increasing ( P_{H_{2}} ) and ( P_{O_{2}} ) D. varies with the concentration of ( O H^{-} ) ions in the cathodic and anodic compartments | 12 |

707 | What happens to molar conductivity when one mole of ( K C l ) dissolved in one litre is diluted to five liters? | 12 |

708 | Which one of the following statements is incorrect? A. Specific conductivity decreases with dilution B. Equivalent and molar conductivities increases with dilution ( mathrm{C} cdot Lambda_{m}^{o} ) for a weak electrolyte cannot be found by extrapolation of ( Lambda_{m} ) to zero concentration D. Molar conductivity of a strong electrolyte increases with dilution because ionization increases with dilution | 12 |

709 | How much electricity in terms of Faraday is required to produce 100 g of Ca from molten ( C a C l_{2} ? ) A . 1 F в. 2 F ( c .3 ) F D. 5 | 12 |

710 | For a cell, the cell reaction is ( M g(s)+ ) ( C u^{2+}(a q) rightarrow M g^{2+}(a q)+C u(s) . ) If the S.R.P. values of ( M g ) and ( C u ) are ( -2.37 V ) and ( +0.34 V ) respectively, the EMF of the cell is: A ( .+2.03 V ) B . ( -2.03 mathrm{V} ) ( mathrm{c} ldots+2.71 mathrm{V} ) D. ( -2.71 V ) | 12 |

711 | Question 4. What does the negative sign in the expression EZ 2+ /Zn) = -0.76V mean? | 12 |

712 | Lead pipes are readily corroded by: A. water B. acetic acid c. conc. ( H_{2} S O_{4} ) D. dil. ( H_{2} S O_{4} ) | 12 |

713 | A galvanic cell is constructed using the redox reaction, it is represented as: ( frac{1}{2} H_{2}(g)+A g C l(s) rightleftharpoons H^{+}(a q)+ ) ( boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{A} boldsymbol{g}(boldsymbol{s}) ) ( mathbf{A} cdot P tleft|H_{2}(g)right| H C l(s o l n .) | A g N O_{3}(s o l n .) mid A g ) B ( cdot A g|A g C l(s)| K C l(s o l n .) mid H C l(text {soln.}), H_{2}(g) mid P t ) ( mathbf{c} cdot P tleft|H_{2}(g)right| K C l(s o l n .) | A g C l(s) mid A g ) ( mathbf{D} cdot P tleft|H_{2}(g), H C l(s o l n .) | A g C l(s)right| A g ) | 12 |

714 | 54 NCERT Exem lectrolysis of aqueous solution of CuSO4 by Q. 23 What will happen during the electrolysis of aqueo using platinum electrodes? (a) Copper will deposit at cathode (b) Copper will dep (C) Oxygen will be released at anode (d) Copper will disso Thinking Process This problem is based on electrolysis of electrolytes. (6) Copper will deposit at anode (d) Copper will dissolve at anode node | 12 |

715 | State the Kohlrausch law of independent migration of ions. Why does the conductivity of a solution decrease with dilution? | 12 |

716 | 2. 29 Can Ecell or 4, Gº for cell reaction ever be equal to zero? | 12 |

717 | What is electrolysis? A solution of ( C u S O_{4} ) is electrolysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode? | 12 |

718 | Process of depositing a thin layer of zinc metal on iron objects is called: A. rusting B. corrosion c. sublimation D. galvanisation | 12 |

719 | ( ln ) a fuel cell ( H_{2} ) and ( O_{2} ) react to produce electricity. In the process ( boldsymbol{H}_{2} ) gas is oxidized at anode and ( O_{2} ) at cathode. If 67.2 litre of ( H_{2} ) at STP reacts in 15 minutes. The average current produced is: ( A cdot 643.33 mathrm{A} ) B. 642.33 А c. ( 682.33 mathrm{A} ) D. None of the above | 12 |

720 | During discharging of lead-storage acid battery following reaction takes place: ( boldsymbol{P b}(s)+boldsymbol{P b O}_{2}(s)+2 boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow ) ( 2 P b S O_{4}(s)+2 H_{2} O ) If 2.5 amp of current is drawn for 965 minutes, ( H_{2} S O_{4} ) consumed is: A. 0.75 mol B. 3.00 mol c. 1.50 mol D. 4.50 mol | 12 |

721 | Fill in the blanks: Electrolysis is the passage of ( _{text {一一一一一一一 }} ) (electricity / electrons) through a liquid or a solution accompanied by a (physical/ chemical) change. | 12 |

722 | When ( X ) amperes of current is passed through molten ( A l C l_{3} ) for 96.5 seconds. 0.09 grams of aluminium is deposited. What is the value of ( X ? ) A . 10 B. 20 ( c . ) 30 ( D cdot 40 ) | 12 |

723 | A zinc electrode is placed in a ( 0.1 mathrm{M} ) solution at ( 25^{0} C . ) assuming that the salt is ( 20 % ) dissociated at this dilutions calculate the electrode reduction potential. ( boldsymbol{E}^{0}left(boldsymbol{Z} boldsymbol{n}^{2+} mid boldsymbol{Z} boldsymbol{n}right)=-mathbf{0 . 7 6} boldsymbol{V} ) | 12 |

724 | At ( 25^{circ} C, ) the equivalent conductance at infinite dilution of ( H C l, C H_{3} C O O N a ) and ( N a C l ) are 426.1,91.0 and ( 126.45 c m^{2} Omega^{-1} e q^{-1} ) respectively, the ( wedge_{infty} ) for ( boldsymbol{C H}_{3} boldsymbol{C O O H}left(boldsymbol{i n} boldsymbol{c m}^{-1} boldsymbol{Omega}^{-1} boldsymbol{e q}^{-1}right) ) is: ( mathbf{A} cdot 391.6 ) B. 390.6 ( c .389 .6 ) D. 388.6 | 12 |

725 | The variation of ( A_{m} ) acetic acid with concentration is correctly represented by: ( A ) B. ( mathbf{c} ) D. | 12 |

726 | Iron can be prevented from rusting by: This question has multiple correct options A. connecting iron to more electropositive metal a case of cathodic protection. B. connecting iron to more electropositive metal a case of anodic protection. c. connecting iron to less electropositive metal a case of anodic protection D. connecting iron to less electropositive metal a case of cathodic protection. | 12 |

727 | Question 8. The conductivity of 0.20M solution of KCl at 298K is 0.0248 S cm . Calculate its molar conductivity. we Molar conductivity is calculated as Ame ‘ mol-‘cm?. So, first convert concentration (mol/L) into mol cm and then calculate molar conductivity. | 12 |

728 | Assertion: Copper sulphate solution can be stored in a zinc vessel. Reason: ( boldsymbol{E}_{boldsymbol{C u}^{2+} mid boldsymbol{C u}}^{ominus}= ) ( mathbf{0 . 3 4} boldsymbol{V}, boldsymbol{E}_{Z n^{2+} mid mathbf{Z} n}^{ominus}=-mathbf{0 . 7 6} boldsymbol{V} ) ( boldsymbol{E}_{A boldsymbol{g}^{oplus} mid A boldsymbol{g}}^{ominus}=mathbf{0 . 8 0} boldsymbol{V} ) A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

729 | Assertion Ionic compounds are bad conductors of electricity. Reason In ionic compounds mobile ions exists. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Assertion is incorrect and the Reason is correct | 12 |

730 | Define fuel cell and write its two advantages. | 12 |

731 | Chemical effect of electric current may cause: A. formation of gas bubbles at the electrodes B. deposit of metal on the electrodes C. change in colour of the solution D. all of above | 12 |

732 | Which of the following quantity is always positive for a spontaneous chemical reaction? A. Standard voltaic potential B. Entropy c. Enthalpy D. Reaction rate E. Gibbs free energy | 12 |

733 | More electronegative elements have: A. negative reduction potential B. tendency to lose electrons C. positive reduction potential D. positive oxidation potential | 12 |

734 | A battery jar contained a solution of copper sulfate. Two electrodes. one made of copper the other a metal object to be copper plated, were placed in the jar and connected to a source of direct current. Which of the following statements concerning this system is correct? A. The object to be placed is the anode B. Oxidation occurs at the anode c. The sulfate ions migrate toward the cathode D. The concentration of the copper sulfate solution increases as electrolysis proceeds E. The copper electrode increases in mass | 12 |

735 | After electrolysis of a sodium chloride solution with inert electrodes for a certain period of time, ( 600 m L ) of the solution was left which was found to be ( 1 N ) in ( N a O H . ) During the same period ( 31.75 g ) of copper was deposited in the copper voltameter in series with the electrolytic cell. Calculate the percentage theoretical yield of ( N a O H ) obtained. | 12 |

736 | The equilibrium constant for the reaction is: ( 2 F e^{3+}+3 I^{ominus} rightleftharpoons F e^{3+}+C e^{3+} ) Given : ( E_{C e^{4+1} C e^{3+}}=1.44 mathrm{V} ) ( E_{F e^{3+} 1 F e^{2+}}^{ominus}=0.68 mathrm{V} ) A . ( 7.236 times 10^{12} ) B . ( 7.386 times 10^{12} ) c. ( 7.158 times 10^{12} ) D. None of these | 12 |

737 | Ihs Q. 65 Assertion (A) Copper sulphate can be stored in zinc vessel. Reason (R) Zinc is less reactive than copper. | 12 |

738 | Limiting molar conductivity of NaBr is: ( mathbf{A} cdot Lambda_{m}^{o} N a B r=Lambda_{m}^{o} N a C l+Lambda_{m}^{o} K B r ) B. ( Lambda_{m}^{o} N a B r=Lambda_{m}^{o} N a C l+Lambda_{m}^{o} K B r-Lambda_{m}^{o} K C l ) ( mathbf{C} cdot Lambda_{m}^{o} N a B r=Lambda_{m}^{o} N a O H+Lambda_{m}^{o} N a B r-Lambda_{m}^{o} N a C l ) ( mathbf{D} cdot Lambda_{m}^{o} N a B r=Lambda_{m}^{o} N a C l-Lambda_{m}^{o} N a B r ) | 12 |

739 | What is the cell reaction occurring in Daniell cell (galvanic cell)? ( mathbf{A} cdot C u(s)+Z n S O_{4}(a q .) rightarrow C u S O_{4}(a q .)+Z n(s) ) B ( cdot Z n(s)+C u S O_{4}(a q .) rightarrow C u(s)+Z n S O_{4}(a q .) ) ( mathbf{c} cdot N i(s)+Z n S O_{4}(a q .) rightarrow N i S O_{4}(a q .)+Z n(s) ) ( mathbf{D} cdot 2 N a(s)+C d S O_{4}(a q .) rightarrow N a_{2} S O_{4}(a q .)+C d(s) ) | 12 |

740 | Assertion: The Nernst equation gives concentration dependence of EMF of the cell. Reason: In a Daniell cell current flows from cathode to anode. A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

741 | Question 2. Can you store copper sulphate solutions in a zinc pot? Consider the Eº values of copper and zinc. More the negative value of E higher is the reactivity and a more reactive metal can displace a less reactive metal from its salt solution. | 12 |

742 | The below reaction is the gold-plating process reaction. [ boldsymbol{A} boldsymbol{u}^{3+}(boldsymbol{a q})+boldsymbol{3} boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{u}(boldsymbol{s}) ] If ( 0.600 g ) of ( A u ) is plated onto a metal how many coulombs are used? ( mathbf{A} cdot 299 C ) B. ( 868 C ) ( c .2,990 C ) D. ( 8,680 C ) | 12 |

743 | ( boldsymbol{Z} boldsymbol{n}(boldsymbol{s})left|boldsymbol{Z} boldsymbol{n} boldsymbol{C l}_{2}(boldsymbol{a} boldsymbol{q}) | boldsymbol{C l}^{-}(boldsymbol{a q})right| boldsymbol{C l}_{2}(boldsymbol{g}) mid boldsymbol{C} ) In the electrochemical cell described by the cell diagram above, what reaction occurs at the anode? A. ( Z n rightarrow Z n^{2+}+2 e^{-} ) B. ( Z n^{2+}+2 e^{-} rightarrow Z n ) c. ( C l_{2}+2 e^{-} rightarrow 2 C l ) D. ( 2 C l^{-} rightarrow C l_{2}+2 e^{-} ) | 12 |

744 | A conductance cell was filled with 0.01 molar KCl. Its resistance was found to be 150 ohm at ( 25^{circ} mathrm{C} ). The conductivity was observed to be ( 0.00177 S c m^{-1} . ) The cell was when washed and filled with 0.05 molar solution of NaCl whose resistance was found to be 325 ohm. Conductivity of NaCl solution is: B. ( 9.168 times 10^{-4} mathrm{Scm}^{-1} ) c. ( 8.169 times 10^{-4} mathrm{Scm}^{-1} ) D. None of these | 12 |

745 | The extent of charge of lead accumulator is determined by: ( mathbf{A} cdot ) amount of ( P b S O_{4} ) in the battery B. amount of ( P b O_{2} ) in the battery C . specific gravity of ( H_{2} S O_{4} ) of the battery D. amount of ( P b ) in the battery | 12 |

746 | Assertion If two half reaction with electrode potential ( E_{1}^{o} ) and ( E_{2}^{o} ) gives a third half reaction, then ( Delta G_{3}^{o}=Delta G_{1}^{o}+Delta G_{2}^{o} ) Reason ( boldsymbol{E}_{mathbf{3}}^{boldsymbol{o}}=boldsymbol{E}_{mathbf{1}}^{boldsymbol{o}}+boldsymbol{E}_{mathbf{2}}^{boldsymbol{o}} ) A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

747 | Answer the following. a. What is done to prevent corrosion of metals? b. What are the metals that make the alloys brass and bronze? | 12 |

748 | The molar conductance (in ( left.mathbf{Omega}^{-1} boldsymbol{c m}^{2} boldsymbol{m o l}^{-1}right) ) of ( boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4} ) solution is: | 12 |

749 | Electrolyte for silver plating is: A. potassium nitrate solution B. dilute sulphuric acid C. double cyanide of silver and potassium solution D. any of the above | 12 |

750 | For the reaction: ( boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{a} boldsymbol{q})+boldsymbol{A} boldsymbol{g}^{+}(boldsymbol{a} boldsymbol{q}) longrightarrow boldsymbol{A} boldsymbol{g}(boldsymbol{s})+ ) ( boldsymbol{F} boldsymbol{e}^{+boldsymbol{3}}(boldsymbol{a} boldsymbol{q}) ) Predict which change will decrease the cell voltage? A. Increase the amount of Agg B. Decrease the concentration of ( A g^{+} ) C. Increase the concentration of ( F e^{+3} ) D. Both ( B ) and ( C ) | 12 |

751 | ( E_{1}, E_{2}, E_{3} ) are the emf values of the three galvanic cells respectively. (i) ( Z nleft|Z n_{1 M}^{2+}right|left|C u_{0.1 M}^{2+}right| C u ) ( (text { ii }) Z nleft|Z n_{1 M}^{2+}right|left|C u_{1 M}^{2+}right| C u ) (iii) ( Z nleft|Z n_{0.1 M}^{2+} | C u_{1 M}^{2+}right| C u ) Which one of the following is true? A ( . E_{2}>E_{3}>E_{1} ) в. ( E_{3}>E_{2}>E_{1} ) c. ( E_{1}>E_{2}>E_{3} ) D. ( E_{1}>E_{3}>E_{2} ) | 12 |

752 | What is electroplating? Explain the process. Give two uses of electroplating | 12 |

753 | Which of the following statement is not true? A. metals produce a ringing sound when struck hard B. copper doesn’t get rusted C. coal and sulphur are soft and dull in appearance D. magnesium and phosphorous burn vigorously in air | 12 |

754 | The standard electrode potential ( left(boldsymbol{E}^{ominus}right) ) for ( boldsymbol{O C l}^{-} mid boldsymbol{C l}^{-} ) and ( boldsymbol{C l}^{-} mid frac{mathbf{1}}{mathbf{2}} boldsymbol{C l}_{2} ) respectively are ( 0.94 mathrm{V} ) and ( -1.36 mathrm{V} ). The ( boldsymbol{E}^{ominus} ) value of ( boldsymbol{O} boldsymbol{C l}^{-} mid frac{boldsymbol{1}}{boldsymbol{2}} boldsymbol{C l}_{2} ) will be: A. ( -0.42 mathrm{v} ) в. ( -2.20 mathrm{v} ) c. ( 0.52 mathrm{v} ) D . 1.04 | 12 |

755 | If ( m ) is the mass of silver deposited at the cathode by ( 2 A ) current flowing for ( 25 m i n ) through a silver voltameter, then the mass deposited by ( 1.5 A ) current flowing for ( 600 s ) is A . в. ( 3 m ) ( mathrm{c} .0 .3 mathrm{m} ) D. None | 12 |

756 | The equilibrium constant for the redox change ( left[2 A gleft(N H_{3}right)_{2}^{+}+C_{6} H_{12} O_{6}+H_{2} O rightarrowright. ) ( boldsymbol{C}_{6} boldsymbol{H}_{12} boldsymbol{O}_{7}+boldsymbol{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s})+boldsymbol{C}_{6} boldsymbol{H}_{12} boldsymbol{O}_{2}+ ) ( left.mathbf{2} boldsymbol{H}^{+}right] ) is: ( mathbf{A} cdot 5.15 times 10^{9} ) В. ( 4,2 times 10^{5} ) c. ( 1.72 times 10^{-11} ) | 12 |

757 | The same quantity of electricity is passed through ( A l_{2}left(S O_{4}right)_{3} ) and ( A g N O_{3} ) solution with platinum electrodes. If ( n ) number of Al atoms are deposited on the cathode, the number of Ag atoms deposited on the cathode will be: ( A ) B. 2n ( c cdot 3 n ) D. n/2 | 12 |

758 | ( Z n ) Amalgam is prepared by the electrolysis of aqueous ( Z n C l_{2} ) using ( H g ) cathode ( (9 mathrm{gm}) . ) How much current should be passed through ( Z n C l_{2} ) solution for 1000 seconds to prepare a ( Z n ) amalgam with ( 25 % Z n ) by weight ? ( (Z n text { atomic weight }=65.4) ) A . ( 5.6 mathrm{A} ) в. 7.2 A ( c cdot 8.85 A ) D. 11.2 A | 12 |

759 | Anodic oxidation of ammonium hydrogen sulphate produces ammonium persulphate. ( N H_{4} H S O_{4} rightarrow N H_{4} S O_{4}^{-}+H^{+} ) ( mathbf{2} boldsymbol{N} boldsymbol{H}_{4} boldsymbol{S} boldsymbol{O}_{4}^{-} rightarrowleft(boldsymbol{N} boldsymbol{H}_{4}right)_{2} boldsymbol{S}_{2} boldsymbol{O}_{8}+boldsymbol{2} boldsymbol{e}^{-} ) (Anodic oxidation) ( 2 H^{+}+2 e^{-} rightarrow H_{2} ) (Cathodic reduction) Hydrolysis of ammonium persulphate forms ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) ( left(N H_{4}right)_{2} S_{2} O_{8}+2 H_{2} O rightarrow ) ( mathbf{2} boldsymbol{N} boldsymbol{H}_{mathbf{4}} boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{O}_{2} ) Current efficiency inn electrolytic process is ( 60 % ). Calculate the amount of current required to produce ( 85 g ) of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) per hour Hydrolysis reaction shows ( 100 % ) yield. | 12 |

760 | The ( E_{c e l l}^{o} ) for ( C uleft|C u^{2+}right|left|A g^{+}right| A g ) in volt is A. +0.449 B. +0.474 c. -0.449 D. -0.474 | 12 |

761 | The ( E_{text {cell }}^{o} ) for ( boldsymbol{C u}left|boldsymbol{C} boldsymbol{u}^{2+} | boldsymbol{A} boldsymbol{g}^{+}right| boldsymbol{A} boldsymbol{g} ) is: A . ( 0.415 V ) в. ( 0.374 V ) c. ( -0.415 V ) D. ( -0.374 V ) | 12 |

762 | For the given cell reaction: ( boldsymbol{F e}^{2+}+ ) ( boldsymbol{C} boldsymbol{e}^{4+} rightleftharpoons boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{C} boldsymbol{e}^{boldsymbol{3}+} . ) The equilibrium constant is: (Given: ( boldsymbol{E}_{C e^{4+} / C e^{3+}}^{circ}= ) ( left.mathbf{1 . 4 4} boldsymbol{V} ; boldsymbol{E}_{boldsymbol{F} e^{2+} / boldsymbol{F} e^{3+}}^{circ}=mathbf{0 . 6 8} boldsymbol{V}right) ) | 12 |

763 | The resistance of a ( frac{N}{10} K C l ) aqueous solution is ( 245 Omega ). If the electrodes in the cell are ( 4 mathrm{cm} ) apart and area having ( 77 mathrm{cm}^{2} ) each, the molar conductance of the solution will be: A . 233 B. 2.12 c. 23.32 D. 0.233 | 12 |

764 | The thermodynamic efficiency of cell is given by: A. ( Delta H / Delta G ) в. ( frac{n F E}{Delta G} ) c. ( frac{-n F E}{Delta H} ) D ( cdot n F E^{ominus} ) | 12 |

765 | Assertion: The density of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) decreases in lead storage cell during discharging. Reason: Calomel electrode is a reference electrode and it is better than hydrogen electrode. A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

766 | The equilibrium constant for the following reaction is: ( 2 F e^{3+} 3 I^{ominus} rightleftharpoons 2 F e^{2+}+I_{3}^{ominus} ) The standard reduction potential in acidic conditions is ( 0.78 V ) and ( 0.54 V ) respectively, for ( boldsymbol{F e}^{mathbf{3}}+ ) ( left|boldsymbol{F} boldsymbol{e}^{2+} boldsymbol{a} boldsymbol{n} boldsymbol{d} boldsymbol{I}_{3}^{ominus}right| boldsymbol{I}^{ominus} ) couples ( mathbf{A} cdot K_{e q}=10^{8} ) В. ( K_{e q}=10^{7} ) ( mathbf{c} cdot K_{e q}=10^{5} ) D. None of these | 12 |

767 | In rusting of iron, iron is oxidised and ( mathrm{O}_{2} ) is reduced. The no. of electrons used during reduction ( mathrm{O}_{2} ) are : | 12 |

768 | What are galvanic cells? Explain the construction and working of galvanic cell with an example? | 12 |

769 | Assertion Iron is protected from corrosion by connecting magnesium metal with it. Reason Iron acts as cathode and magnesium as anode which gradually disappears. | 12 |

770 | Assertion If standard reduction potential for the reaction ( boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g} ) is 0.80 volt, then for the reaction ( 2 A g^{+}+2 e^{-} rightarrow ) 2 Ag.lt will be 1.60 volt. Reason If concentration of ( A g^{+} ) ions is doubled the standard electrode potential is also doubled. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

771 | If the molar concentration of ( boldsymbol{P b I}_{2} ) is ( 1.5 times 10^{-3} ) mol ( L^{-1}, ) then the concentration of iodide ions in ( g ) ion ( L^{-1} ) is: A. ( 3.0 times 10^{-3} ) В. ( 6.0 times 10^{-3} ) D. ( 0.6 times 10^{-6} ) | 12 |

772 | Conductivity (Unit Siemen’s ‘S’) is directly proportional to area of the vessel and the concentration of the solution in it and is inversely proportional to the length of the vessel, then the unit of constant of proportionality is ( mathbf{A} cdot S m m o l^{-1} ) B. ( S m^{2} m o l^{-1} ) c. ( S^{-2} m^{2} ) mol D. ( S^{2} m^{2} ) mol ( ^{-2} ) | 12 |

773 | ( mathbf{Lambda}_{infty} ) of propionic acid cannot be determined experimentally because: A. conductance at high concentration cannot be determined B. conductance at low concentration cannot be determined c. conductance a thigh pressure cannot be determined D. all of the above | 12 |

774 | How many molecules of ( C O_{2} ) are formed when one molecule of ( C_{6} H_{12} O_{6} ) is oxidised in our body? A . 4 B. 2 ( c cdot 6 ) D. | 12 |

775 | a. Calculate e.m.f of cell for the reaction: ( M g_{(s)}+C u^{2+}(0.0001 M) rightarrow ) ( M g^{2+}(0.001 M)+C u_{(s)} ) Given that: ( E_{M g^{2+} / M g}^{o}=-2.37 mathrm{V} ) ( E_{C u^{2+} / C u}^{o}=+0.34 v ) b. i) State Kohlrausch law. ii) What is meant by limiting molar conductance. | 12 |

776 | Predict whether the following equation will take place or not. ( boldsymbol{C u}_{(s)}+mathbf{2 H}_{(a q)}^{+} rightarrow boldsymbol{C u}_{a q}^{2+}+boldsymbol{H}_{2(g)} ) Given that ( boldsymbol{E}_{boldsymbol{C u}^{2+} mid boldsymbol{C u}}^{0}=boldsymbol{0 . 4 4} boldsymbol{V} ; boldsymbol{E}_{boldsymbol{H}^{+} mid boldsymbol{H}_{2}}^{0}= ) 0 | 12 |

777 | The equilibrium constant for the reaction, ( boldsymbol{S n}(boldsymbol{s})+boldsymbol{2} boldsymbol{H}^{+} rightarrow boldsymbol{S} boldsymbol{n}^{2+}+ ) ( boldsymbol{H}_{2}(boldsymbol{g}) boldsymbol{a} boldsymbol{t} boldsymbol{2} boldsymbol{5}^{circ} boldsymbol{C} ) is: ( boldsymbol{E}^{circ}left(boldsymbol{S} boldsymbol{n}^{2+} mid boldsymbol{S} boldsymbol{n}right)=mathbf{0 . 1 4} ) A ( .5 .5 times 10^{4} ) B. ( 2.3 times 10^{2} ) c. ( 1.1 times 10^{2} ) D. 1.009 | 12 |

778 | toppr Q Type your question 19 ( m ) ( ) ( A ) ( B ) ( c ) ( D ) | 12 |

779 | ( boldsymbol{C a}, boldsymbol{N a}, boldsymbol{M} boldsymbol{g}, boldsymbol{Z} boldsymbol{n}, boldsymbol{F e}, boldsymbol{H}, boldsymbol{C u}, boldsymbol{H} boldsymbol{g}, boldsymbol{A} boldsymbol{g}, boldsymbol{A} ) Given elements are in order of decreasing reactivity according to electrochemical series. Half-reaction possible for the shown electrochemical cell at the anode is: A ( cdot C u^{2+}+e^{-} rightarrow C u+ ) B ( cdot Z n(s) rightarrow Z n^{2+}+2 e^{-} ) c. ( Z n^{2+}+2 e^{-} rightarrow Z n(s) ) D. ( C u(s) rightarrow C u^{2+}+2 e^{-} ) E ( cdot C u^{2+}+2 e^{-} rightarrow C u(s) ) | 12 |

780 | An electric spark is struck between two electrodes placed near each other, inside a closed tank full of petrol. What’ll happen? A. Spontaneous combustion of petrol B. Explosion c. Slow combustion of petrol D. Nothing will happen | 12 |

781 | During the working of a galvanic cell and with the passage of time: This question has multiple correct options A. spontaneity of the cell reaction decreases, ( E_{c c l} ) decreases B. reaction quotient Q decreases, E ( _{text {cell } text {increases }} ) C . reaction quotient ( Q ) increases, ( E_{c e l l} ) decreases D. at equilibrium, ( Q=K_{e q}, E_{c e l l}=0 ) | 12 |

782 | The removal of salt bridge from Daniell cell brings in the following changes: A ( cdot E_{Z n / Z n^{2+}}^{o} ) changes B . ( E_{C u / C u^{2+}}^{o} ) changes C. ( E_{text {clu }}^{o} ) drops to zero D. none of the above | 12 |

783 | The factor which is not affecting the conductivity of any solution is A. temperature B. dilution c. nature of electrolyte D. none of the above | 12 |

784 | When copper rod donates electrons to hydrogen ions, it gains charge. A. positive B. negative c. no charge D. can’t say | 12 |

785 | The process in which metal surface is made inactive is called: A. passivation B. galvanising c. corrosion D. pickling | 12 |

786 | Q.41 Solutions of two electrolytes A and B are diluted. 1.5 times while that of A increases 25 times. Which strong electrolyte ? Justify your answer. and B are diluted. The Am of ‘B’ increases lases 25 times. Which of the two is a otion Therefore, | 12 |

787 | Electrolysis is carried out in three cells: ( (A)-1.0 M C u S O_{4}, ) Pt electrodes; ( (B)-1.0 M C u S O_{4}, ) Copper electrodes; ( (C)-1.0 M K C I, ) Pt electrodes. If volume of electrolytic solution is maintained constant in each of the cells, which is correct set of ( mathrm{pH} ) changes in ( (A),(B) ) and ( (C) ) cells respectively: A. increase in all the three B. decrease in all the three c. increase, constant, increase D. decrease, constant, increase | 12 |

788 | Two faraday of electricity is passed through a solution of ( C u S O_{4} ). The mass of copper deposited at the cathode is : (at mass of ( boldsymbol{C u}=mathbf{6 3 . 5} boldsymbol{u} ) ). A. ( 127 g ) в. ( 0 g ) c. ( 63.5 g ) D. ( 2 g ) | 12 |

789 | The reaction which is taking place in nickel- cadmium battery can be represented by which of the following equation? A ( cdot C d+N i O_{2}+2 H_{2} O rightarrow C d(O H)_{2}+N i(O H)_{2} ) B. ( C d+N i O_{2}+2 O H^{-} rightarrow N i+C d(O H)_{2} ) c. ( N i+C d(O H)_{2} rightarrow C d+N i(O H)_{2} ) D. ( N i(O H)_{2}+C d(O H)_{2} rightarrow N i+C d+2 H_{2} O ) | 12 |

790 | Write cell reactions in lead storage battery during discharge. | 12 |

791 | A depolariser used in dry cell batteries is: A. ammonium chloride B. manganese dioxide c. potassuim hydroxide D. sodium phosphate | 12 |

792 | The reduction potential of hydrogen electrode when placed in a buffer solution is found to be -0.413 V. The pH of the buffer is: A . 10 B. 4 ( c cdot 7 ) D. 12 | 12 |

793 | In lead-acid battery electrolyte used is: A. sulphuric acid B. aqueous solution of ( P b S O_{4} ) c. nitric acid D. aqueous solution of ( mathrm{FeSO}_{4} ) | 12 |

794 | The potential of the following cell at ( 25^{circ} C ) is: ( boldsymbol{P t}left|begin{array}{c|c|c}boldsymbol{H}_{2} & boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} & boldsymbol{N a O H} & boldsymbol{H}_{2} \ (boldsymbol{1} boldsymbol{a} boldsymbol{t m}) & boldsymbol{0} . boldsymbol{1} boldsymbol{M} & mid & left(boldsymbol{1 0}^{-3} boldsymbol{M}right)end{array}right|(boldsymbol{1} boldsymbol{a} boldsymbol{t m}) ) A. ( -0.059 V ) B. ( 0.059 V ) ( c .-0.59 V ) D. ( 0.5 V ) | 12 |

795 | ( E^{o} ) values for the half cell reactions are given: ( boldsymbol{C u}^{2+}+boldsymbol{e}^{-} rightarrow boldsymbol{C u}^{+} ; boldsymbol{E}^{o}=mathbf{0 . 1 5 V} ) ( boldsymbol{C u}^{2+}+mathbf{2} e^{-} rightarrow boldsymbol{C u} ; boldsymbol{E}^{o}=mathbf{0 . 3 4} mathbf{v} ) What will be the ( E^{o} ) of the half-cell: ( boldsymbol{C u}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{C u} ? ) A . ( +0.49 v ) в. ( +0.19 v ) ( c .+0.53 v ) D. ( +0.30 v ) | 12 |

796 | Question 9. Why is alternating current used for measuring resistance of an electrolytic solution? | 12 |

797 | What transformation of energy takes place when current is drawn from a cell ? A. Chemical energy changes to electrical energy B. Chemical energy changes to heat energy c. mechanical energy changes to electrical energy D. Chemical energy changes to mechanical energy | 12 |

798 | KCI can be used in salt bridge as electrolyte in which of the following cells? ( mathbf{A} cdot Z nleft|Z n C l_{2} | A g N O_{3}right| A g ) B . ( P bleft|P bleft(N O_{3}right)_{2} | C uleft(N O_{3}right)_{2}right| C u ) c. ( C uleft|C u S O_{4} | A u C l_{3}right| A u ) D. ( F eleft|F e S O_{4} | P bleft(N O_{3}right)_{2}right| P b ) | 12 |

799 | During the purification of copper by electrolysis: This question has multiple correct options A. the anode used is made of copper ore B. pure copper is deposited on the cathode C. the impurities such as ( A g, A u ) present in solution as ions D. concentration of ( C u S O_{4} ) solution remains constant during dissolution of ( C u ) | 12 |

800 | ampere current is passed for 60 seconds into an electrolytic cell. Number of electrons that pass through the solution is : A. ( 6.0 times 10^{23} ) B. ( 1.2 times 10^{24} ) c. ( 37.5 times 10^{19} ) D. ( 7.48 times 10^{21} ) | 12 |

801 | Calculate the equilibrium constant for the reaction: ( mathbf{3} boldsymbol{S} boldsymbol{n}(boldsymbol{s})+boldsymbol{2} boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{2} boldsymbol{8} boldsymbol{H}^{+} rightarrow ) ( mathbf{3} boldsymbol{S} boldsymbol{n}^{+mathbf{4}}+mathbf{4} boldsymbol{C} boldsymbol{r}^{mathbf{3}+}+mathbf{1 4} boldsymbol{H}_{mathbf{2}} boldsymbol{O} ) ( E^{circ} ) for ( S n / S n^{2+}=0.136 V E^{circ} ) for ( boldsymbol{S} boldsymbol{n}^{2+} / boldsymbol{S} boldsymbol{n}^{4}=-mathbf{0 . 1 5 4} boldsymbol{V} ) ( E^{circ} ) for ( C r_{2} O_{7}^{2-} / C r^{3+}=1.33 V ), if the ans is ( K=10^{c}, ) what is c? A . 261 в. 273 ( c cdot 128 ) D. none of these | 12 |

802 | During electrolysis of a salt solution ( 0.05 mathrm{F} ) of electricity deposits ( 1.6 mathrm{g} ) of divalent metal. Theatomic wt. of the metal is : A . 32 B. 16 ( c cdot 64 ) D. 1.6 | 12 |

803 | Which of the following is not true about LED? A. There are two wires (called leads) attached to an LED. B. While connecting to a circuit, the longer lead of LED is always connected to the positive terminal of the battery. C. While connecting to a circuit, the shorter lead of LED is always connected to the positive terminal of the battery. D. LED can be used to detect weak current. | 12 |

804 | Question 20. Write the cell reaction for a lead storage battery when it is discharge. How does the density of the electrolyte change when the battery is discharged? | 12 |

805 | Calculate the current (in mA) required to deposit ( 0.195 g ) of platinum metal in 5.0 hours from a solution of ( left[boldsymbol{P t} C l_{6}right]^{2-} ) (Atomic weight: ( boldsymbol{C r}=mathbf{5 2 . 0} ) ) A . 310 B. 31 c. 21.44 D. 5.36 | 12 |

806 | Calculate the e.m.f. (in ( V ) ) of the cell: ( boldsymbol{P t}left|boldsymbol{H}_{2}(boldsymbol{g})right| boldsymbol{B O H}(boldsymbol{a q}) | boldsymbol{H} boldsymbol{A}(boldsymbol{a q})left|boldsymbol{H}_{2}(boldsymbol{g})right| boldsymbol{P} ) Given: ( boldsymbol{K}_{boldsymbol{a}}(boldsymbol{H} boldsymbol{A})=mathbf{1 0}^{-mathbf{7}}, boldsymbol{K}_{boldsymbol{b}}(boldsymbol{B O H})= ) ( 10^{-5} ) A . ( 0.43 mathrm{V} ) B . ( 0.36 V ) c. ( 0.93 V ) D. None of these | 12 |

807 | The units of conductivity of the solution are: ( mathbf{A} cdot o h m^{-1} ) B. ohms ( mathbf{c} cdot operatorname{ohm}^{-1} c m^{-1} ) D. ( o h m^{-1} e q^{-1} ) | 12 |

808 | A fuel cell is: I.A voltaic cell in which continuous supply of fuels are sent at anode to perform oxidation. II. A voltaic cell in which fuels such as: ( C H_{4}, H_{2} ) and ( mathrm{CO} ) are used up at anode. III. One which involves the reaction of ( H_{2} O_{2} ) fuel cell such as: Anode ( : 2 H_{2}+4 stackrel{ominus}{O} H rightarrow 4 H_{2} O(l)+4 e^{-} ) Cathode ( : O_{2}+2 H_{2} O(l)+4 e^{-} rightarrow 4 stackrel{ominus}{O} H ) IV. The efficiency of ( H_{2}-O_{2} ) fuel cell is 70 to ( 75 % ) A. ( I, I I I ) в. ( I, I I I, I V ) c. ( I, I I, I I I, I V ) D. ( I, I I, I I I ) | 12 |

809 | If for the half-cell reactions ( boldsymbol{C u}^{2+}+boldsymbol{e}^{-} longrightarrow boldsymbol{C u}^{+} boldsymbol{E}^{o}=mathbf{0 . 1 5} boldsymbol{V} ) ( boldsymbol{C u}^{2+}+boldsymbol{2} boldsymbol{e}^{-} longrightarrow boldsymbol{C u} quad boldsymbol{E}^{o}=mathbf{0 . 3 4} boldsymbol{V} ) Calculate ( E^{o} ) of the half cell reaction ( boldsymbol{C u}^{+}+boldsymbol{e}^{-} longrightarrow boldsymbol{C u} ) Also predict whether ( C u^{+} ) undergoes disproportionation or not | 12 |

810 | The maximum amount of electrical energy that can be obtained from one mole of ( N_{2} O_{3} ) is : ( mathbf{A} cdot-245.11 k J ) B. -125.10kJ c . ( -255.43 k J ) D. None of these | 12 |

811 | Which of the following methods is suitable for preventing an iron frying pan from rusting? A. Applying grease B. Applying paint C. Applying a coating of zinc D. All of the above | 12 |

812 | State True or False. Kohlrausch law is valid for weak electrolytes only. A. True B. False | 12 |

813 | The correct order of ( A_{e q}^{infty} ) at infinite dilution is: A . ( operatorname{LiC} mid> ) NaCI ( > ) KCI B. KCI> NaCI> LiCI C . NaCI> KCI > LiCI D. LiCI>KCI> Nacl | 12 |

814 | Assertion Lower parts of the ship or bridge is coated with tar. Reason It is to increase rusting. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

815 | Consider a fuel cell supplied with 1 mol of ( H_{2} ) gas and 10 moles of ( O_{2} ) gas. If fuel cell is operated at 96.3 m ( A ) current, how long will it deliver power? (Assume ( 1 F=96500 C / )mol of electrons) ( mathbf{A} cdot 1 times 10^{6} s ) B . ( 0.5 times 10^{6} s ) C ( .2 times 10^{6} s ) D. ( 4 times 10^{6} s ) E . ( 5 times 10^{6} ) | 12 |

816 | Write the equation occurring at anode in lead battery. | 12 |

817 | A certain current liberated 0.504 gm of hydrogen in 2 hrs. How many grams of copper can be liberated by the same current flowing for the same time in a copper sulphate solution? A. ( 12.7 mathrm{gms} ) B. 15.9 gms c. ( 31.8 mathrm{gms} ) D. ( 63.5 mathrm{gms} ) | 12 |

818 | Two platinum electrodes were immersed in a solution of ( C u S O_{4} ) and electric current was passed through the solution. After some time, it was found that colour of ( C u S O_{4} ) disappeared with evolution of gas at the electrode. The colorless solution contains: A ( . C u S O_{4} ) в. ( H_{2} S O_{4} ) ( c cdot operatorname{both} A & B ) D. None of the above | 12 |

819 | The value of E for elements are as follows: ( boldsymbol{F} boldsymbol{e}^{+mathbf{2}}+boldsymbol{2} boldsymbol{e} rightarrow boldsymbol{F} boldsymbol{e} ; boldsymbol{E}^{boldsymbol{o}}=mathbf{0 . 4 4} boldsymbol{V} ) ( boldsymbol{F} boldsymbol{e}^{+mathbf{3}}+mathbf{1} boldsymbol{e} rightarrow boldsymbol{F} boldsymbol{e}^{+mathbf{2}} ; boldsymbol{E}^{boldsymbol{o}}=+mathbf{0 . 7 7} boldsymbol{V} ) ( boldsymbol{S} boldsymbol{n}^{+mathbf{4}}+boldsymbol{2} boldsymbol{e} rightarrow boldsymbol{S} boldsymbol{n}^{+2} ; boldsymbol{E}^{boldsymbol{o}}=+mathbf{0 . 1 3} boldsymbol{V} ) ( boldsymbol{I}_{2}+boldsymbol{2} boldsymbol{e} rightarrow boldsymbol{2} boldsymbol{I} ; boldsymbol{E}^{o}=+mathbf{0 . 5 4} boldsymbol{V} ) ( boldsymbol{C r}^{3+}+boldsymbol{3} boldsymbol{e} rightarrow boldsymbol{C r} ; boldsymbol{E}^{o}=mathbf{0 . 7 4} boldsymbol{V} ) Based on the above data correct statements are: This question has multiple correct options | 12 |

820 | Question below refers to the overall reaction and half-reactions with standard reduction potentials below. ( 2 F e^{2+}+C l_{2} rightarrow 2 F e^{3+}+2 C l ? ) ( boldsymbol{F e}^{3+}+boldsymbol{e}^{-} rightarrow boldsymbol{F} e^{2+} ; boldsymbol{E}_{r e d}^{o}=0.77 ) volts ( C l_{2}+2 e^{-} rightarrow 2 C l^{-} ; E_{r e d}^{o}=1.36 ) volts Find the overall potential for the reaction? A. 0.18 volt B. 0.59 volts c. ( 1.05 v o l t s ) D. 2.13voolt E. 2.90volts | 12 |

821 | The half cell involving the reaction ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}(boldsymbol{a q})+mathbf{1 4 H}^{+}(boldsymbol{a q})+boldsymbol{6} e rightarrow ) ( 2 C r^{3+}(a q)+7 H_{2} O ) can be represented as: A ( cdot P t, H^{+}(a q), C r_{2} O_{7}^{2-}(a q) ) B . ( P t, H^{+}, C r^{3}+(a q) ) c. ( P t, H_{2}, C r_{2} O_{7}^{2-}(a q), C r^{3+}(a q) ) D. ( P t, H^{+}, C r_{2} O_{7}^{2-}(a q), C r^{3+}(a q) ) | 12 |

822 | Which of the following statement(s) is/are true for the process of anodizing? A. Anodizing is an electrochemical process B. It converts the metal surface into a decorative, durable, corrosion-resistant, anodic oxide finish. C. Aluminum is ideally suited to anodizing, although other nonferrous metals, such as magnesium and titanium, also can be anodized. D. All of the above | 12 |

823 | Current efficiency in electroplating is usually: A . 99% B. 90 to 98% c. 70 to ( 80 % ) D. 50 to 60% | 12 |

824 | Define the term: Corrosion | 12 |

825 | How much will the potential of ( Z n / Z n^{2+} ) change if the solution of ( Z n^{2+} ) is diluted 10 times? A. increase by ( 0.03 mathrm{V} ) B. decreases by ( 0.03 mathrm{V} ) c. increases by ( 0.059 mathrm{V} ) D. decreases by ( 0.059 mathrm{V} ) | 12 |

826 | Cell constant of a conductivity cell is generally obtained by measuring conductance of aqueous solution of A. ( B a C l_{2} ) в. LiCl c. ( K C l ) D. ( M g C l_{2} ) | 12 |

827 | Foe the electrochemical cell: [ begin{array}{c} boldsymbol{Z} boldsymbol{n}(boldsymbol{s}) mid boldsymbol{Z} boldsymbol{n}^{2+}(boldsymbol{a} boldsymbol{q}) | \ boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q})left|boldsymbol{C l}_{2}(boldsymbol{g})right| boldsymbol{P} boldsymbol{t}(boldsymbol{s}) \ text { Given }: boldsymbol{E}_{boldsymbol{Z n}^{2+} / Z boldsymbol{n}}^{o}=-mathbf{0 . 7 6} boldsymbol{V} boldsymbol{o l t} \ boldsymbol{E}_{boldsymbol{C l}^{prime} / boldsymbol{C l}_{2}(boldsymbol{g})}=-mathbf{1 . 3 6} boldsymbol{V} boldsymbol{o l t} boldsymbol{t} end{array} ] From these data one can deduce that: A ( cdot Z n+C l_{2} rightleftharpoons Z n^{2+}+2 C l^{-} ) is a non-spontaneous reaction at standard conditions B . ( Z n^{2+}+2 C l^{-} rightleftharpoons C l_{2}+Z n ) is a spontaneous reaction at standard conditions with ( E_{c e l l}^{o}=2.12 ) volt. C. ( Z n+C l_{2} longrightarrow Z n^{2+}+2 C l^{-} ) is a spontaneous reaction at standard conditions with ( E_{c e l l}^{o}=2.12 ) volt. D. ( Z n+C l_{2} longrightarrow Z n^{2+}+2 C l^{-} ) is a spontaneous reaction at standard conditions with ( E_{c e l l}^{o}=0.60 ) volt. | 12 |

828 | Select the wrong option about rancidity. A. Aerial oxidation of fats B. Aerial oxidation of oils C . Oils left in refrigerator gets rancid D. Chips exposed to air gets rancid | 12 |

829 | 10 g fairly concentrated solution of ( boldsymbol{C u} boldsymbol{S O}_{4} ) is electrolyzed using 0.01 ( mathrm{F} ) of electricity. Calculate: (a) The weight of resulting solution(g) (write the value to the nearest integer). | 12 |

830 | During galvanization of iron, which metal is used for coating iron surface? A. copper B. zinç c. Nickel D. Tin | 12 |

831 | The cell constant of a conductivity cell with electrodes of ( 0.5 mathrm{cm} times 0.5 mathrm{cm} ) with a separation of ( 0.5 mathrm{cm}, ) is: A. ( 0.5 mathrm{cm}^{-1} ) B. ( 2.0 mathrm{cm}^{-1} ) ( c .2 .0 mathrm{cm} ) D. ( 2.0 mathrm{cm}^{-2} ) | 12 |

832 | In Leclanche cell, Zinc rod is placed in: A ( cdot 10 % ) NH ( _{4} ) С। B. 20% NH_CI c. ( 30 % mathrm{NH}_{4} ) С। D . 40% NH ( _{4} ) C | 12 |

833 | The overall formation constant for the reaction of 6 mole of ( C N^{-} ) with cobalt (II) is ( 1 times 10^{19} . ) Given that ( boldsymbol{C o}(boldsymbol{C N})_{boldsymbol{6}}^{boldsymbol{3}-}+boldsymbol{e} rightarrow boldsymbol{C o}(boldsymbol{C N})_{boldsymbol{6}}^{boldsymbol{4}-} ; boldsymbol{E}_{boldsymbol{R} boldsymbol{P}}^{boldsymbol{o}}= ) ( -0.83 V ) ( boldsymbol{C o}^{3+}+boldsymbol{e} rightarrow boldsymbol{C o}^{2+} ; boldsymbol{E}_{R P}^{o}=mathbf{1 . 8 2} boldsymbol{V} ) If the formation constant for the reaction of 6 mole of ( C N^{-} ) with cobalt (III) is ( x times 10^{63} ) then ( 100 x ) is | 12 |

834 | If ( 9 g ) of ( H_{2} O ) is electrolyzed completely with ( 50 % ) current efficiency: A. ( 1 F ) of electricity will be needed B. ( 3 F ) of electricity is needed c. 5.6 L of ( O_{2} ) at ( S T P ) will be formed D. ( 11.2 L ) of ( O_{2} ) at ( S T P ) will be formed | 12 |

835 | As dilution of the solution increases then the conductivity of solution A. increases B. decreases c. remain unchanged D. none of the above | 12 |

836 | Iron articles rust readily whereas steel which is also mainly made of iron will not undergo corrosion. A. True B. False | 12 |

837 | Mark the correct statement: a) Damp air alone supplies both things needed for corrosion. b) Ordinary water supplies both air and water for corrosion. c) Moist air can’t provide both things. ( A cdot a, b ) в. а, ( c cdot b, c ) D. All of the above | 12 |

838 | When a lead storage battery is discharged, then: ( A cdot mathrm{SO}_{2} ) is evolved B. lead is formed c. lead sulphate is consumed D. sulphuric acid is consumed | 12 |

839 | A constant current of ( 30 A ) is passed through an aqueous solution of ( N a C l ) for a time of ( 1.00 h ). What is the volume of ( C l_{2} ) gas at STP produced? A . ( 30.00 L ) B . ( 25.08 L ) c. ( 12.54 L ) D. ( 1.12 L ) | 12 |

840 | Time required to produce 1 kg of ( C l_{2} ) in hrs is ( (40+x) . ) Find value of ( x ) (nearest integer value). | 12 |

841 | Q. 63 Assertion (A) Current stops flowing when Ecell = 0. Reason (R) Equilibrium of the cell reaction is attained. | 12 |

842 | Write three methods of preventing rusting of iron. | 12 |

843 | Given ( : boldsymbol{H}_{2} boldsymbol{O}_{2} rightarrow boldsymbol{O}_{2}+boldsymbol{2} boldsymbol{H}^{oplus}+boldsymbol{2} boldsymbol{e}^{-} ) ( boldsymbol{e}^{oplus}=-mathbf{0 . 6 9} boldsymbol{V} ) ( boldsymbol{H}_{2} boldsymbol{O}_{2}+boldsymbol{2} boldsymbol{H}^{oplus}+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O} ) ( boldsymbol{E}^{oplus}=mathbf{1} . mathbf{7 7} boldsymbol{V} ) ( mathbf{2} boldsymbol{I}^{ominus} rightarrow boldsymbol{I}_{mathbf{2}}+mathbf{2} boldsymbol{e}^{-} ) ( boldsymbol{E}^{ominus}=-mathbf{0 . 5 3 5} boldsymbol{V} ) Assertion: ( H_{2} O_{2} ) acts as an oxidizing agent for ( boldsymbol{I}^{ominus} ) Reason: ( boldsymbol{E}^{ominus} ) is positive. A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Assertion is false but Reason is true Both Assertion and Reason are false | 12 |

844 | stion 14. How much electricity is required in coulomb for the oxidation of (i) 1 mole of H2O to O2? (ii) 1 mole of FeO to Fe2O3? | 12 |

845 | In the above cell cathodic cell reaction and number of electrons involved are: A ( cdot 2 A g^{+}+2 e^{-} rightarrow 2 A g, 2 e^{-} ) B. ( A g^{+}+e^{-} rightarrow A g, 1 e^{-} ) ( mathbf{c} cdot 2 H^{+}+2 e^{-} rightarrow H_{2}, 2 e^{-} ) D. ( H^{+}+e^{-} rightarrow frac{1}{2} H_{2}, e^{-} ) | 12 |

846 | One ampere of current is passed for 9650 seconds through molten ( A l C l_{3} ) What is the weight in grams of ( boldsymbol{A l} ) deposited at cathode? (Atomic weight of ( A l=27 ) ) A . 0.9 в. 9. c. 0.09 D. 90.0 | 12 |

847 | Prevention of corrosion of iron by ( Z n ) coating is called: A . galvanization B. cathodic protection c. electrolysis D. photoelectolysis | 12 |

848 | State True or False. A cell works if its e.m.f. is negative. A. True B. False | 12 |

849 | Select incorrect statement A. If salt-bridge is removed, potential falls to zero B. Liquid-junction potential developed across the boundary of the two solutions of different concentration cells are used c. calomel electrode contains calcium chloride solution in contact with ( P t ) electrode D. Quinhydrone electrode is reversible to ( H^{+} ) | 12 |

850 | The number of coulombs necessary to deposit ( 1 ~ g ) of potassium metal (molar mass ( 39 g m o l^{-1} ) ) from ( K^{+} ) ions is: A ( cdot 96500^{circ} mathrm{C} ) B . ( 1.93 times 10^{50} C ) ( mathbf{c} cdot 1237^{circ} mathrm{C} ) D. 2474 ( ^{circ} mathrm{C} ) | 12 |

851 | Which of the following cells can be used to experimentally determine the reduction potential of Zinc? A ( cdot Z n(s)left|Z n^{2+}(a q)right|left|H^{+}(a q)right| H_{2}(g), P t ) B . ( P t, H_{2}(g)left|H^{+}(a q)right||Z n(s)| Z n^{2+}(a q) ) c. ( Z n(s)left|Z n^{2+}(a q)right|left|C u^{2+}(a q)right| C u(s) ) D. any one of these | 12 |

852 | The reaction ( frac{1}{2} times H_{2}(g)+A g C l(a q) rightarrow ) ( H^{+}(a q)+A g(s) ) can be represented in the galvanic cell as: ( mathbf{A} cdot operatorname{Ag} / mathrm{AgCl}(mathrm{s})left|mathrm{KCl}(mathrm{sol}) | mathrm{AgNO}_{3}(mathrm{sol})right| mathrm{Ag} ) B. PtH ( _{2} ) (g) I HCI(sol) II AgNO ( _{3} ) (sol) ( mid ) Ag C. ( P t, H_{2}(g) mid ) HCI ( (text { sol }) | ) AgCI ( (s) mid A g ) D. ( mathrm{H}_{2}(mathrm{g}) ) | HCI(sol) ( | ) AgCI(s) ( mid ) Ag | 12 |

853 | State Faraday’s first law of electrolysis. | 12 |

854 | A solution of sodium sulphate in water is electrolysed using inert electrodes. The products at the cathode and anode are respectively: A. ( H_{2}, O_{2} ) в. ( O_{2}, H_{2} ) c. ( O_{2}, N a ) D. none of the above | 12 |

855 | A voltaic cell converts: A. electrical energy into chemical energy B. chemical energy into electrical energy C. light energy into electrical energy D. mechanical energy into electrical energy | 12 |

856 | Which of the following is correct regarding mechanical passivity? A. Visible metal oxide film is formed B. Visible metal oxide film prevents dissociation of metal C. Fe, Mn and Pb exhibit mechanical passivity D. All the above | 12 |

857 | Assertion The ratio of speeds of cation and anions of an electrolyte under same potential gradient is ( 2: 3, ) the fall in concentration around anodic and cathodic solution will be in the ratio 1: 1 during the passage of current. Reason The number of ions discharged at either electrode during electrolysis in independent of their relative speed. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

858 | Write the chemistry of recharging lead storage battery highlighting all the materials that are evolved during recharging. | 12 |

859 | 018. How will you identify cathode and anode in electrochemical cell? | 12 |

860 | When galvanic cell is started, with passage of time: This question has multiple correct options A. spontaneity of the cell reaction decreases; ( E_{c e l l} ) decreases B. reaction quotient Q decreases; ( E_{text {cell}} ) increases C . reaction quotient ( mathrm{Q} ) increases; ( E_{c e l l} ) decreases D. at equilibrium ( Q=K_{c} ; E_{c e l l}=0 ) | 12 |

861 | Standard electrode potentials of ( boldsymbol{F} boldsymbol{e}^{2+}+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{F} boldsymbol{e} ) and ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{3} boldsymbol{e}^{-} rightarrow ) ( F e ) are ( -0.440 V ) and ( -0.036 V ) respectively. The standard electrode potential ( left(boldsymbol{E}^{o}right) ) for ( boldsymbol{F} boldsymbol{e}^{mathbf{3}+}+boldsymbol{e}^{-} rightarrow boldsymbol{F} boldsymbol{e}^{2+} ) is: ( mathbf{A} cdot-0.476 V ) В. ( -0.404 V ) c. ( +0.404 V ) D. ( +0.772 V ) | 12 |

862 | Assertion The ratio of specific conductivity to the observed conductance does not depend upon the concentration of the solution taken in the conductivity cell. Reason The specific conductivity decreases with dilution whereas observed conductance increases with the dilution. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

863 | Can you store copper sulphate solutions in a zinc pot? | 12 |

864 | Find out the EMF of the following cells at ( 25^{0} mathrm{C} ) ( p t, B r_{2(l)}left|B r^{-}(0.010 M)right|left|H^{+}(0.030 M)right| H_{2}(1 a ) ( $ $ 1 ) binom ( left{E{{0}}_{-}left{B r_{-}{2} / 2 B r^{wedge}{-}right}=+1.08right. ) ( left.V, R=8.314 J K^{wedge}left{-left.1 m oright|^{wedge}{-1}right},right} ) ( left{F=96,left.500 C m oright|^{wedge}{-1}right} $ ) A. ( 0.872 v ) ( v ) B . -0.872v c. -1.052v D. 1.288v | 12 |

865 | The conductivity of a saturated solution of ( B a S O_{4} ) is ( 3.06 times 10^{-6} ) ohm ( ^{-1} c m^{-1} ) and its molar conductance is ( 1.53 o h m^{-1} c m^{2} m o l^{-1} . ) The ( K_{s p} ) of ( B a S O_{4} ) will be: A ( cdot 4 times 10^{-12} ) В. ( 2.5 times 10^{-9} ) c. ( 2.5 times 10^{-13} ) D. ( 4 times 10^{-6} ) | 12 |

866 | R 1 Which cell will measure standard electrode potential of copper electrode (a) Pt (s) IH,(g, 0.1 bar) H(aq., 1 M) Cu2+ (aq, 1 M) Cu (b) Pt (5) Hy(s, 1 bar) H(aq, 1 M) Cu2+(aq, 2 M) Cu (c) Pt (s) | H (8,1 bar) H(aq, 1 M) Cu2+ (aq, 1 M) Cu (d) Pt (5)|H2/8, 0.1 bar) H*(aq,0.1 M | Cu2+ (aq, 1 M) Cu | 12 |

867 | Edible oils shows rancidity when stored for long period. A . True B. False | 12 |

868 | At ( 25^{circ} mathrm{C} ), the molar conductances at infinite dilution for the strong electrolytes ( N a O H, N a C l ) and ( B a C l_{2} ) ( operatorname{are} 248 times 10^{-4}, 126 times 10^{-4} ) and ( 280 times ) ( 10^{-4} S m^{2} m o l^{-1} ) respectively ( lambda_{m}^{circ} B a(O H)_{2} ) in ( S m^{2} m o l^{-1} ) is ( mathbf{A} cdot 52.4 times 10^{4} ) B ( .524 times 10^{4} ) c. ( 4.2 times 10^{4} ) D ( .262 times 10^{4} ) | 12 |

869 | Which of the following might be the reason that the current in the circuit is weak? A. Circuit of the tester might not be complete B. The material may not be able to conduct electricity as easily as metals. c. The circuit of the tester is complete but still the bulb does not glow. D. Both A and B | 12 |

870 | Rusting of iron is catalysed by which of the following: A . ( F e ) в. ( Z n ) ( c cdot 0_{2} ) ( mathbf{D} cdot H^{+} ) | 12 |

871 | The standard reducation potentials of ( Z n^{2+}left|Z n, C u^{2+}right| C u ) and ( A g^{+} mid A g ) are respectively -0.76,0.34 and ( 0.8 mathrm{V} ). The following cells were constructed. a) ( Z nleft|Z n^{2+}right|left|C u^{2+}right| C u ) b) ( Z nleft|Z n^{2+} | A g^{+}right| A g ) c) ( C uleft|C u^{2+}right|left|A g^{+}right| A g ) What is the correct order ( E_{text {cell }}^{0} ) of these cells? ( A cdot ) b>c ( >a ) B. b>a>c ( c cdot a>b>c ) D. c>asb | 12 |

872 | Assertion Polished iron nails do not rust when kept immersed in a test tube containing boil water covered with a layer of oil. Reason Rust formation can be controlled with coatings such as paint or varnish that isolate the iron from environment. When only temporary protection is needed for storage or transport a thin layer of oil, grease can be applied to an iron surface A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

873 | The emf of a cell corresponding to the reaction, ( Z n+2 H^{+}(a q .) rightarrow Z n^{2+}(0.1 M)+ ) ( H_{2}(g) 1 a t m ) is 0.28 volt at ( 25^{circ} mathrm{C} ). Write the half-cell reactions and calculate the ( p H ) of the solution at the hydrogen electrode. ( boldsymbol{E}_{boldsymbol{Z n}^{2+} / boldsymbol{Z n}}^{circ}=-mathbf{0 . 7 6} boldsymbol{v o l t} ) and ( boldsymbol{E}_{boldsymbol{H}^{+} / boldsymbol{H}_{2}}^{circ}=boldsymbol{0} ) | 12 |

874 | The emf of a galvanic cell, with electrode potentials of ( Z n=+0.76 V ) is: A ( .-1.1 V ) B. ( +1.1 V ) ( mathbf{c} .+0.34 V ) D. ( +0.76 V ) | 12 |

875 | The methods used in protecting the metals are: A. galvanizing B. alloying c. electroplating D. all of these | 12 |

876 | State True or False. Electrolysis of molten ( K C l ) gives ( mathrm{Cl}_{2} ) at cathode. A. True B. False | 12 |

877 | Assertion The Daniell cell becomes dead after some time. Reason Oxidation potential of zinc anode decreases and that of copper increases. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

878 | For the following half cell reactions, ( boldsymbol{E}^{boldsymbol{o}} ) values are also given: ( M n^{2+}+2 H_{2} O rightarrow M n O_{2}+4 H^{+}+ ) ( mathbf{2} e^{-} ; quad boldsymbol{E}^{o}=-mathbf{1 . 2 3} mathbf{V} ) ( M n O_{4}^{-}+4 H^{+}+3 e^{-} rightarrow M n O_{2}+ ) ( 2 H_{2} O ; quad E^{o}=+1.70 V ) Select the correct statements. A. ( M n^{2+} ) reacts with ( M n O_{4}^{-} ) in acid solution to form ( M n O_{2} ) в. ( M nleft(M n O_{4}right)_{2} ) is stable in acid solution c. ( M n O_{2} ) disproportionates to ( M n^{2+} ) and ( M n O_{4}^{-} ) in acid solution D. None of the above | 12 |

879 | Calculate the emf of the following concentration cell at ( 25^{circ} C ) ( boldsymbol{A} boldsymbol{g}(boldsymbol{s}) mid boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3}(mathbf{0} . boldsymbol{0} mathbf{1} boldsymbol{M}) ) ( boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3}(boldsymbol{0} . boldsymbol{0} boldsymbol{5} boldsymbol{M}) mid boldsymbol{A} boldsymbol{g}(boldsymbol{s}) ) A. ( -0.414 V ) в. ( 0.828 V ) c. ( 0.414 V ) D. ( 0.0414 V ) | 12 |

880 | Standard electrode potential of cell ( boldsymbol{H}_{2}left|boldsymbol{H}^{+} | boldsymbol{A} boldsymbol{g}^{+}right| boldsymbol{A} boldsymbol{g} ) is : A. ( 0.8 mathrm{v} ) в. ( -0.8 V ) c. ( -1.2 V ) D. ( 1.2 V ) | 12 |

881 | The number of Faradays required to produce 0.5 mol of free metal from ( mathbf{A} mathbf{l}^{mathbf{3}+} ) is ( A cdot 3 ) B. 2 ( c cdot 6 ) D. 1.5 | 12 |

882 | toppr Q Type your question conductivity of theses reactions is given in List II. Match List I with List II and select the correct using the code given below the lists: List-A ( (P) ) (1) Conductivity decreases and [ left(begin{array}{cc} left.C_{2} H_{5}right)_{3} N+ & text { then increases } \ X & end{array}right. ] [ C H_{2} C O O H ] (Q) (2) Conductivity decreases and [ begin{array}{c} K I(0.1 M)+ \ X end{array} ] [ begin{array}{c} A g N O_{3}(0.01 M) \ Y end{array} ] (R) (3) Conductivity increases and ( C H_{2} C O O+quad ) then does not change much ( K_{Y}^{O H} ) (4) Conductivity does not (S) ( N a O H+quad ) change much and then [ X ] ( H I ) ( Y )( quad ) increases A. 3,4,2,1 B. 4,3,2,1 C. 2,3,4,1 D. 1,4,3,2 | 12 |

883 | The equivalent conductances of two strong electrolytes at infinite dilution in ( H_{2} O ) (where ions move freely through a solution) at ( 25^{circ} mathrm{C} ) are given below [ boldsymbol{C H}_{3} boldsymbol{C O O N a}=91.0 boldsymbol{S c m}^{2} / boldsymbol{e q u i v} ] ( H C l=426.2 mathrm{Scm}^{2} / )equiv What additional information/quantity one needs to calculate the equivalent conductances an aqueous solution of acetic acid? A. The limiting equivalent conductance of Naç B. The limiting equivalent conductance of ( mathrm{CH}_{3} mathrm{COOH} ) C. The limiting equivalent conductance of ( mathrm{H}^{+} ) D. The limiting equivalent conductance of chloroacetic ( operatorname{acid}left(mathrm{ClCH}_{2} mathrm{COOH}right) ) | 12 |

884 | Which battery is used in aeroplanes? A. Dry cell battery. B. Lead acid battery. c. Edission cell. D. None of them. | 12 |

885 | Name the law or principle to which the following observations confirm: (1) When water is added to a ( 1.0 M ) aqueous solution of acetic acid, the number of hydrogen ion ( left(boldsymbol{H}^{+}right) ) increases. (2) When 9650 coulombs of electricity is passed through a solution of copper sulphate, ( 3.175 g ) of copper is deposited on the cathode (atomic weight of ( boldsymbol{C u}= ) 63.5) (3) When ammonium chloride is added to a solution of ammonium hydroxide, the concentration of hydroxyl ions decreases. | 12 |

886 | For hydrogen-oxygen fuel cell, the cell reaction is: ( mathbf{2} boldsymbol{H}_{mathbf{2}}(boldsymbol{g})+boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow mathbf{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ) If ( Delta G_{f}^{o}left(H_{2} Oright)=-237.2 k J m o l^{-1}, ) then emf of this cell is: A . ( +2.46 V ) в. ( -2.46 V ) c. ( +1.23 V ) D. ( -1.23 V ) | 12 |

887 | The unit of molar conductivity is A ( cdot operatorname{scm}^{2} s^{-1} ) B . ( mathrm{S} l^{2} mathrm{mol}^{-1} ) c. ( operatorname{scm}^{2} m o l^{-1} ) D. None of these | 12 |

888 | For the strong electrolytes NaOH, NaCl and ( B a C l_{2}, ) the molar ionic conductances at infinite dilution are ( 248 times 10^{-4}, 126.5 times 10^{-4} ) and ( 280.0 x ) ( 10^{-4} mathrm{s} m^{2} m o l^{-1}, ) respectively. Calculate ( wedge_{m}^{0} ) for ( B a(O H)_{2} ) | 12 |

889 | Which of the following solution of ( N a C l ) has the higher specific conductance? A. ( 1 N ) B. ( 0.01 N ) ( c cdot 0.1 N ) D. ( 0.001 N ) | 12 |

890 | For the cell ( Z n(s)left|Z n^{2+}right|left|C u^{2+}right| C u(s) ) the standard cell voltage, ( boldsymbol{E}_{c e l l}^{ominus} ) is ( 1.10 mathrm{V} ) When a cell using these reagents was prepared in the lab, the measured cell voltage was ( 0.98 mathrm{V} ). One possible explanation for the observed voltage is : A. There were 2.00 mol of ( Z n^{2+} ) but only 1.00 mol of ( C u^{2} ) B. The Zn electrode had twice the surface of the cu electrode C. The ( left[Z n^{2+}right] ) was larger than the ( left[C u^{2+}right] ) D. The volume of the ( left[Z n^{2+}right] ) solution was larger than the volume of the ( C u^{2+} ) solution | 12 |

891 | The concentration of ( Z n^{2+} ) in first compartment after passage of ( 0.1 F ) charge will be: A ( .1 ~ M ) В. 1.05 М c. 1.025 М D. ( 0.5 ~ M ) | 12 |

892 | The amount of charge which the battery must have been used is: A ( .9 .88 F ) в. ( 8.98 F ) c. ( 8.89 F ) D. ( 7.88 F ) | 12 |

893 | What are Galvanic cells? Explain the working of Galvanic cells with one example. | 12 |

894 | The half-cell reaction is the one that: A. takes place at one electrode B. consumes half a unit of electricity C. involves half a mole of electrolyte D. goes half way to completion | 12 |

895 | How many no. of metals among the following obtained from molten salt Electrolysis of their chlorides, oxides or hydroxides ( mathrm{Cu}, mathrm{Ag}, mathrm{Ba}, mathrm{Na}, mathrm{Zn}, mathrm{Fe}, mathrm{Cs} ) | 12 |

896 | Molten ( A l C l_{3} ) is electrolysed with the current of 0.5 empere to produced 27 g Al. Number of Farady used are: ( A cdot 3 ) B. 5 ( c .6 ) D. None of these | 12 |

897 | The voltage of the cell given below is ( -0.46 V ) ( boldsymbol{P t}left|begin{array}{cc}boldsymbol{N a H} boldsymbol{S O}_{3} & boldsymbol{N a}_{2} boldsymbol{S O}_{3} \ boldsymbol{0 . 4} boldsymbol{M} & boldsymbol{6 . 4 4} times mathbf{1 0}^{-3} boldsymbol{M}end{array}right|left|begin{array}{c}boldsymbol{Z} boldsymbol{n}^{2+} \ boldsymbol{0} . boldsymbol{3} boldsymbol{M}end{array}right| ) Also, ( Z n^{2+}+2 e rightarrow Z n(s) ; E^{o}= ) ( -0.763 V ) The value of ( boldsymbol{K}_{2} ) where ( boldsymbol{K}_{2}= ) ( frac{left[boldsymbol{H}^{+}right]left[boldsymbol{S O}_{3}^{2-}right]}{left[boldsymbol{H} boldsymbol{S O}_{3}^{-}right]} mathbf{i s} ) A . ( 6.44 times 10^{-8} ) B. ( 5.43 times 10^{-8} ) c. ( 7.34 times 10^{-8} ) D. None of these | 12 |

898 | What is corrosion? A. When metal is gradually destroyed through chemical reactions B. When metal is created through chemical reactions C. When a redox reaction takes place D. When a metal is destroyed after exposure to a gas E. When a solid is destroyed through chemical reactions | 12 |

899 | ( mathbf{1 0} C l^{-}(a q)+2 M n O_{4}^{-}(a q)+ ) ( mathbf{1 6} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow mathbf{5} boldsymbol{C l}_{2}(boldsymbol{g})+ ) ( 2 M n^{2+}(a q)+8 H_{2} O(l) ) The value of ( E^{o} ) for the above reaction at ( 25^{circ} mathrm{C} ) is ( 0.15 mathrm{V} ). Hence, the value of ( mathrm{K} ) for this reaction is : A . ( 2.4 times 10^{25} ) B . ( 4.9 times 10^{12} ) c. ( 1.2 times 10^{15} ) D. ( 3.4 times 10^{20} ) | 12 |

900 | List I A) Salt bridge Reduction B) Standard hydrogen electrode 2 ) Oxidation C) Cathode 3) Reference electrode D) Anode 4) ( mathrm{KCl}, mathrm{KNO}_{3} ) ( (text { or }) mathrm{NH}_{4} mathrm{NO}_{3} ) The correct match is : A. 3421 B. 4 312 c. 4321 D. 1234 | 12 |

901 | The measured resistance of a conductance cell was ( 100 Omega .left(M_{K C l}=right. ) ( 74.5 g m o l^{-1} ) and cell constant ( = ) ( 1.25 mathrm{cm}^{-1} ) ). If the specific conductance ( operatorname{in} operatorname{oh} m^{-1} c m^{-1} ) is ( 125 times 10^{-x}, ) then what is the value of ( x ? ) | 12 |

902 | toppr ( Q ) туре A large number of atoms/molecules (approximately ( 6.023 times 10^{23} ) ) are present in few grams of any chemical compound varying with their atomic/molecular masses. To handle such large numbers conveniently, the mole concept was introduced. This concept has implications in diverse areas such as analytical chemistry, biochemistry, electrochemistry, and radiochemistry. the following example illustrates a typical case, involving chemical/electrochemical reaction, which requires a clear understanding of the mole concept. A 4.0 molar aqueous solution of NaCl is prepared and ( 500 mathrm{mL} ) of this solution is electrolyzed. This leads to the evolution of chlorine gas at one of the electrodes (atomic mass: ( mathrm{Na}=23, mathrm{Hg}=200 ; 1 ) | 12 |

903 | Consider the statements ( $ 1 ) and ( s 2: ) S1: Conductivity always increases with decrease in the concentration of electrolyte. S2: Molar conductivity always increases with decrease in the concentration of electrolyte. The correct option among the following is: | 12 |

904 | The standard half cell reduction potential for ( A g^{+} mid A g ) is ( 0.7991 V ) at ( 25^{circ} mathrm{C} . ) Given that the experimental value of ( boldsymbol{K}_{s p}=mathbf{1 . 5 6} times mathbf{1 0}^{-mathbf{1 0}} ) for ( boldsymbol{A} boldsymbol{g} boldsymbol{C l} ) calculate the standard half cell reduction potential for the ( boldsymbol{A} boldsymbol{g} mid boldsymbol{A} boldsymbol{g} boldsymbol{C l} ) electrode. A ( .0 .2192 V ) В. ( -0.2192 mathrm{V} ) c. ( -1.2192 mathrm{V} ) D. ( 1.219 V ) | 12 |

905 | Negative terminal of a dry cell is formed by: A. zinc container B. carbon rodd c. graphite rod D. both A and B | 12 |

906 | When electrolysis of ( K C l ) is done in alkaline medium, 10 g of ( K C l O_{3} ) is produced as follows: ( boldsymbol{C l}^{ominus}+mathbf{6} stackrel{ominus}{boldsymbol{O}} boldsymbol{H} rightarrow boldsymbol{C l} boldsymbol{O}_{3}^{ominus}+mathbf{3} boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{6} boldsymbol{e}^{-} ) A current of 2 A is passed for 10.941 hours. The current efficiency (in %) used in the process is ( ( M w t o f K C l O_{3}= ) 122.5 | 12 |

907 | The cost of electricity required to deposit ( 1 g m ) of ( M g ) is ( R s .5 . . ) How much would it cost to deposit 10 gm. of ( A l ?(A t w t . A l=27, M g=24) ) A. ( R s .10 .00 ) B. Rs. 27.00 c. ( R s .44 .44 ) D. Rs. 66.67 | 12 |

908 | A solution is one molar in each of ( N a C l, C d C l_{2}, Z n C l_{2} ) and ( P b C l_{2} . ) To this, tin metal is added. Which of the following is true? Given: ( boldsymbol{E}_{boldsymbol{P b}^{2+} / boldsymbol{P b}}^{circ}=-mathbf{0 . 1 2 6} boldsymbol{V}, boldsymbol{E}_{boldsymbol{S n}^{2+} / boldsymbol{S} n}^{circ}= ) ( -mathbf{0 . 1 3 6} boldsymbol{V} ) ( boldsymbol{E}_{boldsymbol{C d}^{2+} / boldsymbol{C d}}^{circ}=-mathbf{0 . 4 0} boldsymbol{V}, boldsymbol{E}_{Z n^{2+} / Z n}^{circ}= ) ( -mathbf{0 . 7 6 3} boldsymbol{V}, boldsymbol{E}_{N a^{+} / N a}^{circ}=-mathbf{2 . 7 1} boldsymbol{V} ) A. ( S n ) can reduce ( N a^{+} ) to ( N a ) B. ( S n ) can reduce ( Z n^{2+} ) to ( Z n ) ( mathrm{c} cdot operatorname{Sn} ) can reduce ( C d^{2+} ) to ( C d ) D. ( S n ) can reduce ( P b^{2+} ) to ( P b ) | 12 |

909 | of Q. 18 The positive value of the standard electrode potential Cu2+ / Cu indicates that……….. (a) this redox couple is a stronger reducing agent than the H /H, couple (b) this redox couple is a stronger oxidising agent than H+ /H, (c) Cu can displace H, from acid (d) Cu cannot displace H, from acid | 12 |

910 | Fill in the blanks by choosing the appropriate word/words from those given in the brackets: (increases, decreases, positive, efficient, ( 68, ) non-efficient, no ( alpha ) hydrogen, ( alpha ) -hydrogen, negative, Rosenmund’s, greater, Cannizzaro, 74 common-ion effect, lesser, buffer action, diamagnetic, paramagnetic) The more is standard reduction potential of a metal, the is its ability to displace hydrogen from acids. | 12 |

911 | How much silver will be obtained by that quantity of current which displaces 5.6 litre of ( boldsymbol{H}_{2} ) ? A . ( 54 g ) в. ( 13.5 g ) c. ( 20 g ) D. ( 108 g ) | 12 |

912 | Which of the following does not produce ( mathrm{H}_{2} ) at the anode on electrolysing using Pt electrode? This question has multiple correct options A . molten CaH ( _{2} ) B. ( N a C l(a q) ) ( c cdot operatorname{cus} 0_{4}(a q) ) D. ( operatorname{dil} mathrm{H}_{2} mathrm{SO}_{4} ) | 12 |

913 | What should be the state of compounds which decompose on passing electric current? A. Plasma B. Solid c. Gas D. Molten or aqueous | 12 |

914 | One gram atomic weight of metal of the following can be deposited by one Faraday: ( mathbf{A} cdot ) AuCl ( _{3} ) B. Bacla c. Nacı D. cuso | 12 |

915 | At ( 298 mathrm{K} ), the standard reduce potentials are ( 1.51 mathrm{V} ) for ( mathrm{MnO}_{4}^{-}, 1.36 mathrm{V} ) for ( boldsymbol{C l} boldsymbol{l}_{2} mid boldsymbol{C l}^{-}, 1.07 mathrm{V} ) for ( boldsymbol{B} boldsymbol{r}_{2} mid boldsymbol{B r}^{-}, 0.54 mathrm{V} ) for ( I_{2} mid I^{-} . ) At ( p H=3, ) permangnate is expected to oxidize: ( left(frac{R T}{F}=0.059right) ) A ( . C l^{-} ) and ( B r^{-} ) B. ( B r^{-} ) and ( I^{-} ) c. ( I^{-} ) only D. ( C l^{-}, B r^{-} ) and ( I^{-} ) | 12 |

916 | The number of coulombs required to deposit ( 5.4 g ) of Aluminium when the given electrode reaction is represented as ( A l^{3+}+3 e^{-} rightarrow A l ) A ( cdot 1.83 times 10^{5} C ) в. ( 57900 C ) ( mathbf{c} cdot 5.86 times 10^{5} C ) D. ( 3 F ) | 12 |

917 | List ( A ) List ( mathrm{B} ) A. Dry Cell (P) Primary cell B. Lead storage battery (Q) ( 38 % H_{2} S O_{4} ) C. Ni-Cd cell ( (mathrm{R}) M n O_{2}+C ) D. ( H_{2}-O_{2} ) fuel cell (S) Secondary cell A ( cdot ) A-P,R: B-Q,S:C-S:D-S B. A-Q,R: B-P,S:C.C-P:D-Q c. A-P, B-S:C-P,S :D-Q,R D. A-R: B-Q:C-Q,S:D-P | 12 |

918 | Assertion: At infinite dilution, both strong and weak electrolyte have degree of ionization equal to unity. Reason: At infinite dilution of an electrolyte, the equivalent conductance of cations and anions are independent of each other. A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

919 | When hydrogen sulphide gas is passed through a blue solution of copper sulphate, a black precipitate of copper sulphide is obtained and the sulphuric acid so formed remains in the solution. The reaction is an example of: A. a combination reaction B. a displacement reaction c. a decomposition reaction D. a double displacement reaction | 12 |

920 | The potential of a single electrode depends upon: A. the nature of the electrode B. Temperature C. concentration of the ion with respect to which it is reversible D. all the above | 12 |

921 | Number of faradays’ required to generate one gram atom of magnesium from molten ( M g C l_{2} ) is A . 1 B . 2 ( c .3 ) D. | 12 |

922 | Which one of the following cells can convert chemical energy of ( O_{2} ) and ( H_{2} ) directly into electrical energy: A. mercury cell B. danicell cell c. fuel cell D. lead storage cell | 12 |

923 | In which reactants are not contained within the cell but are continuously supplied from external source? A. Fuel cell B. Dry cell c. Lithium battery D. Lead storage battery | 12 |

924 | The EMF of the cell; ( mathbf{M g}left|mathbf{M g}^{2+}(mathbf{0 . 0 1} mathbf{M}) | mathbf{S n}^{2+}(mathbf{0 . 1} mathbf{M})right| mathbf{S} mathbf{n} ) is: ( left(text { Given: } mathbf{E}_{mathbf{M g}^{2+}, mathbf{M g}}^{circ}=-mathbf{2 . 3 4} mathbf{V}, mathbf{E}_{mathbf{S n}^{2+}, mathbf{S n}}^{circ}=right. ) ( -0.14 V) ) ( mathbf{A} cdot 2 cdot 17 V ) в. ( 2.23 mathrm{V} ) c. ( 2.51 V ) D. ( 2.45 V ) | 12 |

925 | For the half cell ( E^{o}=1.30 V . ) At ( p H=3 ) electrode potential is: A . ( 1.30 V ) B. ( 1.20 V ) c. ( 1.10 V ) D . ( 1.48 V ) | 12 |

926 | A current of 3 A has to be passed through a solution of silver nitrate for ( t^{prime} ) sec to coat a metal surface of ( 80 mathrm{cm}^{2} ) with a 0.005 -mm-thick layer, then ( t ) is: (density of silver is 10.5 g ( c m^{-3} ) ) (write your answer to nearest integer) | 12 |

927 | In hydrogen-oxygen fuel cell the carbon rods are immersed in hot aqueous solution of. A . ( K C l ) в. КОН c. ( H_{2} S O_{4} ) D. ( N H_{4} C l ) | 12 |

928 | refers to amount of electricity while ( quad ) refers to rate at which it flows. A. Ampere, coloumb B. Coloumb, ampere c. Faraday, coloumb D. Coloumb, faraday | 12 |

929 | Give the equation for the discharge of ion at the cathode during the electrolysis of acidified water? | 12 |

930 | The value of ( wedge_{m}^{infty} ) for ( K C l ) and ( K N O_{3} ) are 149.86 and ( 154.96 Omega^{-1} c m^{2} m o l^{-1} ) respectively. Also ( lambda_{C l^{-}}^{infty} ) is 71.44 ohm ( ^{-1} mathrm{cm}^{2} ) mol ( ^{-1} ). The value of ( lambda_{N O_{3}^{-}}^{infty} ) is : A ( cdot 76.54 ) ohm ( ^{-1} mathrm{cm}^{2} ) mol ( ^{-1} ) в. 133.08 ohm ( ^{-1} mathrm{cm}^{2} mathrm{mol}^{-1} ) c. 37.7 ohm ( ^{-1} mathrm{cm}^{2} ) mol ( ^{-1} ) D. none of the above | 12 |

931 | The cost at 5 paise / KWH of operating an electri motor for 8 hours which takes 15 ampere at ( 110 mathrm{V} ) is: A. Rs.66 B. 66 paise c. 37 paise D. Rs.6.60 | 12 |

932 | Refining and extraction of metals from impure samples is called: A. electroplating B. cathodization c. electrorefining D. anionization | 12 |

933 | Total world production of iron destroyed by rusting is about: A . ( 10 % ) B. 50 % c. ( 15 % ) D. 40 % | 12 |

934 | Assertion Inert electrolytes like KCI ( , K N O_{3} ) are used in salt bridge. Reason Salt bridge provides an electric contact between the two solutions without allowing them to mix with each other A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

935 | Standard E.M.F. experienced by the person with dental filling is: A . ( +3.89 V ) B . ( 2.89 V ) c. ( 0.93 V ) D. ( +0.43 V ) | 12 |

936 | Q11. What is a standard hydrogen electrode? Clabu | 12 |

937 | On passing a current through a molten aluminium chloride for some time produced 11.28 lit of ( C l_{2} ) at ( mathrm{NTP} ) at anode. The quantity of aluminium deposited at cathode is: A. 27grams B. 18gram c. ( operatorname{ggram} ) D. 36 gram | 12 |

938 | For the redox reaction ( Z n(S)+C u^{2+}(0.1 M) rightarrow ) ( Z n^{2+}(1 M)+C u(s) ) taking place in a cell, ( E_{c e l l}^{0} ) is 1.10 volt. ( E_{text {cell}} ) for the cell will be: ( left(2.303 frac{R T}{F}=0.0591right) ) ( mathbf{A} cdot 2 cdot 14 V ) B. ( 1.80 V ) c. ( 1.07 V ) D. ( 0.82 V ) | 12 |

939 | Q12. What is meant by cell potential? T . 1 | 12 |

940 | What is meant by galvanizing? | 12 |

941 | The molar conductivities of ( K C l, N a C l ) and ( K N O_{3} ) are 152,128 and ( 111 S c m^{2} m o l^{-1} ) respectively. What is the molar conductivity of ( N a N O_{3} ? ) ( mathbf{A} cdot 101 S mathrm{cm}^{2} mathrm{mol}^{-1} ) B. ( 87 S mathrm{cm}^{2} mathrm{mol}^{-1} ) c. ( -101 S mathrm{cm}^{2} mathrm{mol}^{-1} ) D. ( -391 S mathrm{cm}^{2} mathrm{mol}^{-} ) | 12 |

942 | When iron is rusted, it is : A. reduced B. oxidised c. evaporated D. decomposed | 12 |

943 | A reaction: ( frac{1}{2} H_{2}(g)+A g C l(s) rightleftharpoons H^{oplus}(a q)+ ) ( C l^{ominus}(a q)+A g(s) ) occurs in a galvanic cell. The structure of the cell will be: A ( cdot A g, A g C l(s)|K C l(s o l)| A g N O_{3}(s o l), A g ) B . ( P t, H_{2}(g)|H C l(s o l)| A g N O_{3}(s o l), A g ) c. ( P t, H_{2}(g)|H C l(s o l)| A g C l(s), A g ) D. ( P t, H_{2}(g)|K C l(s o l)| A g C l(s), A g ) | 12 |

944 | How much time will it take for a uniform current of ( 6.00 mathrm{A} ) to deposit ( 78 mathrm{g} ) of gold from a solution of ( A u C l_{4}^{-} ? ) What mass of chlorine gas will be formed simultaneously at the anode of the cell? (Atomic mass of ( A u=197 ) ) A ( cdot t=3010 sec , w=35.50 g ) B. ( t=20306 sec , w=45.54 g ) c. ( t=19500 ) sec ( , w=54.5 g ) D. ( t=19139.16 sec , w=42.24 g ) | 12 |

945 | In the electroysis of ( A g N O_{3} ) solution, ( 0.7 mathrm{g} ) of ( mathrm{Ag} ) is deposited after a certain period of time. Calculate the quantity of electricity required in coulomb. (Molar mass of ( A g ) is ( 107.9 g ) mol ( ^{-1} ) ). | 12 |

946 | State the first and second law of electrolysis. | 12 |

947 | Ans.( • 24 What will happen during the electrolysis of aqueous solution or cu the electrolysis of aqueous solution of CuSO4 in the presence of Cu electrodes? (a) Copper will deposit at cathode (b) Copper will dissolve at anode (C) Oxygen will be released at anode (d) Copper will deposit at anode | 12 |

948 | What make(s) water conducting? A. Salts B. Hydrogen c. oxygen D. None of the above | 12 |

949 | An aqueous solution of NaCl on electrolysis gives ( boldsymbol{H}_{2(g)^{prime}}, boldsymbol{C l}_{2(g)} ) and NaOH according to the reaction ( mathbf{2} C l_{(a q)}^{-}+mathbf{2} boldsymbol{H}_{2} boldsymbol{O} rightleftharpoons mathbf{2} boldsymbol{O} boldsymbol{H}_{(a q)}^{-}+boldsymbol{H}_{2(g)}+ ) ( C l_{2(g)} ) A direct current of 25 amperes with a current efficiency of ( 62 % ) is passed through 20 liters of NaCl solution (20% by weight). Write down the reactions taking place at the anode and the cathode. How long will it take to produce ( 1 mathrm{kg} ) of ( C l_{2} ? ) in hrs. (write the value to the nearest integer). | 12 |

950 | The anodic half-cell of lead-acid battery is recharged unsing electricity of 0.05 Faraday. The amount of ( P b S O_{4} ) electrolyzed in g during the process is : (Molar mass of ( boldsymbol{P b S O}_{4}=mathbf{3 0 3 g m o l}^{-1} ) ) A . 22.8 B. 15.2 ( c .7 .6 ) D. 11.4 | 12 |

951 | Calculate the cell potential ( left(E_{c e l l}right) ) of the following cell at ( 298 K ) ( boldsymbol{A} boldsymbol{g}(boldsymbol{s}) mid boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3}(boldsymbol{0} . boldsymbol{0} mathbf{1} boldsymbol{M}) | boldsymbol{A} boldsymbol{g} boldsymbol{N} boldsymbol{O}_{3}(mathbf{1} . boldsymbol{0} boldsymbol{M} ) | 12 |

952 | Which of the following is the cell reaction that occurs when the following half-cells are combined? ( boldsymbol{I}_{2}+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{2} boldsymbol{I}^{-}(boldsymbol{1} boldsymbol{M}) ; boldsymbol{E}^{o}=+boldsymbol{0 . 5 4} mathbf{V} ) ( boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{2} boldsymbol{B} boldsymbol{r}^{-}(boldsymbol{1} boldsymbol{M}) ; boldsymbol{E}^{o}=+mathbf{1} . boldsymbol{0} boldsymbol{9} ) ( mathbf{V} ) A ( cdot 2 B r^{-}+I_{2} rightarrow B r_{2}+2 I^{-} ) В ( cdot I_{2}+B r_{2} rightarrow 2 I^{-}+2 B r^{-} ) c. ( 2 I^{-}+B r_{2} rightarrow I_{2}+2 B r ) D. ( 2 I^{-}+2 B r^{-} rightarrow I_{2} B r_{2} ) | 12 |

953 | Calculate the standard EMF of the following cell ( boldsymbol{C} boldsymbol{d}left|boldsymbol{C} boldsymbol{d}^{2+} | boldsymbol{A} boldsymbol{g}^{+}right| boldsymbol{A} boldsymbol{g} ) Given that ( boldsymbol{E}_{boldsymbol{C d}^{2+} mid boldsymbol{C d}}^{boldsymbol{o}}= ) ( -mathbf{0 . 4 0} V, E_{A g^{o} mid A g}^{o}=mathbf{0 . 8 V} ) | 12 |

954 | 0.22 AH,0 is equal to……. (a) Amen + AINAOH – ANSCH (b) AmHNO + AMIN.NO – ANO (c) AmiHNO, + AINOH – AmiNaNO (d) AMINHOH) + Am(HCI- AmiNH.CH Thinking Process This problem includes concept of Kohlrausch law and its application in determination of molar conductivity of species. This problem can be solved by following three steps. O Write the molar conductance of each species in terms of sum of their constituent ions. (ii) Now operate the equation of each option given above by using information provided in the question (iii) At last if the sum of molar conductivity remaining constituent ions is equal to the molar conductivity of species asked (here Amin.) then that will be the correct choice. | 12 |

955 | topp ( E ) Q туре your question ( C u(s) ) ( boldsymbol{E}_{text {cll }}^{o}=mathbf{1 . 1 0} boldsymbol{V} ) ( boldsymbol{X}-boldsymbol{a} boldsymbol{x} boldsymbol{i} boldsymbol{s}: log _{10} frac{left[boldsymbol{Z} boldsymbol{n}^{2+}right]}{left[boldsymbol{C u}^{2+}right]}, quad Y- ) axis ( : boldsymbol{E}_{c e l l} ) ( A ) B. ( c ) ( D ) | 12 |

956 | Which of the following is/are true regarding rancidity? This question has multiple correct options | 12 |

957 | ( mathrm{Zn}(s)left|mathrm{ZnCl}_{2}(mathrm{aq})right| mathrm{Cl}^{-}(mathrm{aq})left|mathrm{Cl}_{2}(g)right| mathrm{C}(s) ) According to the above cell diagram the electrochemical cell described, the reaction at anode is : A ( cdot z n rightarrow z n^{2+}+2 e^{-} ) B. ( z n^{2+}+2 e^{-} rightarrow ) Zn c. ( mathrm{cl}_{2}+2 mathrm{e}^{-} rightarrow 2 mathrm{Cl}^{-} ) D . 2CI- ( rightarrow mathrm{Cl}_{2}+2 mathrm{e}^{-} ) E. ( z n+C l_{2} rightarrow Z n C l_{2} ) | 12 |

958 | Maintenance-free batteries, now in use, in place of common batteries, have : A. Electrodes made of lead-lead oxide B. Electrodes made of calcium-containing lead alloy C. Non-aqueous solvents as medium D. Platinum electrodes | 12 |

959 | The standard reduction potential of ( E_{B i^{3+} / B i}^{o} ) and ( E_{C u^{2+} / C u}^{o} ) are ( 0.226 mathrm{V} ) and ( 0.344 mathrm{V} ) respectively. A mixture of salts of Bi and Cu at unit concentration each is electrolysed at ( 25^{circ} mathrm{C} ). To what value ( operatorname{can}left[C u^{2+}right] ) be brought down before bismuth starts to deposit during electrolysis? В. ( 10^{-3} M ) c. ( 10^{-5} M ) D. ( 10^{-2} M ) E ( cdot 10^{-6} M ) F. ( 10^{-1} M ) G. ( 10^{-7} M ) | 12 |

960 | In the process of electroplating, ( boldsymbol{m} boldsymbol{g} ) of silver is deposited when 4 ampere of current flows for 2 minutes. The amount (in ( g ) ) of silver deposited by 6 ampere of current flowing for 40 seconds will be: A. ( 4 m ) в. ( frac{m}{2} ) c. ( frac{4 m}{3} ) D. ( 3 m ) | 12 |

961 | Cell equation ( : boldsymbol{A}+mathbf{2} boldsymbol{B}^{+} rightarrow boldsymbol{A}^{2+}+mathbf{2} boldsymbol{B} ) ( boldsymbol{A}^{2+}+boldsymbol{2} boldsymbol{e} rightarrow boldsymbol{A} boldsymbol{E}^{circ}=+mathbf{0 . 3 4} boldsymbol{V} ) and ( log _{10} K=15.6 ) at ( 300 K ) for cell reactions Find ( boldsymbol{E}^{circ} ) for ( boldsymbol{B}^{+}+boldsymbol{e} rightarrow boldsymbol{B} ) Given ( left[frac{2.303 R T}{n F}=0.059right]_{a t 300 K} ) A . 0.80 B. 1.26 c. -0.54 D. +0.94 | 12 |

962 | Assume that impure copper contains only ( F e, A u ) and ( A g ) as impurities. After passage of 140 ampere for 482.5 sec the mass of anode decreased by 22.260 ( g ) and the cathode increased in mass by 22.011 g. Calculate the percentage of iron and percentage of copper originally present A. ( F e=3 % C u=93 % ) в. ( F e=2.5 % C u=89 % ) c. ( F e=3.5 % C u=93 % ) D. None of these | 12 |

963 | How many Faradays of electricity are required to deposit 10 g of calcium from molten calcium chloride using inert electrodes? (molar mass of calcium = ( left.40 text { g } m o l^{-1}right) ) A . ( 0.5 mathrm{F} ) B. 1 c. ( 0.25 mathrm{F} ) D. 2 | 12 |

964 | The cell ( boldsymbol{P t}left(boldsymbol{H}_{2}right)(boldsymbol{1} boldsymbol{a} boldsymbol{t m}) mid boldsymbol{H}^{+}(boldsymbol{p} boldsymbol{H}=?), boldsymbol{I}^{-}(boldsymbol{a}= ) 0. The electrode potential for the reaction ( boldsymbol{A} boldsymbol{g} boldsymbol{l}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g}+boldsymbol{I}^{ominus} boldsymbol{i} boldsymbol{s}- ) 0.151 volt. Calculate the ( p H ) value :- A . 3.37 B. 5.26 ( c .2 .56 ) D. 4.62 | 12 |

965 | In a galvanic cell electron flow will be from: A. negative electrode to positive electrode B. positive electrode to negative electrode C. there will be no flow of electrons D. cathode to anode in the extenal circuit | 12 |

966 | A constant current(0.5 amp) is passed for 1 hour through (i) aqueous ( A g N O_{3} ) (ii) aqueous ( C u S O_{4} ) and (iii) molten ( A l F_{3}, ) separately. The ratio of the mass of the metals deposited on the cathode is? ( left[M_{A g}, M_{C u}, M_{A l} ) are molar masses right. of the respective metals]. A ( cdot M_{A g}: 2 M_{C u}: 3 M_{A l} ) B. ( M_{A g}: M_{C u}: M_{A l} ) ( mathbf{c} cdot 6 M_{A g}: 3 M_{C u}: 2 M_{A l} ) D. ( 3 M_{A g}: 2 M_{C u}: M_{A} ) | 12 |

967 | During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 to 1.139 g ( m l^{-1} ) and sulphuric acid of the density of ( 1.294 mathrm{g} ) ( m l^{-1} ) is ( 39 % ) by mass and that of the density of 1.139 g ( m l^{-1} ) is ( 20 % ) by mass. The battery holds 3.5 litre of acid and the volume practically remained constant during the discharge. Calculate the no. of ampere hour for which the battery must have been used. The charging and discharging reactions are: ( boldsymbol{P b}+boldsymbol{S O}_{4}^{2-} rightarrow boldsymbol{P b S O}_{4}+boldsymbol{2 e} Longrightarrow ) charging ( boldsymbol{P b O}_{2}+boldsymbol{4} boldsymbol{H}^{+}+boldsymbol{S O}_{4}^{2-}+boldsymbol{2} e rightarrow ) ( P b S O_{4}+2 H_{2} O Longrightarrow ) discharging A . ( 2.5 A ) в. ( 1.7 A ) ( c .3 .2 A ) D. None of these | 12 |

968 | Faraday can be defined as: A. the magnitude of the charge of 1 mole of electrons B. the magnitude of the electric dipole C. a fundamental constant of nature equal to ( 6.63 times ) ( 10^{-34} J s / )photon D. a constant that accounts for the existence of ions in solution E. the assignment of charges to individual atoms | 12 |

969 | The standard electrode potential of Zinc is ( 0.76, ) V. The potential of ( 0.1 mathrm{M} ) zinc electrode is: ( mathbf{A} cdot 0.8196 mathbf{V} ) B. 0.7895 V c. ( 0.9484 mathrm{V} ) D. ( 0.7508 mathrm{V} ) | 12 |

970 | The standard potential of the following cell is ( 0.23 V ) at ( 15^{circ} C ) and ( 0.21 V ) at ( 25^{circ} C ) ( boldsymbol{P t H}_{2}(boldsymbol{g})|boldsymbol{H} boldsymbol{C l}(boldsymbol{a q} .) | boldsymbol{A} boldsymbol{g} C l(s)| boldsymbol{A} boldsymbol{g}(s) ) (i) Write cell reaction. (ii) Calculate ( triangle H^{circ} ) and ( triangle S^{circ} ) for the cell reaction by assuming that these quantities remain unchanged in the range ( 15^{circ} mathrm{C} ) to ( 35^{circ} mathrm{C} ) (iii) Calculate the solubility of ( A g C l ) in water at ( 25^{circ} C . ) Given the standard reduction potential of the ( boldsymbol{A} boldsymbol{g}^{+} / boldsymbol{A} boldsymbol{g} ) couple is 0.80 volt at ( 25^{circ} mathrm{C} ) | 12 |

971 | Which one is wrong if electrolysis of ( C H_{3} C O O N a(a q) ) is made using ( P t ) electrodes? A. ( p H ) of solution increases B. Molar ratio of gases at anode and cathode is 3: 1 ( mathrm{c} cdotleft[C H_{3} C O O^{ominus}right] ) in solution decreases D. The molar ration of gases at anode and cathode is 2 : 1 | 12 |

972 | The e.m.f of the cell obtained by combining Zn and Cu electrode of a Daniel cell with ( mathrm{N} ) calomel electrode in two different arrangements are ( 1.083 mathrm{V} ) and ( 0.018 mathrm{V} ) respectively at ( 25^{circ} mathrm{C} ). If the standard reduction potential of ( mathrm{N} ) calomel electrode is ( 0.28 mathrm{V} ) the emf (V) of Daniel cell is (write the value to the nearest integer) | 12 |

973 | During the electrolysis of a concentrated brine solution. Calculate the moles of chlorine gas produced by the passage of ( 4 F ) electricity. | 12 |

974 | In electro-chemical corrosion of metals, the metal undergoing corrosion: A. Becomes anode B. Becomes cathode c. Becomes inert D. None is correct | 12 |

975 | A current of 9.65 amp flowing for 10 minute deposits ( 3.0 g ) of a metal. The equivalent wt. of the metal is: A . 10 B. 30 c. 50 D. 96.5 | 12 |

976 | ( ln ) a ( H_{2}-O_{2} ) fuel cell. ( 6.72 L ) of hydrogen at NTP reacts in 15 minutes, the average current produced in amperes is: A. 64.3 amp B. 643.3 amp c. 6.43 amp D. 0.643 amp | 12 |

977 | Given the limiting molar conductivity as: ( A_{m}^{infty}(H C l)=126.4 Omega^{-1} c m^{2} m o l^{-1} ) ( A_{m}^{infty}(N a C l)=425.9 Omega^{-1} c m^{2} m o l^{-1} ) ( A_{m}^{infty}left(C H_{3} C O O N aright)= ) ( 91 Omega^{-1} c m^{2} m o l^{-1} ) The molar conductivity at infinite dilution of acetic acid ( left(i n Omega^{-1} c m^{2} m o l^{-1}right) ) will be: ( mathbf{A} cdot 481.5 ) B. 390.5 ( mathbf{c} cdot 299.5 ) D . 516.9 | 12 |

978 | State True or False. In an electrochemical cell, in the inner circuit current is carried by ions and in the external circuit, current of electrons flows through the metal conductors. A. True B. False | 12 |

979 | Which of the following takes place in discharge process at anode? ( mathbf{A} cdot P b O_{2}+4 H^{+}+S O_{4}^{2-}+2 e^{-} rightarrow P b S O_{4}+2 H_{2} O ) B ( cdot P b S O_{4}+2 H_{2} O rightarrow P b O_{2}+4 H^{+}+S O_{4}^{2-}+2 e^{-} ) ( mathbf{c} cdot P b S O_{4}+2 e^{-} rightarrow P b+S O_{4}^{2} ) ( mathbf{D} cdot P b S O_{4}+4 H_{2} O rightarrow P b O_{2}+8 H^{+}+S O_{4}^{2-}+2 e^{-} ) | 12 |

980 | ( mathbf{A} ) 0.1 M solution of a monobasic acid has a specific resistance of ‘r’ ohm-cm. Its molar conductivity is: A ( cdot frac{10}{r} ) в. ( 10 r ) c. ( frac{10^{4}}{r} ) D. ( frac{10^{4}}{2 r} ) | 12 |

981 | Question 5. Calculate the emf of the cell in which the following reaction takes place : Ni(s) + 2 Ag+ (0.002 M) Ni2+ (0.160 M) + 2Ag(s) Given that Ecell = 1.05 V | 12 |

982 | Calculate the useful work of the reaction ( boldsymbol{A} boldsymbol{g}(boldsymbol{s})+mathbf{1} / mathbf{2} boldsymbol{C l}_{2}(boldsymbol{g}) rightarrow ) ( A g C l(s) ) ( operatorname{Given} boldsymbol{E}_{c_{2} / C l^{-}}^{0}=+mathbf{1 . 3 6} boldsymbol{V} ) ( boldsymbol{E}_{A boldsymbol{g}|A boldsymbol{g} C l| C l^{-}}^{0}=mathbf{0 . 2 2} boldsymbol{V} ) if ( boldsymbol{P}_{C l_{2}}=mathbf{1} boldsymbol{a} boldsymbol{t m} ) and ( boldsymbol{T}=mathbf{2} mathbf{9} mathbf{8} boldsymbol{K} ) A. 110 kJ/mol B. 220 kJ/mol c. 55 kJ/mol D. 1000 kJ/mol | 12 |

983 | A current of ( 1 times 10^{-5} A ) is passed through a solution of single atom thick layer of ( A g N O_{3} ) for 16 min ( 5 s, ) using plantinum electrodes. A uniform single atom thick layer of Ag is deposited covering ( 90 % ) of cathode surface. The total surface area ( left(text { in } c m^{2}right) ) of cathode if each silver atom covers an area of ( mathbf{5 . 6} times mathbf{1 0}^{-mathbf{1 6}} mathbf{c m}^{mathbf{2}} mathbf{i s} ) | 12 |

984 | The process of zinc plating on iron sheet is known as A. annealing B. roasting c. galvanization D. smelting | 12 |

985 | Calculate the e.m.f of the cell in ( mathbf{V} ) ( boldsymbol{P t}left|boldsymbol{H}_{2}right|(mathbf{1} . mathbf{0} boldsymbol{a} boldsymbol{t m}) mid boldsymbol{C H}_{3} boldsymbol{C O O H}(mathbf{0 . 1} boldsymbol{M}) ) ( boldsymbol{K}_{boldsymbol{a}}left(boldsymbol{C} boldsymbol{H}_{3} boldsymbol{C O O H}right)=mathbf{1 . 8} times ) ( mathbf{1 0}^{-mathbf{5}}, boldsymbol{K}_{boldsymbol{B}^{prime}}left(boldsymbol{N} boldsymbol{H}_{3}right)=mathbf{1 . 8} times mathbf{1 0}^{-mathbf{5}} . ) if the value is ( -46 times 10^{-x}, ) then what is the value of ( x ? ) | 12 |

986 | Find the distance between (345) plane is a cubic batteries of length ( 7-7 A ) | 12 |

987 | What is the reduction electrode potential (in volts) of copper electrode when ( left[C u^{2+}right. ) ( =0.01 mathrm{M} ) in a solution at ( 25^{0} mathrm{C} ) ? (EO of ( left.C u^{2+} / C u text { electrode is }+0.34right) ) A . 0.399 B. 0.2809 c. 0.3105 D. 0.3695 | 12 |

988 | In an experimental set-up for the measurement of emf of a half-cell using a reference electrode and a salt bridge, when the salt bridge is removed, the voltage: A. does not change B. increases to maximum c. decreases half the value D. drops to zero | 12 |

989 | The limiting molar conductivity and molar conductivity of acetic acid are ( 390.5 s . c m^{2} . m o l^{-1} ) and ( 48.15 s . c m^{2} . m o l^{-1} ) respectively Calculate the degree of dissociation of the weak acid? ( mathbf{A} cdot 1.233 ) B. 12.33 c. 0.1233 D. 0.01233 | 12 |

990 | Which of the following, when dissolved in distilled water, makes it a good conductor? A. Potassium iodide B. common salt c. Potassium dichromate D. All of the above | 12 |

991 | Arrange the following metals in the order in which they displace each other from the solution of their salts. ( A l, C u, F e, M g ) and ( Z n ) | 12 |

992 | The resistance of a decinormal solution of an electrolyte in a conductivity cell was found to be 245 ohms Calculate the equivalent conductivity of the solutions. | 12 |

993 | Calculate the potential of hydrogen electrode in contact with a solution of ( 5 times 10^{-3} M ) of ( B a(O H)_{2} ) at 1 atm pressure and ( 298 mathrm{K} ) temperature: A . – ( 0.059 v ) B. 0.059v c. ( 0.59 v ) D – -0.59V | 12 |

994 | In a galvanic cell, the salt bridge: A. does not participate chemically in the cell reaction B. stops the diffusion of ions from one electrode to another C. is necessary for the occurrence of the cell reaction D. ensures mixing of the two electrolytic solutions | 12 |

995 | At ( 25^{circ} C, Delta H_{f}left(H_{2} O, Iright)= ) ( -56700 J / ) mol and energy of ionization of ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{I})=mathbf{1 9 0 5 0} boldsymbol{J} / )moll the reversible EMF at ( 25^{circ} mathrm{C} ) of the cell is ( 414 times 10^{-x}, ) then the value of ( x ) is ( ? ) ( boldsymbol{P t}left|boldsymbol{H}_{2}(boldsymbol{g})(boldsymbol{1} boldsymbol{a} boldsymbol{t m})right| boldsymbol{H}^{+} | boldsymbol{O} boldsymbol{H}^{-} mid boldsymbol{O}_{2}(boldsymbol{g})(boldsymbol{1} ) if at ( 26^{circ} mathrm{C} ) the emf increase by 0.001158 ( mathbf{V} ) Ans in ( mathrm{V} ) | 12 |

996 | Chemically, rust is ( mathrm{Fe}_{2} mathrm{O}_{3} cdot mathrm{XH}_{2} mathrm{O} ) If true enter 1 , else enter 0 . | 12 |

997 | Which of the following which has the highest molar conductivity? ( mathbf{A} cdotleft[C oleft(N H_{3}right)_{5} C lright] B r ) в. ( left[C oleft(N H_{3}right)_{5} C lright] S O_{4} ) ( mathbf{c} cdotleft[operatorname{Co}left(N H_{3}right)_{5} C lright] N O_{2} ) D. ( left[operatorname{Co}left(N H_{3}right)_{4} C lright] cdot 2 H_{2} O ) | 12 |

998 | During an electrochemical process, A. Gibbs free energy increases B. Gibbs free energy remain constant C. No prediction can be made about Gibbs free energy D. Gibbs free energy of decreases | 12 |

999 | The redox potential of ( boldsymbol{F e}^{mathbf{3}+} mid boldsymbol{F e}^{mathbf{2}+} ) electrode at ( mathrm{pH}=4 ) is: A. ( 0.8 mathrm{v} ) B. 0.5 c. ( 0.2 v ) D. 0.1 | 12 |

1000 | If aq. NaCl is electrolysed using graphite as anode and Hg as cathode than products are: A. ( C l_{2} ) gas at anode and Na at cathode B. ( C l_{2} ) gas at anode and ( H_{2} ) gas at cathode c. ( O_{2} ) gas at anode and ( H_{2} ) gas at cathode D. ( C l_{2} ) gas at anode and ( O_{2} ) gas at cathode | 12 |

1001 | Question 3. Under what condition is E cell = 0 or A, G = 0? :1: 1 1 | 12 |

1002 | Match the List-I with List-II and List-III: List – I (Ouantity) List – II (Symbol) (Quantity) (a) Conductivity ( (p) ) ( wedge_{m} ) ( (b) ) Cell constant ( (q) ) ( K ) (c) Molar conductance ( quad(mathrm{r}) quad wedge_{e} ) (d) Equivalent conductance ( quad(mathrm{s}) ) ( mathbf{A} cdot(a-q, u),(b-s, v),(c-d, w),(d-r, x) ) B . ( (a-q, u),(b-s, v),(c-p, w),(d-r, x) ) C ( .(a-b, u),(b-s, v),(c-p, w),(d-r, x) ) D . ( (a-p, u),(b-s, v),(c-p, w),(d-r, x) ) | 12 |

1003 | What happens when An iron rod is placed in ( C u S O_{4} ) solution? | 12 |

1004 | Galvanization is applying a coating of A ( . C r ) в. ( C u ) ( c cdot Z n ) D. ( P b ) | 12 |

1005 | Why do we apply paint on iron articles? | 12 |

1006 | In LEDs, the longer lead is connected to and the shorter lead is connected to A. negative terminal; positive terminal B. positive terminal; negative terminal c. negative terminal; neutral terminal D. positive terminal; neutral terminal | 12 |

1007 | What is a voltaic cell? ( A cdot A ) cell in which a spontaneous redox reaction produces electricity B. A cell in which an oxidation reaction produces electricity. C . A cell that produces voltage. D. A cell full of volts. E. Any cell that undergoes a spontaneous reaction. | 12 |

1008 | Draw a neat labelled diagram of ( boldsymbol{H}_{2}- ) ( O_{2} ) fuel cell. Write the reaction occurs at cathode of the cell. | 12 |

1009 | Q. 28 Can absolute electrode potential of an electrode be measured ? murod This is due | 12 |

1010 | Hiu Question 16. Which reference electrode is used to measure the 11 electrode potential of other electrodes? | 12 |

1011 | Grills of doors and windows are always painted before they are used : A. To look beautiful B. To avoid corroison c. To protect from rain D. None of these | 12 |

1012 | The redox reaction involving the reducing power of hydrogen sulphide is: [ begin{array}{c} boldsymbol{S}+mathbf{2} boldsymbol{H}^{+}+mathbf{2} boldsymbol{e}^{-} rightarrow \ boldsymbol{H}_{2} boldsymbol{S}, quad boldsymbol{E}_{boldsymbol{S} / boldsymbol{H}_{2} boldsymbol{S}}^{circ}=+mathbf{0 . 1 4} boldsymbol{V} end{array} ] Two other half equations are: [ boldsymbol{F} e^{3+}+boldsymbol{e}^{-} rightarrow boldsymbol{F} boldsymbol{e}^{2+} quad boldsymbol{E}_{boldsymbol{F} e^{3+} / boldsymbol{F} e^{2+}}^{mathrm{O}}= ] [ begin{array}{l} +mathbf{0 . 7 7} V \ B r_{2}+2 e^{-} rightarrow 2 B r^{-} quad E_{B r_{2} / B r^{-}}^{0}= end{array} ] ( mathbf{1 . 0 7} V ) Under standard conditions, hydrogen sulphide reacts with iron ( (I I I) ) ions If this statement is true enter 1 , else enter 0 | 12 |

1013 | Which of the following forms vortex ring? A ( cdot P_{2} O_{5} ) в. ( P H_{3} ) c. ( N H_{3} ) D. None of the above | 12 |

1014 | Question 6. Depict the galvanic cell in which the cell reaction is Cu+ 2Ag 2Ag + Cu2+ | 12 |

1015 | An electrolytic cell is constructed for preparing hydrogen. For an average current of 1 ampere in the circuit, the time required to produced ( 450 m L ) of hydrogen at NTP is approximately. A. 30 min B. 1 hour c. 2 hours D. 5 hours | 12 |

1016 | The electric charge for electrode deposition of one gram equivalent of a substance is: A ( cdot 1 ) ampere ( s^{-1} ) B. 96500 coulomb ( s^{-1} ) c. 1 ampere hour ( ^{-1} ) D. 1 coulomb ( s^{-1} ) | 12 |

1017 | The Gibbs energy for the decomposition of ( A l_{2} O_{3} ) at ( 500^{circ} C ) is as follows: ( frac{2}{3} A l_{2} O_{3} rightarrow frac{4}{3} A l+O_{2} ; triangle_{r} G= ) ( +966 k J m o l^{-1} ) The potential difference needed for the electrolytic reduction of ( A l_{2} O_{3} ) at ( 500^{circ} ) is at least. ( mathbf{A} cdot 2.5 V ) в. ( 5.0 mathrm{V} ) c. ( 4.5 V ) D. 3.0 ( V ) | 12 |

1018 | The two half-cell reactions of an electrochemical cell is given as ( boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{e}^{-} longrightarrow boldsymbol{A} boldsymbol{g} ; boldsymbol{E}_{boldsymbol{A} boldsymbol{g}^{+} mid boldsymbol{A} boldsymbol{g}}= ) ( -0.3995 V ) ( boldsymbol{F} boldsymbol{e}^{2+} longrightarrow boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{e}^{-} ; boldsymbol{E}_{boldsymbol{F} e^{3+} mid boldsymbol{F} e^{2+}}= ) ( -0.7120 V ) The value of cell EMF will be: A. ( -0.3125 V ) B. ( 0.3125 V ) c. ( 1.114 V ) D. ( -1.114 V ) | 12 |

1019 | If ( 0.5 L ) of ( 0.6 M S n S O_{4} ) solution is electrolysed for a period somin using a current of | 12 |

1020 | a) Define Kohlrausch’s law of independent migration of ions. Give its applications. b) Describe the salient features of the Collision theory of reaction rates of bimolecular reactions. | 12 |

1021 | If ( 0.01 M ) solution of an electrolyte has a resistance of 40 ohms in a cell having a cell constant ( 0.4 mathrm{cm}^{-1} ) then its molar conductance would be: A ( cdot 10^{4} ) B . ( 10^{3} ) ( c cdot 10^{2} ) D. 10 | 12 |

1022 | Assertion ( boldsymbol{H}_{2}+boldsymbol{O}_{2} ) fuel cell gives a constant voltage throughout its life. Reason In this fuel cell, ( H_{2} ) reacts with ( O H^{-} ) ions, yet the overall concentration of ( O H^{-} ) ions does not change A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

1023 | For the given data ( boldsymbol{A}+boldsymbol{B} rightleftharpoons boldsymbol{C}+boldsymbol{D} ; boldsymbol{E}^{o}=boldsymbol{a} boldsymbol{v} boldsymbol{o l} boldsymbol{t} ; boldsymbol{K}_{c}=boldsymbol{K}_{1} ) ( mathbf{2} boldsymbol{A}+mathbf{2} boldsymbol{B} rightleftharpoons mathbf{2} boldsymbol{C}+mathbf{2} boldsymbol{D} ; boldsymbol{E}^{boldsymbol{o}}= ) ( boldsymbol{b} boldsymbol{v} boldsymbol{o l} boldsymbol{t} ; boldsymbol{K}_{c}=boldsymbol{K}_{2} ) Select the correct choices: This question has multiple correct options ( mathbf{A} cdot a=b ) В. ( K_{2}=K_{1}^{2} ) ( mathbf{c} cdot a neq b ) ( mathbf{D} cdot b=a^{2} ) | 12 |

1024 | Galvanisation is a method of protecting iron from rusting, by coating with a thin layer of: A . galliummmmmmmmmmmaliuunmmmmmm B. aluminium c. zinc D. silver | 12 |

1025 | Following reactions are taking place in a Galvanic cell, ( Z n rightarrow Z n^{2+}+ ) ( mathbf{2} e^{-} ; boldsymbol{A} boldsymbol{g}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{A} boldsymbol{g} ) Which of the given representations is the correct method of depicting the cell? A ( cdot Z n_{(s)}left|Z n_{(a q)}^{2+}right|left|A g_{(a q)}^{+}right| A g_{(s)} ) B . ( Z n^{2+}|Z n | A g| A g^{+} ) c. ( Z n_{(a q)}left|Z n_{(s)}^{2+}right|left|A g_{(s)}^{+}right| A g_{(a q)} ) D. ( Z n_{(s)}left|A g_{(a q)}^{+}right|left|Z n_{(a q)}^{2+}right| A g_{s s} ) | 12 |

1026 | Consider the following cell: [ begin{array}{c} boldsymbol{P t}, boldsymbol{H}_{2}(boldsymbol{g}) mid boldsymbol{2} boldsymbol{M} boldsymbol{C H}_{3} boldsymbol{C O O N H}_{4}(boldsymbol{a} boldsymbol{q}) | mathbf{2} boldsymbol{n} \ 20 end{array} ] ( a+m ) 0.2 atm Given, ( boldsymbol{p} boldsymbol{K}_{boldsymbol{a}} boldsymbol{o} boldsymbol{f} boldsymbol{C H}_{3} boldsymbol{C O O H}= ) 4.74 and ( p K_{b} ) of ( N H_{4} ) OHis4.74. If ( E ) is e.m.f. of the cell in volt, then the value of ( 1000 mathrm{E} ) is ( left[text { Take } frac{2.303 R T}{F}=right. ) 0.059]( (text { e.g. }, text { if the value is } 56, ) then write answer as ( 6) ) | 12 |

1027 | Molten ( A l C l_{3} ) is electrolysed with a current of 0.5 ampere to produce 27 g Al. How many g-atom of ( A l ) are formed? | 12 |

1028 | What is corrosion? | 12 |

1029 | The specific conductivity of ( 0.1 mathrm{N} ) KCl solution is 0.0129 ohm ( ^{-1} mathrm{cm}^{-1} ). The resistance of the solution in the cell is 100 ( Omega ). The cell constant of the cell will be A . 1.10 B. 1.29 c. 0.56 D. 2.80 | 12 |

1030 | W WUMU U U CICUUUiyul cell ons of electrolytes is not correct? Q. 7 Which of the statements about solutions of electroly (a) Conductivity of solution depends upon size of ions (b) Conductivity depends upon viscosity of solution (c) Conductivity does not depend upon solvation of ions present (d) Conductivity of solution increases with temperature on of ions present in solution conductivit | 12 |

1031 | The conductivity of saturated solution of ( A g C l ) is found to be ( 1.86 times ) ( 10^{-6} ) ohm ( ^{-1} c m^{-1} ) and that of water is ( 6 times 10^{-8} o h m^{-1} c m^{-1} . ) If ( lambda^{0} A g C l ) is 138 ( o h m^{-1} c m^{2} e q^{-1} ) the solubility product of ( A g C l ) is: A ( cdot 1.3 times 10^{-5} ) В. ( 1.69 times 10^{-10} ) C ( .2 times 10^{-10} ) D. ( 2.7 times 10^{-10} ) | 12 |

1032 | Write Faraday’s laws of electrolysis. | 12 |

1033 | The rusting of iron takes place as follows ( 2 H^{+}+2 e+frac{1}{2} O_{2} rightarrow H_{2} O(l) ; E^{o}= ) ( +1.23 V ) ( F e^{2+}+2 e rightarrow F e(s) ; E^{o}=-0.44 V ) ( Delta G^{o} ) for the net process is: В. ( -161 k J ) mol ( ^{-1} ) C. -152 kJ ( m o l^{-1} ) D. ( -76 k J ) mol( ^{-1} ) | 12 |

1034 | When 96500 coulombs of electricity are passed through nickel sulphate solution, the amount of nicke deposited will be: A . 1 mol ( c .0 .1 mathrm{mol} ) D. 2 mol | 12 |

1035 | A constant electric current flows for 4 hours through two electrolytic cells connected in series. One contains ( mathrm{AgNO}_{3} ) solution and second contains ( mathrm{CuCl}_{2} ) solution. During this time 4 grams of Ag are deposited in the first cell. (a) How many grams of Cu are deposited in the second cell? (b) What is the current flowing in amperes? | 12 |

1036 | Which step(s) in glycolysis require the input of energy? A. The glucose priming step B. The phosphorylation of glucose c. The phosphorylation of fructose 6-phosphate D. All of these steps require the input of energy | 12 |

1037 | Draw a labelled diagram of ‘Standard Hydrogen Electrode’. | 12 |

1038 | For ( 2 A g^{+}+C_{6} H_{12} O_{6}+H_{2} O rightarrow ) ( mathbf{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s})+boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{mathbf{1 2}} boldsymbol{O}_{boldsymbol{7}}+boldsymbol{2} boldsymbol{H}^{+}, ) In K of the change is: ( mathbf{A} cdot 66.13 ) B. 58.38 c. 28.30 D. 46.29 | 12 |

1039 | calculate ( Delta G_{f}^{ominus} ) of the reaction: ( boldsymbol{A} boldsymbol{g}^{oplus}(boldsymbol{a} boldsymbol{q})+boldsymbol{C l}^{ominus}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{A} boldsymbol{g} boldsymbol{C l}(boldsymbol{s}) ) Given ( : Delta G^{ominus_{A g C l}}=-109 k J m o l^{-1} ) ( Delta G_{left(C l^{ominus}right)}^{ominus}=-129 k J m o l^{-1} ) ( Delta G_{left(A g^{oplus)}right.}^{ominus}=-77 k J m o l^{-1} ) в. ( -57 k J ) mol( ^{-} ) c. ( 57 k J ) mol ( ^{-1} ) D. ( 97 k J ) mol ( ^{-1} ) | 12 |

1040 | The reduction potential of hydrogen electrode at ( p H=10 ) is: A ( .-0.059 mathrm{V} ) B. -0.59 c. ( 0.59 v ) D. ( 0.0 mathrm{V} ) | 12 |

1041 | Draw a neat and labelled diagram of lead storage battery. | 12 |

1042 | Classify the following substances under three headings. Strong electrolytes, Weak electrolytes | 12 |

1043 | The negative Zn pole of Daniel cell, sending a constant current through a circuit, decreases in mass by 0.13 g in 30 minutes. If the chemical equivalent of Zn and Cu and 32.5 and 31.5 respectively, the increase in the mass of the positive Cu pole in this time is : A. 0.180 g B. 0.141g c. ( 0.126 mathrm{g} ) D. 0.242 | 12 |

1044 | In the atmosphere of industrial smog, copper corrodes to form: This question has multiple correct options A. Basic copper carbonate B. Copper sulphide c. Basic copper sulphate D. copper oxide | 12 |

1045 | When ammonia is added to the solution, ( p H ) is raised to ( 11 . ) Which half- cell reaction is affected by ( p H ) and by how much? ( mathbf{A} cdot mathrm{E}_{mathrm{oxd}} ) will increase by a factor of 0.65 from ( mathrm{E}_{text {oxd }}^{circ} ) are B. ( mathrm{E}_{text {oxd }} ) will decrease by a factor of 0.65 from ( mathrm{E}_{text {oxd }}^{circ} ) C ( cdot mathrm{E}_{text {red }} ) will increase by a factor of 0.65 from ( mathrm{E}_{text {red }}^{circ} ) D. ( mathrm{E}_{text {red }} ) will decrease by a factor of 0.65 from ( mathrm{E}^{circ} ) red | 12 |

1046 | Which of the following electrolytic solutions has the least specific conductance? A. ( 0.02 N ) n B. ( 0.2 N ) ( c cdot 2 N ) D. ( 0.002 N ) | 12 |

1047 | The process of coating of zinc over iron is known as A. Calcination B. Metallurgy c. Tinning D. Galvanisation | 12 |

1048 | Some of the batteries have alkaline electrolytes- ¡) Nickel – cadmium ii) Mercury battery iii) Modified Leclanche cell Cell potential is independent of ( left[mathrm{OH}^{-}right] ) in : B. ii, ii c. i, ii, iii D. iii only | 12 |

1049 | On electrolysing ( K_{2} S O_{4} ) solution using inert electrodes, ( 1.68 L(mathrm{STP}) ) of gases was obtained. How many moles of ( M n O_{4}^{-} ) could be reduced to ( M n^{2+} ) by the same quantity of electricity? A . 0.10 B. 0.20 c. 0.15 D. 0.02 | 12 |

1050 | For the circuit shown in the adjoining figure, match the entries of column with the entries of column II | 12 |

1051 | The specific conductance of a saturated solution of ( A g C l ) at ( 298 mathrm{K} ) is found to be ( 1.386 times 10^{-6} mathrm{Scm}^{-1} . ) Calculate its solubility. ( left(lambda_{A g^{+}}^{circ}=62.0 S c m^{2} m o l^{-1} text {and } lambda_{C l^{-}}^{circ}=7right. ) | 12 |

1052 | Define Reference electrode. | 12 |

1053 | Calculate EMF of ( left.Z nright|_{(0.01 M)} ^{Z n^{2+}} |_{(0.1 M)}^{A g^{+}} mid A g ) ( E_{Z n / Z n^{+2}}^{0}=0.762 V E_{A g^{+} / A g}^{0}=+0.80 V ) A. ( 1.56 v ) B. 2.36V c. ( 0.236 v ) D. 0.118v | 12 |

1054 | Which molecule electrolysis temperature is maximum? ( mathbf{A} cdot A s H_{3} ) B . ( N H_{3} ) ( mathbf{c} cdot P H_{3} ) ( mathbf{D} cdot S b H_{3} ) | 12 |

1055 | If ( 9 g m H_{2} O ) is electrolysed completely with the current of ( 50 % ) efficiency then : A. 96500 charge is required B. ( 2 times 96500 C ) charge is required c. ( 5.6 L ) of ( O_{2} ) at STP will be formed D. ( 11.2 L ) of ( O_{2} ) at STP will be formed | 12 |

1056 | In the diagram above, what is the half reaction that occurs at the cathode? A ( cdot A l rightarrow A l^{3+}+3 e^{-} ) B. ( N i^{2+}+2 e^{-} rightarrow N i ) ( mathbf{C} cdot N i rightarrow N i^{2+}+2 e^{-} ) ( mathbf{D} cdot 2 A l^{3+}+6 e^{-} rightarrow 2 A l ) E. None of these | 12 |

1057 | What will be the emf of a cell of two hydrogen electrodes, if a negative electrode is in contact with ( 10^{-8} M H^{+} ) ion positive electrode is in contact with ( mathbf{0 . 0 2 5 M} boldsymbol{H}^{+} mathbf{?} ) A. ( -0.18 V ) в. ( -0.28 V ) c. ( -0.38 V ) D. – ( 0.48 V ) | 12 |

1058 | Q. 14 The cell constant of a conductivity cell ……… (a) changes with change of electrolyte (b) changes with change of concentration of electrolyte (c) changes with temperature of electrolyte (d) remains constant for a cell | 12 |

1059 | Column II gives name of material use for device given in column I: | 12 |

1060 | Given standard ( E^{ominus}: ) ( F e^{3+}+3 e^{-} rightarrow F e ; E^{ominus}=-0.036 V ) ( F e^{2+}+2 e^{-} rightarrow F e ; E^{ominus}=-0.440 V ) The ( E^{ominus} ) of ( F e^{3+}+e^{-} rightarrow F e^{2+} ) is: A. ( 0.476 V ) ( V ) в. ( 0.404 V ) c. ( 0.604 V ) D. ( 0.772 V ) | 12 |

1061 | Grills of doors and windows are always painted before they are used? Give reason | 12 |

1062 | Assertion To protect iron from rusting it is coated with a thin layer of zinc. Reason The zinc forms a barrier against corrosion in that the steel underneath does not come into contact with water moisture in the air A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

1063 | Stand electrode potential are; ( boldsymbol{F e}^{+2} / mathrm{Fe} quad mathrm{E}=0.44 ) ( boldsymbol{F} boldsymbol{e}^{+boldsymbol{3}} / boldsymbol{F} boldsymbol{e}^{+mathbf{2}} quad mathbf{E}=mathbf{0 . 7 7} ) If ( F e^{+2}, F e^{+3} ) and ( mathrm{Fe} ) block re kept together, then: A ( cdot F e^{+3} ) increases B. ( F e^{+3} ) decreases c. ( frac{F e^{+2}}{F e^{+3}} ) reamins unchanged D. ( F e^{+2} ) decreases | 12 |

1064 | A current of ( 3.7 mathrm{A} ) is passed for six hours between ( N i ) electrode in 0.5 litre of ( 2 M ) solution of ( N ileft(N O_{3}right)_{2} . ) The molarity of solution at the end of electrolysis is: | 12 |

1065 | The potential of the cell containing two hydrogen electrodes as represented below, is: ( boldsymbol{P t}, boldsymbol{H}_{2(g)}left|boldsymbol{H}^{+}left(mathbf{1 0}^{-6} boldsymbol{M}right) | boldsymbol{H}^{+}left(mathbf{1 0}^{-4} boldsymbol{M}right)right| boldsymbol{H} ) ( operatorname{at} 298 K ) A. ( -0.118 V ) B . ( -0.0591 V ) c. ( 0.118 V ) D. ( 0.0591 V ) | 12 |

1066 | The temperature coefficient of the e.m.f. of cell, ( left(frac{d E}{d T}right)_{p} ) is given by: A ( cdot frac{n F}{Delta S} ) в. ( frac{Delta S}{n F} ) c. ( frac{Delta S}{n F T} ) D. ( -n F E ) | 12 |

1067 | Which of the following reactions does not take place during rusting? A ( cdot H_{2} C O_{3} rightleftharpoons 2 H^{+}+C O_{3}^{2} ) B. ( 4 F e^{2+}+O_{2(d r y)} rightarrow F e_{2} O_{3} ) C. ( 4 F e^{2+}+O_{2}+4 H_{2} O rightarrow 2 F e_{2} O_{3}+8 H^{+} ) D. ( F e_{2} O_{3}+x H_{2} O rightarrow F e_{2} O_{3} cdot x H_{2} O ) | 12 |

1068 | ( H_{2} S O_{4} ) solution attached to a bulb in a beaker: A. cannot light the bulb B. can light the bulb c. diffuses the bulb D. none of above | 12 |

1069 | The standard reduction potential for ( C u^{2+} 1 C u ) is +0.34 V. The reduction potential at ( mathrm{pH}=14 ) for the above couple is: ( boldsymbol{K}_{s p} ) of ( boldsymbol{C u}(boldsymbol{O H})_{2} ) is ( 1.0 times 10^{-19} ) ( mathbf{A} cdot 0.34 V ) B . ( 0.56 V ) c. ( -0.22 V ) D. None of these | 12 |

1070 | The negative Zn pole of a Daniel cell, sending a constant current through a circuit, decreases in mass by 0.13 g in 30 minutes. If the electrochemical equivalent of Zn and Cu are 32.5 and 31.5 respectively, the increase in the mass of the positive Cu pole in this time is: A. 0.180 g B. 0.141 g c. ( 0.126 mathrm{g} ) D. 0.242 | 12 |

1071 | While charging the lead storage battery A. ( P b S O_{4} ) anode is reduced to ( P b ) B. ( P b S O_{4} ) cathode is reduced to Pb ( mathrm{c} cdot P b S O_{4} ) cathode is oxidised to ( mathrm{Pb} ) D. ( P b S O_{4} ) anode is oxidised to ( P b O_{2} ) | 12 |

1072 | Question 6. The cell in which the following reaction occurs, 2 Fe3+ (aq) + 21 (aq) →→2Fe2+ (aq) + 12(s) has E = 0.236V at 298 K, calculate the standard Gibbs energy and the equilibrium constant of the cell reaction. (0) Gibbs energy, 4, Gº = – OFEcell where, n is the number of electons taking part in the reaction, so write two half reactions to find the value of n and then calculate the standard Gibbs energy by using the formula AG (1) Equilibrium constant is related to Gibbs energy as log Ko=; 2.030 RT So, calculate K. by using this formula. | 12 |

1073 | The standard reduction potential of normal calomel electrode and reduction potential of saturated calomel electrodes are 0.27 and 0.33 volt respectively. What is the concentration of ( C l^{-} ) in saturated solution of ( K C l ? ) A . ( 0.1 M ) в. ( 0.01 M ) c. ( 0.001 M ) D. None | 12 |

1074 | Ten gram of a fairly concentrated solution of cupric sulphate is electrolysed using 0.01 faraday of electricity. Calculate: (i) The mass of the resulting solution. (ii) The number of equivalents of acid or alkali in the solution. | 12 |

1075 | The molar conductivities at infinite dilution of ( K C l, K N O_{3} ) and ( A g N O_{3} ) at ( mathbf{2 9 8} boldsymbol{K} ) are 0.01499 mho ( m^{2} m o l^{-1}, 0.01250 m h o r ) and 0.01334 mho ( m^{2} m o l^{-1} ) respectively. What is the molar conductivity of ( A g C l ) infinite dilution at this temperature? | 12 |

1076 | 3 Faradays of electricity was passed through an aqueous solution of iron ( (I I) ) bromide. The weight (in ( g ) ) of iron metal (atomic weight ( =mathbf{5 6} ) amu) deposited at the cathode is: A . 56 B. 84 ( c cdot 112 ) D. 168 | 12 |

1077 | What will be the molar conductance ‘ ( boldsymbol{Lambda} ); if resistivity is ( x ) for ( 0.1 mathrm{N} mathrm{H}_{2} mathrm{SO}_{4} ? ) A ( . quad Lambda=frac{x times 1000}{0.1} ) в. ( Lambda=frac{2 times 1000}{x times 0.1} ) c. ( _{Lambda}=frac{x times 1000}{0.5} ) D. ( _{Lambda}=frac{0.5}{1000 x} ) | 12 |

1078 | When ( 4 A ) of current is passed through a ( mathbf{1} . mathbf{0} boldsymbol{L}, mathbf{0 . 1 0} boldsymbol{M} boldsymbol{F} mathbf{e}^{mathbf{3}+}(mathbf{a q}) ) solution for ( mathbf{1} boldsymbol{h} ) it is partly reduced to ( F e(s) ) and partly of ( F e^{2+}(a q) ) Identify the correct statement(s). This question has multiple correct options A. 0.10 mole of electrons are required to convert all ( F e^{3+} ) to ( F e^{2} ) B. 0.025 mol of ( F e(s) ) will be deposited. c. 0.075 mol of iron remains as ( F e^{2} ) D. 0.050 mol of iron remains as ( F e^{2} ) | 12 |

1079 | The process of zinc-plating on iron sheet is known as: A. annealing B. roasting c. galvanisation D. smelting | 12 |

1080 | ( 10 g ) fairly concentrated solution of ( boldsymbol{C u} boldsymbol{S O}_{4} ) is electrolysed using ( mathbf{0 . 0 1} ) faraday of electricity. Calculate the mass of the resulting solution. A. ( 7.6025 g ) в. ( 9.6025 g ) c. ( 6.6025 g ) D. ( 77.6025 g ) | 12 |

1081 | Standard free energies of formation (in kJ/mol) at ( 298 mathrm{K} ) are -237.2,-394.4 and -8.2 for ( boldsymbol{H}_{2} boldsymbol{O}(l), boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) ) and pentane ( (g) ) respectively The value of ( E_{c e l l}^{0} ) for the pentane-oxygen fuel cell is: A ( .1 .0968 mathrm{V} ) в. ( 0.0968 V ) c. ( 1.968 V ) D. ( 2.0968 V ) | 12 |

1082 | For a solution of an electrolyte at a particular concentration and temperature, which of the following is not the function of cell constant? 1) specific conductance 2) molar conductance 3) equivalent conductance 4) conductance A ( cdot 1,2 ) B. 1,2,3 c. 2,3,4 D. 1,4 | 12 |

1083 | Three copper wires of lengths and cross sectional areas are ( (ell, boldsymbol{A}),(2 ell, boldsymbol{A} / 2) ) and ( (ell / 2,2 A) . ) Resistance is minimum in: A. wire of cross-sectional area ( A / 2 ) B. wire of cross-sectional area A c. wire of cross-sectional area ( 2 A ) D. same in all the three cases | 12 |

1084 | The conductance of a solution of an electrolyte is equal to that of its specific conductance. The cell constant of the conductivity cell is equal to A. Resistance B. Faraday c. zero D. Unity | 12 |

1085 | Why do we apply paint on iron articles? | 12 |

1086 | Which of the following reaction is used to make a fuel cell ? ( mathbf{A} cdot 2 H_{2}(g)+O_{2}(g) rightarrow 2 H_{2} O(l) ) B. ( 2 F e(s)+O_{2}(g)+4 H^{+}(a q) rightarrow 2 F e^{2+}(a q)+2 H_{2} O(l) ) ( mathbf{c} cdot P b(s)+P b O_{2}(s)+2 H_{2} S O_{4}(a q) rightarrow 2 P b S O_{4}(s)+ ) ( H_{2} O(l) ) D. ( C d(s)+2 N i(O H)_{3}(s) rightarrow C d O(s)+2 N i(O H)_{2}+ ) ( 2 H_{2} O(l) ) | 12 |

1087 | If equal quantities of electricity are passed through three voltmeter containing ( boldsymbol{F} boldsymbol{e} boldsymbol{S} boldsymbol{O}_{4}, boldsymbol{F} boldsymbol{e}_{2}left(boldsymbol{S} boldsymbol{O}_{4}right)_{3} ) and ( F eleft(N O_{3}right)_{2}, ) then which of the following is not true? A. Amount of iron deposited in ( F e S O_{4} ) and ( F e_{2}left(S O_{4}right)_{3} ) is equal B. Amount of iron deposited in ( F eleft(N O_{3}right)_{3} ) is ( frac{2}{3} ) of the amount of iron deposited in ( F e S O_{4} ) C. Amount of iron deposited in ( F e_{2}left(S O_{4}right)_{3} ) and ( F eleft(N O_{3}right)_{3} ) are equal D. Same gas will evolve in all three cases at anode | 12 |

1088 | Corrosion of metals can be prevented when contact between metal and is cut off. A. nitrogen B. hydrogen c. oxygen D. carbon | 12 |

1089 | Which of the following changes will increase the EMF of the cell: ( boldsymbol{C o}(boldsymbol{s})left|boldsymbol{C o C l}_{2}left(boldsymbol{M}_{1}right) | boldsymbol{H} boldsymbol{C l}left(boldsymbol{M}_{2}right)right|left(boldsymbol{H}_{2}, boldsymbol{g}right) ) This question has multiple correct options A. Increase the volume of ( C o C l_{2} ) solution from ( 100 mathrm{mL} ) to 200 mL. B. Increase ( M_{2} ) from 0.01 M to 0.50 M. C. Increase the pressure of the ( H_{2}(g) ) from 1.0 to 2.0 atm. D. Increase ( M_{1} ) from 0.01 M to 0.50 ( mathrm{M} ) | 12 |

1090 | Question 8. What is electrode potential? | 12 |

1091 | Molar conductivity of 0.15 M solution of KCl at ( 298 mathrm{K} ), if its conductivity is ( 0.0152 mathrm{S} mathrm{cm}^{-1} ) will be: A ( cdot 124 Omega^{-1} mathrm{cm}^{2} mathrm{mol}^{-} ) B. ( 204 Omega^{-1} mathrm{cm}^{2} mathrm{mol}^{-} ) c. ( 101 Omega^{-1} mathrm{cm}^{2} ) mol ( ^{-1} ) D. ( 300 Omega^{-1} mathrm{cm}^{2} ) mol ( ^{-1} ) | 12 |

1092 | If ( C u ) reacts with conc. ( H_{2} S O_{4}, ) then what reactions take place: A ( . C u ) is oxidised to ( C u^{2} ) B. ( S O_{4}^{2-} ) is reduced to ( S O_{2} ) c. Both of the above reactions take place D. None of the above reaction take place | 12 |

1093 | 0.37 Why is alternating current used for measuring resistance of an electrolytic solution? | 12 |

1094 | On electrolysis, water splits into A. positively charged hydrogen ions and negatively charged oxygen ions. B. negatively charged hydrogen ions and positively charged oxygen ions C. hydrogen and oxygen atoms having positive and negative charges respectively. D. hydrogen and oxygen atoms having negative and positive charges respectively. | 12 |

1095 | The process of formation of polymers from respective monomers is called: A. Polyacrylonitrile B. Co-polymerization c. Polymerization D. None of these | 12 |

1096 | Question 7. Why does the conductivity of a solution decrease with dilution? @ Conductivity Number of ions per unit volume. | 12 |

1097 | The values of the limiting molar conductivity ( left(wedge^{circ}right) ) for ( N a C l, H C l ) and NaOAc are 126.4,425.9 and ( 91.0 S mathrm{cm}^{2} ) mol ( ^{-1}, ) respectively. For ( H O A c, wedge^{circ} ) in ( S c m^{2} m o l^{-1} ) is: A. 390.5 B . 299.5 c. 208.5 D. 217.4 | 12 |

1098 | Edible oil is not allowed to stand for a long time in an iron or tin container Give reasons. | 12 |

1099 | Ouestion 18. Write the Nernst equation for the cell reaction in the Daniel cell. How will the E cell be affected when concentration of Zn2+ ions is increased? | 12 |

1100 | A silver wire dipped in ( 0.1 mathrm{M} mathrm{HCl} ) solution saturated with AgCl develops a potential -0.25V. If ( E^{0}_{A g / A g^{+}}= ) ( -0.799 V, K_{S P} ) of AgCl in pure water will be A ( .2 .95 times 10^{-11} ) B . ( 5.30 times 10^{-11} ) c. ( 3.95 times 10^{-11} ) D. ( 1.95 times 10^{-11} ) | 12 |

1101 | When 0.1 mol ( operatorname{CoCl}_{3}left(N H_{3}right)_{5} ) is treated with excess of ( A g N O_{3}, 0.2 ) mole of ( A g C l ) are obtained. The conductivity of solution will correspond to A. 1: 3 electrolyte B. 1: 2 electrolyte c. 1: 1 electrolyte D. 3: 1 electrolyte | 12 |

1102 | Express the relation among cell constant, resistance of the solution in the cell and conductivity of the solution. How is molar conductivity of a solution related to its conductivity? | 12 |

1103 | In a cell, the following reaction takes place: ( boldsymbol{F} boldsymbol{e}+boldsymbol{C u} boldsymbol{S O}_{4} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{C u} ) The cell can be represented as: A ( cdot C uleft|C u S O_{4} | F eright| F e S O_{4} ) B . ( P tleft|C u S O_{4} | F e S O_{4}right| P t ) c. ( F eleft|F e S O_{4} | C u S O_{4}right| C u ) D. ( C u S O_{4}left|C u | F e S O_{4}right| F e ) | 12 |

1104 | The specific conductance of saturated solution of ( C a F_{2} ) is ( 3.86 times 10^{-5} ) ohm ( c m^{-1} ) and that of water used for solution is ( 0.15 times 10^{-5} ). The specific conductance of ( C a F_{2} ) alone is: A. ( 3.71 times 10^{-5} ) В. ( 4.01 times 10^{-5} ) c. ( 3.7 times 10^{-4} ) D . ( 3.86 times 10^{-4} ) | 12 |

1105 | Quinhydrone half cell is not reversible to: This question has multiple correct options ( mathbf{A} cdot mathbf{H}^{+} ) B. quinone c. quinol D. он | 12 |

1106 | Calculate the electrode potential of the electode ( Z n / Z n^{2+}(text {conc.}=0.1 M) ) at ( 25^{circ} C ) Given that ( boldsymbol{E}_{Z n, Z n^{2+}}^{circ}=mathbf{0 . 7 6 1 8} ) volt. | 12 |

1107 | The molar conductivity of ( 0.1 M C H_{3} C O O H ) solution is ( 4 S c m^{2} m o l^{-1} . ) What is the specific conductivity and resistivity of the solution. | 12 |

1108 | Internal resistance of a battery cell increases with: A. increase in concentration of electrolyte B. increase in distance between two electrodes C. increase in area of the plates inside the electrolyte D. increase in size of the electrodes | 12 |

1109 | In a fuel cell the fuel is fed to which compartment? A. Anode compartment B. Cathode compartment c. Both the compartments D. None of the above | 12 |

1110 | ( E_{C l O_{4}^{-} / C l O_{3}^{-}}^{o} ) and ( E_{C l O_{3}^{-} / C l O_{2}^{-}}^{o} operatorname{are}+0.36 V ) and ( +0.33 V ) respectively. The equilibrium concentration of per chlorate ion for the given reaction would be: [ begin{array}{rcc} & mathbf{2 C l O}_{mathbf{3}}^{-} rightleftharpoons mathbf{C l O}_{mathbf{2}}^{-}+mathbf{C l O}_{mathbf{4}}^{-} \ boldsymbol{t}=mathbf{0} & mathbf{0 . 1} mathbf{M} & mathbf{0} end{array} ] A ( .0 .19 M ) B. 0.024 c. 0.24 D. 0.019 | 12 |

1111 | As a lead storage battery is charged. A. Lead dioxide dissolves B. Sulphuric acid is regenerated C. Lead electrode becomes coated with lead sulphate D. The concentration of sulphuric acid decreases | 12 |

1112 | In an electrochemical cell, anode and cathode are A. Positively and negatively charges ions B. Positively and negatively charges electrodes C. Negatively and positively charged electrodes D. Negatively and positively charged ions | 12 |

1113 | The specific conductance of a ( N / 10 K C I ) at ( 25^{0} C ) is 0.0112 oh ( m^{-1} c m^{-1} . ) The resistance of cell containing solution at the same temperature was found to be 55ohms. The cell constant will be: A ( cdot 6.16 mathrm{cm}^{-1} ) B. ( 0.616 c m^{-1} ) c. ( 0.0616 mathrm{cm}^{-1} ) D. ( 616 mathrm{cm}^{-1} ) | 12 |

1114 | Which of the following is true for an electrolytic cell? A. An electric current causes an otherwise nonspontanteous chemical reaction to occur B. Reduction occurs at the anode. C. A spontaneous electrochemical reaction produces an electric current D. The electrode to which electrons flow is where oxidation occurs E. None of the above | 12 |

1115 | Q Type your question following apparatus was set up. Which among the following statement(s) is(are) correct? (i) Bulb will not glow because electrolyte is not acidic. (ii) Bulb will glow because NaOH is a strong base and furnishes ions for conduction. (iii) Bulb will not glow because circuit is incomplete. (iv) Bulb will not glow because it depends upon the type of electrolytic solution. ( A cdot ) (i) and (iii) B. (ii) and (iv) c. (ii) only D. (iv) only | 12 |

1116 | VUVCHI Q.55 Match the items of Column I and Column items of Column I and Column II on the basis of data given below Ff/f = 2.871. Ex = -3.5V. FAU3+ /Au = 1.4V, E = 1.09V Bro/Br Column 1 A. 1. BLI 2. C. Au3+ 3. D. Br 4. E AU 5. 6 7. Column II Metal is the strongest reducing agent Metal ion which is the weakest oxidising agent Non-metal which is the best oxidising agent Unreactive metal Anion that can be oxidised by Au+| Anion which is the weakest reducing agent Metal ion which is an oxidising agent | 12 |

1117 | The reduction potential of a hydrogen electrode containing a solution of ( boldsymbol{p} boldsymbol{H}=boldsymbol{4} ) is: A . 0.336 B. 4.059 ( v ) c. – ( 0.236 v ) D. 3.941 | 12 |

1118 | Fuel cells are better than other cells. Give any two reasons. | 12 |

1119 | The potential of a hydrogen electrode in a solution with ( p O H=4 ) at ( 25^{circ} C ) is: A . -0.059 B. 0.059 c. -0.59 D. 0.59 | 12 |

1120 | List 1 and List 2 contains four entries each. Entries of List 1 are to be matched with some entries of List 2. One or more than one entries of List 1 may have the matching with the same entries of List 2 | 12 |

1121 | Which metals does not corrode easily? A . Gold B. Iron c. Aluminium D. zinc | 12 |

1122 | The current inside a copper voltameter: A. is half the outside value B. is the same as the outside value C. is twice the outside value D. depends on the concentration of ( C u S O_{4} ) | 12 |

1123 | Which of the following statements regarding fuel cell is (are) true? This question has multiple correct options A. They have efficiency of about ( 60-70 % ) B. There efficiency is less then conventional methods C. They do not cause pollution D. They can supply indefinite amount of energy until outside supply of reactants is maintained | 12 |

1124 | Which is true according to the Faraday Law of electrolysis? Here ( m ) is the mass deposited at an electrode, ( Q ) is the charge at the electrode and ( I ) is the current passed. ( A cdot m propto I^{2} ) в. ( m propto Q ) ( mathrm{c} cdot m propto Q^{2} ) D. ( m ) does not depend on ( Q ) | 12 |

1125 | The reference electrode is made from which of the following? A. ( Z n C l_{2} ) в. ( mathrm{CuSO}_{4} ) c. ( H g_{2} C l_{2} ) D. ( H g C l_{2} ) | 12 |

1126 | Ammonium chloride used in dry cell acts as A. Catalyst B. Electrolyte C. Polariser D. Both (1) and (3) | 12 |

1127 | Number of coulombs required to liberate 0.5 mol of ( boldsymbol{O}_{2} ) is: A . 19300 B. 193000 c. 96500 D. 9650 | 12 |

1128 | What happens when you join the free ends of the tester for more than a few minutes? A. Cells of the battery will drain quickly. B. The current will not be able to pass. c. There would be no conduction of electricity D. All of the above | 12 |

1129 | How many faradays are released when ( 12.7 g ) of copper metal is changed into copper ions? | 12 |

1130 | The term infinite dilution refers when: A. ( alpha rightarrow 1 ), for weak electrolytes B. an electrolyte is 100% dissociated c. all interionic effects disappears D. all of the above | 12 |

1131 | ( left[A u(C N)_{2}right]^{ominus} ) is a very stable complex under certain conditions. The concentration of cyande ion which is required to keep 99 mol% of the gold in the form of the cyanide complex is: [Given ( left.K_{f}left[A u(C N)_{2}right]^{ominus}=4 times 10^{28}right] ) A ( .2 times 10^{-28} M ) в. ( 3 times 10^{-14} M ) c. ( 5 times 10^{-28} M ) D. ( 5 times 10^{-14} M ) | 12 |

1132 | The standard reduction potential ( E^{circ} ) for half reaction are: ( Z n rightarrow Z n^{2+}+2 e^{-} ; E^{o}=+0.76 V ) ( boldsymbol{F e} rightarrow boldsymbol{F} boldsymbol{e}^{2+}+boldsymbol{2} boldsymbol{e}^{-} ; boldsymbol{E}^{o}=+boldsymbol{0 . 4 1} boldsymbol{V} ) The EMF of the cell reaction is: ( boldsymbol{F} boldsymbol{e}^{2+}+boldsymbol{Z} boldsymbol{n} rightarrow boldsymbol{Z} boldsymbol{n}^{2+}+boldsymbol{F} boldsymbol{e} ) A. ( -0.35 V ) в. ( +0.35 V ) ( mathrm{c} cdot+1.17 V ) D. -1.17V | 12 |

1133 | ( 4.5 g ) of aluminium (At. mass ( =27 ) atm is deposited at cathode from ( boldsymbol{A} boldsymbol{l}^{mathbf{3}+} ) solution by a certain quantity of electric charge. The volume of hydrogen produced at STP from ( boldsymbol{H}^{+} ) ions in solution by the same quantity of electric charge will be A . ( 44.8 L ) B. 22.4 L c. ( 11.2 L ) D. ( 5.6 L ) | 12 |

1134 | Arrange the following reducing agents in the order of increasing strength under standard state condition. Justify the answer. Element Al(s) ( mathrm{Cu}(mathrm{s}) quad mathrm{cl}(mathrm{aq}) ) ( E^{o} quad v^{-1.66} ) ( 1.36 mathrm{v} ) ( 0.34 mathrm{V} ) | 12 |

1135 | Consider the following equation for a cell ( boldsymbol{A}+boldsymbol{B} rightleftharpoons boldsymbol{C}+boldsymbol{D} ) ( boldsymbol{E}^{o}= ) ( boldsymbol{X} boldsymbol{v o l t}, quad boldsymbol{K}_{e q}=boldsymbol{K}_{1} ) ( mathbf{2 A}+mathbf{2 B} rightleftharpoons mathbf{2 C}+mathbf{2 D} ; quad boldsymbol{E}^{boldsymbol{o}}= ) ( boldsymbol{y} ) volt, ( quad boldsymbol{K}_{e q}=boldsymbol{k}_{2} ) A. ( X=y, K_{1}=K_{2} ) B . ( X=2 y, K_{1}^{2}=K_{2} ) C . ( X=y, K_{1}^{2}=K_{2} ) D. ( X^{2}=y, K_{1}^{2}=K_{2} ) | 12 |

1136 | Statement ( 1: ln ) an electrolytic cell, the anode becomes positive and the cathode becomes negative. Statement 2: Anions migrate to the anode and cations migrate to the cathode. A. Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1 B. Both the Statement 1 and Statement 2 are correct, but Statement 2 is NOT the correct explanation of Statement 1. c. Statement 1 is correct, but Statement 2 is not correct D. Statement 1 is not correct, but Statement 2 is correct | 12 |

1137 | Number of Faraday required to get ( 1 g ) atom of ( M g ) from ( M g C l_{2} ) is: A. ( 0.0035 F ) в. ( 2 F ) ( c .1 F ) D. ( 0.2 F ) | 12 |

1138 | The cell in which the following reaction occurs: ( 2 F e^{3+}(a q)+2 I^{-}(a q) rightarrow 2 F e^{2+}(a q)+ ) ( boldsymbol{I}_{2}(boldsymbol{s}) ) has ( E_{c e l l}^{circ}=0.236 V ) at ( 298 K . ) Calculate the standard Gibbs energy of the cell reaction. (Given : ( 1 boldsymbol{F}= ) ( left.mathbf{9 6}, mathbf{5 0 0} boldsymbol{C} boldsymbol{m o l}^{-mathbf{1}}right) ) | 12 |

1139 | Give Nernst equation: Calculate the electrode potential of the following single electrode. ( boldsymbol{C u}_{(a q)}^{++}(boldsymbol{C}=mathbf{0 . 0 1 M}) / boldsymbol{C u} ;left(boldsymbol{E}^{circ}=right. ) ( +0.337 V) ) | 12 |

1140 | The pH of solution in a cell : Reference electrode ( | boldsymbol{H}_{3} boldsymbol{O}^{+}(?) boldsymbol{H}_{2} mid boldsymbol{P} boldsymbol{t} ) can be determined by using the formula ( boldsymbol{p} boldsymbol{H}= ) ( -frac{left[boldsymbol{E}_{text {cell}}+boldsymbol{E}_{text {ref}}right]}{mathbf{0 . 0 5 9}} . ) However, the use of hydrogen electrode to determine pH is usually ignored. Which are the correct facts about this observation? This question has multiple correct options A. The use of H-electrode hinders in the establishment of the equilibrium at the surface and the electrode no Ionger behaves reversibly B. The use of H-electrode is usually restricted if solution contains reducible materials c. The use of H-electrode is usually restricted as it is easily poisoned D. The use of quinhydrone electrode as electrode is usually preferred as reference electrode ( left|H_{3} O^{+}, Q, Q H_{2}right| A u ) | 12 |

1141 | The molar conductivity of a solution of a weak acid ( boldsymbol{H} boldsymbol{X}(mathbf{0 . 0 1} boldsymbol{M}) ) is ( mathbf{1 0} ) times smaller than the molar conductivity of a solution of a weak acid ( boldsymbol{H} boldsymbol{Y}(mathbf{0 . 1} boldsymbol{M}) . ) If ( boldsymbol{lambda}_{boldsymbol{X}^{-}}^{circ} approx boldsymbol{lambda}_{boldsymbol{Y}^{-}}^{circ}, ) the difference in their ( boldsymbol{p} boldsymbol{K}_{boldsymbol{a}} ) values, ( boldsymbol{p} boldsymbol{K}_{boldsymbol{a}}(boldsymbol{H} boldsymbol{X})-boldsymbol{p} boldsymbol{K}_{boldsymbol{a}}(boldsymbol{H} boldsymbol{Y}), ) is (consider degree of ionization of both acids to be ( <<1 ) ) | 12 |

1142 | The reaction taking place is: ( mathbf{A} cdot H g_{2} C l_{2}(s)+2 A g(s) rightarrow 2 A g C l(s)+2 H g(l) ) B ( cdot 2 H g_{2} C l_{2}(s)+2 A g(s) rightarrow 4 A g C l(s)+2 H g(l) ) ( mathbf{c} cdot H g_{2} C l_{2}(s)+3 A g(s) rightarrow A g C l(s)+2 H g(l) ) D. None of these | 12 |

1143 | Question 13. How much electricity in terms of Faraday is requir produce. (i) 20.0 g of Ca from molten CaCl ? (ii) 40.0 g of Al from molten Al2O3? | 12 |

1144 | What is the electrode potential in (in ( V ) ) of the following electrode at ( mathbf{2 5}^{o} boldsymbol{C}>boldsymbol{N} boldsymbol{i}^{2+}(mathbf{0 . 1} boldsymbol{M}) mid boldsymbol{N} boldsymbol{i}(boldsymbol{s}) ) (standard reaction potential of ( left.N i^{2+} / N i text { is }-0.25 Vright) ) A . ( -0.28 v ) B. -0.34 V c. ( -0.82 v ) D. -0.22V | 12 |

1145 | Arrange the following compounds in order of their Molar conductance: (।) ( boldsymbol{K}left[boldsymbol{C o}left(boldsymbol{N} boldsymbol{O}_{2}right)_{4}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}right] ) ( (|)left[boldsymbol{C r}(boldsymbol{O} boldsymbol{N} boldsymbol{O})_{3}left(boldsymbol{N} boldsymbol{H}_{3}right)_{3}right] ) ( (||)left[boldsymbol{C r}left(boldsymbol{N} boldsymbol{H}_{3}right)_{6}right] boldsymbol{C l}_{3} ) ( (mathrm{IV}) M gleft[C rleft(N O_{2}right)_{5}left(N H_{3}right)right] ) ( A cdot|<I<I V<| 1 ) B. II IV ( <1<11 ) c. ( |<1=1 V<| ) D. IV <III <II<I | 12 |

1146 | A Faraday is: A. the magnitude of the charge of 1 mole of electrons B. the magnitude of the electric dipole C. a fundamental constant of nature equal to ( 6.63 times ) ( 10^{-34} J s / )photon D. a constant that accounts for the existence of ions in solution | 12 |

1147 | The specific conductance of a solution is ( 0.3568(o h m)^{-1} mathrm{cm}^{-1} mathrm{When} ) placed in a cell the conductance is 0.0268 oh ( m^{-1} ) The cell constant is: A ( cdot 1.331 mathrm{cm}^{-1} ) B. ( 13.31 c m^{-1} ) ( mathbf{c} cdot 0665 mathrm{cm}^{-1} ) D. ( 6.65 mathrm{cm}^{-1} ) | 12 |

1148 | The efficiency of a fuel cell is given by: A ( cdot frac{Delta s}{Delta G G} ) в. ( frac{Delta H}{Delta G} ) c. ( frac{Delta G}{Delta S G} ) D. ( frac{Delta G}{Delta H} ) | 12 |

1149 | The density of copper is ( 8.94 m L^{-1} ) Find out the number of coulombs needed to plate an area ( 10 times 10 mathrm{cm}^{2} ) to a thickness of ( 10^{-2} mathrm{cm} ) using ( mathrm{Cu} ) SO solution as electrolyte. (At. mass of ( boldsymbol{C u}=mathbf{6 3 . 6}) ) | 12 |

1150 | Assertion Zinc is used in the galvanization of iron. Reason Its coating on iron articles increases their life by protecting them from rusting. A. If both Assertion and Reason are correct and Reason is the correct explanation of Assertion B. If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion C. If Assertion is correct but Reason is incorrect D. If Assertion is incorrect but Reason is correct | 12 |

1151 | The potential value of standard hydrogen electrode is | 12 |

1152 | When electricity is passed through a solution of ( A l C l_{3} ) and ( 13.5 g ) of ( A l ) is deposited, the number of Faraday required must be: A . 0.5 в. 1.0 c. 1.5 D. 2.0 | 12 |

1153 | ( boldsymbol{Z} boldsymbol{n}_{(s)}left|boldsymbol{Z} boldsymbol{n}_{(boldsymbol{a q})}^{boldsymbol{2}+}(boldsymbol{1} boldsymbol{M}) | boldsymbol{N} boldsymbol{i}_{(boldsymbol{a q})}^{2+}(boldsymbol{1} boldsymbol{M})right| boldsymbol{N} boldsymbol{i}_{(s)} ) Which is incorrect for the above given cell? A. Electrochemical cell B. Voltaic cell c. Galvanic cell D. Daniel cell | 12 |

1154 | Which one of the following species has maximum conductance in their aqueous solutions? A ( cdot K_{2} P t C l_{6} ) в. ( P t C l_{4} cdot 2 N H_{3} ) c. ( P t C l_{4} cdot 3 N H_{3} ) D. ( P t C l_{4} cdot 5 N H_{3} ) | 12 |

1155 | If ( F e^{3+}+y^{4-} rightleftharpoons F e Y^{ominus} ; K_{f}=1.3 times ) ( 10^{25} ) ( F e^{3+}+Y^{4-} rightleftharpoons F e Y^{2-} ; K_{f}=2.1 times 10^{14} ) And ( F e^{3+}+e^{-} rightleftharpoons F e^{2+} ; E^{ominus}=+0.77 V ) ( boldsymbol{E}^{ominus} ) for ( boldsymbol{F} boldsymbol{e} boldsymbol{Y}^{ominus}+boldsymbol{e}^{-} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{Y}^{2-} ) A . 0.13 v B. ( 0.26 mathrm{v} ) c. ( 1.2 v ) D. 1.6 | 12 |

1156 | Which of the following statements is false? A. Vegetables conduct electricity B. Passage of electric current will not change the colour of a solution C. An electrode conducts electricity D. Electroplating is one of the applications of chemical effects of electrical current | 12 |

1157 | Maximum conductance is shown by: A . ( 0.1 M ) NaCl в. ( 0.1 M ) Н ( _{2} ) SO ( _{4} ), c. ( 0.1 M ) sucrose D. ( 0.1 M ) glucose | 12 |

1158 | Consider the cell: ( boldsymbol{P t}left|boldsymbol{H}_{2}left(boldsymbol{p}_{1} boldsymbol{a t m}right)right| boldsymbol{H}^{oplus}left(boldsymbol{x}_{1} boldsymbol{M}right) | boldsymbol{H}^{oplus}left(boldsymbol{x}_{2} boldsymbol{N}right. ) The cell reaction be spontaneous if This question has multiple correct options ( mathbf{A} cdot p_{1}=p_{2} ) and ( x_{1}>x_{2} ) B . ( p_{1}=p_{2} ) and ( x_{1}p_{2} ) D. ( x_{1}=x_{2} ) and ( p_{1}<p_{2} ) | 12 |

1159 | Which of the following metals is used to prevent rusting of iron, as per electrochemical method? ( A cdot Z n ) B. Sn c. ( mathrm{Ni} ) D. cu | 12 |

1160 | A current of ( 2.0 mathrm{A} ) is passed for 5 hours through a molten metal salt deposits 22.2 ( g ) of metal (At. mass: 177 u). The oxidation states of the metal in metal salt is: ( A cdot+1 ) ( B .+2 ) ( c cdot+3 ) ( D cdot+4 ) | 12 |

1161 | Fuel cell involves which of the following reaction(s)? This question has multiple correct options ( mathbf{A} cdot O_{2}(g)+2 H_{2} O(l)+4 e^{-} rightarrow 4 O H^{-}(a q .)(text { at cathode }) ) B. ( O_{2}(g)+2 H_{2} O(l)+4 e^{-} rightarrow 4 O H^{-}(a q .) ) (at anode) ( mathbf{c} cdot 2 H_{2}(g)+4 O H^{-}(a q) rightarrow 4 H_{2} O(l)+4 e^{-}(a t text { anode }) ) D. ( 2 H_{2}(g)+4 O H^{-}(a q .) rightarrow 4 H_{2} O(l)+4 e^{-} ) (at cathode) | 12 |

1162 | When metal atoms are deposited on the cathode: A. the mass of the cathode and anode increases by an equal amount B. the mass of the cathode decreases and the mass of the anode increases by an equal amount c. the mass of the cathode increases and the mass of the anode decreases by an equal amount D. the mass of the cathode increases more than the mass of the anode that decreases | 12 |

1163 | A current of 0.965 ampere is passed through ( 500 mathrm{ml} ) of ( 0.2 mathrm{M} ) solution of ( Z n S O_{4} ) for 10 minutes. The molarity of ( Z n^{2+} ) after deposition of zinc is: A. 0.1 B. 0.5 ( M ) c. ( 0.8 mathrm{M} ) D. 0.194 M | 12 |

1164 | State True or False. In recharging of lead storage cell, sulphuric acid is produced. A. True B. False | 12 |

1165 | In electrochemical passivity: A. thin visible oxide film is formed B. thin invisible oxide film is formed C. thick visible oxide film is formed D. thick invisible oxide films formed | 12 |

1166 | In fuel cells, the reaction that takes place at the anode is: A ( cdot H_{2}(g)+2 O H^{-}(a q) rightarrow 2 H_{2} O(l)+2 e^{-} ) в. ( O_{2}(g)+2 H_{2} O(l)+4 e^{-} rightarrow 4 O H^{-}(a q) ) c. ( 4 O H^{-} rightarrow O_{2}+2 H_{2} O+4 e^{-} ) D. ( 2 H^{+}+2 e^{-} rightarrow H_{2} ) | 12 |

1167 | The factors, which influence the conductance of solutions: This question has multiple correct options | 12 |

1168 | Faraday’s second law of electrolysis is related to the: A. molecular mass of the electrolyte B. Equivalent weight of the cation /anion C. Atomic weight of the electrolyte D. Atomic number of the cation/anion | 12 |

1169 | Plots of ( E_{text {cell}} ) with ( log _{10} Q ) for the reaction, ( Z n(s)+C u^{2+}(a q .) rightleftharpoons ) ( boldsymbol{C u}(boldsymbol{s})+boldsymbol{Z} boldsymbol{n}^{2+}(boldsymbol{a q} .) ) gives a straight line with an intercept ( 1.10 . ) If ( boldsymbol{E}_{c e l l}= ) ( 1.1591 V ), then value of ( Q ), i.e. ( frac{left[Z n^{2+}right]}{left[C u^{2+}right]} ) is: A . 0.01 B. ( 0 . ) c. 100 D. 10 | 12 |

1170 | On heating, sodium and sulphur can be melted. Molten sodium and molten sulphur are used? A. For refining lead B. As a medium for extracting metals c. As catalysts D. As electrodes in a modern kind of battery | 12 |

1171 | Differentiate between the terms strong electrolyte and weak electrolyte. (sating any two differences) | 12 |

1172 | A conductance cell was calibrated by filling it with a ( 0.02 M ) solution of potassium chloride (specific conductance ( =0.2768 ) oh ( m^{-1} m^{-1} ) and measuring the resistance at ( 298 K ) which was found to be 457.3 ohm. The cell was then filled with a calcium chloride solution containing ( 0.555 g ) of ( mathrm{CaCl}_{2} ) per litre. The measure resistance was 1050 ohm. Calculate the molar conductivity of ( C a C l_{2} ) solution. | 12 |

1173 | Given the standard potential of the following at ( 25^{circ} mathrm{C} . M n O_{2} rightarrow M n^{3+} ) ( boldsymbol{E}^{ominus}=mathbf{0 . 9 5} boldsymbol{V} ) ( M n^{3+} rightarrow M n^{2+} ; E^{ominus}=1.51 V ) The standard potential of ( M n O_{2} rightarrow ) ( M n^{2+} ) is : A . ( 1.23 mathrm{v} ) B. 0.2 ( v ) c. ( 0.02 mathrm{v} ) D. None of these | 12 |

1174 | Lead storage battery is most widely used in automobiles. A. True B. False | 12 |

1175 | Select the correct statements about the electrolysis This question has multiple correct options A. Electric current is used to drive a non spontaneous reaction B. ( Delta G ) is positive for chemical process during electrolysis C. Cations and anions move towards the anode in the anode and cathode respectively D. Over voltage is generally associated with anode in the electrolysis of ( N a C l(a q) ) | 12 |

1176 | In three test tubes ( P, Q, ) and ( R ) iron nails, water, oil and anhydrous calcium chloride is taken. Among these test tubes, in which test tubes corrosion of nails will not take place? ( A cdot P, Q ) and ( R ) B. ( P ) and ( R ) ( c . P ) and ( Q ) D. ( Q ) and ( R ) | 12 |

1177 | During the electrolysis of ( 0.1 mathrm{M} ) Cu SO solution using copper electrodes, a depletion of ( left[C u^{2+}right] ) occurs near the cathode with a corresponding excess near the anode, owing to inefficient stirring of the solution. If the concentrations of ( left[C u^{2+}right] ) near the anode ( & ) cathode are respectively 0.12 M & 0.08 M, calculate the back e.m.f. developed. Temperature ( =298 mathrm{K} ) A . 22 ( mathrm{mv} ) B. 5.2 mv c. ( 29 mathrm{mv} ) D. 59 mv | 12 |

1178 | What is the time (in sec) requried for depositing all the silver present in ( 125 m L ) of ( 1 M A g N O_{3} ) solution by passing a current of ( 241.24 A ? ) ( (1 F=96500 text { coulombs }) ) A . 10 B. 50 c. 100 D. 90 | 12 |

1179 | Reduction occurs at cathode in: A. galvanic cell B. electrolytic cell C. both galvanic and electrolytic cell D. neither galvanic nor electrolytic cell | 12 |

1180 | For the galvanic cell : ( boldsymbol{A l}(boldsymbol{s})left|boldsymbol{A} boldsymbol{l}^{3+}(boldsymbol{a} boldsymbol{q})(boldsymbol{0} cdot boldsymbol{1} boldsymbol{M})right| boldsymbol{A} boldsymbol{g}^{+}(boldsymbol{a} boldsymbol{q})(boldsymbol{0} cdot boldsymbol{1} boldsymbol{M}) ) which of the following is/are correct? This question has multiple correct options A. Reaction quotient ( Q=1.0 times 10^{-2} ) в. ( log _{10} Q=2 ) c. ( Q=1.0 times 10^{3} ) D. ( Q=1.0 times 10^{2} ) | 12 |

1181 | What is the main principle involved in voltaic cell? A. Conversion of chemical energy into heat energy B. Conversion of heat energy into electrical energy C. Conversion of chemical energy into electrical energy D. Conversion of electrical energy into chemical energy | 12 |

1182 | Which of the following devices can be used to detect a weak current? A. Use of electric bulb in tester B. Use of LED in tester c. A tester using magnetic effects of current D. Both B and C | 12 |

1183 | If a current of 0.3 ampere is drawn from a Daniell cell for 1 hour, what would be the change in mass of electrodes? (At. mass of ( C u=63.5 ) and ( Z n=65.37 ) | 12 |

1184 | For which of the following electrolytic solution ( wedge_{m} ) and ( wedge_{e} ) are equal? A. ( B a C l_{2} ) в. ( K C l ) ( mathbf{c} cdot A l_{2}left(S O_{4}right) ) D. ( operatorname{CaCl}_{2} ) | 12 |

1185 | No rusting takes place in absence of moisture. A . True B. False | 12 |

1186 | A conductivity cell filled with ( 0.01 M A g N O_{3} ) solution gives at ( 25^{circ} C ) a resistance of ( 1442 Omega ). If the molar conductivity of ( 0.01 M A g N O_{3} ) solution is ( 124.8 Omega^{-1} c m^{2} m o l^{-1}, ) what is the cell constant? | 12 |

1187 | For the cell Pt ( mid mathbf{H}_{2}(0.4 text { at } m) mid mathbf{H}^{+}(p H=1) ) ( left.|(p H=2) mid H_{2} 90.1 text { atm }right) mid P t . ) The measured potential at ( 25^{circ} mathrm{C} ) is: A . ( -0.1 V ) B. ( -0.5 V ) c. ( -0.041 V ) D. ( -0.030 V ) | 12 |

1188 | Jamila started noticing some kind of reddish brown particles around a photo frame, which is an old one. Why it could have happened and what is it? | 12 |

1189 | The ionization constant of a weak acid is ( 1.6 times 10^{-5} ) and the molar conductivity at infinite dilution is ( 380 times 10^{-4} S m^{2} m o l^{-1} . ) If the cell constant is ( 0.01 mathrm{m}^{-1} ) then conductance of ( 0.01 M ) acid solution is: A ( cdot 1.52 times 10^{-5} mathrm{S} ) в. ( 1.52 times 10^{-7} ) S c. ( 1.52 times 10^{-3} ) S D. ( 1.52 times 10^{-4} ) S | 12 |

1190 | Q29. Given the standard electrode potentials, K*/K = -2.93 V, Ag/Ag = 0.80 V, Hg2+/Hg = 0.79 V, Mg2+/Mg = -2.37 V, Cr**/Cr = -0.74 V. Arrange these metals in increasing order of their reducing power. | 12 |

1191 | The more negative the standard potential, the ( ldots ) is its ability to displace hydrogen from acids. A. Greater B. Lesser c. Negetivity of the satndard potential has nothing to do with displacement of hydrogen D. Depends on the acid | 12 |

1192 | Assertion The voltage of mercury cell remains constant for longer period of time. Reason It is because net cell reaction does not involve ions. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

1193 | Find the time required to liberate 1 litre of ( boldsymbol{H}_{2} ) at ( mathrm{STP} ) in an electrolytic cell operating at 5 A. A . 19 min B. 24 min c. 29 min D. 14.5 min | 12 |

1194 | 3 faraday of electricity are passed through molten ( A l_{2} O_{3}, ) aqueous solution of ( C u S O_{4} ) and molten NaCl taken in three different electrolytic cells. The amount of ( mathrm{Al}, mathrm{Cu}, ) and ( mathrm{Na} ) deposited at the cathodes will be in the ratio of A. 1 mole : 2 mole : 3 mole B. 3 mole:2 mole:1 mole c. 1 mole : 1.5 mole : 3 mole D. 1.5 mole : 2 mole : 3 mole | 12 |

1195 | In an electrolytic cell: This question has multiple correct options A. anode is positively charged B. cathode is negatively charged C. oxidation takes place at anode D. reduction takes place at cathode | 12 |

1196 | Which metal pairs when coupled will get maximum emf for a voltaic cell? ( A cdot F e ) and ( C u ) B. Pb and Cu c. Cu and Au D. ca and cu | 12 |

1197 | Q. 6 An electrochemical cell can behave like an electrolytic cell when (a) Ecell = 0 (b) Ecell >Eext (c) Eext > Ecell (d) Ecell = Eext Dumin noll and increased reactic | 12 |

1198 | Which of the following will be most easily corroded in moist air? A. ( Z n ) в. ( F e ) c. ( N i ) D. ( S n ) | 12 |

1199 | If the values of ( wedge_{infty} ) of ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{C l}, boldsymbol{N} boldsymbol{a} boldsymbol{O H} ) and ( N a C l ) are 130,217 and 109 ohm ( ^{-1} cdot c m^{2} cdot e q u i v^{-1} ) respectively, the ( wedge_{infty} ) of ( N H_{4} O H ) in ( o h m^{-1} cdot c m^{2} cdot e q u i v^{-1} ) is: A .238 в. 198 c. 22 D. 456 | 12 |

1200 | Daniel cell can be represented in which of the following way? A ( cdot Z n_{(s)}left|Z n_{(a q)}^{2+}right|left|C u_{(s)}right| C u_{(a q)}^{2} ) B. ( Z n_{(s)}left|Z n_{(a q)}^{2+}right|left|C u_{(a q)}^{2+}right| C u_{(s)} ) c. ( C u_{(s)}left|C u_{(a q)}^{2+}right|left|Z n_{(a q)}^{2+}right| Z n_{(s)} ) D. ( Z n_{(a q)}^{2+}left|Z n_{(s)}right|left|C u_{(a q)}^{a+}right| C u_{(s)} ) | 12 |

1201 | Faraday’s laws of electrolysis are related to the: A. the atomic number of the cation B. the atomic number of anion c. the equivalent weight of the electrolyte D. the speed of the cation | 12 |

1202 | 09. Why is standard hydrogen electrode called reversible electrode? 11. T ib lootnodi A | 12 |

1203 | Marshall’s acid or perdisulphuric acid ( left(H_{2} S_{2} O_{8}right) ) can be prepared by electrolytic oxidation of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) as : ( mathbf{2} boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow boldsymbol{H}_{2} boldsymbol{S}_{2} boldsymbol{O}_{8}+boldsymbol{2} boldsymbol{H}^{oplus}+boldsymbol{2} boldsymbol{e}^{-} ) ( O_{2} ) and ( H_{2} ) are byproducts. In such an electrolysis ( 9.72 mathrm{L} ) of ( H_{2} ) and ( 2.35 mathrm{L} ) of ( O_{2} ) were produced at S.T.P. What is the weight of ( boldsymbol{H}_{2} boldsymbol{S}_{2} boldsymbol{O}_{8} ) formed? | 12 |

1204 | Calculate ( E^{ominus} ) for the reactions: ( Z n Y^{2-}+2 e^{-} rightleftharpoons Z n(s)+Y^{4-} ) is the completely deprotonated anion of EDTA. The formation constant for ( Z n Y^{2-} ) is ( 3.5 times ) ( mathbf{1 0}^{mathbf{1 6}} mathbf{a n d} boldsymbol{E}^{ominus} operatorname{for} boldsymbol{Z} boldsymbol{n} rightarrow boldsymbol{Z} boldsymbol{n}^{mathbf{2}+}+mathbf{2} boldsymbol{e}^{-} ) is ( 0.76 mathrm{V} ) A . ( -1.25 V ) B. ( 0.48 V ) ( c .+0.68 V ) D. ( -0.27 V ) | 12 |

1205 | Which one of the following has a potential more than zero? A ( cdot P t, frac{1}{2} H_{2}(operatorname{latm}) mid H C l(1 M) ) в. ( P t_{2} frac{1}{2} H_{2}(1 a t m) mid H C l(2 M) ) c. ( quad P t, frac{1}{2} H_{2}(1 a t m) mid H C l(0.1 M) ) D ( cdot operatorname{Pt}, frac{1}{2} H_{2}(1 text { at } m) mid H C l(0.5 M) ) | 12 |

1206 | Heat of reaction for the change ( Z n+ ) ( boldsymbol{C u}^{2+}(mathbf{0 . 1} boldsymbol{M}) rightarrow boldsymbol{Z} boldsymbol{n}^{2+}(mathbf{1} boldsymbol{M})+boldsymbol{C u} mathbf{a t} ) ( 27^{circ} C ) is: A. ( -2.17 times 10^{5} mathrm{J} ) В. ( -2.29 times 10^{5} mathrm{J} ) c. ( -2.24 times 10^{5} J ) D. ( -1.84 times 10^{5} mathrm{J} ) | 12 |

1207 | The process of giving a coating of to copper or brass is called tinning. A. zinç B. copper ( c . ) tin D. iron | 12 |

1208 | Which of the following reactions is used to make a fuel cell? ( mathbf{A} cdot C d(s)+2 N i(O H)_{3}(s) rightarrow C d O(s)+2 N i(O H)_{2}(s)+ ) ( H_{2} O(l) ) ( mathbf{B} cdot P b(s)+P b O_{2}(s)+2 H_{2} S O_{4}(a q) rightarrow 2 P b S O_{4}(s)+ ) ( 2 H_{2} O(l) ) ( mathbf{c} cdot 2 H_{2}(g)+O_{2}(g) rightarrow 2 H_{2} O(l) ) D. ( 2 F e(s)+O_{2}(g)+4 H^{+}(a q) rightarrow 2 F e^{2+}(a q)+2 H_{2} O(l) ) | 12 |

1209 | The equilibrium constant ( boldsymbol{K}_{c} ) for the reaction: ( boldsymbol{C u}(boldsymbol{s})+boldsymbol{2} boldsymbol{A} boldsymbol{g}^{+}(boldsymbol{a} boldsymbol{q} cdot) rightleftharpoons boldsymbol{C} boldsymbol{u}^{2+}(boldsymbol{a} boldsymbol{q} cdot)+ ) ( mathbf{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s})left(boldsymbol{E}_{c e l l}^{circ}=mathbf{0 . 4 6} boldsymbol{V}right) ) will be: A. antilog 15.6 B. antilog 2.5 c. antilog 1.5 D. antilog 12.2 | 12 |

1210 | Cell constant has unit: A ( cdot s m^{-1} ) B . ( m s^{-1} ) ( mathrm{c} cdot m^{-1} ) D. ( m^{-2} ) | 12 |

1211 | Lead storage cell is a secondary cell. If true enter 1 , else enter 0 | 12 |

1212 | The cell, ( Z nleft|Z n^{2+}(1 M) | C u^{2+}(1 M)right| C u, ) was allowed to be completely discharged at 298 K. The relative concentration of ( Z n^{2+} ) to ( C u^{2+}left(frac{left[Z n^{2+}right]}{left[C u^{2+}right]}right) ) is : ( left[boldsymbol{E}_{c e l l}^{0}=mathbf{1 . 1 0} boldsymbol{V}right] ) ( mathbf{A} cdot 9.65 times 10^{4} ) B . antilog (24.08) c. 37.3 D. ( 10^{37.3} ) | 12 |

1213 | Which of the following statements are true? A. During electrolysis, charge flows through electrolytic solution via electrons. B. The randomly moving electrons in a metal wire will start moving in a particular direction when a potential difference is applied across it. C. A negatively charged particle has higher electric potential than a positively charged particle. D. Charge flows only through negative charge carriers like electrons. | 12 |

1214 | Corrosion occurs due to: a) action of water on the metal. b) action of air on the metal. c) action of temperature on the metal ( A cdot a, b ) в. b, ( c cdot ) а, D. all of the above | 12 |

1215 | The cell constant of a given cell is 0.47 ( c m^{-1} . ) The resistance of a solution placed in this cell is measured to be 31.6 ohm. The conductivity of the solution ( left(text { in } S c m^{-1} text {where } S ) has usual right. meaning) is: A . 0.15 в. 1.5 c. 0.015 D. 150 | 12 |

1216 | The secondary battery is such a battery: A. which cannot be recharged B. which can be recharged C. which can be reused after replacing its chemical D. which is charged by primary cells | 12 |

1217 | For ( boldsymbol{C u}(boldsymbol{s})+boldsymbol{N O}_{3}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow ) ( boldsymbol{C u}^{2+}(boldsymbol{a q})+boldsymbol{N O}_{2}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(l), ) which of the following takes place? A. ( C u(s) ) is oxidized B . ( H^{+}(a q) ) is oxidized c. ( C u(s) ) is reduced D. ( H^{+}(a q) ) is reduced E . ( N O_{3}^{-} ) is oxidized | 12 |

1218 | A half cell reaction: ( boldsymbol{A} boldsymbol{g}_{2} boldsymbol{S}(boldsymbol{s})+boldsymbol{2} boldsymbol{e}^{-} rightarrow ) ( mathbf{3} A boldsymbol{g}(s)+boldsymbol{S}^{2-} ) is carried out in a half ( operatorname{cell} P t_{A g_{2}} s mid A g, H_{2} S(0.1 M) boldsymbol{a t}left[boldsymbol{H}^{oplus}right]= ) ( 10^{-3}, ) The EMF of the half cell is: ( left[boldsymbol{E}_{A boldsymbol{g}^{oplus} mid boldsymbol{A} boldsymbol{g}}^{ominus}=mathbf{0 . 8 0} boldsymbol{V}, boldsymbol{K}_{aleft(boldsymbol{H}_{2} boldsymbol{S}right)}=right. ) ( left.mathbf{1 0}^{-mathbf{2 1}}, boldsymbol{a n d} boldsymbol{K}_{s p} boldsymbol{o} boldsymbol{f} boldsymbol{A} boldsymbol{g}_{2} boldsymbol{S}=mathbf{1 0}^{-49}right] ) ( mathbf{A} cdot-0.1735 V ) в. ( -0.19 V ) c. ( +0.1735 V ) D. ( +0.19 V ) | 12 |

1219 | In moist air, iron is oxidized to give: ( A cdot ) iron ( [I I] ) oxide B. iron ( [I I I] ) oxide c. iron[II] hydroxide D. iron[II] sulphide | 12 |

1220 | During an electrolysis of conc. ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) perdisulphuric acid ( left(boldsymbol{H}_{2} boldsymbol{S}_{2} boldsymbol{O}_{8}right) ) and ( boldsymbol{O}_{2} ) form in equimolar amount. The amount of ( boldsymbol{H}_{2} ) that will form simultaneously will be: ( left(2 H_{2} S O_{4} rightarrow H_{2} S_{2} O_{8}+2 H^{+}+right. ) ( 2 e^{-} ) A. Thrice that of ( mathrm{O}_{2} ) in moles B. Twice that of ( 0_{2} ) in moles c. Equal to that of ( mathrm{O}_{2} ) in moles D. Half of that of ( mathrm{O}_{2} ) in moles | 12 |

1221 | Electrolysis is the passage of electricity through a liquid or a solution accompanied by a chemical change. A. True B. False | 12 |

1222 | 1 g metal ( mathrm{M}^{2+} ) was discharged by the passage of ( 1.81 times 10^{22} ) electrons. What is atomic mass of metal (write answer as the nearest after diving atomic mass by 20)? | 12 |

1223 | Question 1. Arrange the following metals in the order in which they displace each other from the solution of their salts. Al, Cu, Fe, Mg and Zn. Consider the order of reactivity of metals, as a more reactive metal can displace the less reactive metal from its salt solution. | 12 |

1224 | What is an electrochemical series? How is it useful in predicting whether a metal can liberate hydrogen from acid or not? | 12 |

1225 | State True or False. Corrosion of iron is a redox process. A. True B. False | 12 |

1226 | A current of 2 amp when passed for 5 hour through a molten salt deposits ( 22.2 g ) of metal of atomic mass 177 Then calculate the positive oxidation state of the metal in the metal salt. | 12 |

1227 | If fully charged battery contains 1.5 L of ( 5.00 mathrm{M} mathrm{H}_{2} mathrm{SO}_{4} ) in and ( 1.5 mathrm{mol} ) of ( mathrm{H}_{2} mathrm{SO}_{4} ) is consumed, concentration of ( H_{2} S O_{4} ) after current is drawn is: A . 3.50 B. 2.00 M c. ( 4.25 mathrm{M} ) D. 4.00 M | 12 |

1228 | Calculate the current strength which was passed for 15 min to liberated ( 193.11 c m^{3} ) of hydrogen gas at ( 273 K ) and ( 760 m m ) of ( H g ) pressure during electrolysis of acidulated water | 12 |

1229 | The following are some equations about Nernst equations. I) For metal electrode: ( E=E^{0}- ) ( frac{2.303 R T}{n F} log frac{[M]}{left[M^{n+}right]} ) II) For metal electrode: ( E=E^{0}+ ) ( frac{2.303 R T}{n F} log c ) III) For non-metal electrode: ( E=E^{0}- ) ( frac{0.059}{n} log cleft[A^{n-}right] ) IV) For non-metal electrode: ( E=E^{0}- ) ( frac{2.303 R T}{n F} log cleft[A^{n-}right] ) The correct answer is : A. only I and III are correct B. only II and IV are correct C. only I and IV are correct D. all are correct | 12 |

1230 | By process of electrolysis chemical energy gets converted into electrical energy. | 12 |

1231 | In the reaction, ( boldsymbol{2} boldsymbol{A l}(boldsymbol{s})+boldsymbol{6} boldsymbol{H} boldsymbol{C l}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{2} boldsymbol{A} boldsymbol{l}^{3+}(boldsymbol{a} boldsymbol{q} cdot)+ ) ( mathbf{6} C l^{-}left(a q_{cdot}right)+3 H_{2}(g) ) ( mathbf{A} cdot 11.2 H_{2}(g) ) at ( mathrm{STP} ) is produced for every mole of ( H C l(a g .) ) consumed B. 6 LHCl ( (text { ag. }) ) is consumed for every 3 L ( H_{2}(E ) ) produced C ( .33 .6 L H_{2}(g) ) is produced regardless of temperature and pressure for every mole of ( mathrm{Al} ) that reacts D. ( 67.2 L H_{2}(g) ) at SIT is produced for every mac of Al that reacts | 12 |

1232 | A big irregular shaped vessel container water, the specific conductance of which was ( 2.56 times 10^{-5} mathrm{mhocm}^{-1} .500 mathrm{g} ) of ( N a C l ) was the added to the water and the specific conductance after the addition of ( N a C l, ) was found to be ( 3.10 times 10^{-5} mathrm{mhocm}^{-1} . ) The capacity of the vessel if it is fulfilled with water is : ( left(lambda_{infty} N a C l=149.9right) ) B . ( V=2.59 times 10^{6} mathrm{cm}^{-3} ) c. ( V=3.14 times 10^{9} mathrm{cm}^{-3} ) D. none of the above | 12 |

1233 | The technique of protecting a metal from corrosion by connecting it to a second metal (that is more easily oxidised) is called: A. annealing B. galvanisation c. cathodic protection D. anodic protection | 12 |

1234 | The molar conductivity of ( N a C l, H C l ) and ( C H_{3} C O O N a ) at infinite dilution are 126.45,426.16 and ( 91 S c m^{2} m o l^{-1} ) respectively. The molar conductivity of ( C H_{3} C O O H ) at infinite dilution is: A ( .201 .28 S mathrm{cm}^{2} mathrm{mol}^{-1} ) B. ( 698.28 S mathrm{cm}^{2} mathrm{mol}^{-1} ) c. ( 390.71 S mathrm{cm}^{2} mathrm{mol}^{-1} ) D. ( 540.48 S mathrm{cm}^{2} mathrm{mol}^{-1} ) | 12 |

1235 | Assertion The transfer of electrons from zinc to copper takes place through metal wire connecting the two rods. Reason Electricity from solution in one beaker to other flows by migration of ions through the salt bridge. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

1236 | Equivalent conductivity of acetic acid at infinite dilution is ( 390.7 mathrm{mho} mathrm{cm}^{2} mathrm{gm} ) equiv and for ( 0.1 mathrm{M} ) acetic acid is 5.2 mho ( c m^{2} ) gm.equiv ( ^{2} ). Calculate degree of dissociation, ( boldsymbol{H}^{+} ) ion concentration and dissociation constant of the acid. | 12 |

1237 | Q. 60 Assertion (A) Mercury cell does not give steady potentia Reason (R) In the cell reaction, ions are not involved action, ions are not involved in solution. AA is stood | 12 |

1238 | Match the following: | 12 |

1239 | For given half cell; ( A l^{+3}+3 e^{-} rightarrow A l ; ) on increasing ( left[A l^{+3}right], ) the electrode potential: A. Increases B. Decreases c. No change D. First increases then decreases | 12 |

1240 | From the given cells: Lead storage cell, Mercury cell, Fuel cell and Dry cell Answer the following: (i) Which cell is used in hearing aids? (ii) Which cell was used in Apollo Space Programme? (iii) Which cell is used in automobiles and inverters? (iv) Which cell does not have long life? | 12 |

1241 | Which of these half-reactions represents an oxidation? I. ( boldsymbol{S} boldsymbol{n}^{boldsymbol{4}+} rightarrow boldsymbol{S} boldsymbol{n}^{2+} ) II. ( M n O_{4}^{-} rightarrow M n^{2+} ) III. ( boldsymbol{C l}_{2} rightarrow boldsymbol{C l O}_{mathbf{3}}^{-} ) A. I only B. II only c. III only D. I and II only E. II and III only | 12 |

1242 | Which of the following is not true? A. The electrode which pushes electrons into external circuit is known as anode B. The electrode which pulls electrons out of external circuit is known as cathode C. Weak electrolytes conduct relatively small quantity of electricity than strong electrolytes D. Effect of dilution on conductance of strong electrolyte can be explained by Arrhenius theory. | 12 |

1243 | Q. 54 Match the items of Column I and Column II. Column 1 Column II A. Lechlanche cell 1 Cell reaction 2H, +O, — 210 B. Ni-Cd cell 2. Does not involve any ion in solution and is used in hearing aids C. Fuel cell 3. Rechargeable D. Mercury cell 4. Reaction at anode, Zn → Zn²+ + 2e 5. Converts energy of combustion into electrical energy | 12 |

1244 | ( H_{2}-O_{2} ) fuel cell is: A. primary cell B. secondary cell ( c cdot ) both D. cant be predicted | 12 |

1245 | For an electrolyte solution of ( mathbf{0 . 0 5} boldsymbol{M} ) the conductivity has been found to be ( 0.0110 mathrm{S} mathrm{cm}^{-1} . ) The molar conductivity is: A. ( 0.055 mathrm{Scm}^{2} mathrm{mol}^{-1} ) B. ( 550 mathrm{Scm}^{2} mathrm{mol}^{-1} ) c. ( 0.22 mathrm{Scm}^{2} mathrm{mol}^{-1} ) D. ( 220 mathrm{Scm}^{2} mathrm{mol}^{-1} ) | 12 |

1246 | The standard reduction potentials of ( Z n^{2+} mid Z n ) and ( C u^{2+} mid C u ) are ( -0.76 V ) and ( +0.34 mathrm{V} ) respectively. What is the cell EMF of the following cell? ( Z nleft|Z n^{2+}(0.05 M)right|left|C u^{2+}(0.005 M)right| C u ) ( left[frac{R T}{F}=0.059right] ) A . 1.1295 в. 1.0705 V c. 1.1000 D. 1.0412 v | 12 |

1247 | Which solution will conduct the current? A. Sugar in water B. Sugar in ethanol c. lodine in ethanol D. ( M g C l_{2} ) in water | 12 |

1248 | Which of the following energy changes occur in galvanic cell? A. Electrical energy ( rightarrow ) Chemical Energy B. Chemical Energy ( rightarrow ) Electrical Energy C. Chemical Energy ( rightarrow ) Internal Energy D. Internal Energy ( rightarrow ) Electrical Energy | 12 |

1249 | Conductivity of a saturated solution of a sparingly soluble salt ( A B ) at ( 298 K ) is ( 1.85 times 10^{-5} S m^{-1} . ) Solubility product of the salt ( A B ) at ( 298 K ) is : ( left[text { Given } boldsymbol{Lambda}_{boldsymbol{m}}^{o}(boldsymbol{A B})=mathbf{1 4 0} timesright. ) ( left.10^{-4} S m^{2} m o l^{-1}right] ) A. ( 1.32 times 10^{-12} ) В. ( 1.74 times 10^{-12} ) C ( .5 .7 times 10^{-12} ) D. ( 7.5 times 10^{-12} ) | 12 |

1250 | In hydrogen fuel cell the catalyst used ¡s/are: This question has multiple correct options A . ( A g ) в. ( F e ) ( c cdot P t ) D. ( Z n ) | 12 |

1251 | Battery charging equipment is generally installed: A . in well ventilated location B. in clean and dry place. c. as near as practical to the battery being charged D. in location having all above features | 12 |

1252 | In which of the following cells, use of salt bridge to eliminate liquid junction potential is not necessary? A ( cdot P t H_{2}(g)|H C l| A g C l(s) mid A g ) B . ( H gleft|H g_{2} C l_{2}(s)right| K C l )saturated( |H C l(a q)| H_{2}(g) P t ) c. ( Z nleft|Z n S O_{4} | C u S O_{4}right| C u ) D. ( Z nleft|Z n S O_{4}right| F e^{3+}(a q), F e^{2+}(a q) mid P t ) | 12 |

1253 | Conductivity of a solution is affected by: A. addition of water B. process of heating c. addition of acetic acid D. all of the above | 12 |

1254 | ions is lectrode potential for the oxidation of cl Q. 34 Value of standard electrode potential for the oxid more positive than that of water, even then in the ele aqueous sodium chloride, why is Cl- oxidised at anode instead of water? water at | 12 |

1255 | Specific conductance of ( 0.1 mathrm{M} ) NaC solution is ( 1.01 times 10^{-2} ) ohm ( ^{-1} mathrm{cm}^{-1} ) Its molar conductance in ohm ( ^{-1} mathrm{cm}^{2} ) ( m o l^{-1} ) is: A ( cdot 1.01 times 10^{2} ) B . ( 1.01 times 10^{3} ) c. ( 1.01 times 10^{4} ) D. 1.01 | 12 |

1256 | The number of electrons involved in electrode reaction by 1 coulomb charge is: A ( cdot 6.85 times 10^{14} ) B. ( 19.85 times 10^{18} ) c. ( 6.85 times 10^{18} ) D. ( 16.85 times 10^{15} ) | 12 |

1257 | Which of the following statements is true? A. Electrolysis is one of the applications of chemical effects of current B. A metal wire shows chemical effect when a current is passed through it c. Like charges attract each other D. Charge flows only through negative charge carriers | 12 |

1258 | If for the following half-cell reactions: ( boldsymbol{C u}^{2+}+boldsymbol{e}^{-} rightarrow boldsymbol{C u}^{oplus} ) ( boldsymbol{E}^{oplus}=mathbf{1 . 7 7} boldsymbol{V} ) ( boldsymbol{C u}^{2+}+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{C u} ) ( boldsymbol{E}^{ominus}=-mathbf{0 . 3 4} ) The ( E^{ominus} ) of the half-cell reaction will be ( (text { in } V) ) ( boldsymbol{C u}^{oplus}+boldsymbol{e}^{-} rightarrow boldsymbol{C u} ) | 12 |

1259 | How many electrons flow when a current of 5 amperes is passed through a conductor for 200 seconds? A ( cdot 6.25 times 10^{21} ) B. ( 6.025 times 10^{21} ) c. ( 6.25 times 10^{22} ) D. ( 6.025 times 10^{22} ) | 12 |

1260 | Which is correct relation? ( mathbf{A} cdot A_{e q cdot(K O O C cdot C O O N a)}=frac{1}{2} lambda_{K^{+}}+frac{1}{2} lambda_{N a^{+}}+frac{1}{2} lambda_{O X^{2}} ) B. ( A_{e q .(text {KOOC} cdot text {COONa})}=lambda_{K^{+}}+lambda_{N a^{+}}+lambda_{O X^{2-}} ) C ( cdot A_{text {eq. }(text { KOOC } cdot text { COON } a)}=lambda K^{+}+lambda_{N a^{+}}+frac{1}{2} lambda_{O X^{2}-} ) D. ( A_{e q .(text {KOOC} cdot text {COONa})}=frac{1}{2} lambda_{K^{+}}+frac{1}{2} lambda_{N a^{+}}+lambda_{O X^{2}} ) | 12 |

1261 | The equation representing the process by which standard reduction potential of zinc can be defined is ( mathbf{A} cdot Z n^{2+}(s)+2 e^{-} rightarrow Z n ) ( mathbf{B} cdot Z n(g) rightarrow Z n^{2+}(g)+2 e^{-} ) ( mathbf{c} cdot Z n^{2+}(g)+2 e^{-} rightarrow Z n ) D. ( Z n^{2+}(a q .)+2 e^{-} rightarrow Z n(s) ) | 12 |

1262 | A steady current of 10.0 Amps is passed through a nickel production cell of 15 minutes. Which of the following is the correct expression for calculating the number of grams of nickel produced? Note: | 12 |

1263 | The battery is an arrangement of an electrolytic cell connected in series. A. True B. False | 12 |

1264 | The resistance of ( frac{1}{10} mathrm{M} ) solution is ( 2.5 times ) ( 10^{3} ) ohm. What is the molar conductivity of solution? (cell constant= ( 1.25 mathrm{cm}^{-1} ) ) A. 3.5 ohm ( ^{-1} c m^{2} ) mol ( ^{-} ) B. 5.0 ohm ( ^{-1} c m^{2} ) mol ( ^{-} ) c. 2.5 ohm( ^{-1} mathrm{cm}^{2} ) mol ( ^{-1} ) D. 2.0 ohm ( ^{-1} mathrm{cm}^{2} ) mol- | 12 |

1265 | During the charging of lead storage battery, the reaction at anode is represented by: A ( cdot P b^{2+}+S O_{4}^{2-} rightarrow P b S O_{4} ) B . ( P b S O_{4}+2 H_{2} O rightarrow P b O_{2}+S O_{4}^{2-}+4 H^{+}+2 e ) c. ( P b rightarrow P b^{2+}+2 e ) ( mathbf{D} cdot P b^{2+}+2 e rightarrow P b ) | 12 |

1266 | For ( Z n^{2+} / Z n, E^{circ}=-0.76 V, ) for ( boldsymbol{A} boldsymbol{g}^{+} / boldsymbol{A} boldsymbol{g}, boldsymbol{E}^{circ}=mathbf{0 . 7 9 9} boldsymbol{V} . ) The correct statement is: A. the reaction Zn getting reduced Ag getting oxidized is spontaneous B. Zn undergoes reduction and Ag is oxidized C. zn undergoes oxidation Ag gets reduced D. No suitable answer | 12 |

1267 | Q Type your question ( A ) ( B ) ( c ) ect presenta | 12 |

1268 | Which metal is usefull for protection of iron by corrosion? A. Aluminium B. Sodium c. zinc D. copper | 12 |

1269 | Which of the following is an example of simple fuel cell? A. Lead storage battery B. Leclanche cell c. ( H_{2} O_{2} ) D. All of the above | 12 |

1270 | The following are some statements about galvanic cell. 1) The cell reaction will be obtained by summing up the reactions in the two half cells. 2) ( E^{0} ) cell ( =E^{0} ) cathode ( -E_{text {Anode }}^{0} ) 3) ( E_{C e l l}^{0}=E_{text {reduction electrode }}^{0}-E_{text {oxidation electrode }}^{0} ) 4) ( E^{0} ) Cell ( =E^{0}_{L . H . E}-E^{0} R . H . E ) The correct combination is : A. only I and III are correct B. only I and II are correct C. only I,II,III are correct D. all are correct | 12 |

1271 | Solution. Methane (CH) and neu (o Question 15. Explain how rusting of iron is envisaged as setting up of an electrochemical cell. se Rusting of iron is a redox reaction, it involves the oxidation of Fe and Fe* and reduction of O2. | 12 |

1272 | Which one is the most powerful oxidizing agent? ( mathbf{A} cdot C l_{2}+2 e^{-} rightarrow 2 C l^{-}, quad E^{o}=1.36 V ) B. ( N a^{+}+e^{-} rightarrow N a, quad E^{o}=-2.71 V ) ( mathbf{c} cdot M n O_{4}^{-}+2 H_{2} O+3 e^{-} rightarrow M n O_{2}+4 O H^{-}, quad E^{o}= ) ( 0.6 V ) ( mathbf{D} cdot H_{2} O_{2}+2 H^{+}+2 e^{-} rightarrow 2 H_{2} O, quad E^{o}=1.78 V ) | 12 |

1273 | Electrolysis of water to form hydrogen and oxygen gas is called A. precipitation B. oxidation-reduction c. distillation D. hydration E. condensation | 12 |

1274 | Assertion In electrochemical cell, we can not use KCl in the salt bridge if anodic or cathodic compartment consists of ( mathrm{Ag}^{+} ) or ( P b^{2+} ) ion. Reason Salt bridge is employed to maintain the electrical neutrality and to minimize the liquid-liquid junction potential. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion. B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion. C. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

1275 | The ( Delta H ) for the reaction at ( 0^{circ} mathrm{C} ) ( Z n+2 A g C l rightarrow Z n C l_{2}+2 A g ) is -52.05 kcal. If the e.m.f. of the cell is 1.015 volt, the temperature coefficient of the cell at ( 0^{circ} mathrm{C} ) in ( V /^{o} C ) is: A . ( -4.311 times 10^{-4} ) В . ( 2.388 times 10^{-4} ) c. ( 4.311 times 10^{-4} ) D. ( 4.311 times 10^{-5} ) | 12 |

1276 | Chromium metal can be plated out from an acidic solution containing ( boldsymbol{C r} boldsymbol{O}_{3} ) according to the following equation. [ begin{array}{c} boldsymbol{C r} boldsymbol{O}_{3}(boldsymbol{a q})+boldsymbol{6} boldsymbol{H}^{+}+boldsymbol{6} boldsymbol{e}^{-} rightarrow \ boldsymbol{C r}(boldsymbol{s})+boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O} end{array} ] How many grams of chromium will be plated out by 24000 coulombs? A. ( 0.78 g ) B. ( 0.45 g ) c. ( 1.2 g ) D. None of these | 12 |

1277 | Consider the following ( E^{0} ) values: ( E_{F e^{3+} / F e^{2+}}^{0}=+0.77 V ; E_{S n^{2+} / S n}^{0}=-0.14 V ) Under standard conditions the EMF for the reaction ( S n_{(s)}+2 F e_{(a q)}^{3+} rightarrow 2 F e^{2+}_{(a q)}+S n_{(a q)}^{2+} ) is : A . ( 1.68 mathrm{v} ) B . ( 1.40 mathrm{V} ) c. ( 0.91 v ) D. ( 0.63 mathrm{v} ) | 12 |

1278 | Question 17. Consider a cell given below Cu Cu2+||0rCl2, Pt. Write the reactions that occur at anode and cathode. 2+ | 12 |

1279 | The standard reduction potentials of ( boldsymbol{C u}^{2+} / boldsymbol{C u} ) and ( boldsymbol{C u}^{2+} / boldsymbol{C u}^{+} ) are ( boldsymbol{0 . 3 3 7} ) and ( 0.153 mathrm{V} ) respectively. The standard electrode potential of ( C u^{+} / C u ) half cell is: A . ( 0.184 mathrm{v} ) B. ( 0.827 mathrm{V} ) c. ( 0.521 mathrm{v} ) D. ( 0.490 v ) | 12 |

1280 | For the galvanic cell pictured below, determine the electrochemical potential for the system at ( 25^{circ} mathrm{C} ) Note: ( boldsymbol{C u}_{(a q)}^{2+}+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{C u}_{(s)} boldsymbol{E}^{circ}= ) ( mathbf{0 . 3 3 7} mathbf{V} ) ( Z n_{(a q)}^{2+}+2 e^{-} rightarrow Z n_{(s)} E^{circ}=-0.763 V ) A. ( -0.426 V ) В. ( -1.10 v ) ( mathbf{c} .+0.426 V ) D. ( +1.10 v ) | 12 |

1281 | Explain the following terms with one example each. (a) Corrosion (b) Rancidity | 12 |

1282 | What is ( X ), in the following reaction? ( boldsymbol{K} boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{F}_{2} rightarrow boldsymbol{H} boldsymbol{F}+boldsymbol{X} ) A. ( K_{2} S O_{4} ) в. ( K_{2} S_{2} O_{4} ) ( mathbf{c} cdot K_{2} S_{2} O_{3} ) D. ( K_{2} S_{2} O_{8} ) | 12 |

1283 | What is Primary Battery? Give one example. | 12 |

1284 | How many electrons constitute current of one micro ampere in one second? ( mathbf{A} cdot 6.25 times 10^{8} ) B. ( 6.25 times 10^{12} ) ( mathbf{C} cdot 6.25 times 10^{9} ) D. ( 6.25 times 10^{15} ) | 12 |

1285 | Conductivity of ( 2.5 times 10^{-4} ) M methanoic acid is ( 5.25 times 10^{-5} S c m^{-1} . ) Calculate it molar conductivity and degree of dissociation. ( left(text { Given: } boldsymbol{lambda}^{0}left(boldsymbol{H}^{+}right)=right. ) ( mathbf{3 4 9 . 5 s} mathrm{cm}^{2} ) mol ( ^{-1} ) and ( lambda^{0}left(mathrm{HCOO}^{-}right)= ) ( left.50.5 S c m^{2} m o l^{-1}right) ) | 12 |

1286 | Calculate the potential of hydrogen electrode in contact with a solution whose ( p H ) is 10 | 12 |

1287 | For the following sequential reaction ( boldsymbol{E}^{boldsymbol{o}} ) values in volts at ( 298 mathrm{K} ) are given: ( M n O_{4}^{-0.564}^{V} M n O_{4}^{-2}^{2.26 V} ) ( M n O_{2} stackrel{0.95}{rightarrow} M n^{+3} stackrel{1.51 V}{rightarrow} M n^{+2} ) Calculate ( boldsymbol{E}^{o} ) for ( boldsymbol{M} boldsymbol{n} boldsymbol{O}_{boldsymbol{4}}^{-} rightarrow boldsymbol{M} boldsymbol{n}^{+2} ) A. -1.81 volt B. -1.18 volt c. 1.51 volt D. 1.18 volt | 12 |

1288 | When one faraday of electricity is passed through three electrolytic cells containing ( boldsymbol{A} boldsymbol{g}^{+}, boldsymbol{N} boldsymbol{i}^{2+} ) and ( boldsymbol{C} boldsymbol{r}^{3+} ) ions respectively, the deposited ( A g ) (At. mass ( =108), N i(text { At. mass }=59) ) and ( boldsymbol{C r}(boldsymbol{A} boldsymbol{t} . boldsymbol{m} boldsymbol{a} boldsymbol{s} boldsymbol{s}=mathbf{5} boldsymbol{2}) ) are A. ( A g=108 g, N i=29.5 g, C r=17.3 mathrm{g} ) в. ( A g=108 g, N i=59 g, C r=52 g ) c. ( A g=108 g, N i=108 g, C r=17.3 g ) D. ( A g=108 g, N i=29.5 g, C r=166 g ) | 12 |

1289 | What is SHE? Explain its construction and application. | 12 |

1290 | Assertion A greenish layer appears on copper vessels, if left uncleaned. Reason It is due to the formation of a layer of basic copper carbonate. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

1291 | A certain current liberated 0.504 g of hydrogen in 2 hours. How many grams of copper can be liberated by the same current flowing for the same time in copper sulphate solution? A. ( 31.8 mathrm{g} ) B. ( 16.0 mathrm{g} ) c. ( 12.7 mathrm{g} ) D. ( 63.5 mathrm{g} ) | 12 |

1292 | When a lead storage battery is discharged: A. ( S O_{2} ) is evolved B. lead sulphate is consumed ( mathrm{c} ). lead is formed D. sulphuric acid is consumed | 12 |

1293 | ( N_{2}+O_{2}+H e a t rightarrow 2 N O ) ( (g) ) ( boldsymbol{q} ) ( boldsymbol{C}_{(boldsymbol{s})}+boldsymbol{O}_{boldsymbol{2}(boldsymbol{g})} rightarrow boldsymbol{C} boldsymbol{O}_{boldsymbol{2}(boldsymbol{g})}+boldsymbol{Q} ) What information do you get from the above equations ? Comment. Write an activity about how you conduct an experiment to show that more reactive metals replace less reactive metals from their compounds. | 12 |

1294 | In hydrogen evolution type of corrosion with respect to hydrogen electrode which of the following is correct? A. the metal with more negative SRP value under the given conditions B. the metal with more positive SRP value under the given conditions C. the metal with both negative and positive SRP values D. All the above | 12 |

1295 | A solution of ( X S O_{4} ) is electrolyed. When a constant current of 2.0 amperes is applied for 800 minutes, ( 4.5 g ) of the unknown metal X is deposited. Identify the unknown metal, X. A. ( C d ) в. ( B e ) c. ( M g ) D. ( C u ) | 12 |

1296 | During electrolysis, cations move towards the positive terminal. A. True B. False | 12 |

1297 | Electrochemistry 75 Question 10. If a current of 0.5 ampere flows through a metallic wire for 2 h, then how many electrons would flow through the wire? (0) Find charge by using. Q = it. (ii) When charge 1 Faraday (96500 C) flows; number of electrons is equal to 6.022 x102. So, calculate the number of electrons when charge is Qby unitary method. | 12 |

1298 | Which of the following statements is true for fuel cells? A. They are more efficient B. They are free from pollution c. They run till reactants are active D. All of the above | 12 |

1299 | Substance which give good conducting aqueous solution are called: A. weak electrolytes B. strong electrolytes c. non-electrolytes D. catalysts | 12 |

1300 | The weight of silver (At. Wt. = 108) displaced by a quantity of electricity which displaces ( 5600 mathrm{ml} ) of ( O_{2} ) at STP will be A. ( 5.4 mathrm{g} ) B. ( 10.8 mathrm{g} ) c. ( 54.0 mathrm{g} ) D. ( 108.0 mathrm{g} ) | 12 |

1301 | SULLULLLERI LETTULLE Q28. Arrange the following metals in the order in which they displace each other from the solution of their salts. Al, Cu, Fe, Mg and Zn. Ttia bang Tha | 12 |

1302 | Question 2. Given the standard electrode potentials, K/K =-2.93 V, Agt / Ag=0.80 V Hg2+ /Hg = 0.79V, Mg2+ /Mg=-2.37 V, Cr3+/ Cr=-0.74 V Arrange these metals in their increasing order of reducing power. Reducing power & Reduction potential – i.e., as the reduction potential decreases, reducting power increases. So, arrange the given metals on this basis. | 12 |

1303 | A current of ( 10.0 mathrm{A} ) flows for ( 2.00 mathrm{hrs} ) through an electrolytic cell containing a molten salt of metal ( X . ) This results in the decomposition of 0.250 mol of metal ( X ) at the cathode. The oxidation state of ( X ) in the molten salt is: ( (F= ) ( 96500 C) ) ( A cdot+1 ) ( B cdot+2 ) ( c cdot+3 ) ( D cdot+4 ) | 12 |

1304 | According to the Nernst equation, the potential of an electrode changes by ( mathbf{5 9 . 2} boldsymbol{m} boldsymbol{V} ) whenever the ratio of the oxidized and the reduced species changes by a factor of 10 at ( 25^{circ} mathrm{C} ). What would be the corresponding change in the electrode potential if the experiment is carried out at ( 30^{circ} mathrm{C} ) ? A. ( 59.2 mathrm{mV} ) в. ( 71.0 mathrm{mV} ) c. ( 60.2 mathrm{mV} ) D. None of above | 12 |

1305 | What is corrosion? Explain whether gold ornaments corrode or not | 12 |

1306 | Given the standard potential of the following at ( 25^{circ} mathrm{C} . M n O_{2} rightarrow M n^{3+} ) ( boldsymbol{E}^{ominus}=mathbf{0 . 9 5} boldsymbol{V} ) ( M n^{3+} rightarrow M n^{2+} ; E^{ominus}=1.51 V ) The standard potential of ( M n O_{2} rightarrow ) ( M n^{2+} ) is: A. ( -0.56 V ) B . ( -2.46 V ) c. ( -1.23 V ) D. ( 1.23 V ) | 12 |

1307 | How many moles of electrons wil together contribute to the charge of 289500 coulomb? | 12 |

1308 | An electrolytic cell contains a solution of ( A g_{2} S O_{4} ) and has platinum electrodes. A current is passed until ( 1.6 g ) of ( O_{2} ) has been liberated at anode. The amount of silver deposited at cathode will be A. ( 108 g ) B. ( 1.6 g ) ( mathrm{c} .0 .8 mathrm{g} ) D. 21.60 ( g ) | 12 |

1309 | Explain rancidity. | 12 |

1310 | Silver is monovalent and has an atomic mass of ( 108 . ) Copper is divalent and has an atomic mass of ( 63.6 . ) The same electric current is passed, for the same length of time through a silver coulometer and a copper coulometer. If ( 27.0 mathrm{g} ) of silver is deposited, then the corresponding amount if copper deposited is: A. ( 31.80 g ) B. 15.90 g c. ( 7.95 mathrm{g} ) D. none of these | 12 |

1311 | Explain the term with example:Oxidant | 12 |

1312 | What is the other name of ( S H E ? ) A. Concentration cell B. Inactive electrode c. Reference electrode D. Active electrode | 12 |

1313 | Internal resistance of a battery cell decreases with: A. an increase in area of the plates inside the electrolyte B. an increase in distance between the two electrodes c. a decrease in size of the electrodes D. an increase of age of the battery | 12 |

1314 | Given that the standard reduction potentials for ( M^{+} / M ) and ( N^{+} / N ) electrodes at ( 298 K ) are ( 0.52 V ) and ( 0.25 V ) respectively. Which of the following is correct in respect of the following electrochemical cell? ( boldsymbol{M}left|boldsymbol{M}^{+} | boldsymbol{N}^{+}right| boldsymbol{N} ) A. The overall cell reaction is a spontaneous reaction B. The standard EMF of the cell is ( -0.27 V ) c. The standard EMF of the cell is ( 0.77 V ) D. The standard EMF of the cell is ( -0.77 V ) E. The standard EMF of the cell is ( 0.27 V ) | 12 |

1315 | In producing chlorine through electrolysis 100 watt power at 125 V is being consumed. How much chlorine per minute is liberated? Electrochemical Equivalent of chlorine is ( 0.367 times 10^{-6} ) kg/coulomb: | 12 |

1316 | Write two methods of preventing the rusting of iron | 12 |

1317 | Calculate the standard oxidation potentials of zinc electrode form the following data. The EMF of the cell : ( boldsymbol{L} boldsymbol{i}|boldsymbol{L} boldsymbol{i} oplus(mathbf{0 . 0 5} boldsymbol{M}) | boldsymbol{A} boldsymbol{n}| boldsymbol{Z} boldsymbol{n}^{2+}(boldsymbol{0} . boldsymbol{5} boldsymbol{M}), boldsymbol{E} ) ( -3.045 V, ) is ( 2.35 mathrm{V} ) at ( 25^{circ} mathrm{C} ) | 12 |

1318 | Why do caesium ( (C s) ) and potassium ( K ) ) find applications in photoelectric cells? | 12 |

1319 | The molar conductivities of ( boldsymbol{K} boldsymbol{C} boldsymbol{I} ) ( N a C l ) and ( K N O_{3} ) are 152,128 and ( 111 S c m^{2} m o l^{-1} ) respectively. What is the molar conductivity of ( N a N O_{3} ? ) A ( cdot 101 S mathrm{cm}^{2} mathrm{mol}^{-1} ) B. ( 87 S mathrm{cm}^{2} mathrm{mol}^{-1} ) c. ( -101 S mathrm{cm}^{2} mathrm{mol}^{-1} ) D. ( -391 S mathrm{cm}^{2} mathrm{mol}^{-} ) | 12 |

1320 | topp Tropovur precipitation. Which of the following netric titration vs NaO axis ( Rightarrow ) Volume of alkali adde y-axis ( Rightarrow ) conductivity | 12 |

1321 | State Faraday’s first law of electrolysis. | 12 |

1322 | Which of the following indicates that a potato is a conductor of electricity? A. Greenish blue spot on potato around one wire. B. Greenish blue spot on potato around both wires. c. Blue color spot on potato around one wire. D. Blue color spot on potato around both wires | 12 |

1323 | When electric current is passed through water, hydrogen is deposited over: A. positive pole B. negative pole c. no dissociation D. both the poles | 12 |

1324 | In a cell that utilizes the reaction ( Z n(s) ) ( +2 H^{+}(a q) rightarrow Z n^{2+}(a q)+H_{2}(g) ) addition of ( mathbf{H}_{2} mathbf{S} mathbf{O}_{4} ) to cathode compartment, will: A. lower the E and shift equilibrium to the left B. lower the E and shift the equilibrium to the right c. increase the ( mathrm{E} ) and shift the equilibrium to the right D. increase the E and shift the equilibrium to the left | 12 |

1325 | Primary battery is a battery: A. which can be recharged. B. which cannot be reconditioned by replacing chemical. c. which cannot be reused. D. which cannot be recharged. | 12 |

1326 | The standard electrode potentials of ( Z n ) and ( N i ) respectively are ( -0.76 mathrm{V} ) and ( -0.25 mathrm{V} . ) Then the standard emf of the spontaneous cell by coupling these under standard conditions is: ( A cdot+1.01 v ) B. – 0.51 V ( c cdot+0.82 v ) ( D cdot+0.25 v ) ( mathrm{E} cdot+0.51 mathrm{v} ) | 12 |

1327 | Number of faradays required to convert 1 mole of ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-} ) into ( boldsymbol{C r}^{mathbf{3}+} ) ions is ( A cdot 6 ) B. 4 ( c cdot 3 ) D. none of these | 12 |

1328 | Total charge required for the oxidation of two moles ( M n_{3} O_{4} ) in to ( M n O_{4}^{2-} ) in presence of alkaline medium is: A. ( 5 F ) в. 10F c. २० D. None of these | 12 |

1329 | Question 12. Unlike dry cell, the mercury cell has a constant cell potential throughout its useful life why? | 12 |

1330 | The potential of the cell at ( 25^{circ} mathrm{C} ) is Given ( p K_{a} ) of ( C H_{3} C O O H ) and ( p K_{b} ) of ( N H_{4} O H=4.74 ) A . ( -0.04 V ) В. ( 0.04 V ) ( c .-0.189 V ) ( V ) D. ( 0.189 V ) | 12 |

1331 | When electric current is passed through water, the dissociation is indicated A. in the form of bubbles B. by color change ( c . ) both a and ( b ) D. none of above | 12 |

1332 | A constant voltage is applied between the two ends of a uniform metallic wire. Some heat is developed in it. The heat developed is double if: A. both the length and radius of wire are halved B. both length and radius of wire are doubled c. the radius of wire is doubled D. the length of the wire is doubled | 12 |

1333 | A flash light cell reaction is : ( mathbf{2} M n O_{2}+Z n^{2+}+2 e^{-} longrightarrow Z n+ ) ( M n_{2} O_{4} . ) The current rating of the flashlight is ( 4.6 mathrm{mA} ). The time for which we can use this light, if we start with 3.5 g of ( M n O_{2} ) is: A ( .8 .44 times 10^{5} s ) B. ( 8.76 times 10^{5} s ) c. ( 8.96 times 10^{5} s ) D. None of these | 12 |

1334 | On passing ( 1.5 F ) charge, the number of moles of aluminum deposited at the cathode is: [Molar mass of ( boldsymbol{A l}=mathbf{2 7} ) gram mol ( ^{-1} ) ] A . 1.0 в. 13.5 c. 0.50 D. 0.75 | 12 |

1335 | Assertion n electrolysis, the quantity of electricity needed for depositing 1 mole of silver is different from that required for 1 mole of copper. Reason The molecular weights of silver and copper are different. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Both Assertion and Reason are incorrect | 12 |

1336 | What is Kohlrausch’s law? | 12 |

1337 | Which of the following statement(s) is correct while conducting electricity through vegetable oil? A. The liquid (vegetable oil) allows the electric current to pass through. since, it is a good conductor of electricity. B. The circuit of the tester is complete but the bulb does not glow. c. The circuit of the tester is not complete and hence the bulb does not glow. D. Both A and B | 12 |

1338 | If mercury is used as cathode in the electrolysis of aqueous NaCl solution, the ions discharged at cathode are: ( mathbf{A} cdot mathbf{H}^{mathbf{t}} ) B. Nat c. он D. cᅵ | 12 |

1339 | Consider the following half-cell reactions and associated standard half- cell potentials and determine the maximum voltage that can be obtained by combination resulting in spontaneous processes: ( boldsymbol{A u} boldsymbol{B r}_{4}^{-}(boldsymbol{a q})+boldsymbol{3} boldsymbol{e}^{-} rightarrow boldsymbol{A u}(boldsymbol{s})+ ) ( 4 B r^{-}(a q) ; E^{circ}=-0.86 V ) ( boldsymbol{E} boldsymbol{u}^{3+}(boldsymbol{a} boldsymbol{q})+boldsymbol{e}^{-} rightarrow boldsymbol{E} boldsymbol{u}^{2+}(boldsymbol{a} boldsymbol{q}) ; boldsymbol{E}^{circ}= ) ( -0.43 V ) ( boldsymbol{S} boldsymbol{n}^{2+}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{S} boldsymbol{n}(boldsymbol{s}) ; boldsymbol{E}^{circ}= ) ( -0.14 V ) ( boldsymbol{I O}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{H}_{2} boldsymbol{O}(l)+boldsymbol{2} boldsymbol{e}^{-} rightarrow ) ( boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{O} boldsymbol{H}^{-}(boldsymbol{a} boldsymbol{q}) ; boldsymbol{E}^{circ}=+mathbf{0 . 4 9} boldsymbol{V} ) ( mathbf{A} cdot+0.72 ) B. +1.54 c. +1.00 D. +1.35 | 12 |

1340 | Rusting of iron is prevented by A. applying paint B. keeping in contact with water c. keeping in contact with oxygen D. reacting with acid | 12 |

1341 | Coulomb is an unit of charge while ampere is the rate at which it flows. If true enter 1 , else enter 0 . | 12 |

1342 | Pure water is a ( -=—— ) conductor of electricity. A. good B. bad c. semi D. none of the above | 12 |

1343 | A current of ( 4.0 mathrm{A} ) is passed for 5 hours through 1L of 2M solution of nitrate using two nickel electrodes. The molarity of the solution at the end of the electrolysis will be: A . 1.5 м в. 1.2 c. ( 2.5 mathrm{M} ) D. 2.0 M | 12 |

1344 | requires a salt bridge. A. Voltaic cell B. Electrolytic cell C . Geiger counter D. pH meter E . Calorimeter | 12 |

1345 | Electrolysis of dilute aqueous ( mathrm{NaCl} ) solution was carried out by passing 10 milli ampere current. The time required to liberate 0.01 mol of ( mathbf{H}_{2} ) gas at the cathode is (1 Faraday ( =mathbf{9 6 5 0 0 C} ) mol ( ^{-1} ) ) A ( cdot 9.65 times 10^{4} mathrm{sec} ) B . ( 19.3 times 10^{4} mathrm{sec} ) c. ( 28.95 times 10^{4} ) sec D. ( 38.6 times 10^{4} mathrm{sec} ) | 12 |

1346 | Which of the following equations are correctly represented for ( 0.10 mathrm{M} ) solution of acetic acid in water? ( mathbf{A} cdot[H O A c]=[H O A c c]_{e q .}+left[O A c^{-}right]_{e q .}=0.10 mathrm{M} ) B . ( left[H^{+}right]_{e q .}=left[O A c^{-}right]_{e q .}+left[O H^{-}right]_{e q} ) ( mathbf{c} cdotleft[H^{+}right]>left[O H^{-}right] ) D. All of the above | 12 |

1347 | At ( 25^{circ} C ), the standard emf of a cell having reaction involving two electrons change is found to be ( 0.295 V ). The equilibrium constant of the reaction is ( mathbf{A} cdot 29.5 times 10^{-2} ) B. 10 ( c cdot 1 times 10^{10} ) 0 D . ( 29.5 times 10^{10} ) | 12 |

1348 | In which of the following the corrosion of iron will be most rapid? A. In pure water B. In pure oxygen C. In air and moisture D. In air and saline water | 12 |

1349 | Cathodic standard reduction potential minus anodic standard reduction potential is equal to: A. Faraday B. Coulomb c. cell potential D. Ampere | 12 |

1350 | The standard free energies of formation of ( boldsymbol{H}_{2} boldsymbol{O}_{(l)}, boldsymbol{C} boldsymbol{O}_{2}(g) ) an n-pentane are ( -237.2 k J,-394.4 k J,-8.2 k J . ) Then the value of ( E^{0} ) for pentane-oxygen fuel cell is: A . ( 1.1 V ) в. ( 0.1 V ) ( c .2 .0 V ) D. 2.3V | 12 |

1351 | What is standard hydrogen electrode? How is it prepared? Explain with labelled diagram? | 12 |

1352 | Expalin the following: The ( E^{o} c u^{21} / c u ) for copper metal is positive ( (+0.34), ) unlike the remaining members of the first transition series | 12 |

1353 | The unit of conductance is and that of specific conductance is ( mathbf{A} cdot operatorname{oh} m^{-1} ; o h m^{-1} c m^{2} ) B . ( o h m^{-1} c m^{2} ; ) ohm ( ^{-1} c m^{-1} ) ( mathbf{c} cdot o h m^{-1} c m^{-1} ; o h m^{-1} c m^{2} ) D. ( o h m^{-1} ; o h m^{-1} c m^{-1} ) | 12 |

1354 | Galvanizing is a process of coating iron with a metal to prevent it from rusting. The metal is: A . tin B. zinç c. copper D. silver | 12 |

1355 | At ( 25 C ) molar conductance of 0.1 molar aqueous solution of ammonium hydroxide is 9.54 ohm ( ^{1} c m^{2} ) mol ( ^{1} ) and at infinite dilution its molar conductance is 238 ohm ( ^{1} mathrm{cm}^{2} ) mol ( ^{1} ). The degree of ionisation of ammonium hydroxide at the same concentration and temperature is: A. ( 2.080 % ) B. 20.800 % c. 4.008 % D. ( 40.800 % ) | 12 |

1356 | Assertion The cell potential of mercury cell is ( 1.35 V, ) which remains constant. Reason In mercury cell, the electrolyte is a paste of ( K O H ) and ( Z n O ) | 12 |

1357 | After electrolysis of a sodium chloride solution with inner electrodes for a certain period of time, ( 600 mathrm{mL} ) of the ( 1 mathrm{N} ) solution was left which was found to be NaOH. During the same time 31.80 g of Cu was deposited in copper voltameter in series with the electrolytic cell. The % yield of NaOH obtained will be: (Atomic mass of ( C u=63.6 .) ) | 12 |

1358 | Explain corrosion on the basis of following points : (i) Definition (ii) Factors affecting any two (iii) Prevention of corrosion any two | 12 |

1359 | Assertion Reason A. assertion is true, reason is true; reason is correct explanation for assertion. B. assertion is true, reason is true; reason is NOT a correct explanation for assertion. C. assertion is true, reason is false. D. assertion is false, reason is true. | 12 |

1360 | The standard reduction potentials ( boldsymbol{E}^{circ} ) for ( boldsymbol{O C l}^{-} / boldsymbol{C l}^{-} ) and for ( boldsymbol{C l}^{-} / mathbf{1} / mathbf{2 C l}_{2} ) are ( 0.86 V ) and -1.10 volt respectively. The ( boldsymbol{E}^{circ} ) value of ( boldsymbol{O C l}^{-} / mathbf{1} / mathbf{2} boldsymbol{C l}_{mathbf{1}} ) will be ( boldsymbol{?} ) ( mathbf{A} cdot+1.96 V ) B . ( -1.96 V ) c. ( +0.24 V ) D. ( -0.24 V ) | 12 |

1361 | Explain normal or standard hydrogen electrode. | 12 |

1362 | When electricity is passed through a solution of ( A l C l_{3}, 13.5 ) g of Al are deposited. The number of Faradays of electricity passed is: ( write your answer to nearest integer) | 12 |

1363 | Which cell of the following will measure standard electrode potential of copper electrode? A ( cdot P t_{(s)}left|H_{2}(g, 0.1 b a r)right| H^{+}(a q, 1 M) | C u^{2+}(a q, 1 M) mid C u ) B . ( P t_{(s)}left|H_{2}(g, 1 b a r)right| H^{+}(a q, 1 M)|| C u^{2+}(a q, 2 M) mid C u ) C ( cdot P t_{(s)}left|H_{2}(g, 1 b a r)right| H^{+}(a q, 1 M)|| C u^{2+}(a q, 1 M) mid C u ) D. ( P t_{(s)}left|H_{2}(g, 1 b a r)right| H^{+}(a q, 0.1 M)|| C u^{2+}(a q, 1 M) mid C u ) | 12 |

1364 | Using the information in the preceding problem, calculate the solubility product of ( A g I ) in water at ( 25^{0} C ) ( left[boldsymbol{E}_{boldsymbol{A} boldsymbol{g}^{+}, boldsymbol{A} boldsymbol{g}}^{boldsymbol{o}}=+mathbf{0 . 7 9 9} quad boldsymbol{v o l t}right] ) A ( cdot 1.97 times 10^{-17} ) В. ( 7.91 times 10^{-17} ) c. ( 1.79 times 10^{-17} ) D. ( 9.17 times 10^{-17} ) | 12 |

1365 | Assertion: The standard potential of ( boldsymbol{C l}^{ominus}|boldsymbol{A} boldsymbol{g} boldsymbol{C l}| boldsymbol{A} boldsymbol{g} ) half cell is related to that of ( boldsymbol{A} boldsymbol{g}^{ominus} mid boldsymbol{A} boldsymbol{g} ) Reason: ( boldsymbol{E}_{boldsymbol{A} boldsymbol{g}^{ominus} mid boldsymbol{A} boldsymbol{g}}^{ominus}=boldsymbol{E}_{C l^{ominus}|A boldsymbol{g} C l| boldsymbol{A} boldsymbol{g}}^{ominus}+frac{boldsymbol{R} boldsymbol{T}}{boldsymbol{F}} ln boldsymbol{K}_{s p} ) ( (A g C mid) ) A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

1366 | To protect iron from corrosion and rust, it is coated by: A. Tin B. Copper c. zinc D. Mercury | 12 |

1367 | In the manufacture of ( A l, A l_{2} O_{3} ) is dissolved in ( N a_{3} A l F_{6} ) at ( 300 K ) and electrolysed between ( A l ) and carbon electrodes following the net reaction, ( mathbf{2} boldsymbol{A} boldsymbol{l}_{2} boldsymbol{O}_{3}(boldsymbol{s} boldsymbol{o l u t i o n})+boldsymbol{3} boldsymbol{C} rightarrow boldsymbol{4} boldsymbol{A l}(l)+ ) ( mathbf{3} boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) ) The minimum voltage required between the electrodes if the Gibbs energy change for the above reaction is -1370 ( k J m o l^{-1} ) is ( _{-1} ) (write nearest integer) | 12 |

1368 | A lead storage battery has initially ( 200 g ) of lead and ( 200 g ) of ( P b O_{2}, ) plus excess ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} . ) How long could this cell deliver a current of 10 amp, without recharging, if it was possible to operate it so that the reaction goes to completion? A. 2.48 hour B. 3.48 hour c. 4.48 hour D. 6.48 hour | 12 |

1369 | A solution containing ( boldsymbol{N} boldsymbol{a}^{oplus}, boldsymbol{N} boldsymbol{O}_{3}^{ominus}, boldsymbol{C l}^{ominus} ) and ( S O_{4}^{2-} ) ions, all at unit concentrations, is electrolyzed between nickel anode and plantinum cathode. As the current is passed through the cell : This question has multiple correct options A. pH of the cathode increases B. Oxygen is the major product at anode c. Nickel is deposited at cathode D. Chlorine is the maior product at anode | 12 |

1370 | Question 12. Consider the reaction, Cr 0- +14H+ + 6e 2 Cr3+ + 7H,0 What is the quantity of electricity in coulombs needed to reduce 1 mole of Cr2O ? | 12 |

1371 | The number of electrons delivered at the cathode during electrolysis by a current of 1 ampere in 60 seconds is : (charge on an electron is ( 1.60 times ) ( left.10^{-19} Cright): ) ( mathbf{A} cdot 3.75 times 10^{20} ) B . ( 7.48 times 10^{23} ) ( c cdot 6 times 10^{23} ) D. ( 6 times 10^{20} ) | 12 |

1372 | Given the standard half-cell potentials ( left(E^{o}right) ) of the following as ( Z n=Z n^{2+}+2 e^{-} ; quad E^{o}=+0.76 mathrm{V} ) ( boldsymbol{F e}=boldsymbol{F} boldsymbol{e}^{2+}+boldsymbol{2} boldsymbol{e}^{-} ; quad boldsymbol{E}^{o}=+mathbf{0 . 4 1} mathbf{V} ) Then the standard e.m.f. of the cell with the reaction ( boldsymbol{F e}^{2+}+boldsymbol{Z n} rightarrow boldsymbol{Z n}^{2+}+boldsymbol{F e} ) is? A . ( -0.35 v ) B. ( +0.35 v ) c. ( +1.17 v ) D. ( -1.17 v ) | 12 |

1373 | What two metals are often used in electrochemical cells? A. zinc and copper B. Zinc and sulfur c. carbon and copper D. zinc and carbon E. Sulfur and copper | 12 |

1374 | Cadmium amalgam is prepared by electrolysis of a solution of ( C d C l_{2} ) using a mercury cathode. Find how long a current of 5 ampere should be passed in order to prepare ( 12 % C d-H g ) amalgam on a cathode of ( 2 g ) mercury. At. mass of ( C d=112.40 ) | 12 |

1375 | The standard reduction potential at ( 25^{circ} mathrm{C} ) of the reaction ( 2 H_{2} O+2 e^{-} rightleftharpoons ) ( H_{2}+2 stackrel{ominus}{O} H ) is ( -0.8277 mathrm{V} . ) The equilibrium constant for the reaction ( 2 H_{2} O rightleftharpoons H_{3} O^{oplus}+stackrel{ominus}{O} ) at ( 25^{circ} C ) is: A ( cdot K_{w}=9.35 times 10^{-15} ) В. ( K_{w}=9.83 times 10^{-15} ) C . ( K_{w}=9.14 times 10^{-15} ) D. None of these | 12 |

1376 | Which substances are needed for iron to rust? A. Carbon dioxide and oxygen B. Oxygen only c. water and carbon dioxide D. water and oxygen | 12 |

1377 | If a salt bridge is not used between two half cells, what happens to the voltage? A. Drops to zero B. Does not change c. Increases gradually D. Increases rapidly | 12 |

1378 | The electrolysis of molten NaOH liberates ( 0_{2} ) at anode. If true enter 1 , else enter 0 . | 12 |

1379 | ( K C l ) is used in salt bridge because: A. it forms a good jelly with agar-agar B. it is a strong electrolyte c. it is a good conductor of electricity D. the transference number of ( K^{+} ) and ( C l^{-} ) ions are almost equal | 12 |

1380 | ven in Column I with the items given in Column II. Α. Λm Q.51 Match the terms given in Column I with the Column 1 Column II 1. Intensive property 2. Depends on number of ions/volume 3. Extensive property Increases with dilution B. Ecell D A , Gcell | 12 |

1381 | For which cell e.m.f. is independent of the concentrations of electrolytes used? ( mathbf{A} cdot F e|F e O(s)| K O H(a q)|N i O(s)| N i_{2} O_{3}(s) mid N i ) ( mathbf{B} cdot P tleft(H_{2}right)|H C l| P tleft(C l_{2}right) ) ( mathbf{c} cdot Z nleft|Z nleft(N O_{3}right)_{2}right|left|C u S O_{4}right| C u ) D. ( H g, H g C l_{2}left|K C l | A g N O_{3}right| A g ) | 12 |

1382 | Q17. How can CuSo solution not be stored in an iron vessel? 27 | 12 |

1383 | Which among the following metals is employed to provide cathodic protection to iron? A. zinc B. Nickel ( c . ) Tin D. Lead | 12 |

1384 | The cell potential of ( mathbf{A} mathbf{g}|mathbf{A} mathbf{g} mathbf{B} mathbf{r}(mathbf{s})| mathbf{H} mathbf{B} mathbf{r}_{(0.02 mathrm{M})}left|mathbf{H}_{mathbf{2}(mathbf{0 . 5} mathrm{atm})}right| mathbf{P} mathbf{t}(mathbf{G} mathbf{i} ) is: A . ( 0.26 v ) B. -0.26V c. ( 0.16 v ) D . -0.16v | 12 |

1385 | For a cell reaction ( 2 H_{2}(g)+O_{2}(g) longrightarrow ) ( 2 H_{2} O(l) ; triangle_{r} S_{298}^{circ}=-0.32 k J / K . ) What is the value of ( triangle_{f} H_{298}^{circ}left(H_{2} O, lright) ? ) Given ( quad O_{2}(g)+4 H^{+}(a q .)+4 e^{-} longrightarrow ) ( 2 H_{2} O(l) ; quad E^{0}=1.23 V ) A. ( -285.07 k J / ) mol в. ( -570.14 mathrm{kJ} / mathrm{mol} ) c. ( 285.07 k J / ) mol D. None of these | 12 |

1386 | Select correct statement. A. In lead storage battery, galvanic cells are linked in series B. Cathode and anode compartments are not separated in a battery as oxidizing agents and reducing agents both are solids C. Recharging of storage battery is a non spontaneous process D. All are correct statements | 12 |

1387 | Question 21. Why on dilution the Am of CH3COOH increases drastically, while that of CH3COONa increases gradually? | 12 |

1388 | ( Z nleft|Z n^{2+}(a q)right|left|C u^{2+}(a q)right| C u . E^{o} ) for ( C u ) and ( Z n ) are 0.35 and -0.76 respectively: Find EMF of cell (nearest integer) if ( Z n^{2+} ) and ( C u^{2+} ) are 1 M each. | 12 |

1389 | The specific conductance of a ( 0.1 N K C l ) solution at ( 23^{circ} C ) is 0.0112 oh ( m^{-1} c m^{-1} . ) The resistance of the cell containing the solution at the same temperature was found to be ( mathbf{5 5} ) ohm. The cell constant will be: A. ( 0.142 mathrm{cm}^{-1} ) B. ( 0.918 mathrm{cm}^{-1} ) c. ( 1.12 mathrm{cm}^{-1} ) D. ( 0.616 mathrm{cm}^{-1} ) | 12 |

1390 | Assertion ( left(H_{2}+O_{2}right) ) fuel cell gives a constant voltage throughtout its life. Reason In this fuel cell, ( H_{2} ) reacts with ( stackrel{ominus}{O H} ) ions, yet the over all ( [stackrel{ominus}{O} boldsymbol{H}] ) does not change. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

1391 | Which of the following is an additive property? A. conductance B. Viscosity c. Surface tension D. None of these | 12 |

1392 | Which of the following has the highest oxidation potential? A. ( N a ) в. ( A g ) c. ( A l ) D. ( Z ) n | 12 |

1393 | Same quantity of electricity being used to liberate iodine (at anode) and a metal (at cathode). The mass of metal liberated at cathode is 0.617 g and the liberated iodine completely reduced by ( 46.3 mathrm{ml} ) of ( 0.124 mathrm{M} ) sodium thiosulphate solution. What is equivalent weight of metal? A . 23 ( g ) в. ( 127 mathrm{g} ) c. ( 108 mathrm{g} ) D. 46 | 12 |

1394 | In an electrochemical cell, cathode is: A. always neutral B. always positive C. the electrode at which reduction takes place D. always negative | 12 |

1395 | What is the difference between galvanic cell and electrolytic cell? A. In galvanic cell, electrical energy is produced while in electrolytic cell electrical energy is consumed B. In galvanic cell, anode is (-) ve while in electrolytic cell anode is ( (+) ) ve c. In galvanic cell, cathode is ( (+) ) ve while in electrolytic cell anode is ( (-) v e ) D. All are correct | 12 |

1396 | If same quantity of electricity is passed through three electrolytic cells containing ( boldsymbol{F} boldsymbol{e} boldsymbol{S} boldsymbol{O}_{4}, boldsymbol{F} boldsymbol{e}_{2}left(boldsymbol{S} boldsymbol{O}_{4}right)_{3}, ) and ( boldsymbol{F} boldsymbol{e}left(boldsymbol{N} boldsymbol{O}_{3}right)_{3}, ) then: This question has multiple correct options A. the amount of iron deposited in ( F e S O_{4} ) and ( F e_{2}left(S O_{4}right)_{3} ) are equal B. the amount of iron deposited in ( F e S O_{4} ) is 1.5 times of the amount of iron deposited in ( F eleft(N O_{3}right)_{3} ) C. the amount of iron deposited in ( F eleft(S O_{4}right)_{3} ) and ( F eleft(N O_{3}right)_{3} ) are equal D. the same amount of gas is evolved in all three cases of the anode. | 12 |

1397 | Which of the following methods is employed to prevent rusting? A. Annealing B. Alloying c. Enamelling D. both (b) and (c) | 12 |

1398 | If the cell voltage is 1.23 V for the ( H_{2}-O_{2} ) fuel cell and for the half cell : ( O_{2}+2 H_{2} O+4 e^{-} rightleftharpoons 4^{ominus} H ) ( boldsymbol{E}^{ominus}=mathbf{0 . 4 0} boldsymbol{V}, ) then ( boldsymbol{E}^{ominus} ) for ( boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}+ ) ( mathbf{2} e^{-} rightleftharpoons boldsymbol{H}_{2}+mathbf{2} stackrel{ominus}{O} boldsymbol{H} ) will be: ( mathbf{A} cdot 0.56 V ) в. ( 0.73 V ) c. ( 0.41 V ) D. ( 0.83 V ) | 12 |

1399 | Q. 13 The quantity of charge required to obtain one mole of aluminium from AL203 is ………. (b) 6 F (c) 3 F (a) 1 F (d) 2 F . | 12 |

1400 | A secondary cell is one that: A. can be recharged B. can be recharged by passing current through it in the same direction C. can be recharged by passing current through it in the opposite direction D. can not be recharged | 12 |

1401 | Which of the following units is correctly matched? A. SI units of conductivity is ( S m^{-1} ) B. ( S I ) units of molar conductivity is ( S mathrm{cm}^{2} mathrm{mol}^{-1} ) c. ( S I ) unit of conductance is ( S^{-1} ) D. All of these | 12 |

1402 | The rusting of iron takes place as follows: ( mathbf{2} boldsymbol{H}^{oplus}+mathbf{2} e^{-}+frac{mathbf{1}}{mathbf{2}} boldsymbol{O}_{2} rightarrow ) ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ; boldsymbol{E}^{ominus}=+mathbf{1} cdot boldsymbol{2} boldsymbol{3} boldsymbol{V} ) ( boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{e}^{-} rightarrow boldsymbol{F} boldsymbol{e}(s) ; boldsymbol{E}^{ominus}= ) ( -0.44 V ) Calculate ( Delta G^{ominus} ) for the net process. B. ( -152 k J ) mol( ^{-1} ) c. ( -76 k J ) mol ( ^{-1} ) D. – ( 161 k J ) mol ( ^{-1} ) | 12 |

1403 | The specific conductance of a saturated solution of silver bromide is ( kappa mathbf{S} mathrm{cm}^{-1} ) The limiting ionic conductivity of ( A g^{+} ) and ( B r^{-} ) ions are ( x ) and ( y ) respectively. The solubility of silver bromide in ( mathrm{gL}^{-1} ) is: [molar mass of ( mathrm{AgBr}=188 ) A. ( frac{kappa times 100}{x-y} ) B. ( frac{kappa}{x+y} times 188 ) c. ( frac{kappa times 1000 times 188}{x+y} ) D. ( frac{x times y}{kappa} times frac{1000}{188} ) | 12 |

1404 | At what ( frac{left[boldsymbol{B r}^{+}right]}{sqrt{left[boldsymbol{C O}_{3}^{2-}right]}} ) does the following cell have its reaction at equilibrium? ( boldsymbol{A} boldsymbol{g}(boldsymbol{s})left|boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C} boldsymbol{O}_{3}(boldsymbol{s})right| boldsymbol{N} boldsymbol{a}_{2} boldsymbol{C O}_{3}(boldsymbol{a} boldsymbol{q}) | boldsymbol{K} boldsymbol{B} boldsymbol{r} ) ( boldsymbol{K}_{s p}=mathbf{8} times mathbf{1 0}^{-12} ) for ( boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C} boldsymbol{O}_{2} ) and ( boldsymbol{K}_{s p}=mathbf{4} times mathbf{1 0}^{-13} ) for AgBr. A. ( sqrt{1} times 10^{-7} ) B . ( sqrt{2} times 10^{-7} ) c. ( sqrt{3} times 10^{-7} ) D. ( sqrt{4} times 10^{-7} ) | 12 |

1405 | If the molar conductance values of ( C a^{2+} ) and ( C l^{-} ) at infinite dilution are respectively ( 118.88 times ) ( 10^{-4} m^{2} ) mho mol ( ^{-1} ) and ( 77.33 times ) ( 10^{-4} m^{2} ) mho mho ( ^{-1} ) then that of ( C a C l_{2} ) is: A . ( 118.88 times 10^{-4} ) B . ( 154.66 times 10^{-4} ) c. ( 273.54 times 10^{-4} ) D. ( 196.21 times 10^{-4} ) | 12 |

1406 | What happens when the current passing through the circuit is too weak? A. The filament does not get heated sufficiently and the bulb does not glow. B. The filament gets heated but the bulb does not glow c. The filament does not get heated but the bulb glows D. The filament gets heated and the bulb glows | 12 |

1407 | The internal resistance of a dry cell is of the order of: A. 0.2 to 0.4 ohm. B. 1 to 1.4 Ohm. c. 2 to 5 ohm. D. 1 to 15 Ohm. | 12 |

1408 | Which of the following statements are correct regarding the galvanic cell? This question has multiple correct options A. A reaction is spontaneous from left to right if ( E_{text {cell}}>0 ) B. A reaction occurs from right to left if ( E_{text {cell}}<0 ) C. If the system is at equilibrium no net reaction occurs D. ( E_{text {cell}} ) is temperature-independent | 12 |

1409 | By virtue of Faradays second law of electrolysis, the electrochemical equivalent of the two metals liberated at the electrodes has the same ratio as that of their: A. Atomic masse B. Molecular masses c. Equivalent masses D. All the above | 12 |

1410 | The graph of ( sqrt{C} ) vs ( Lambda_{m} ) for an aqueous solution of which substance is not obtained as a straight line? A. ( H C l ) в. ( N a O H ) c. ( N a C l ) D. ( H C N ) | 12 |

1411 | The reduction potential of a hydrogen electrode at ( p H 10 ) at ( 298 K ) is ( :(P= ) 1 ( (a t m) ) A. 0.51 volt B. 0 volt c. 0.591 volt D. 0.059 volt | 12 |

1412 | Which of the following are concentration cells? This question has multiple correct options ( mathbf{A} cdot P tleft|H_{2}(g)right| H C lleft|H_{2}(g)right| P t ) B. ( P t: P t: / begin{array}{l}H C l / / H C l / H_{2}: P t \ left(P^{H}=4right)^{prime} /left(P^{H}=2right)end{array} ) ( mathbf{c} . A g / A g C l / / A g B r / A g ) ( (1 M) quad 1 M ) ( mathbf{D} cdot A g|A g C l| C_{c_{1}}^{-}(a q)|| B_{c_{2}}^{-}(a q)|A g B r| A g ) | 12 |

1413 | In a hydrogen-oxygen fuel cell, combustion of hydrogen occurs to: A. generate heat B. create potential difference between the two electrodes c. produce high purity water D. remove absorbed oxygen from electrode surfaces | 12 |

1414 | The conductivity of saturated solution of ( B a S O_{4} ) is ( 3.06 times 10^{-6} ) mho ( c m^{-1} ) and its equivalent conductance 1.53 ( operatorname{mhocm}^{2} e q^{-1} . ) The ( K_{s p} ) for ( B a S O_{4} ) will be: A ( cdot 10^{3} M ) В. ( 4 times 10^{6} M ) c. ( 10^{-3} M ) D. ( 4 times 10^{-6} M ) | 12 |

1415 | Find out the volume of gasses evolved by passing 0.965 A current for 1 hr through an aqueous solution of ( C H_{3} C O O N a ) at ( 25^{0} C ) and 1 atm: A . ( 0.036 L ) B. 1.76 L c. ( 0.072 mathrm{L} ) D. 1.12 L | 12 |

1416 | Flow of current though electrolyte solution is due to migration of : A. Ions B. Electrons c. Protons D. Nucle | 12 |

1417 | Anode in the galvanic cell is : A. Negative electrode B. Positive electrode c. Neutral electrode D. None of the above | 12 |

1418 | The factors that promote electro chemical corrosion are A. the nature of the impurity metal with which the metal under consideration is associated. B. the concentration of ( O_{2} ) in contact with the surface of the metal. C. highly conducting solutions. D. all the above. | 12 |

1419 | A current liberates ( 0.50 g ) of hydrogen in 2 hours. The weight of copper(At.wt. ( = ) 63.5 ) deposited at the same time by the same current through copper sulphate solution is: ( mathbf{A} cdot 63.5 g ) в. ( 31.8 g ) c. ( 15.9 g ) D. ( 15.5 g ) | 12 |

1420 | Match the following and choose the correct option given below. Compound / Type A. Dry ice I. Anti-knocking compound B. ( quad ) II. Electronic diode or triode Semiconductor C. Solder III. Joining circuits IV. Refrigerant for preserving D. TEL ( quad ) food A. ( A-I, B-11, C-1 V, D-111 ) B. ( A-11, B-111, C-1, D-1 V ) C. ( A-I V, B-I I I, C-11, D-1 ) D. ( A-I V, B-11, C-111, D-1 ) | 12 |

1421 | ulatur below find out the strongest reducing agent. (d) Mn2+ (c) CM3+ . 8 Using the data given below find out the strong Eczo-/Cr3+ = 1.33V; E ®Cl2/cl” = 1.30V E®Mnoz /Mn2+ = 1.51V; EⓇCr3+/Cr = -0.74V (a) CI (6) Cr Thinking Process m includes concept of electrochemical series and standard reduction potential of the metal. Higher the negative value of standard reduction potential, strongest will be the reducing agent As value of SRP increases from negative to positive value nature of species changes from reducing to oxidising nature. | 12 |

1422 | The magnitude of charge present on one azide ion in coulombs is: ( mathbf{A} cdot 96500 ) B . ( 4.8 times 10^{19} ) c. ( 4.8 times 10^{-19} ) D. ( 1.6 times 10^{-19} ) | 12 |

1423 | The time required to produce ( 2 mathrm{F} ) of electricity with a current of 2.5 amperes is: A. 21.44 B. 1200 min c. 50000 s D. 1.5 ( h ) | 12 |

1424 | A cell with two electrodes, one of grey tin and the other white tin, both dipped in solution of ( left(N H_{4}right)_{2} S n C l_{6} ) showed zero e.m.f. at ( 18^{circ} mathrm{C} ). What conclusion may be drawn from this? A. The e.m.f. developed at the electrode-solution phase boundary cancels the normal e.m.f. B. Grey tin being non-metallic ceases to provide a reversible electrode reaction C. Electrode surface develops a protective layer and the cell develops a very large internal resistance D. The Gibbs energy change of the cell becomes zero | 12 |

1425 | (a) An organic compound (A) of molecular formula ( C_{2} H_{4} O ) is prepared by the reduction of compound (B) of molecular formula ( C_{2} H_{3} N ) dissolved in ether, with ( S n C l_{2} ) and ( H C l . ) Compound (A) reduces Tollen’s reagent. When a drop of conc. ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) is added to compound (A), it polymerises to give a cyclic compound (C). Identify (A), (B) and (C). Explain the reactions? (b) Ionic conductance at infinite dilution of ( A l^{3+} ) and ( S O_{4}^{2-} ) are 189 ohm ( ^{-1} mathrm{cm}^{2} ) gm.equiv ( ^{-1} ) and 160 ohm ( ^{-1} mathrm{cm}^{2} ) gm.equiv ( ^{-1} ). Calculate equivalent and molar conductance of the electrolytes at infinite dilution? | 12 |

1426 | At equilibrium, if ( boldsymbol{K}_{boldsymbol{p}}=mathbf{1}, ) then: ( mathbf{A} cdot Delta G^{o}>1 ) В. ( Delta G^{o}<1 ) c. ( Delta G^{o}=0 ) D. ( Delta G^{o}=1 ) | 12 |

1427 | Corrosion can be prevented by using | 12 |

1428 | ( boldsymbol{P t}left|left(boldsymbol{H}_{2}right)right| boldsymbol{p} boldsymbol{H}=boldsymbol{2} | boldsymbol{p} boldsymbol{H}=boldsymbol{3} midleft(boldsymbol{H}_{2}right) boldsymbol{P} boldsymbol{t} . ) The cell reaction for the given cell is : A. spontaneous B. non-spontaneous c. equilibrium D. None of the above | 12 |

1429 | Sonal has dropped her golden ring in ( mathrm{CuSO}_{4}, ) solution. Does she need to worry? ( E_{A u^{3+} mid A u}^{o}=1.50 V, E_{C u^{2+} mid C u} V ) | 12 |

1430 | The change in potential of the half-cell ( C u^{2+} / C u, ) when aqueous ( C u^{2+} ) solution is diluted 100 times at ( 298 K ? ) ( left[frac{2.303 R T}{F}=0.06right] ) A. Increases by ( 120 mathrm{mV} ) B. Decreases by ( 120 mathrm{mV} ) c. Increases by ( 60 mathrm{mV} ) D. Decreases by ( 60 mathrm{mV} ) E. No change | 12 |

1431 | Balance the reaction of copper sulphide with dilute hydrochloric acid. ( mathbf{A} cdot C u_{2} S+2 H C l rightarrow 2 C u C l+H_{2} S ) B ( cdot C u_{2} S+H C l rightarrow C u C l+H_{2} S ) ( mathbf{c} cdot C u_{2} S+H C l rightarrow C u C l_{2}+H_{2}+S ) D. ( 2 C u_{2} S+2 H C l rightarrow 2 C u C l_{2}+S_{2}+H_{2} S ) | 12 |

1432 | Copy and complete the following table which refers to two practical applications of electrolysis. Anode Electrolyte silver Solution of plating a potassium spoo argentocya | 12 |

1433 | Molar conductivities at infinite dilution of ( N a C l, H C l ) and ( C H_{3} C O O N a ) are 126.4,425.9 and ( 91.0 mathrm{Scm}^{2} ) mol ( ^{-1} ) respectively. Molar conductivity for ( boldsymbol{C H}_{3} boldsymbol{C O O H} ) will be: | 12 |

1434 | The number of electrons required for deposition of one mole of copper on the cathode during the electrolysis of CuSO ( _{4} ) is: B . 1.2×10 ( ^{2} ) c. ( 4.8 times 10^{24} ) D. 3×10 ( ^{23} ) | 12 |

1435 | Approximate ( K_{c} ) for the reaction at ( 25^{circ} C ) will be: ( boldsymbol{Z} boldsymbol{n}(boldsymbol{s})+boldsymbol{C u}^{2+}(boldsymbol{a q})=boldsymbol{Z} boldsymbol{n}^{3+}(boldsymbol{a q})+ ) ( boldsymbol{C u}(boldsymbol{s}) ) ( boldsymbol{E}_{Z n^{2+} / Z n}^{o}=-mathbf{0 . 7 6} boldsymbol{V} boldsymbol{E}_{C u / C u^{2+}}^{o}= ) ( -mathbf{0 . 3 4} V ) ( mathbf{A} cdot 10^{11} ) B. ( 10^{3} ) ( mathbf{c} cdot 10^{18} ) D. ( 10^{14} ) | 12 |

1436 | (a) Define molar conductivity of a solution and explain how molar conductivity changes which change in concentration of solution for a weak and a strong electrolyte? (b) The resistance of a conductivity cell containing ( 0.001 M ) KCl solution at 298 Kis ( 1500 Omega ). What is the cell constant if the conductivity of ( 0.001 mathrm{M} ) KCl solution at ( 298 mathrm{K} ) is ( 0.146 times 10^{-3} mathrm{S} mathrm{cm}^{-1} ) ? | 12 |

1437 | 10g fairly concentrated solution of ( boldsymbol{C u} boldsymbol{S O}_{4} ) is electrolysed using ( mathbf{0 . 0 1} ) faraday of electricity. The mass of resulting solution is : A. ( 9.6025 mathrm{g} ) B. ( 10.6005 mathrm{g} ) c. ( 6.6025 mathrm{g} ) D. None of these | 12 |

1438 | Which modifications are necessary to determine resistance of solutions by usual method of conductance measurement? This question has multiple correct options | 12 |

1439 | ( Delta H^{ominus} ) for the cell reaction assuming that these quantities remain unchanged in the range ( 15^{circ} C ) to ( 35^{circ} mathrm{C} ) is: A. ( -99.97 k J mathrm{mol}^{-1} ) B. ( 99.97 k J ) mol ( ^{-1} ) ( mathbf{c} .-9.99 k J mathrm{mol}^{-1} ) D. ( 9.99 mathrm{kJ} mathrm{mol}^{-1} ) | 12 |

1440 | Question 7. Value of standard electrode potential for the oxidation of Clions is more positive than that of water, even then in the electrolysis of aqueous sodium chloride, why is cl oxidised at anode instead of water? | 12 |

1441 | Actual efficiency of fuel cell is only around: A. 60-70% в. 20-30% c. ( 100 % ) D. 30-40% | 12 |

1442 | What will be standard cell potential of galvanic cell with the following reaction? ( boldsymbol{2} boldsymbol{C r}_{(s)}+boldsymbol{3} boldsymbol{C} boldsymbol{d}_{(a q)}^{2+} rightarrow boldsymbol{2} boldsymbol{C r}_{(a q)}^{3+}+boldsymbol{3} boldsymbol{C} boldsymbol{d}_{(s)} ) ( left[text { Given: } boldsymbol{E}_{C r^{3+} / C r}^{o}=-mathbf{0 . 7 4 V} ) and right. ( boldsymbol{E}_{C d^{2+} / C d}^{o}=-mathbf{0 . 4 0 V} ) ( mathbf{A} cdot 0.74 mathrm{v} ) B. ( 1.14 mathrm{V} ) c. ( 0.34 v ) D. ( -0.34 mathrm{v} ) | 12 |

1443 | Assertion The presence of ( C O_{2} ) in the air accelerates corrosion. Reason ( C O_{2} ) is a poisonous gas. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 12 |

1444 | Resistance of a conductivity cell filled with a solution of an electrolyte of concentration ( 0.1 M ) is 100 ohm. The conductivity of this solution is ( 1.29 S m^{-1} . ) Resistance of the same cell when filled with ( 0.2 ~ M ) of the same solution is 520 ohm. The molar conductivity of ( 0.02 M ) solution of the electrolyte will be: A ( cdot 124 times 10^{-4} mathrm{S} mathrm{m}^{2} mathrm{mol}^{-1} ) В. ( 1240 times 10^{-4} mathrm{S} ) m ( ^{2} ) mol ( ^{-1} ) c. ( 1.24 times 10^{-4} ) S ( m^{2} ) “nol ( ^{-1} ) D. ( 12.4 times 10^{-4} mathrm{S} mathrm{m}^{2} mathrm{mol}^{-} ) | 12 |

1445 | Q. 45 Consider a cell given below Cu Cu2+ || CL CL2., Pt Write the reactions that occur at anode and cathode. | 12 |

1446 | A current of ( 9.65 A ) flowing for 10 minutes deposits ( 3.0 g ) of the metal which is monovalent. The atomic mass of the metal is: | 12 |

1447 | The following are some statements about electrolysis: I) Involves flow of electrons from anode to cathode II) Involves no chemical reaction at electrodes III) Oxidation occurs at anode and reduction at cathode IV) Anions migrate towards cathode A. Only I and III are correct B. Only I and II are correct c. onlyı, I land III are correct D. All are correct | 12 |

1448 | A resistance of ( 50 Omega ) is registered when two electrodes are suspended into a beaker containing a dilute solution of a strong electrolyte such that exactly half of the them are submerged into solution. If the solution is diluted by adding pure water (negligible conductivity) so as to just completely submerge the electrodes, the new resistance offered by the solution would be: A . ( 50 Omega ) B. ( 100 Omega ) ( c .25 Omega ) D. 200 ( Omega ) | 12 |

1449 | A current of 2 amp when passed for 5 hours through a molten salt deposits ( 22.2 g ) of metal of atomic mass ( 177 . ) The oxidation state of the metal in the metal salt is: A. +1 B. +2 ( c cdot+3 ) D. +4 | 12 |

1450 | Sulphuric acid is used in lead-acid storage batteries. A. True B. False | 12 |

1451 | The quantity of charge (in Faraday) required to reduce 96 g Mg from molten solution of ( mathrm{MgCl}_{2} ) is : | 12 |

1452 | In an electro chemical process, a salt bridge is used a) to maintain electro neutrality in each solution. b) to complete the circuit so that current can flow c) as an oxidising agent d) as a colour indicator A. only a is correct B. a and b are correct c. a, b and care correct D. all are incorrect | 12 |

1453 | In a salt solution, the flow of current is: A. same as the direction of positive ions B. opposite to the direction of negative ions c. both a and b D. opposite to the direction of positive ions | 12 |

1454 | Which of the following statement (s) differentiate between electrochemical cell and electrolytic cell? This question has multiple correct options A. Spontaneous or non-spontaneous nature of the chemical process. B. Chemical reactions occurring at the electrodes c. Positive and negative nature of anode D. Dependence on Faraday’s law | 12 |

1455 | Lead accumulator is: A. acid storage cell B. alkali storage cell ( c cdot ) both D. cant be predicted | 12 |

1456 | Q. 26 Molar conductivity of ionic solution depends on ……. (a) temperature (b) distance between electrodes (c) concentration of electrolytes in solution (d) surface area of electrodes | 12 |

1457 | How much will the reduction potential of a hydrogen electrode change when its solution initially at ( mathrm{pH}=0 ) is neutralised to ( mathrm{pH}=7 ? ) A. Increases by ( 0.059 mathrm{V} ) B. Decreases by ( 0.059 mathrm{V} ) c. Increases by ( 0.41 V ) D. Decreases by ( 0.41 V ) | 12 |

1458 | The weights of various ions liberated by passing the same current through different electrolytes are in the ratio of their: A. Atomic weights B. Equivalent weights c. Molecular weights D. Atomic numbers | 12 |

1459 | Question 15. In an aqueous solution how does specific conductivity of electrolytes change with addition of water? | 12 |

1460 | The EMF of the cell : ( boldsymbol{P t}, boldsymbol{H}_{2}(boldsymbol{1} boldsymbol{a} boldsymbol{t m})left|boldsymbol{H}^{oplus}(boldsymbol{a} boldsymbol{q}) | boldsymbol{A} boldsymbol{g} boldsymbol{C l}right| boldsymbol{A} boldsymbol{g} ) is 0.27 and ( 0.26 mathrm{V} ) at ( 25^{circ} mathrm{C} ) and ( 35^{circ} mathrm{C} ) respectively. The posituve value of heat of the reaction occurring inside the cell ( operatorname{at} 25^{circ} Cleft(i n k J K^{-1}right) ) is: ( ( ) write your answer to nearest integer) | 12 |

1461 | ( boldsymbol{E}^{o} ) value of ( boldsymbol{N} boldsymbol{i}^{2+} / boldsymbol{N} boldsymbol{i} ) is ( -mathbf{0 . 2 5} ) V and ( A g^{+} / A g ) is ( +0.80 V . ) If a cell is made by taking the two electrodes what is the feasibility of the reaction? A. since ( E^{circ} ) value for the cell will be positive, redox reaction is feasible B. since ( E^{o} ) value for the cell will be negative, redox reaction is not feasible c. Ni cannot reduce ( A g^{+} ) to Ag hence reaction is not feasible D. Ag can reduce ( N i^{2+} ) to Ni hence reaction is feasible | 12 |

1462 | The standard potential of the following cells is ( 0.23 mathrm{V} ) at ( 15^{circ} mathrm{C} ) and ( 0.21 mathrm{V} ) at ( 35^{circ} mathrm{C} ) ( boldsymbol{P t}left|boldsymbol{H}_{2}(boldsymbol{g})right| boldsymbol{H} boldsymbol{C l}(boldsymbol{a q})|boldsymbol{A} boldsymbol{g} boldsymbol{C l}(boldsymbol{s})| boldsymbol{A} boldsymbol{g}(boldsymbol{s}) ) Calculate ( -Delta H^{o} ) (in ( mathrm{kJ} ) ) for the cell reaction by assuming that these quantities remain unchanged in the range ( 15^{circ} mathrm{C} ) to ( 35^{circ} mathrm{C}( ) to the nearest integer) | 12 |

1463 | Net reaction taking place when amalgam is in contact with Al foil: A ( cdot 2 H_{2} O+O_{2} rightarrow 2 H_{2} O ) B. ( 4 A l+3 O_{2}+12 H^{oplus} rightarrow 4 A l^{3+}+6 H_{2} O ) c. ( A l+O_{2}+stackrel{delta}{O} rightarrowleft[A l(O H)_{4}right]^{ominus}+H_{2} O ) D. ( 4 A l+3 O_{2} rightarrow 2 A l_{2} O_{3} ) | 12 |

1464 | The EMF of a galvanic cell is determined by using a: A. voltmeter B. potentiometer c. coulometer D. ammeter | 12 |

1465 | Assertion: In a galvanic cell, the half-cel with higher reduction potential provides a reducing agent Reason: Easily reducible substances are good oxidants. A. Both Assertion and Reason are true and Reason is the correct explanation of Assertion B. Both Assertion and Reason are true but Reason is not the correct explanation of Assertion c. Assertion is true but Reason is false D. Assertion is false but Reason is true E. Both Assertion and Reason are false | 12 |

1466 | The standard electrode potential of Cu/Cu ( ^{+2} ) electrode is ( 0.336 . ) It corresponds to the reaction: A. ( C u rightarrow C u^{+2}+2 e^{-} ) В ( cdot frac{1}{2} C u^{+2}+e^{-} rightarrow frac{1}{2} C u ) ( mathrm{c} cdot mathrm{Cu}^{+2}+2 e^{-} rightarrow mathrm{Cu} ) D. ( 2 C u^{+} rightarrow C u+2 e^{-} ) | 12 |

1467 |