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

#### List of thermodynamics Questions

Question No | Questions | Class |
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1 | The significance of ( boldsymbol{T} boldsymbol{Delta} boldsymbol{S} ) in ( boldsymbol{Delta} boldsymbol{G}= ) ( Delta H-T Delta S ) is a quantitative measure of the randomness of the: B. space c. both of the above D. none of the above | 11 |

2 | Which one of the following equations does not correctly represent the first law of thermodynamics for the given processes involving an ideal gas? (Assume non-expansion work is zero) A. Cylic process : ( q=-w ) B. Isothermal process : ( q=-w ) c. Adiabatic process: ( Delta U=-w ) D. Isochoric process: ( Delta U=q ) | 11 |

3 | Q Type your question Substance Mass(gm) in moles ( begin{array}{ll}C H_{3} C O O H & 0.742end{array} ) 0.0 ( H ) 195 Beaker The two liquids ( C H_{3} C O O C H_{3} ) and ( C H C l_{3} ) combine in such away that they form a single H-bond between each pair of molecules. In an experiment to determine the approximate strength of this bond, samples of the two liquids were mixed in an insulated glass beaker and the temperature was found to rise by ( 1^{0} C . ) Other data are given in the table. The approximate strength of the H bond according to the above experiment (in kJ/mole) will be: | 11 |

4 | Work done during isothermal expansion depends on change in A. volume B. pressure c. both (a) and (b) D. none of these | 11 |

5 | ( boldsymbol{H}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) boldsymbol{Delta} boldsymbol{H}= ) ( -242 k J m o l^{-1} ) Bond energy of ( H_{2} ) and ( O_{2} ) are 436 and ( mathbf{5 0 0} k J mathrm{mol}^{-1} ) respectively. The bond energy of ( 0-H ) bond is : A ( cdot 434 k J mathrm{mol}^{-1} ) B. ( 464 k J ) mol ( ^{-1} ) ( mathbf{c} cdot 452 k J mathrm{mol}^{-1} ) D. ( 485 k J ) mol ( ^{-1} ) | 11 |

6 | For the pressure-volume work expression, the term pressure in the expression refers to gas pressure. ( mathbf{A} cdot W=-P_{e x} cdot Delta P ) ( mathbf{B} cdot W=-P_{e x} cdot Delta V ) ( mathbf{C} cdot W=-P_{e x} cdot Delta C ) ( mathbf{D} cdot W=-P_{e x} cdot Delta D ) | 11 |

7 | Spontaneous reactions are: A. Endergonic B. Exergonic C . Energy neutral D. Exer-endergonic reactions | 11 |

8 | A diatomic gas ( (lambda=1.4) ) does 200 Jof work when it is expanded isobarically. Find the heat given to the gas in the process. | 11 |

9 | In exothermic reaction ( mathbf{A} cdot H_{R}=H_{P} ) В ( cdot H_{R}>H_{P} ) ( mathbf{c} cdot H_{R}<H_{P} ) D. ( Delta H=0 ) | 11 |

10 | A certain mass of gas is expanded from ( (1 mathrm{L} .10 mathrm{atm}) ) to ( (4 mathrm{L} .5 mathrm{atm}) ) against a constant external pressure of 1 atm. If initial temperature of gas is ( 300 mathrm{K} ) and the heat capacity of process is ( 50 mathrm{J} /^{circ} mathrm{C} ) Then the enthalpy change during the process is: ( (-1 mathrm{L} text { atm } 100 mathrm{J}) ) A ( . Delta H=15 mathrm{kJ} ) в. ( Delta H=15.7 mathrm{k} ) c. ( Delta H=14.4 mathrm{kJ} ) D. ( Delta H=14.7 mathrm{kJ} ) | 11 |

11 | The heat of atomization of methane and ethane are ( 360 mathrm{kJ} / mathrm{mol} ) and ( 620 mathrm{KJ} / mathrm{mol} ) respectively. The longest wavelength of light capable of breaking the ( C-C ) bond is: (Avogadro number ( =6.02 times 10^{23}, h= ) ( 6.62 times 10^{-34} mathrm{Js} ) A ( cdot 2.48 times 10^{4} mathrm{nm} ) B . ( 1.49 times 10^{3} ) nm c. ( 2.48 times 10^{3} mathrm{nm} ) D. ( 1.49 times 10^{4} ) nm | 11 |

12 | An ideal gas at ( 27^{circ} C ) is compressed adiabatically to ( frac{8}{27} ) of its original volume. The rise in temperature is (Take ( gamma=5 / 3) ) ( mathbf{A} cdot 475 K ) в. ( 150 K ) c. ( 275 K ) D. 375K | 11 |

13 | The difference between ( Delta H ) and ( Delta U ) for the combustion reaction of benzene at ( 127^{circ} mathrm{C} ) is: A. ( -200 R ) в. ( -600 R ) c. ( 200 R ) D. ( 600 R ) | 11 |

14 | The free energy changes for the two reactions given below are: ( mathbf{a} . boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) longrightarrow ) ( boldsymbol{S} boldsymbol{O}_{2} boldsymbol{C l}_{2}(boldsymbol{g}), boldsymbol{Delta} boldsymbol{G}=-boldsymbol{2} 270 boldsymbol{c} boldsymbol{a} boldsymbol{l} ) b. ( S(R h o m b)+O_{2}(g)+C l_{2}(g) longrightarrow ) ( boldsymbol{S O}_{2} boldsymbol{C l}_{2}(boldsymbol{g}), boldsymbol{Delta} boldsymbol{G}=-mathbf{7 4 0 6 0 c a l} ) Find ( Delta G ) for the reaction ( S(r h o m)+ ) ( O_{2}(g) longrightarrow S O_{2}(g) ) A ( . Delta G=-71790 c a l ) в. ( Delta G=+71790 ) са ( l ) c. ( Delta G=-9670 c a l ) D. None of these | 11 |

15 | The temperature of ( 3 mathrm{kg} ) of nitrogen is raised from ( 10^{circ} mathrm{C} ) to ( 100^{circ} mathrm{C} ). Compute the heat added, the work done, and the change in internal energy if this is done at constant volume A . ( 199800 mathrm{J} ) B. 19000 J c. 199000 J D. 190000 J | 11 |

16 | A reversible adiabatic path on a P-V diagram for an ideal gas passes through sate A where ( boldsymbol{P}=mathbf{0 . 7} times ) ( mathbf{1 0}^{5} boldsymbol{N} / boldsymbol{m}^{-2} ) and ( boldsymbol{v}=mathbf{0 . 0 0 4 9} boldsymbol{m}^{3} . ) The ratio of specific heat of the gas is 1.4 The slope of path at ( A ) is: A . ( 2.0 times 10^{7} N m^{-5} ) B . ( 1.0 times 10^{7} mathrm{Nm}^{-5} ) c. ( -2.0 times 10^{7} mathrm{Nm}^{-5} ) D. ( -1.0 times 10^{7} mathrm{Nm}^{-5} ) | 11 |

17 | Assertion In adiabatic process work is independent of path. Reason In adiabatic process work done is equal to negative of change in internal 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 | 11 |

18 | Water is boiled under a pressure of 1.0atm. When an electric current of ( 0.50 A ) from a ( 12 V ) supply is passed for 300 second through a resistance in thermal contact with it, it is found that ( 0.789 g ) of water is vapourized. The molar internal energy change at boiling point (373.15K) is A. ( =37.9 k J m o l^{-1} ) В. ( =27.5 k J ) mol ( ^{-1} ) ( mathbf{c} .=47.5 k J m o l^{-1} ) ( mathbf{D} cdot=17.5 k J m o l^{-1} ) | 11 |

19 | In a constant volume calorimeter, 5 g of a gas with molecular weight 40 was burnt in excess of oxygen at ( 298 mathrm{K} ). The temperature of the calorimeter was found to increase from ( 298 mathrm{K} ) to ( 298.75 mathrm{K} ) due to combustion process. Given that the heat capacity of the calorimeter is ( 2.5 mathrm{kJ} K^{-1} ), the numerical value for the ( Delta U ) of combustion of the gas in ( mathrm{kJ} ) ( m o l^{-1} ) is: A . 15 B. 12 c. 90 D. 8 | 11 |

20 | Magnitude of Seebeck emf between the junctions does not depend on A. thermocouple B. temperature of cold junction c. temperature of hot function D. neutral temperature | 11 |

21 | According to the first law of thermodynamics, ( Delta U=q+w . ) In special cases the statement can be expressed in different ways. Which of the following is not a correct expression? A. At constant temperature: ( q=-w ) B. When no work is done: ( Delta U=q ) C. In gaseous system: ( Delta U=q+P Delta V ) D. When work is done by the system: ( Delta U=q+w ) | 11 |

22 | A steam engine delivers ( 5.4 times 10^{8} ) Jof work per minute and services ( 3.6 times 10^{9} ) Jof heat per minute from its boiler What is the efficiency of the engine? How much heat is wasted per minute? | 11 |

23 | Properties of substances like pressure, temperature and density, in thermodynamic coordinates are A. path function B. point function c. cyclic function D. real function | 11 |

24 | Q13. Given : N,(o) + 3H,(g) 2NH2(g); 4.HⓇ = -92.4 kJ moll. What is the standard enthalpy of formation of NH, gas? | 11 |

25 | The quantity of heat required by 1 gram of a substance to raise its temperature by ( 1 mathrm{K} ) is called its specific heat. State whether given statement is True/False A. True B. False | 11 |

26 | If the pressure of ( N_{2} / H_{2} ) mixture in a closed apparatus is 100 atm and ( 20 % ) of the mixture reacts then the pressure at the same temperature would be: A. 100 B. 90 c. 85 D. 80 | 11 |

27 | Two moles of an ideal monoatomic gas is heated from ( 27^{circ} C ) to ( 627^{circ} C ) reversibly and isochorically. The entropy of gas: A. increases by ( 2 R ln 3 ) B. increases by ( 3 R ln 3 ) c. decreases by ( 2 R ln 3 ) D. decreases by ( 3 R ln 3 ) | 11 |

28 | List I and List II contains four entries each. Entries of Column I are to be matched some entries of List II. One or more than one entries of List I may match with the same entry of List II | 11 |

29 | Calculate the work done (in J) when 4.5 g of ( H_{2} O_{2} ) reacts against a pressure of 1.0 ( operatorname{atm} operatorname{at} 2 H_{2} O_{2} rightarrow O_{2}+2 H_{2} O ) A . ( -1.63 times 10^{2} ) В. ( 4.5 times 10^{2} ) c. ( 3.2 times 10^{2} ) D. ( -6.1 times 10^{2} ) | 11 |

30 | Internal energy per mole of gas depends on A. viscosity B. density c. temperature D. thermal conductivity | 11 |

31 | toppr Q Type your question to the other end of the piston, it moves down. If air in the enclosure is cooled from temperature ( boldsymbol{T} ) to ( boldsymbol{T}-triangle boldsymbol{T}, ) the piston moves back to its original position. Then ( triangle boldsymbol{T} / boldsymbol{T} ) is close to (Assuming air to be an ideal gas, ( boldsymbol{g}= ) ( 10 m / s^{2}, ) atmospheric pressure is ( 10^{5} ) Pascal) ( mathbf{A} cdot 0.01 ) B. 0.02 c. 0.04 D. 0.09 | 11 |

32 | Two substances ( P ) and ( Q ) when brought together, form substance R with the evolution of heat. The properties of R are different from both ( mathrm{P} ) and ( mathrm{Q} ). What is substance R? A. A compound B. An element c. A metal D. A mixture | 11 |

33 | Assertion It is not possible for a system unaided by an external agency to transfer heat from a body at lower temperature to another at a higher temperature. Reason It is not possible to violate the 2 nd law of thermodynamics. 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 | 11 |

34 | For an isolated system, the entropy: A. Either increases or remains constant B. Either decreases or remains constant c. can never decrease D. can never increase | 11 |

35 | Three bodies ( A, B ) and ( C ) are in thermal equilibrium. The temperature of ( B ) is ( 45^{circ} mathrm{C}, ) then the temperature of ( C ) is A ( cdot 45^{circ} mathrm{C} ) в. ( 50^{circ} mathrm{C} ) ( mathbf{c} cdot 40^{circ} C ) D. Any temperature | 11 |

36 | Which is the amount of energy that must be added to raise the temperature of 1 gram of a substance by ( 1^{circ} mathrm{C} ? ) A. Enthalpy change B. Entropy change c. Gibbs free energy change D. Activation energy E. Specific heat capacity | 11 |

37 | The thermal capacity of calorimeter system is ( 17.7 k J K^{-1} .(R= ) ( 8.313 m o l^{-1} K^{-1} ) ) (only magnitude in nearest integer in kJ/mol) | 11 |

38 | ( operatorname{In} ) a reaction ( Delta H ) and ( Delta S ) both are positive. In which of the following cases, the reaction would not be spontaneous? A ( . Delta H>T Delta S ) в. ( T Delta S>Delta H ) c. ( Delta H=T Delta S ) D. All of these | 11 |

39 | For the reaction: ( 2 H_{2(g)}+2 C l_{2(g)} rightarrow ) ( 4 H C l(g) ; Delta H^{0}=-92.3 K J, ) choose the correct statement(s) out of the following: (i) If the reaction equation is reversed, the ( Delta H^{0} ) value will become ( 92.3 K J ) (ii) The ( 4(H-C l) ) bond in ( 4 H C l ) is stronger than the ( 2(H-H) ) and ( mathbf{2}(boldsymbol{C l}-boldsymbol{C l}) ) bonds in ( mathbf{2} boldsymbol{H}_{2} ) and ( mathbf{2} boldsymbol{C l} mathbf{l}_{mathbf{2}} ) respectively. (iii) The ( Delta H^{0} ) value will be ( -92.3 K J ), if the ( H C l ) is produced as a liquid. A. (i) only B. (i) and (ii) only C. (ii) and (iii) only D. All of these | 11 |

40 | Consider the following statements and arrange in the order of true/false as given in the codes. ( S_{1}: ) Change in state function between two states is a definite quantity and does not depend on path. ( S_{2}: ) Intensive properties cannot be algebraically added or subtracted. ( S_{3}: ) Ratio of two extensive properties result in a parameter that depends on the amount of substance. ( S_{4}: ) Molar heat capacity is a state function. The correct order to true/false of the above statements is: ( A ). FT FT B. FF FT c. TT FT D. TTTF | 11 |

41 | A piston exerting a pressure of 1.0 atmosphere rests on the surface of water at ( 100^{circ} mathrm{C} ). The pressure is reduced to smaller extent and as a result 10 g of water evaporates and absorbs ( 22.2 mathrm{kJ} ) of heat. The change in internal energy is: A . 18.24 k B. 20.477 kJ c. 22.05 kJ D. 23.923 kJ | 11 |

42 | A thermodynamic system goes from states (i) ( P_{1}, V ) to ( 2 P_{1}, V ) (ii) ( P_{1}, V_{1} ) to ( P_{1}, 2 V_{1} . ) Then work done in the two cases is respectively A .0,0 в. ( 0, P_{1} V_{1} ) c. ( P_{1} V_{1}, 0 ) D. ( P_{1} V_{1}, P_{1} V_{1} ) | 11 |

43 | Assertion ( C_{p}-C_{V}=R ) for an ideal gas. Reason ( left[frac{partial boldsymbol{E}}{partial boldsymbol{V}}right]_{T}=mathbf{0} ) for an ideal 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 | 11 |

44 | At what temperature the linear kinetic energy of a gas molecule will be equal to that of an electron accelerated through a potential difference of 10 volt? A . ( 77.3 times 10^{3} mathrm{K} ) B. 38.65 x 10 ( ^{3} ) к c. ( 19 . times 10^{3} mathrm{K} ) D. 273 K | 11 |

45 | What is meant by the notation, ( triangle G, triangle S ) and ( triangle H ? ) Give the relationship between them. | 11 |

46 | on the P-T phase diagram of carbon dioxide: (a) At what temperature and pressure can the solid, liquid and vapour phases of ( C O_{2} ) co-exits in equilibrium? (b) What is the effect of decrease of pressure on the fusion and boiling point of ( boldsymbol{C} boldsymbol{O}_{2} ? ) (c) What are the critical temperature and pressure for ( C O_{2} ) ? what is their significance ? (d) Is ( C O_{2} ) solid, liquid or gas at ( (a) ) ( -70^{circ} mathrm{C} ) under 1 atm, ( (mathrm{b})-60^{circ} mathrm{C} ) under 10 ( operatorname{atm},(c) 15^{circ} C ) under 56 atm ( ? ) | 11 |

47 | A gas consisting of rigid diatomic molecules is expanded adiabatically. How many times has the gas to be expanded to reduce the r.m.s. velocity of the molecules to ( left(frac{2}{3}right) ) rd of initial value. A . 0.13 B. 7.6 ( c .5 ) D. 3.8 | 11 |

48 | In which of the following change entropy decreases? A. Crystallisation of sucrose from solution B. Dissolving sucrose in water c. Melting of ice D. Vaporisation of camphor | 11 |

49 | The mean kinetic energy of gas molecules is zero at ( A cdot O^{o} C ) B. -273 ( ^{circ} mathrm{C} ) c. ( 100 mathrm{k} ) D. ( 100^{circ} mathrm{C} ) | 11 |

50 | What happens when a thermos flask containing liquid is vigorously shaken? Will there be any change in the temperature of the liquid? | 11 |

51 | What is chemical kinetics and chemical thermodynamics? | 11 |

52 | A system undergoes a cyclic process in which it absorbs ( Q_{1} ) heat and gives out ( Q_{2} ) heat. The efficiency of the process is ( eta ) and the work done is ( W ) This question has multiple correct options A ( . W=Q_{1}-Q_{2} ) в. ( eta=frac{W}{Q_{1}} ) c. ( eta=frac{Q_{2}}{Q_{1}} ) D. ( eta=1-frac{Q_{2}}{Q_{1}} ) | 11 |

53 | In the combustion of ( 2.0 mathrm{gm} ) of methane 25 kcal heat is liberated, heat of combustion of methane would be A. 100 kcal B. 200 kcal c. 300 kcal D. 400 kcal | 11 |

54 | For a particular reaction, ( Delta boldsymbol{H}^{o}= ) ( -38.3 k J ) and ( Delta S^{o}= ) ( -113 J K^{-1} m o l^{-1} . ) This reaction is: A. spontaneous at all temperatures B. non-spontaneous at all temperatures C. spontaneous at temperatures below ( 66^{circ} mathrm{C} ) D. spontaneous at temperatures above ( 66^{circ} mathrm{C} ) | 11 |

55 | Natural processes are: A. reversible. B. irreversible. C. isothermal. D. adiabatic. | 11 |

56 | . 46 How will you calculate work done on an ideal gas in a compression, when change in pressure is carried out in infinite steps? in pressure it is a reversible | 11 |

57 | A sample of ( 0.16 g C H_{4} ) was subjected to the combustion at ( 27^{circ} C ) in a bomb calorimeter. The temperature of the calorimeter. The temperature of the calorimeter system (including water) was found to rise by ( 0.5^{circ} mathrm{C} ). Calculate the heat of combustion of methane at (i) constant volume and (ii) constant pressure. the thermal capacity of calorimeter system is ( 17.0 k J K^{-1} ) and ( R= ) ( 8.314 J K^{-1} m o l^{-1} ) | 11 |

58 | ( 2.1 g ) of ( F e ) combines with ( S ) evolving ( 3.77 k J . ) The heat of formation of ( F e S ) in ( k J / m o l ) is: A. -3.77 B . -1.79 c. -100.5 D. None of these | 11 |

59 | One mole of a gas expands by ( 3 L ) against a constant pressure of 3 atmosphere. Calculate the work done in L atmosphere. | 11 |

60 | A liquid boils at such a temperature at which the saturated vapour pressure, as compared to atmospheric pressure, is A. one-third B. equal c. half D. doubl | 11 |

61 | Which is not correct relationship between ( Delta G^{ominus} ) and equilibrium constant ( boldsymbol{K}_{boldsymbol{P}} ) This question has multiple correct options ( mathbf{A} cdot K_{P}=-R T log Delta G^{ominus} ) В ( . K_{P}=[e / R T]^{Delta G^{ominus}} ) ( mathbf{C} cdot K_{P}=-frac{Delta G^{circ}}{R T} ) ( mathbf{D} cdot K_{P}=e^{-Delta G^{ominus} / R T} ) | 11 |

62 | Which of the following is/are state property/properties? This question has multiple correct options A. Internal energy B. Volume c. Heat D. Enthalpy | 11 |

63 | 8.33 Match the following parameters with description for spontaneity. A(Parameters) Description 4,HⓇ A, S A,G A + + 11. Non-spontaneous at high temperature B. – – + at high T 2. Spontaneous at all temperatures 3. Non-spontaneous at all temperatures C – + – | 11 |

64 | Which portion of the heating curve for water shown above would there be both liquid and solid water present? ( A cdot A-B ) 3. ( B-C ) ( c cdot C-D ) D. ( D-E ) | 11 |

65 | A boiled egg show a/an in entropy A. increase B. decrease c. no chnage D. none of these | 11 |

66 | Out of boiling point (I), entropy (II), pH (III) and e.m.f. of a cell (IV). how many of them are intensive | 11 |

67 | A ( 2 k W ) electric heater is placed in 2.5 kg of water at ( 25^{circ} mathrm{C} ). calculate the time taken to increase the temperature by ( 50^{circ} mathrm{C} ) A. 4 min 38 sec B. 5 min 03 sec c. 2 min D. 159 sec | 11 |

68 | The value of entropy of solar system is : A. increasing B. decreasing c. constant D. zero | 11 |

69 | A system is said to be isolated if it can neither exchange matter nor energy with surroundings. If true enter 1 , else enter 0 . | 11 |

70 | The thermal motion means A. motion due to heat engine B. disorderly motion of the body as a whole C. motion of the body that generates heat D. random motion of molecules | 11 |

71 | Q. 9 The entropy change can be calculated by using the expression AS = ? When water freezes in a glass beaker, choose the correct statement amongst the following. (a) AS (system) decreases but AS (surroundings) remains the same (b) AS (system) increases but AS (surroundings) decreases (C) AS (system) decreases but AS (surroundings) increases (d) AS (system) decreases but AS (surroundings) also decreases | 11 |

72 | Rate of disappearance of the reactant ( mathbf{A} ) at two different temperature is given by ( boldsymbol{A} rightleftharpoons boldsymbol{B} ) ( frac{-d[A]}{d t}=left(2 times 10^{-2} S^{-1}right)[A]-4 times ) ( mathbf{1 0}^{-mathbf{3}} boldsymbol{S}^{-mathbf{1}}[boldsymbol{B}] ; mathbf{3 0 0} boldsymbol{K} ) ( frac{-d[A]}{d t}=left(4 times 10^{-2} S^{-1}right)[A]-16 times ) ( mathbf{1 0}^{-4} boldsymbol{S}^{-1}[boldsymbol{B}] ; mathbf{4 0 0} boldsymbol{K} ) Calculate heat of reaction in the given temperature range, when equilibrium is set up. A. ( 8.03 mathrm{kJ} ) B. 16.06 k c. 32.12 k D. None of these | 11 |

73 | Hess’s Law is used A. When a directly measured enthalpy change of reaction is not available B. To calculate an enthalpy change value through multiple steps C. Because enthalpy is a State Function D. As an easy way to calculate the enthalpy change of a reaction E. All of these options(A,B,C,D) are correct | 11 |

74 | For a first order reaction rate constant is ( 1 times 10^{-5} sec ^{-1} ) having ( E_{a}= ) ( 1800 k J / ) mol. Then the value of ( ell n A ) at ( boldsymbol{T}=mathbf{6 0 0} boldsymbol{K} ) is: A . 151.7 в. 349.3 c. 24.7 D. 11.34 | 11 |

75 | Two isothermals are shown in figure at temperature ( T_{1} ) and ( T_{2} . ) Which of the following relations is correct? A ( cdot T_{1}>T_{2} ) в. ( T_{1}<T_{2} ) ( c cdot T_{1}=T_{2} ) ( T_{1}=(1 / 2) T_{2} ) | 11 |

76 | An athlete is given ( 100 g ) of glucose ( C_{6} H_{12} O_{6} ) of energy equivalent to ( 1560 k J . ) He utilizes ( 50 % ) of this gained energy in an event. In order to avoid storage of energy in the body what is the weight of water, he would need to perspire? The enthalpy of evaporation of water is ( 44 k J / ) mol. A. ( 319 g ) в. ( 638 g ) c. ( 14040 g ) D. 35.45 g | 11 |

77 | For the reaction, ( boldsymbol{X}_{2} boldsymbol{O}_{4}(l) longrightarrow ) ( mathbf{2} boldsymbol{X} boldsymbol{O}_{2}(boldsymbol{g}) ) ( Delta U=2.1 k c a l, Delta S=20 operatorname{cal} K^{-1} mathrm{at} ) ( 300 mathrm{K} ) Hence ( , Delta G ) is A . +2.7 kcal B. -2.7 kcal c. +9.3 kcal D. – -9.3 kcal | 11 |

78 | (i) ( boldsymbol{C a O}(boldsymbol{s})+boldsymbol{H}_{2} boldsymbol{O}(l)=boldsymbol{C a}(boldsymbol{O H})_{2}(boldsymbol{s}) ) ( Delta H_{180^{circ} C}=-15.26 k c a l ) (ii) ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l})=boldsymbol{H}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) ) ( boldsymbol{Delta} boldsymbol{H}_{180^{circ} C}=mathbf{6 8 . 3 7} boldsymbol{k c a l} ) (iii) ( C a(s)+frac{1}{2} O_{2}(g)=C a O(s) ) ( boldsymbol{Delta} boldsymbol{H}_{180^{circ} C}=-151.80 k c a l ) From the following data, the heat of formation of ( boldsymbol{C a}(boldsymbol{O H})_{2}(boldsymbol{s}) ) at ( mathbf{1 8}^{circ} boldsymbol{C} ) is: A . -98.69 kcal B . -235.43 kcal c. 194.91 kcal D. 98.69 kcal | 11 |

79 | At ( 27^{circ} C ) a gas is compressed suddenly such that its pressure becomes ( left(frac{1}{8}right) ) th of original pressure. Final temperature will be ( (gamma=5 / 3) ) ( mathbf{A} cdot 450 K ) B. ( 300 K ) c. ( -142^{circ} mathrm{C} ) D. ( 327^{circ} ) | 11 |

80 | Select from below, how are temperature and kinetic energy of molecules related to each other? A. Temperature is directly proportional to average kinetic energy B. Temperature is indirectly proportional to kinetic energy C. Temperature and kinetic energy have no relation D. Temperature is directly proportional to mechanical energy | 11 |

81 | An ideal gas ( left(C_{v}=frac{3}{2} Rright) ) is maintained in a vessel of volume ( 83 times 10^{-4} m^{3} ) at pressure ( 1.6 times 10^{6} N m^{-2} ) and temperature ( 300 K . ) If ( 2.49 times 10^{4} J ) heat is given to this vessel, then its final temperature will be ( mathbf{A} cdot 600 K ) B. ( 625 K ) ( mathbf{c} .650 K ) D. ( 675 K ) | 11 |

82 | What is the quantity of heat released per kg of water per ( 1^{circ} mathrm{C} ) fall in temperature? | 11 |

83 | At ( 227^{0} C, 60 % ) of 2 moles of ( P C l_{5} ) gets dissociated in a two-litre. the value of ( boldsymbol{K}_{boldsymbol{p}} ) will be ( A cdot 450 R ) B. 400 R ( c . ) 50 D. 100 R | 11 |

84 | The Sl unit of heat is A. joul B. kilojoule c. both a and D. None of these | 11 |

85 | Two mole of ideal diatomic gas ( left(C_{V, m}=5 / 2 Rright) ) at ( 300 mathrm{K} ) and 5 atm expanded irreversibly and adiabatically to a final pressure of 2 atm against a constant pressure of 1 atm.Calculate ( q ) ( mathrm{w}, Delta boldsymbol{H} ) and ( Delta boldsymbol{U} ) | 11 |

86 | For the following concentration cell,to be spontaneous ( boldsymbol{P t}left(boldsymbol{H}_{2}right) boldsymbol{P}_{1} boldsymbol{a} boldsymbol{t m} mid boldsymbol{H} boldsymbol{C l} | boldsymbol{P t}left(boldsymbol{H}_{2}right), boldsymbol{P}_{2} boldsymbol{a} boldsymbol{t m} ) Which of the following is correct? A ( cdot P_{1}=P_{2} ) в. ( P_{1} P_{2} ) | 11 |

87 | The standard enthalpies of n-pentane, isopentane and neopentane are -35.0,-37.0 and ( -40.0 K ) cal / mole respectively. The most stable isomer of pentane in terms of energy is A. n-pentane B. isopentane c. neopentane D. n-pentane and isopentane | 11 |

88 | Study the given graph and choose the correct option. A. ( Delta H ) is the net heat absorbed from the surroundings B. ( Delta H ) is the net heat given to the surroundings ( mathrm{c} cdot Delta H ) is positive for the reaction D. ( Delta H ) is the total energy possessed by the reactants | 11 |

89 | One mole of hydrogen, assumed to be ideal, is adiabatically expanded from its initial state ( left(P_{1}, V_{1}, T_{1}right) ) to the final state ( left(P_{2}, V_{2}, T_{2}right) . ) The decreases in the internal energy of the gas during this process will be given by A. ( C_{v}left(T_{1}-T_{2}right) ) в. ( C_{p}left(T_{1}-T_{2}right) ) c. ( frac{C_{P}+C_{V}}{2}left(T_{1}-T_{2}right) ) D. ( left(C_{p}-C_{v}right)left(T_{1}-T_{2}right) ) | 11 |

90 | Assertion A reaction which is spontaneous and accompanied by decrease of randomness must be exothermic. Reason All exothermic reactions are accompanied by decrease of randomness. 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 | 11 |

91 | 5 mole of oxygen are heated at constant volume from ( 10^{circ} mathrm{C} ) to ( 20^{circ} mathrm{C} ). What will be the change in the internal energy of gas? The molar heat of oxygen at constant pressure, ( C_{P}=7.03 mathrm{cal} ) ( m o l^{-1} d e g^{-1} ) and ( R= ) ( 8.31 J ) mol( ^{-1} d e g^{-1} ) | 11 |

92 | The enthalpy change when 1 mol of graphite is converted into diamond is known as the enthalpy of transition. If true enter 1 else 0 A. | 11 |

93 | A cylinder of mass ( 1 mathrm{kg} ) is given heat of ( 20000 mathrm{J} ) at atmospheric pressure. If initially temperature of cylinder is ( 20^{circ} mathrm{C} ) find change in internal energy of the cylinder. (Given that Specific heat capacity of cylinder ( =400 mathrm{J} mathrm{kg}^{-10} mathrm{C}^{-1}, ) Coefficient of volume expansion ( =mathbf{9} times mathbf{1 0}^{-mathbf{5} mathbf{0}} mathbf{C}^{-mathbf{1}} ) Atmospheric pressure ( =10^{5} N / m^{2} ) and Density of cylinder ( =9000 mathrm{kg} / mathrm{m}^{3} ) ) A. 39999.95 J. в. 29999.95 c. 19999.95 s D. 59999.95 J. | 11 |

94 | A Carnot engine has an efficiency of ( 1 / 6 ) When the temperature of the sink is reduced by ( 62^{circ} mathrm{C} ), its efficiency is doubled. The temperatures of the source and the sink are, respectively A ( cdot 124^{circ} mathrm{C}, 62^{circ} mathrm{C} ) B . ( 37^{circ} C, 99^{circ} mathrm{C} ) c. ( 62^{circ} mathrm{C}, 124^{circ} mathrm{C} ) D. ( 99^{circ} mathrm{C}, 37^{circ} mathrm{C} ) | 11 |

95 | L I ELUPY Utail aliueal ulystal. Q13. (a) Under what condition, the heat evolved or absorbed in a reaction is equal to its free energy change? (6) Calculate the entropy change for the following reversible process H2O(s) = H,O(1) AH is 6.0 kJ mol-1 | 11 |

96 | A gas is expanded from volume ( V_{1} ) to volume ( V_{2} ) in three processes, shown in the figure. If ( U_{A}, U_{B} ) and ( U_{C} ) and ( U_{D} ) represent the internal energies of the gas in state ( A, B, C ) and ( D ) respectively, the which of the following is not correct. A. ( U_{B}-U_{A}>0 ) B. ( U_{C}-U_{A}=0 ) c. ( U_{D}-U_{A}<0 ) D. ( U_{B}=U_{C}=U_{D} ) | 11 |

97 | The equilibrium constant of a reaction at ( 298 K ) is ( 5 times 10^{-3} ) and at ( 1000 K ) is ( 2 times 10^{-5} . ) What is the sign of ( Delta H ) for the reaction? ( mathbf{A} cdot Delta H ) is ( +v e ) B. ( Delta H ) is -ve ( mathbf{c} cdot Delta H propto 0 ) D. ( Delta H ) is ( pm v e ) | 11 |

98 | Due to irreversibility of a process, A. initial state of the process cannot be restored B. final state is not in equilibrium with the initial state. C. the intermediate states are not in equilibrium with each other. D. All of the above. | 11 |

99 | Which of the following statement is true as per the second law of thermodynamics for an isolated, ordered system? A. Heat will flow into the system c. work will be done by the system D. Work will be done on the system E. The entropy withing the system will increase | 11 |

100 | For a particular reversible reaction at temperature ( T, Delta H ) and ( Delta S ) were found to be both +ve. If ( T_{e} ) is the temperature at equilibrium, the reaction would be spontaneous when: A ( cdot T_{e}>T ) в. ( T>T_{e} ) ( mathbf{c} cdot T_{e} ) is 5 times ( T ) D. ( T=T_{e} ) | 11 |

101 | Q. 56 Assertion (A) Spontaneous process is an irreversible process and may be reversed by some external agency. Reason (R) Decrease in enthalpy is a contributory factor for spontaneity. (a) Both A and Rare true and R is the correct explanation of A (b) Both A and Rare true but is not the correct explanation of A (c) A is true but R is false (d) A is false but R is true | 11 |

102 | The cycle on a ( P V ) diagram is represented as ( A ) B. ( c ) D. none of these | 11 |

103 | Numerical value of work done is maximum in case of: ( mathbf{A} cdot C_{3} H_{8}(g)+50_{2}(g) longrightarrow 3 C O_{2}(g)+4 H_{2} O(l) ) B. ( C(s)+C O_{2}(g)+longrightarrow 2 C O(g) ) ( mathbf{c} cdot F e(s)+4 H_{2} O(g)+longrightarrow F e_{3} O_{4}(s)+4 H_{2}(g) ) ( mathbf{D} cdot N H_{4} C l(s) longrightarrow N H_{3}(g)+H C l(g) ) | 11 |

104 | If ( R ) is universal gas constant, the amount of heat needed to raise the temperature of 2 moles of an ideal monoatomic gas from 273 ( K ) to 373 ( K ) when no work is done ( mathbf{A} cdot 100 R ) в. ( 150 R ) c. ( 300 R ) D. ( 500 R ) | 11 |

105 | Carnot cycle works with isentropic compression ratio of 5 bar and isothermal ratio of 2. The volume of air at beginning of the isothermal expansion is ( 0.3 m^{3} . ) If the temperature and pressure is limited to ( 550 mathrm{K} ) and 21 bar, Determine Minimum temperature in the cycle. | 11 |

106 | A rigid diatomic ideal gas undergoes an adiabatic process at room temperature,. The relation between temperature and volume of this process is ( boldsymbol{T} boldsymbol{V}^{boldsymbol{x}}= ) constant, then ( boldsymbol{x} ) is : A ( cdot frac{5}{3} ) B. ( frac{2}{5} ) ( c cdot frac{2}{3} ) D. ( frac{3}{5} ) | 11 |

107 | In a constant volume calorimeter, 5 g of gas with molecular weight 40 was burnt in excess of oxygen at 298 K. The temperature of the calorimeter was found to increase from ( 298 mathrm{K} ) to 298.75 K due to the combustion process. Given that the heat capacity of the calorimeter is ( 2.5 mathrm{kJK}^{-1} ), the numerical value for the ( triangle boldsymbol{U} ) of combustion of the ( operatorname{gas} operatorname{in} mathrm{kJ} operatorname{mol}^{-1} mathrm{is} ) A . 15 в. 12 ( c cdot ) э० D. | 11 |

108 | The pressure of a monoatomic gas increases linearly from ( 4 times ) ( 10^{5} N m^{-2} t o 8 times 10^{-5} N m^{-2} ) when its volume increases from ( 0.2 m^{3} ) to ( 0.5 m^{3} ) calculate (a) work done by the gas, (b) increase in internal energy (c) mass of heat supplied and (d) molar heat capacity of the gas. | 11 |

109 | Which of the following is not a state function? A. Temperature c. work D. volume | 11 |

110 | Which law of thermodynamics states that energy can neither be created nor be destroyed, it can change from one to another? A. First law B. Second law c. zero law D. None of these | 11 |

111 | Which of the following statements is true?The entropy of the universe: A. increases and tends towards maximum value B. decreases and tends to be zero c. remains constant D. decreases and increases with a periodic rate | 11 |

112 | Q4. AUⓇ of combustion of methane is – X kJ mol-1. The value of AH® is (i) = AU (ii) > AU (iii) < AU (iv) 0 | 11 |

113 | Which of the following expressions is known as Clausius inequality? A ( cdot oint frac{d q}{T} leq 0 ) В ( cdot oint frac{d q}{T}=0 ) c. ( oint frac{T}{d q} leq 0 ) ( mathbf{D} cdot oint frac{d q}{T} geq leq 0 ) | 11 |

114 | Assertion The second law of thermodynamics states that the entropy of a closed or isolated system always increases. This means that all available energy is used up and there is no more potential for further useful work. Reason The system becomes disordered and also degraded 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 | 11 |

115 | Assertion (A): Internal energy is a state function and extensive property. Reason ( ( mathrm{R} ) ): Internal energy of a substance depends on gravitational force of attraction. A. A and R are true and ( mathrm{R} ) is correct explanation of B. A and R are true and R is not correct explanation of A c. A is true, R is false D. A is false, R is true | 11 |

116 | The bond disssociation energies of ( operatorname{gases} H_{2}, C l_{2} ) and ( H C l ) are 104,58 and ( mathbf{1 0 3} ) kcal ( m o l^{-1} ) respectively. Calculate the enthalpy of formation of ( boldsymbol{H} boldsymbol{C l}(boldsymbol{g}) ) | 11 |

117 | In a cyclic heat engine operating between a source temperature of ( 600^{0} C ) and a sink temperature of ( 20^{0} C ), the least rate of heat rejection per kW net output of the engine is, A. ( 0.505 mathrm{kW} ) B. 0.49 okw c. ( 0.333 mathrm{kw} ) D. none of the above | 11 |

118 | What is the specific heat of a ( 2.0 g ) sample of metal which requires the addition of ( 8 J ) to be heated from ( 293 K ) to ( 303 K ? ) A . 0.4 B. 0.02 c. 0.6 D. 2.5 | 11 |

119 | A point on ( P-V ) diagram represents A. the condition of a system c. work done in a cyclic process D. a thermodynamic process | 11 |

120 | Statement I: The entropy of a solid decreases when it is dissolved Because Statement II : It becomes less ordered 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 and 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. E. Both the Statement 1 and Statement 2 are not correct. | 11 |

121 | Heat of atomisation of ( boldsymbol{N} boldsymbol{H}_{3} ) and ( boldsymbol{N}_{2} boldsymbol{H}_{4} ) ( operatorname{are} boldsymbol{x} boldsymbol{k} boldsymbol{c a l} boldsymbol{m o l}^{-1} ) and ( boldsymbol{y} boldsymbol{k} c boldsymbol{a l} boldsymbol{m o l}^{-1} ) respectively. Average bond energy of ( N-N ) bond is: A ( frac{3 y-4 x}{3} ) kcal ( m o l^{-1} ) в. ( frac{3 y-x}{5} ) kcal ( m o l^{-1} ) c. ( frac{2 y-4 x}{4} ) kcal ( m o l^{-1} ) D. None of these | 11 |

122 | Slope between PV and P at constant temperature is: A . zero B. ( c cdot frac{1}{2} ) D. ( frac{1}{sqrt{2}} ) | 11 |

123 | Which of the following is/are correct? This question has multiple correct options ( mathbf{A} cdot Delta H=Delta U+Delta(P V) ) when ( P ) and ( V ) both changes B. ( Delta H=Delta U+P Delta V ) when pressure is constant C ( . Delta H=Delta U+V Delta P ) when volume is constant D. ( Delta H=Delta U+P Delta V+V Delta P ) when ( P ) and ( V ) both changes | 11 |

124 | The bond dissociation energy of ( boldsymbol{C}-boldsymbol{H} ) in ( C H_{4} ) from the equation ( boldsymbol{C}(boldsymbol{g})+boldsymbol{4} boldsymbol{H}(boldsymbol{g}) rightarrow boldsymbol{C} boldsymbol{H}_{4}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H}= ) ( -397.8 k c a l ) is: ( mathbf{A} cdot+99.45 k c a l ) B . – 99.45 k cal c. ( +397.8 k c a l ) D. ( +198.9 k c a l ) | 11 |

125 | The figure shows the ( P ) – ( V ) plot of an ideal gas taken through a cycle ABCDA. The part ( A B C ) is a semi-circle and CDA is half of an ellipse. Then This question has multiple correct options A. the process during the path ( A rightarrow B ) is isotherma B. heat flows out of the gas during the path ( B rightarrow C rightarrow D ) c. work done during the path ( A rightarrow B rightarrow C ) is zero D. positive work is done by the gas in the cycle ABCDA | 11 |

126 | Find the heat transferred to the water, when the temperature of a 20 gram sample of water is increased from ( 10^{circ} mathrm{C} ) to ( 30^{circ} mathrm{C} ? ) A. 400 calories B. 600 calories c. 20 calories D. 200 calories E. 30 calories | 11 |

127 | Woolen clothes keep the body warm because the wool: A. decreases the temperature of the body B. is a good conductor of heat C. increases the temperature of the body D. is a bad conductor of heat | 11 |

128 | The standard enthalpy of formation of ( N H_{3} ) is ( -46 k J m o l^{-1} . ) If the enthalpy of formation of ( boldsymbol{H}_{2} ) from its atoms is ( -436 k J m o l^{-1} ) and that of ( N_{2} ) is ( -712 k J m o l^{-1}, ) the average bond enthalpy of ( N-H ) bond in ( N H_{3} ) is: A ( .+1056 k J m o l^{-1} ) В. ( -1102 k J ) mol ( ^{-1} ) c. ( -964 k J m o l^{-1} ) D. ( +352 k J m o l^{-1} ) | 11 |

129 | 75 g of water at ( 10^{0} C ) is heated by supplying ( 25200 J ) of heat energy. If the specific heat of water is ( 4.2 J g^{-10} C^{-1} ) Calculate the final temperature of water. | 11 |

130 | Identify the incorrect statement? A. Energy can be converted into matter B. Matter can be converted into energy C. Energy can be converted into matter, and matter can be converted into energy D. Matter can be converted into energy, but energy cannot be converted into matter E. Energy can be measured in units of joules and calories | 11 |

131 | Figure represents two processes, a and b for a given sample of gas. Let ( triangle Q_{1} ) and ( triangle Q_{2} ) be the heat absorbed by the systems in the two cases respectively. Which of the following relations is correct? ( mathbf{A} cdot triangle Q_{1}=triangle Q_{2} ) B ( cdot triangle Q_{1}>triangle Q_{2} ) ( mathbf{c} cdot triangle Q_{1} leq triangle Q_{2} ) ( mathbf{D} cdot triangle Q_{1}<triangle Q_{2} ) | 11 |

132 | Calculate the least amount of work that must be done to freeze one gram of water at ( 0^{0} C ) by means of the refrigerator.The temperature of the surrounding is ( 27^{0} C . ) How much heat is passed on the surrounding in this process? Latent heat of fusion ( boldsymbol{L}= ) ( 80 mathrm{cal} / mathrm{g} ) ( mathbf{A} cdot 87.91 mathrm{cal} ) B. 97.91 cal c. 88.95 cal D. 89.95 cal | 11 |

133 | Calculate y (ratio of ( C_{p} ) and ( C_{v} ) ) for triatomic linear gas at high temperature. Assume that the contribution of the vibrational degree of freedom is ( 75 % ) A . 1.29 B. 1.121 c. 1.18 D. 1.33 | 11 |

134 | What is a heat engine? | 11 |

135 | The heat of combustion of carbon to ( boldsymbol{C O}_{2}(boldsymbol{g}) ) is ( -boldsymbol{3} boldsymbol{9} boldsymbol{3} . boldsymbol{5} boldsymbol{k} boldsymbol{J} quad boldsymbol{m} boldsymbol{o l}^{-1} ) Calculate the heat released upon formation of ( 35.2 g ) of ( C O_{2}(g) ) from carbon and oxygen gas. ( mathbf{A} cdot-315 k J ) в. ( 315 J ) c. ( 215 k J ) D. ( -215 . J ) | 11 |

136 | ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{I}_{2}(boldsymbol{g}) longrightarrow 2 boldsymbol{H} boldsymbol{I}(boldsymbol{g}) ) For this reaction, relate ( Delta H ) and ( Delta U ) ( mathbf{A} cdot Delta H=Delta U ) в. ( Delta H>Delta U ) ( mathbf{c} cdot Delta H<Delta U ) D. None of these | 11 |

137 | Use of thermometer is based on which law of thermodynamics? A. zeroth B. First c. second D. Third | 11 |

138 | Efficiency of a heat engine whose sink is at a temperature of ( 300 K ) is ( 40 % ). To increase the efficiency to ( 60 % ), keeping the sink temperature constant, the source temperature must be increased by : ( mathbf{A} cdot 750 K ) B. ( 500 K ) c. ( 250 K ) D. ( 1000 K ) | 11 |

139 | For spontaneous reaction, ( Delta G ) is: A . -ve B. +ve c. zero D. None of these | 11 |

140 | Which of the following statements are not true? This question has multiple correct options A. Heat is a macroscopic physical property B. Heat is an intrinsic property of a body C. Heat is stored in a body as internal energy D. Heat is path independent | 11 |

141 | Which heat depends on the direction of current? A. Joule heat B. Peltier heat c. Thompson effect D. None of these | 11 |

142 | A certain mass of gas is expanded from ( (1 L, 10 a t m) ) to ( (4 L, 5 a t m) ) against a constant external pressure of 1 atm. If the initial temperature of the gas is ( 300 K ) and the heat capacity of the process is ( 50 J /^{circ} C . ) Then the enthalpy change during the process is: ( (1 L a t m simeq 100 J) ) A ( . triangle H=15 k J ) в. ( triangle H=15.7 k J ) c. ( triangle H=14.4 k J ) D. ( triangle H=14.7 k J ) | 11 |

143 | ( n ) moles of an ideal gas undergoes a process ( A rightarrow B ) as shown in the figure. Maximum temperature of the gas during the process is: A ( cdot frac{3 P_{o} V_{o}}{2 n R} ) B. ( frac{9 P_{o} V_{o}}{4 n R} ) c. ( frac{9 P_{o} V_{o}}{2 n R} ) D. ( frac{9 P_{o} V_{o}}{n R} ) | 11 |

144 | If enthalpies of formation for ( C_{2} H_{4}(g), C O_{2}(g) ) and ( H_{2} O(I) ) at ( 25^{0} C ) and 1 atm pressure are ( 52 ;-394 ) and ( -286 k J / m o l ) respectively, then enthalpy of combustion of ( C_{2} H_{4}(g) ) will be? | 11 |

145 | ope cess ILLUSTRATION 14.12 P-T curve of PT a cyclic process is shown. Find p. 1 ——12B out the work done by the gas in the given process if number of p. moles of the gas are n. Solution. Since path AB and CD are isochoric therefore work done .). | 11 |

146 | A mass ( m_{1} ) of a substance of specific heat capacity ( c_{1} ) at temperature ( t_{1} ) is mixed with a mass ( m_{2} ) of other substance of specific heat capacity ( c_{2} ) at a lower temperature ( t_{2} . ) Deduce the expression for the temperature of the mixture. State the assumption made, if any. A ( cdot frac{m_{1} t_{1}+m_{2} t_{2}}{m_{1}+m_{2}} ) В. ( frac{m_{1} t_{1}+m_{2} t_{2}}{m_{1} c_{1}+m_{2} c_{2}} ) ( mathbf{c} cdot frac{m_{1} c_{1}+m_{2} c_{2}}{m_{1}+m_{2}} ) D. ( frac{m_{1} c_{1} t_{1}+m_{2} c_{2} t_{2}}{m_{1} c_{1}+m_{2} c_{2}} ) | 11 |

147 | Standard Gibbs Free energy change ( Delta G^{o} ) for a reaction is zero. The value of equilibrium constant of the reaction will be: ( A cdot O ) B. ( c cdot 2 ) ( D cdot 3 ) | 11 |

148 | From the following data at constant volume for combustion of benzene, calculate the heat of this reaction at constant pressure condition. ( boldsymbol{C}_{6} boldsymbol{H}_{6}(boldsymbol{l})+mathbf{1 5} / mathbf{2} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{6} boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+ ) ( mathbf{3} boldsymbol{H}_{mathbf{2}} boldsymbol{O}(boldsymbol{l}) ) ( Delta U ) at ( 25^{circ} C=-3268.12 k J ) | 11 |

149 | Which of the following thermodynamic processes can be reversed? A. Heating of an oven B. Combustion of petrol. c. Free expansion of gases D. Isothermal expansion of an ideal gas in a cylinder with frictionless piston. | 11 |

150 | Select the correct statements. a. There is asymmetry between converting work to heat and converting heat to work. b. No process is possible in which the sole result is the absorption of heat from a reservoir and its complete conversion into work. c. For every chemical reaction at equilibrium, standard change in Gibbs free energy is zero. At constant temperature and pressure, chemical reactions are spontaneous in the direction of decreasing Gibbs energy. This question has multiple correct options A. Statement a B. Statement b c. statement c D. Statement d | 11 |

151 | Given the following bond dissociation enthalpies (kJ mol-1) : begin{tabular}{c|c} ( boldsymbol{P} equiv boldsymbol{P} ) & ( mathbf{4 9 0} ) \ ( boldsymbol{P}-boldsymbol{P} ) & ( mathbf{2 0 9} ) \ ( boldsymbol{N} equiv boldsymbol{N} ) & ( mathbf{9 4 6} ) \ ( boldsymbol{N}-boldsymbol{N} ) & ( mathbf{1 6 0} ) end{tabular} Compare the enthalpy changes for the process and comment if the reactions are possible (i) ( 2 P_{2}(g) longrightarrow P_{4}(g) ) (ii) ( 2 N_{2}(g) longrightarrow N_{4}(g) ) A . (i) possible (II) not possible B. (i) possible (II) possible ( c cdot ) (i) not possible (II) possible D. (i) not possible (II)not possible | 11 |

152 | An ideal gas is expanded irreversible against 10 bar pressure from 20 litre to 30 litre. Calculate ‘ ( q^{prime} ) if process is isoenthalpic. ( mathbf{A} cdot mathbf{0} ) в. ( +100 J ) ( c cdot-100 J ) D. ( +10 k J ) | 11 |

153 | Which of the process is not the irreversible process? A. The free expansion of gas B. When a vessel is heated its base is warmer than other parts C. The quasi-static isothermal expansion of ideal gas in cylinder fitted with frictionless piston D. Diffusion of gas from cylinder | 11 |

154 | The most ideal gas among real gases is: A. Hydrogen B. Helium c. Carbon dioxide D. Nitrogen | 11 |

155 | For the reaction taking place at certain temperature ( N H_{2} C O O N H_{4}(s) rightleftharpoons ) ( mathbf{2} N boldsymbol{H}_{3}(boldsymbol{g}) ) if equilibrium pressure is ( mathbf{3} boldsymbol{X} ) bar then ( Delta G^{circ} ) would be: A. ( -R T ln 9-3 R T ln X ) B. ( R T ln 4-3 R T ln X ) c. ( -3 R T ln 4 X ) D. none of these | 11 |

156 | Given ( boldsymbol{S}_{(s)}+boldsymbol{O}_{2(g)} rightarrow boldsymbol{S} boldsymbol{O}_{2(g)} ; quad boldsymbol{Delta} boldsymbol{H}= ) ( -mathbf{2 9 8 . 2 k J} ) ( boldsymbol{S} boldsymbol{O}_{2(g)}+frac{1}{2} boldsymbol{O}_{2(g)} rightarrow boldsymbol{S} boldsymbol{O}_{3(g)} ; quad boldsymbol{Delta} boldsymbol{H}= ) ( -98.7 k J ) ( boldsymbol{S O}_{boldsymbol{3}(boldsymbol{g})}+boldsymbol{H}_{2} boldsymbol{O}_{(l)} rightarrow boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4(l)} ; boldsymbol{Delta} boldsymbol{H}= ) ( -130.2 k J ) ( boldsymbol{H}_{2(g)}+frac{1}{2} boldsymbol{O}_{2(g)} rightarrow boldsymbol{H}_{2} boldsymbol{O}_{(l)} ; boldsymbol{Delta} boldsymbol{H}= ) ( -287.3 k J ) The enthalpy of formation of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) will be : ( mathbf{A} cdot-814.4 k J ) В. ( +320.5 k J ) c. ( -650.3 k J ) D . ( -933.7 k J ) | 11 |

157 | The efficiency of carnot’s engine is ( 50 % ) The temperature of its ( operatorname{sink} ) is ( 7^{circ} mathrm{C} ). To increase its efficience ( 70 % ). What is the increase in temperature of the source? | 11 |

158 | Which of the following processes described below is irreversible? A. The increase in temperature of an iron rod by hammering it. B. A gas in a small container at a temperature ( T_{1} ) is brought in contact with a big reservoir at a higher temperature ( T_{2} ) which increases the temperature of the gas. C. An ideal gas is enclosed in a piston cylinder arrangement with adiabatic walls.A weight ( mathrm{W} ) is added to the piston resulting in compression of gas. D. All of above | 11 |

159 | Assertion In an ideal thermodynamically reversible process, the energy from work performed by or on the system would be maximized, and that from heat would be minimized. Reason A reversible process is a process whose direction can be “reversed” by inducing infinitesimal changes to some property of the system via its surroundings, while not increasing entropy. 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 | 11 |

160 | Assertion Specific heat does not depend upon the mass of the substance. Reason Thermal capacity depends on the mass of the substance. 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 | 11 |

161 | Which of the following statements are correct? This question has multiple correct options A. ( Delta H ) is -ve for exothermic reaction B. ( Delta H ) is +ve for exothermic reactions C. The heat of neutralization of strong acids and strong bases is constant D. The enthalpy of fusion is positive | 11 |

162 | An ideal gas is allowed to expand from ( 5 L ) to ( 15 L ) once rapidly and once very slowly. The magnitude of work done in two processes are ( W_{1} ) and ( W_{2} ), they are related as: A. ( W_{1}=W_{2} ) в. ( W_{1}>W_{2} ) c. ( W_{1}<W_{2} ) D. data is insufficient | 11 |

163 | A negative value for this term indicates that a reaction process will occur spontaneously. A. Gibbs Free Energy B. Entropy c. Enthalpy D. Calorimetry | 11 |

164 | 7. If Cp and C, denote the specific heats of nitrogen per unit mass at constant pressure and constant volume. respectively, then (a) Cp-C= R/28 (b) Cp-C, = R/14 (c) Cp – C, = R (d) Cp-C, = 28 R (AIEEE 2007) | 11 |

165 | 45. A sphere, a cube and a thin circular plate are made of same substance and all have same mass. These are heated to 200°C and then placed in a room. Then the (a) Temperature of sphere drops to room temperature at last (b) Temperature of cube drops to room temperature at last (C) Temperature of thin circular plate drop to room temperature at last (d) Temperatures of all the three drop to room temperature at the same time | 11 |

166 | If the Gibbs free energy change when 1 mole of ( N a C l ) is dissolved in water at ( 298 mathrm{K} ) is ( x mathrm{kJ}, ) then ( -1000 x ) is Given that, (a) Lattice energy of ( N a C l= ) ( 778 k J m o l^{-1} ) (b) Hydration energy of ( N a C l= ) ( -774.3 k J m o l^{-1} ) (c) Entropy change at ( 298 K= ) 43 Jmol( ^{-1} ) A. 9117 B. 9441 c. 9114 D. 9141 | 11 |

167 | 25. It moles of diatomic gas and 1 mole of monatomic gas are mixed, then the ratio of specific heats for the mixture is 61 + | 11 |

168 | Which of the following engines is more efficient? A. Heat utilised – 80 kilojoules, work done – 32 kilojoules B. Heat utilised – 60 kilojoules, work done – 12 kilojoules C. Heat utilised – 50 kilojoules, work done – 25 kilojoules D. Heat utilised – 90 kilojoules, work done – 27 kilojoules | 11 |

169 | Heat of combustion of ( boldsymbol{C H}_{4}, boldsymbol{C}_{2} boldsymbol{H}_{6} ) and ( C_{3} H_{8} ) are respectively -210,-368.4 and ( -526.8 mathrm{Kcal} ) mol ( _{1} ) Hence, heat of combustion of ( C_{8} H_{16} ) is approximately: A. -1267.2 Kcal / mol в. -684 Кса( / ) (тод c. ( -840 K c a l / m o l ) D. ( -1000 K ) cal ( / ) mol | 11 |

170 | 14. 100 g of water is heated from 30°C to 50°C. Ignoring the slight expansion of the water, the change in its internal energy is (specific heat of water is 4184 J/Kg/K) (a) 4.2 kJ (b) 8.4 kJ (c) 84 kJ (d) 2.1 kJ (AIEEE 2011) | 11 |

171 | The specific heat capacities of two bodies ( A ) and ( B ) is 1: 2 and masses in the ratio 3: 4 respectively. The ratio of their heat capacities is : A .3: 2 B. 2:3 ( c cdot 7: 16 ) D. 3:8 | 11 |

172 | Q2. When is bond energy equal to bond dissociation energy? | 11 |

173 | Assertion Woolen clothes keep the body warm in winter Reason Air is a bad conductor of heat. 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 | 11 |

174 | The specific heat of an ideal gas varies as ( mathbf{A} cdot T^{3} ) в. ( T^{2} ) c. ( T^{text {। }} ) D. ( T^{circ} ) | 11 |

175 | If ( Delta G ) standard is zero, this means: A. the reaction is spontaneous at standard conditions B. the reaction is non spontaneous at standard conditions C. the system is at equilibrium at standard conditions D. the reaction is both non spontaneous and at equilibrium E. the reaction is both spontaneous and at equilibrium | 11 |

176 | Heat absorbed or lost by a substance is proportional to and | 11 |

177 | Q12. What is the condition for spontaneity in terms of free energy change? Yeva | 11 |

178 | Assertion The endothermic reactions are favoured at lower temperature and the exothermic reactions are favoured at higher temperature. Reason When a system in equilibrium is disturbed by changing the temperature, it will tend to adjust itself so as to overcome the effect of the 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 | 11 |

179 | Steam engines of Indian railways are replaced with diesel engine. Justify this move with two scientific reasons. | 11 |

180 | A reaction that absorbs heat is: A. Endothermic B. An equilibrium process c. spontaneous D. Non-spontaneous E. Exothermic | 11 |

181 | A quantity of heat ‘Q’ is supplied to a mono-atomic ideal gas which expands at constant pressure. The fraction of heat that goes into work done by the gas is: A ( cdot frac{2}{5} ) B. ( frac{3}{5} ) ( c cdot frac{2}{3} ) D. | 11 |

182 | ( P-V ) diagram of an ideal gas for a process ( A B C ) is as shown in the figure. If the total heat absorbed or released by the gas during the process ( A B C ) is ( operatorname{given} operatorname{by} boldsymbol{H}=-boldsymbol{x} boldsymbol{P}_{0} boldsymbol{V}_{0}, ) what is the value of ( x ) ? | 11 |

183 | A gas mixture 3.67 L in volume contain ( C_{2} H_{4} ) and ( C H_{4} ) is proportion of 2: 1 by moles and is at ( 25^{circ} mathrm{C} ) and 1 atm. If the ( boldsymbol{Delta} boldsymbol{H}_{C}^{circ}left(boldsymbol{C}_{2} boldsymbol{H}_{4}right) ) and ( boldsymbol{Delta} boldsymbol{H}_{C}^{circ}left(boldsymbol{C} boldsymbol{H}_{4}right) ) are -1400 and ( -900 mathrm{kJ} / mathrm{mol} ) find heat evolved on burning this mixture A. ( 20.91 mathrm{kJ} ) J. B. 50.88 kJ c. 185 k D. 160 k | 11 |

184 | Assertion ( C_{P}-C_{V}=R ) for an ideal gas. Reason ( left[frac{partial E}{partial V}right]_{T}=0 ) for an ideal 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. Both Assertion and Reason are incorrect | 11 |

185 | Which of the following is an intensive property? A. Specific heat capacity B. Heat capacity c. Gibb’s energy D. Entropy | 11 |

186 | A thermodynamical system is changed from state ( left(P_{1}, V_{1}right) ) to ( left(P_{2}, V_{2}right) ) by two different processes, the quantity which will remain same will be A. ( Delta Q ) в. ( Delta W ) c. ( Delta Q+Delta W ) D. ( Delta Q-Delta W ) | 11 |

187 | Which of the following options is correct regarding spontaneity of a process occurring on a system in which only pressure-volume? work is involved and S, ( G, C I, H, V, ) and ( P ) have usual meaning as in thermodynamics? A ( cdot(d G)_{U, V}0 ) B . ( (d H) s, v<0,(d G)_{T, P}<0 ) c. ( (d U)_{s, V}<0,(d G)_{T, V}0,(d G)_{T, P}<0 ) | 11 |

188 | When a solution of 500 m ( L ) of ( 2 M ) ( K O H ) is added to ( 500 m L ) of ( 2 M H C l ) then the rise temperature ( T_{1} ) is noted. When the same experiment is repeated by mixing ( 250 m L ) of each solution, the rise in temperature ( T_{2} ) is noted : A ( cdot T_{1}=T_{2} ) В. ( T_{1}=2 T_{2} ) ( mathbf{c} cdot T_{2}=2 T_{1} ) D. ( T_{1}=4 T_{2} ) | 11 |

189 | Dissociation of water takes place in two steps: ( boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{H}^{+}+boldsymbol{O} boldsymbol{H}^{-} ; boldsymbol{Delta} boldsymbol{H}=+497.8 mathrm{kJ} ) ( O H^{-} rightarrow H^{+}+O^{2-} ; Delta H=+428.5 mathrm{kJ} ) What is the bond energy of ( 0-H ) bond? A . ( 463.15 mathrm{kJ} mathrm{mol}^{-1} ) В. 428.5 k ( mathrm{mol}^{-1} ) c. ( 69.3 mathrm{kJ} mathrm{mol}^{-1} ) D. 926.3 kJ ( m o l^{-1} ) | 11 |

190 | A gas is filled in a cylinder, its temperature is increased by ( 20 % ) on kelvin scale and volume is reduced by 10%. How much percentage of the gas will leak out: A . ( 40 % ) B. 30% c. ( 15 % ) D. ( 25 % ) | 11 |

191 | van’t Hoff equation is This question has multiple correct options ( mathbf{A} cdot(d / d T) ln K=-Delta H / R T^{2} ) B ( cdot(d / d T) ln K=+Delta H / R T^{2} ) ( mathbf{c} cdot(d / d T) ln K=-Delta H / R T ) D ( cdot K=A e^{Delta H / R T} ) | 11 |

192 | The incorrect IUPAC convention is – (May have one or more correct answers) This question has multiple correct options A. Heat gained by system +ve sign B. Work done by system – ve sign C. Work done on the system +ve sign D. Heat gained by system -ve sign | 11 |

193 | divided into three parts ( A, B ) and ( C ) Piston I and II are connected by a rigid rod and can move without friction inside the cylinder. Piston I is perfectly conducting while piston II is perfectly insulating. The initial state of ( operatorname{gas}(gamma= ) 1.5) present in each compartment ( mathbf{A}, mathbf{B} ) and ( C ) is as shown. Now, compartment ( A ) is slowly given heat through a heater ( H ) such that the final volume of ( C ) becomes ( frac{4 V_{0}}{9} . ) Assume the gas to be ideal and find the heat supplied by the heater. A ( .18 P_{o} V_{o} ) B. ( 12 P_{o} V_{o} ) ( mathrm{c} cdot 9 P_{o} V_{o} ) D. ( 25 P_{o} V_{o} ) | 11 |

194 | ( ln ) a closed system ( : boldsymbol{A}(s) rightleftharpoons 2 boldsymbol{B}(boldsymbol{g})+ ) ( 3 C(g) ) if the partial pressure ( C ) is of doubled then partial pressure B wil be: A. Twice the original pressure B. Half of its original pressure c. ( frac{1}{2 sqrt{2}} ) times, the original pressure D. ( 2 sqrt{2} ) times its original pressure | 11 |

195 | Two moles of an ideal mono-atomic gas is taken through a cyclic process as shown in the ( P-T ) diagram. In the process ( B C, P T^{2}= ) constant. Then the ratio of heat absorbed and heat released by the gas during the process ( A B ) and process ( B C ) respectively is:- ( A cdot 2 ) B. 3 ( c .5: 6 ) ( D . ) | 11 |

196 | Assertion An endothermic reaction has a positive ( Delta H ) value because Reason In an endothermic reaction, the total enthalpy (heat content) of the products is greater than that of the reactants. 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 | 11 |

197 | Closed system is A . Perfectly sealed B. Perfectly insulated C. Both perfectly insulated and sealed D. Neither insulated nor sealed | 11 |

198 | What is Mechanical equilibrium? A. When no mechanical work is done by one part of the system on any other part of the system. B. When no chemical work is done by one part of the system on any other part of the system. C. When mechanical work is done by one part of the system on any other part of the system. D. None of these | 11 |

199 | toppr Q Type your question. experiment to verify the value of ( Delta H_{text {solution}} ) for ammonium nitrate. She places a known amount of water in a coffee-cup calorimeter and adds a known quantity of solid ammonium nitrate. She traces the course of the reaction by use of a digital thermometer Using ( boldsymbol{q}_{text {solute}} ) and ( boldsymbol{q}_{text {water}} ) to represent the quantity of heat gained or lost by the ammonium nitrate solute itself and the water in the calorimeter, and using ( triangle boldsymbol{T} ) to represent the temperature change that she expects to observe, which combination below correctly describes the signs for ( q_{text {solute}}, boldsymbol{q}_{text {water}}, ) and ( Delta boldsymbol{T} ) ? ( A ) begin{tabular}{|c|c|} hline Variable & Sign \ hline q ( _{text {solute }} ) & ( + ) \ qwater & ( – ) \ ( Delta mathbf{T} ) & ( + ) \ hline end{tabular} в. begin{tabular}{|c|c|} hline Variable & Sign \ hline q ( _{text {solute }} ) & ( – ) \ qwater & ( + ) \ ( Delta mathbf{T} ) & ( + ) \ hline end{tabular} ( c ) begin{tabular}{|c|c|} hline Variable & Sign \ hline q solute & ( + ) \ qwater & ( – ) \ ( Delta mathbf{T} ) & ( – ) \ hline end{tabular} D. begin{tabular}{|c|c|} hline Variable & Sign \ hline q ( _{text {solute }} ) & ( – ) \ qwater & ( + ) \ ( Delta mathbf{T} ) & ( – ) \ hline end{tabular} | 11 |

200 | Which process occurs when the pressure or the volume of a system changes so dramatically and instantaneously that the other (pressure or volume in this case) does not have time to catch up. A . Reversible B. Irreversible c. Isothermal D. Adiabatic | 11 |

201 | Which one of the following pairs represents the intensive properties? A. Specific heat and temperature B. Entropy and density c. Enthalpy and mole fraction D. Heat and temperature | 11 |

202 | ( Delta H ) and ( Delta S ) for the system ( boldsymbol{H}_{2} boldsymbol{O}(l) rightleftharpoons boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) at 1 atmospheric pressure are ( 40.63 k J m o l^{-1} ) and ( 108.8 J K^{-1} m o l^{-1} ) respectively. Calculate the temperature at which the rates of forward and backward reactions will be the same. Predict the sign of free energy for this transformation above this temperature | 11 |

203 | The molar heat capacities at constant pressure (assume constant with respect to temperature) of ( A, B ) and ( C ) are in the ration of 1.5: 3.0: 2.0 If enthalpy change for the exothermic reaction ( A+2 B rightarrow 3 C ) at ( 300 K ) is ( -10 k J / m o l ) ( & C_{p, m}(B) ) is ( 300 J / m o l ) then enthalpy change at ( 310 K ) is: A . ( -8.5 k J / m o l ) B. ( 8.5 k J / ) mol c. ( -11.5 k J / ) mol D. none of these | 11 |

204 | toppr LoGıN Q Type your question the combustion reaction is ( boldsymbol{C}_{8} boldsymbol{H}_{18}+mathbf{1 2 . 1} boldsymbol{O}_{2} rightarrow mathbf{0 . 8} boldsymbol{C O}+ ) [ mathbf{7} . mathbf{2} boldsymbol{C} boldsymbol{O}_{mathbf{2}}+mathbf{9} boldsymbol{H}_{mathbf{2}} boldsymbol{O} ] Calculate the temperatures of the Gases just at the time of maximum compression and Write sum of these two temperatures. Exhaust gases leaving the cylinder if the final pressure in the cylinder is ( 200 k p a ) Relevant data neede for one burn cycle is given below: Compound ( boldsymbol{Delta} boldsymbol{H}_{f}left(boldsymbol{k} boldsymbol{J} boldsymbol{m o l}^{-1}right) ) mol ( N_{2}(g) ) 0.0 ( O_{2}(g) ) 0.0 ( mathcal{P}(g) ) -110.53 ( mathcal{P} O_{2}(g) ) -395.51 -241.82 ( H_{2} O(g) ) sooctane -187.82 | 11 |

205 | Assertion (A): According to the principle of conservation of energy all heat can be converted into mechanical work Reason (R): Due to various losses, it is impossible to convert all heat into mechanical work A. Both Assertion and Reason are true and reason is correct explanation of Assertion B. Both Assertion and Reason are true but reason is not correct explanation of Assertion c. Assertion is true but reason is false D. Both assertion and reason are false | 11 |

206 | ( Delta S_{text {Total}}=-40 k J / m o l times K ) ( boldsymbol{Delta} boldsymbol{H}_{s y s}=mathbf{2 0 0 0} boldsymbol{k J} / boldsymbol{m o l} ) ( boldsymbol{T}=mathbf{4 0 0} boldsymbol{K} ) Find out value of ( Delta S_{text {system}} ) at equilibrium? A. ( -35 k J / m o l times K ) в. ( -5 k J / m o l times K ) c. ( -20 k J / m o l times K ) D. ( -10 k J / m o l times K ) | 11 |

207 | Use the bond energies to estimate ( Delta boldsymbol{H} ) for this reaction: ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{g}) ) begin{tabular}{|c|c|} hline Bond & Bond energy \ hline ( mathrm{H}-mathrm{H} ) & ( 436 mathrm{kJ} mathrm{mol}^{-1} ) \ hline ( 0-0 ) & ( 142 mathrm{kJ} mathrm{mol}^{-1} ) \ hline ( 0=0 ) & ( 499 mathrm{kJ} mathrm{mol}^{-1} ) \ hline ( mathrm{H}-0 ) & ( 460 mathrm{k} mathrm{mol}^{-1} ) \ hline end{tabular} A. ( -127 k J ) ( J ) в. ( -109 k J ) c. ( -400 k J ) D. ( -800 k J ) | 11 |

208 | A heat engine is supplied with ( 250 mathrm{kJ} / mathrm{s} ) of heat at a constant fixed temperature of ( 227^{0} C ; ) the heat is rejected at ( 27^{0} C ) the cycle is reversible, then what amount of heat is rejected? A . 24kJ/s B. 223kJ/s c. ( 150 k J / ) D. none of the above | 11 |

209 | If ( Delta S=frac{q_{r e v}}{T}, ) then choose the incorrect statement(s). This question has multiple correct options A. ( Delta S ) is defined only for reversible process. B. For irreversible process and same process taking place reversibly, ( Delta S ) is same C. ( Delta S_{s y s} ) is always negative for irreversible process D. None of the above | 11 |

210 | A carnot engine works as a refrigerator in between ( 250 mathrm{K} ) and ( 300 mathrm{K} ). If it acquires 750 calories from heat source at low temperature, then what is the heat generated at higher temperature. (in calories)? | 11 |

211 | Q. 14 Which of the following is not correct? (a) AG is zero for a reversible reaction. (b) AG is positive for a spontaneous reaction. (c) AG is negative for a spontaneous reaction. (d) AG is positive for a non-spontaneous reaction. | 11 |

212 | For the reaction ( : boldsymbol{C l}_{2}(boldsymbol{g}) longrightarrow boldsymbol{2} boldsymbol{C l}(boldsymbol{g}) ) ( A cdot Delta H ) is positive, ( Delta ) s is positive B. ( Delta ) H is positive, ( Delta ) s is negative c. ( Delta ) H is negative, ( Delta ) s is negative D. ( Delta ) H is negative, ( Delta ) s is positive | 11 |

213 | Assertion When a vessel is heated,the heat is transferred from base to another part,bringing the vessel to uniform temperature.This process is cannot be reversed. Reason If the process is reversed it will violate the second law of thermodynamics as the part of the vessel will not get cooler spontaneously and warm up at the base. 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 | 11 |

214 | Q7. In a process, 701 J of heat is absorbed by a system and 394 ) of work is done by the system. What is the change in internal energy for the process? | 11 |

215 | Following are the thermochemical reactions: ( C(text { graphite })+frac{1}{2} O_{2} rightarrow C O ; Delta H= ) ( -110.5 mathrm{kJ} / mathrm{mol} ) ( C O+frac{1}{2} O_{2} rightarrow C O_{2} ; Delta H=-283.2 ) kJ/mol The heat of reaction (in kJ/mol) for the following reaction is: ( C(text { graphite })+O_{2} rightarrow C O_{2} ) ( mathbf{A} cdot+393.7 ) В. -393.7 c. -172.7 D. +172.7 | 11 |

216 | Heating of a wheel on applying brakes is due to the relation ( ^{mathrm{A}} cdot_{P} propto frac{1}{V} ) в. ( P propto T ) ( c . W propto Q ) D. ( V propto T ) | 11 |

217 | One mole of an ideal gas at ( 300 mathrm{K} ) is heated at constant volume ( left(V_{1}right) ) until its temperature is doubled, then it is expanded isothermally till it reaches the original the pressure. Finally, the gas is cooled at the constant pressure till system reached to the half of original volume ( left(frac{V_{1}}{2}right) . ) Determine the total work done ( (boldsymbol{w}) ) in calories. [Use ( boldsymbol{operatorname { l n }} mathbf{2}=mathbf{0 . 7 0 , 0} boldsymbol{R}=mathbf{2} mathbf{c a l} mathbf{K}^{-mathbf{1}} boldsymbol{m o l}^{-1} mathbf{j} ) | 11 |

218 | When potassium chloride is dissolved in water A. Entropy increases B. Entropy decreases C. Entropy increases and then decreases D. Free energy increases | 11 |

219 | In figure a certain mass of gas traces three path 1,2,3 from state ( A ) to the state B.If work done by the gas along the three paths are ( W_{1}, W_{2}, W_{3} ) respectively,then: A ( . W_{1} ) в. ( W_{1}=W_{2}=W_{3} ) c. ( W_{1}>W_{2}>W_{3} ) D. cannot say | 11 |

220 | Which has the highest entropy per mol of the substance? A ( . H_{2} ) at ( 25^{circ} mathrm{C} ) and 1 atm B. ( H_{2} ) at STP C. ( H_{2} ) at ( 100 mathrm{K} ) and ( 1 mathrm{atm} ) ( D cdot H_{2} ) at ( 0 mathrm{K} ) and 1 atm | 11 |

221 | A process is approximately reversible. In real life scenarios, this happens only when: A. system variables are constant B. the change in system variables is very fastt c. the change in system variables is very slow D. A or | 11 |

222 | Study the following graph and fill in the blanks. ( A ) Liquid Gas Freezing point Melting point B. Boiling Melting Boiling point Melting point ( c ) usion Vaporisation Melting point Boiling poin D. vap | 11 |

223 | Consider the below diagram of heat transfer and work transfer for a system. What will be the first law equation for the below system? A ( cdot(Q 1-Q 2)=E(W 2+W 3+W 1) ) B . ( (Q 1+Q 2)=E+(W 2+W 3+W 1) ) c. ( (Q 1-Q 2)=E+(W 2+W 3-W 1) ) D. None of the above | 11 |

224 | The products of combustion of an aliphatic thiol (RSH) at ( 298 K ) are A ( cdot C O_{2}(g), H_{2} O(g), ) and ( S O_{2}(g) ) B . ( C O_{2}(g), H_{2} O(l), ) and ( S O_{2}(g) ) c. ( C O_{2}(l), H_{2} O(l), a n d S O_{2}(g) ) D. ( C O_{2}(g), H_{2} O(l), ) and ( S O_{2}(l) ) | 11 |

225 | air expands from 5 liters to 10 liters at 2 atm pressure. External workdone is A . ( 10 J ) в. ( 1000 J ) c. ( 3000 J ) D. 300J | 11 |

226 | Diffusion of a gas in a room is not reversible because: A. entropy of a system cannot decrease. B. entropy of a system remains constant. c. entropy of universe cannot decrease D. None of the above | 11 |

227 | State whether true or false: In Carnot cycle there are total 4 processes which takes place? A. True B. False | 11 |

228 | Q19. For the reaction 2A(g) + B(g) — 2D(g) AUⓇ = – 10.5 k) and AS = – 44.1 k-1 Calculate AGe for the reaction, and predict whether the reaction may occur spontaneously. | 11 |

229 | State two factors upon which the heat absorbed by a body depends. | 11 |

230 | ( mathbb{R} ) 4 4 6 | 11 |

231 | The molar heat capacity of a monoatomic gas is: A. ( 4 / 2 R ) в. ( 3 / 2 R ) c. ( 5 / 2 R ) D. zero | 11 |

232 | Two moles of a monoatomic ideal gas undergo a cyclic process ABCDA as shown in figure. BCD is a semicircle. Find the efficiency of the cycle in ( % ) | 11 |

233 | Calculate the amount of heat energy required to raise the temperature of ( 2 g ) of mercury (Specific heat Capacity ( left.0.12 J g^{-1} o C^{-1}right) ) from ( 10^{circ} C ) to ( 30^{circ} C ) A . ( 1.2 J ) в. 2.4 c. ( 4.8 J ) D. 9.6 .5 | 11 |

234 | On a two-component solid-liquid phase diagram, an isopleth indicates which of the following? A. A region where the composition of the system is constant B. An area above which only the liquid phase exists C. A region where the pressure is constant D. An area below which only the solid phase exists | 11 |

235 | The standard enthalpy of formation of carbon – di – sulphide ( ( l ) ) is: Given the standard enthalpy of combustion of carbon (s), sulphur (s) & carbon – di – sulphide ( ( l ) ) are : -393.3,-293.72 and ( -1108.76 k J m o l^{-1} ) respectively. A. ( 128.02 mathrm{kJ} ) J. B. 456.21kJ c. 232.56 kJ D. 871.25 kJ | 11 |

236 | A reaction in which heat is absorbed is called an endothermic reaction.If true enter 1 else 0 ( A ) | 11 |

237 | Calculate the value of ( log boldsymbol{K}_{boldsymbol{p}} ) (nearest integer) for the reaction, ( N_{2}(g)+ ) ( mathbf{3} boldsymbol{H}_{mathbf{2}}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{N} boldsymbol{H}_{mathbf{3}}(boldsymbol{g}) ) at ( mathbf{2 5}^{circ} boldsymbol{C} . ) The standard enthalpy of formation of ( N H_{3}(g) ) is ( -46 mathrm{kJ} ) and standard entropies of ( N_{2}(g), H_{2}(g), N H_{3}(g) ) are ( mathbf{1 9 1}, mathbf{1 3 0}, mathbf{a n d} mathbf{1 9 2} mathbf{J K}^{-mathbf{1}} mathbf{m o l}^{-mathbf{1}} ) respectively. ( left(boldsymbol{R}=mathbf{8 . 3} boldsymbol{J} boldsymbol{K}^{-1} boldsymbol{m o l}^{-1}right) ) | 11 |

238 | Match List I with List II and select the answer from the given codes. List I List II A. ( C(s)+O_{2}(g) longrightarrow C O_{2}(g) ) ( mathbf{1} mathbf{Delta} boldsymbol{H}=mathbf{Delta} boldsymbol{U}+boldsymbol{R} boldsymbol{T} ) B. ( N_{2}(g)+3 H_{2}(g) longrightarrow 2 N H_{3}(g) ) 2. ( Delta boldsymbol{H}=boldsymbol{Delta} boldsymbol{U} ) C. ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{H} boldsymbol{S}(boldsymbol{s}) longrightarrow boldsymbol{N} boldsymbol{H}_{3}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g}) ) 3. ( Delta boldsymbol{H}=boldsymbol{Delta} boldsymbol{U}-boldsymbol{2} boldsymbol{R} boldsymbol{T} ) D. ( boldsymbol{P C l}_{5}(boldsymbol{g}) longrightarrow boldsymbol{P C l}_{3}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) ) 4. ( Delta boldsymbol{H}=boldsymbol{Delta} boldsymbol{U}+boldsymbol{2} boldsymbol{R} boldsymbol{T} ) E. ( 2 S O_{2}(g)+O_{2}(g) longrightarrow 2 S O_{3}(g) ) 5. ( Delta boldsymbol{H}=boldsymbol{Delta} boldsymbol{U}-boldsymbol{R} boldsymbol{T} ) A. ( A-1, B-2, C-3, D-4, E-5 ) B. ( A-5, B-2, C-3, D-4, E-1 ) c. ( A-1, B-3, C-4, D-2, D-5 ) D. ( A-2, B-3, C-4, D-1, E-5 ) | 11 |

239 | 4. The work done in compressing 1 kg-mol of a gas adiabatically is 146 kJ. in this process, the temperature of the gas increases by 7°C. The gas is (R = 8.3 J/mol-K) (a) diatomic (b) triatomic (c) a mixture of monatomic and diatomic (d) monatomic (AIEEE 2006) пс | 11 |

240 | A solid of mass 250 g at ( 90^{0} C ) is dropped in a calorimeter containing 100 ( g ) of water at ( 15^{0} C . ) The resulting temperature of mixture becomes ( 40^{0} C ) The mass of calorimeter is 100 g and its specific heat capacity is ( 0.1 mathrm{cal} / mathrm{g}^{0} mathrm{C} ) Find the specific heat capacity of the solid. | 11 |

241 | Calculate net work done by the gas. | 11 |

242 | Which of the following statement(s) is/are true? “Internal energy of an ideal gas A. Decreases in an isobaric process B. Remains constant in an isothermal process c. Increases in an isobaric process D. Decreases in an isobaric expansion | 11 |

243 | The cycle is shown in figure is made of one mole of perfect gas in a cylinder with a piston. The processes ( A ) to ( B ) and ( mathrm{C} ) to ( mathrm{D} ) are isochoric whereas process ( mathrm{B} ) to ( C ) and ( D ) to ( A ) are adiabatic, the work done in one cycle is ( left(V_{A}=V_{B}=V, V_{C}=right. ) ( left.V_{D}=2 V text { and } Upsilon=5 / 3right) ) A ( cdotleft[1-4^{3 / 2}right]left(P_{B}-P_{A}right) V ) B ( cdot frac{3}{2}left[1-3^{2 / 3}right]left(P_{B}-P_{A}right) V ) c. ( frac{3}{2}left[1-2^{-2 / 3}right]left(P_{B}-P_{A}right) V ) D. ( frac{5}{2}left[1-2^{-2 / 3}right]left(P_{B}-P_{A}right) V ) | 11 |

244 | 2.48 Enthalpy diagram for a particular reaction is given in figure. Is it possible to decide spontaneity of a reaction from given diagram. Explain. Products 4, H, Net heat absorbed from | surroundings Reactants Reaction coordinate – | 11 |

245 | Four ( 2 c m times 2 c m times 2 c m ) cubes of ice are taken out from a refrigerator and are put in ( 200 mathrm{ml} ) of a drink at ( 10^{circ} mathrm{C} ) (a) Find the temperature of the drink when thermal equilibrium is attained in it. (b) If the ice cubs do not do not melt completely, find the amount melted. Assume that no heat is lost to the outside of the capacity. Density of ice ( =900 k g / m^{3}, ) density of the drink ( = ) ( 1000 k g / m^{3}, ) specific heat capacity of the drink ( 4200 mathrm{J} / mathrm{kg}-mathrm{K} ), latent heat of fusion of ice ( 3.4 times 10^{5} J / k g ) | 11 |

246 | ( V=kleft(frac{P}{T}right)^{0.33} ) where ( k ) is constant. It is an: A. isothermal process B. adiabatic process c. isochoric process D. isobaric process | 11 |

247 | ( Delta_{f} H^{ominus} ) per mole of ( N H_{3}(g), N O(g) ) and ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ) are ( -mathbf{1 1 . 0 4},+mathbf{2 1 . 6 0} ) and ( -68.32 K c a l, ) respectively. Calculate the standard heat of reaction at constant pressure and at a constant volume for the reaction: ( mathbf{4} boldsymbol{N} boldsymbol{H}_{3}(boldsymbol{g})+mathbf{5} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{4} boldsymbol{N} boldsymbol{O}(boldsymbol{g})+ ) ( mathbf{6} boldsymbol{H}_{mathbf{2}} boldsymbol{O}(boldsymbol{l}) ) A. ( Delta H=-279.36 K c a l Delta U=-276.38 K c a l ) В. ( Delta H=+279.36 K c a l Delta U=-276.38 K ) сад. c. ( Delta H=-279.36 K c a l Delta U=+276.38 K c a l ) D. None of these | 11 |

248 | A series combination of two Carnots engines operate between the temperatures of ( 180^{0} C ) and ( 20^{0} C . ) If the engines produce equal amount of work,then what is the intermediate temperature(ln ( ^{0} C ) )? ( A cdot 80 ) B. 90 ( c cdot 100 ) D. 110 | 11 |

249 | Assertion When a salt such as NaCl dissolves, the ( N a^{+} ) and ( C l^{-} ) ions leaving the crystal lattice acquire far greater freedom. Reason In thermodyanamic terms, the formation of solution occurs with a favourable change in free energy, i.e. ( triangle H ) has a high positive value and ( T triangle S ) a low negative vaiue. 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 | 11 |

250 | The ratio of the relative rise in pressure for adiabatic compression to that for isothermal compression is : ( A cdot gamma ) B. ( frac{1}{gamma} ) c. ( 1-gamma ) D. ( frac{1}{1-gamma} ) | 11 |

251 | The enthalpies of the elements in their standard states are assumed to be: A. zero at 298 k B. unit at 298 к c. zero at all temperatures D. zero at 273 K | 11 |

252 | A vessel contains ( N ) molecules of a gas at temperature ( T . ) Now the number of molecules is doubled, keeping the total energy in the vessel constant. The temperature of the gas is. A. ( T ) в. 27 c. ( frac{T}{2} ) D. ( sqrt{2} T ) | 11 |

253 | If there were no atmosphere, the average temperature on earth surface would be A. lower B. higher c. same D. ( 0^{circ} mathrm{C} ) | 11 |

254 | Consider the process on a system shown in fig. During the process, the work done by the system A. Continuously increases B. Continuously decreases C. First increases then decreases D. First decreases then increases | 11 |

255 | When a certain amount of ethylene was burnt, ( 622 mathrm{kJ} ) heat was evolved. If heat of combustion of ethylene is 1411 kJ, the volume of ( boldsymbol{O}_{2} ) that entered into the reaction is: A ( .296 .5 mathrm{mL} ) B . 29.62 L c. ( 6226 times 22.4 ) 느 D. 22.4 mL | 11 |

256 | The molar heat capacity ( left(C_{p}right) ) of ( C D_{2} O ) is 10 cals at ( 1000 K . ) The change in entropy associated with cooling of ( 32 g ) of ( C D_{2} O ) vapour from ( 1000 K ) to ( 100 K ) at constant pressure will be: ( (D=text { deutrium, at. mass }=2 u) ) A. -23.03 cal deg ( ^{-1} ) в. 2.303 саг de ( g^{-1} ) c. 23.03 cal deg ( ^{-1} ) D. -2.303 cal de ( g^{-1} ) | 11 |

257 | Statement As ice absorbs heat and begins to melt, its temperature remains constant Because Statement II Changes of state bring about changes in a substances potential energy, not in its kinetic energy 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 and 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. E. Both the Statement 1 and Statement 2 are not correct | 11 |

258 | Under which of the following conditions is the relation, ( Delta H=Delta U+P Delta V ) valid for closed system? A. constant pressure B. Constant temperature c. constant temperature and pressure D. constant temperature, pressure and composition | 11 |

259 | Consider the following reactions: ( C(s)+O_{2}(g) rightarrow C O_{2}(g)+x k J ) ( C O(g)+frac{1}{2} O_{2}(g) rightarrow C O_{2}(g)+y k J ) The heat of formation of ( mathrm{CO}(mathrm{g}) ) is : ( A cdot-(x+y) k J / m o l ) B. ( (x-y) ) kJ/mol c. ( (y-x) ) k) ( int m o ) D. None of these | 11 |

260 | 2. 22 Standard molar enthalpy of formation, A,Hº is just a special case of enthalpy of reaction, A.H. Is the A, for the following reaction same as A, H®? Give reason for your answer. Ca0(s)+ CO2(g) → Caco, (s);A ,H=-178.3 kJ mol | 11 |

261 | ΔΗ – ΔΟ Q9. Calculate 4.G® for conversion of oxygen to ozone, 3/2 0,8) ► 03(8) at 298 K. If K, for this conversion is 2.47 x 10-29. | 11 |

262 | When ( Delta G ) is zero: A. reaction moves in forward direction B. reaction moves in backward direction C . system is at equilibrium D. none of these | 11 |

263 | The specific heat of is negative. ( A cdot C O_{2} ) B. Ne c. saturated vapoures D. none | 11 |

264 | For the equilibrium ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) rightleftharpoons boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) at 1 atm and ( 298 K ) A. standard free energy change is equal to zero ( left(triangle G^{circ}=right. ) 0) B. free energy change is less than zero ( ( triangle G<0 ) ) c. standard free energy change is less than zero ( left(triangle G^{circ}0right) ) | 11 |

265 | The bond dissociation energies of ( X_{2}, Y_{2} ) and ( X Y ) are in the ratio of 1 ( 0.5: 1 . Delta H ) for the formation of ( X Y ) is ( -200 k J m o l^{-1} . ) The bond dissociation energy of ( boldsymbol{X}_{2} ) will be: В. 200 kJ mol- c. ( 400 mathrm{kJ} mathrm{mol}^{-1} ) D. 100 k J mol( ^{-} ) | 11 |

266 | The quantity of heat required to raise the temperature of unit mass of a given body through ( 1^{circ} C ) is known as | 11 |

267 | A Carnot refrigerator extracts heat from water at ( 0^{circ} mathrm{C} ) and rejects it to a room at ( 24.4^{circ} mathrm{C} . ) The work required by the refrigerator for every ( 1 mathrm{kg} ) of water converted into ice is (Latent heat of ice ( =336 mathrm{kj} mathrm{kg}^{-1} ) ) A . ( 24.4 k j ) в. ( 30 k j ) c. ( 336 k j ) D. ( 11.2 k j ) | 11 |

268 | Which statement is true for second law of thermodynamics? A. Heat can flow spontaneously from a cold object to a hot object. B. You can not create a heat engine which extracts heat and converts it all to useful work c. According to Plank-Kelvin’s law under some circumstances a perfect heat engine is possible. D. None of these. | 11 |

269 | When enthalpy and entropy changes for a chemical reaction are ( 2.5 times 10^{3} ) cals and 7.4 cals ( operatorname{deg}^{-1}, ) respectively. The reaction at ( 298 K ) will be : A. spontaneous B. reversible c. irreversible D. non-spontaneous | 11 |

270 | A gas is at ( 10 P a ) pressure with a volume ( 8 m^{3} . ) When ( 100 J ) of heat is supplied to the gas, it expands to ( 10 m^{3} ) at constant pressure. The change in its internal energy is : A . ( 80 J ) В. ( -80 J ) c. ( 20 J ) D. ( -20 J ) | 11 |

271 | For a reaction to be spontaneous in neither direction, which of the following is/are correct regarding the closed system? (1) ( (Delta G)_{T, P}=0 ) (2) ( (Delta G)_{T, P}0 ) codes: A. 1,2,3 are correct B. 1 and 2 are correct c. 2 and 4 are correct D. 1 and 3 are correct | 11 |

272 | Q16. How are internal energy change, free energy change and entropy change are related to one another? ar rar connotantra procurel | 11 |

273 | When ( 1.0 g ) of oxalic acid ( left(H_{2} C_{2} O_{4}right) ) is burned in a bomb calorimeter whose heat capacity is ( 8.75 k J / K ), the temperature increases by ( 0.312 K . ) The enthalpy of combustion of oxalic acid at ( mathbf{2 7}^{circ} boldsymbol{C} ) is : ( boldsymbol{H}_{2} boldsymbol{C}_{2} boldsymbol{O}_{4}(boldsymbol{l})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l})+ ) ( 2 C O_{2}(g) ) A . ( -245.7 k J / ) mol B . ( -244.452 k J / ) mol c. ( -246.947 k J / ) mol D. none of these | 11 |

274 | How much energy is given off when ( 22 g ) of ( C_{3} H_{8} ) burns? The heat of combustion for ( C_{3} H_{8} ) is ( mathbf{2}, mathbf{2 2 0} boldsymbol{k} boldsymbol{J} / boldsymbol{m o l} ) A ( .2242 k J ) в. ( 1110 k J ) c. ( 2220 k J ) D. ( 1500 k J ) | 11 |

275 | Change in internal energy of the gas in the isobaric process is: A ( .2 .5 times 10^{4} J ) В. ( 1.2 times 10^{6} J ) c. ( 3 times 10^{5} J ) D. ( 0.5 times 10^{3} J ) | 11 |

276 | ( frac{1}{1} ) ( frac{1}{2} ) ( frac{1}{2} ) | 11 |

277 | A barometer made of very narrow tube is placed at normal temperature and pressure. The coefficient of volume expansion of mercury is 0.00018 per ( ^{circ} C ) and that of the tube is negligible. The temperature of mercury in the barometer is now raised by ( 1^{circ} mathrm{C} ), but the temperature of the atmosphere does not change. Then the mercury height in the tube remains unchanged. A. True B. False | 11 |

278 | Effect to pressure on ( Delta boldsymbol{H} ) is negligible if ( Delta n= ) | 11 |

279 | The standard molar heats of formation of ethane, ( C O_{2} ) and ( H_{2} O(l) ) are respectively -21.1,-94,1 and ( -68.3 k c a l . ) The standard molar heat of combustion of ethane will be: A. ( -372 k c a l ) В. ( -240 k c a l ) c. ( 162 k c a l ) D. ( 183.5 k c a l ) | 11 |

280 | The cause of irreversibility of a natura process is: state B. A process often involves dissipative effects c. Both A and B D. None of the above | 11 |

281 | The temperature-entropy diagram of a reversible engine cycle is given in the figure. Its efficiency is- ( A cdot frac{1}{2} ) B. ( frac{1}{4} ) ( c cdot frac{1}{3} ) D. 2 | 11 |

282 | Calculate work done. A .12 atm ( times 1 ) B. ( 24 operatorname{atm} times 1 ) c. 48 atm ( x ) ।t D. 36 atm/l | 11 |

283 | When 0.2 mole of ethane is burnt completely in a bomb calorimeter, the temperature of calorimeter system increased by ( 2 K ). What should be the increase in temperature of the same calorimeter system, when 0.4 mole of ( C H_{4} ) is burnt? Given: ( Delta_{C} U_{C_{2} H_{6}(g)}=-400 K c a l / m o l ) and ( Delta_{c} U_{C H_{4}(g)}=-200 K c a l / m o l ) A . ( 2 K ) в. 4 К ( c cdot 1 k ) D. 3 K | 11 |

284 | Two vessels each of volume ( V ) have air at pressure ( boldsymbol{P}_{1} ) and temperature ( boldsymbol{T}_{1} ). They are connected through a narrow tube and in one of the vessel the temperature changes from ( T_{1} ) to ( T_{2} ) keeping the other at ( T_{1} ). Find the pressure of the gas.Assume the volume of gas is negligible. A ( cdot frac{2 P_{1} T_{1}}{T_{1}+T_{2}} ) в. ( frac{2 P_{1}}{T_{1}+T_{2}} ) c. ( frac{2 P_{1} T_{2}}{T_{1}+T_{2}} ) D. None of these | 11 |

285 | What is the enthalpy of vaporisation of liquid water in ( k J ) mol ( ^{-1} ) if: ( (mathrm{i}) boldsymbol{H}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{H}_{2} boldsymbol{O}(l)+ ) ( 285.77 k J m o l^{-1} ) ( (text { ii }) boldsymbol{H}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{v})+ ) ( 241.84 k J ) mol ( ^{-1} ) ( mathbf{A} cdot+43.93 ) B . -43.93 c. +527.61 D. -527.61 | 11 |

286 | Q10. What do you mean by entropy? in of randon | 11 |

287 | The cyclic process from ( X ) to ( Y ) is an isothermal process. If the pressure of the gas at ( X ) is ( 4.0 mathrm{kPa} ) and the volume is 6.0 cubic meters, and if the pressure at ( Y ) is ( 8.0 mathrm{kPa} ), what is the volume of the gas at ( Y ? ) A . 12.0 cubic meters B. 16.0 cubic meters c. 3.0 cubic meters D. 4.0 cubic meters E . 2.0 cubic meters | 11 |

288 | The amount of heat energy required to raise the temperature of 1 g of Helium at ( mathrm{NTP}, ) from ( boldsymbol{T}_{1} boldsymbol{K} ) to ( boldsymbol{T}_{2} boldsymbol{K} ) is A ( cdot frac{3}{8} N_{a} k_{B}left(T_{2}-T_{1}right) ) B ( cdot frac{3}{2} N_{a} k_{B}left(T_{2}-T_{1}right) ) c. ( frac{3}{4} N_{a} k_{B}left(T_{2}-T_{1}right) ) D. ( frac{3}{4} N_{a} k_{B}left(frac{T_{2}}{T_{1}}right) ) | 11 |

289 | One mole of helium gas is heated in a vessel with variable volume so that the pressure is fixed at 1 atmosphere. When the temperature increased from ( 273 mathrm{K} ) to ( 274 mathrm{K}, ) it was found that ( 21 J ) of heat energy was absorbed. The value of ( Delta U, ) and ( Delta H, ) respectively, are: A. 4.4 Jand ( 12.7 mathrm{J} ) B. 12.7Jand21J c. 21 Jand ( 29.3 mathrm{J} ) D. 29.3Jand21J | 11 |

290 | A system absorbs ( 10^{3} ) cal of heat and the system does ( 1677.3 J ) work. The internal energy of the system increases by ( 2515 . J . ) The value of J is A. ( 4.19 mathrm{J} / mathrm{cal} ) в. 4.18 cal ( / J ) c. ( 42 J / ) cal ( l ) D. ( 420 J / c a l ) | 11 |

291 | Q3. Many thermodynamically feasible reactions do not occur under ordinary conditions. Why? montants may be less | 11 |

292 | ( 200 g ) water is heated from ( 40^{circ} mathrm{C} ) to ( 60^{circ} mathrm{C} . ) Ignoring the slight expansion of water, the change in its internal energy is close to: (Given specific heat of water ( = ) ( 4184 J / k g / K) ) A. ( 167.4 k J ) в. ( 16.7 k J ) c. ( 8.4 k J ) D. ( 4.2 k J ) | 11 |

293 | For adiabatic expansion of a monoatomic perfect gas, the volume increases by ( 2.4 % . ) What is the percentage decreases in pressure? A . ( 2.4 % ) в. ( 4.0 % ) c. ( 4.8 % ) D. ( 7.1 % ) | 11 |

294 | 29. 5 g of water at U) 41.2 min at 30°C and 5 g of ice at -20°C are mixed a calorimeter. Find the final temperature of the ssume water equivalent of calorimeter to be ible. sp. heats of ice and water are 0.5 and 1 calo co together in a calorin mixture. Assume wa negligible, sp. heats of (a) 0°C (C) -30°C and latent heat of ice is 80 callo (b) 10°C (d) >10°C vessel contains Moramo of | 11 |

295 | Assertion Under free expansion, ( left(frac{d U}{d V}right)_{T} ) is ( +v e ) when attractive forces are dominant between gas molecules [U, V, T represent internal energy, volume and temperature of gas respectively]. Reason Internal energy is a state function. 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 | 11 |

296 | 300 gm of water at ( 25^{circ} mathrm{C} ) is added to 100 ( mathrm{gm} ) of ice at ( 0^{circ} mathrm{C} ). Final temperature of the mixture is: A ( cdot-frac{5^{circ}}{3} C ) В. ( -frac{5^{circ}}{2} C ) ( mathbf{c} cdot-5^{circ} C ) D. ( 0^{circ} mathrm{C} ) | 11 |

297 | Calculate the heat of formation of methane, given that heat of formation of water ( = ) ( -286 k J quad m o l^{-1} ) heat of combustion of methane ( = ) ( -890 k J quad m o l^{-1} ) heat of combustion of carbon ( = ) ( -393.5 k J quad m o l^{-1} ) A ( .75 .5 ~ k J ~ m o l- ) – В. ( -75.5 mathrm{kJ} mathrm{mol}^{-1} ) c. ( -55.5 ~ k J ) mol ( ^{-1} ) D. ( 55.5 ~ k J ) mol ( ^{-1} ) | 11 |

298 | For the combustion reaction at ( 298 K ) ( mathbf{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s})+mathbf{1} / mathbf{2} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{2} boldsymbol{A} boldsymbol{g}_{2} boldsymbol{O}(boldsymbol{s}) ) Which of the following alternative is correct? ( mathbf{A} cdot Delta H=Delta U ) в. ( Delta H>Delta U ) c. ( Delta H<Delta U ) D. ( Delta )Hand( Delta U ) bear no relation with each other | 11 |

299 | Which of the following is true about refrigeration? A. Heat is removed from the inside of the refrigerator B. Cold air is produced inside the refrigerator C. Hot air is removed from the inside of the refrigerator D. Hot air is changed to a cold condensate inside the refrigerator E. Hot air inside the refrigerator is expanded to remove its heat | 11 |

300 | Identify the best curve which represents how pressure and volume change in an isothermal process? ( A ) в. c. D. E. | 11 |

301 | When an ideal diatomic gas is heated at constant pressure, the fraction of the heat energy supplied which increased the internal energy of the gas is: A ( cdot frac{2}{5} ) B. ( frac{3}{5} ) ( c cdot frac{3}{7} ) D. | 11 |

302 | For a process to be in equilibrium: A. ( Delta S_{text {system}}+Delta S_{S u r r}=0 ) B. ( Delta S_{text {system}}=0 ) c. ( Delta S_{text {system}}=Delta S_{text {Surr}} ) D. ( Delta S_{S u r r}=0 ) | 11 |

303 | The thermal capacity of 10 gm of the substance is 8 calories. Then its specific heat is. A. 0.8 в. 1.25 c. 0.4 D. ( 0 . ) | 11 |

304 | Q5. At what temperature entropy of a substance is zero? | 11 |

305 | What is intensive property? Give one example. | 11 |

306 | If heat of formation of ( C a C l_{2} ) and ( N a C l ) are 191 and 97.5 kcal, the heat of reaction for ( boldsymbol{C a} boldsymbol{C l}_{2}+boldsymbol{2} boldsymbol{N} boldsymbol{a} longrightarrow ) ( 2 N a C l+C a ) is: | 11 |

307 | UUUUULILLLILUL LUI DULU. Q. 4 The volume of gas is reduced to half from its original volume. The specific heat will be (a) reduce to half apab (b) be doubled (c) remain constant (d) increase four times . | 11 |

308 | The specific heat capacity of water is: A ( cdot 1 ) cal ( g^{-1} ) в. 10 cal ( g^{-1} ) c. 2 cal ( g^{-1} ) D. 30 cal ( g^{-1} ) | 11 |

309 | An ideal gas having molar specific heat capacity at constant volume is ( frac{3}{2} R, ) the molar specific heat capacities at constant pressure is : A ( cdot frac{1}{2} R ) в. ( frac{5}{2} ) R c. ( frac{7}{2} ) R D. ( frac{9}{2} ) R | 11 |

310 | Which of the following is a path function? A. Internal Energy B. Enthalpy c. work D. All of the above | 11 |

311 | ( 2 H I(g) longrightarrow H_{2}(g)+I_{2}(g) ) For this reaction relate ( Delta H ) and ( Delta U ) A. ( Delta H=Delta U ) в. ( Delta H>Delta U ) c. ( Delta H<Delta U ) D. None of these | 11 |

312 | What is abbreviated as ‘H’? A. Standard voltaic potential B. Entropy c. Enthalpy D. Reaction rate | 11 |

313 | How do you define specific heat ? What is specific heat of water? | 11 |

314 | Q9. Calculate the number of kl of heat necessary to raise the temperature of 60 g of aluminium from 35°C to 55°C. Molar heat capacity of Al is 24 J mol-1 K-I. | 11 |

315 | ( boldsymbol{C a} boldsymbol{C O}_{3}(boldsymbol{s}) longrightarrow boldsymbol{C a O}(boldsymbol{s})+boldsymbol{C O}_{2}(boldsymbol{g}) ) For this reaction relate ( Delta H ) and ( Delta U ) A. ( Delta H=Delta U ) в. ( Delta H>Delta U ) c. ( Delta H<Delta U ) D. None of these | 11 |

316 | Using equipartition of energy, the specific heat ( left(operatorname{in} J k g^{-1} K^{-1}right) ) of aluminium at high temperature can be estimated to be (atomic weight of aluminium ( =27) ) A . 25 B. 1850 ( c cdot 410 ) D. 923 | 11 |

317 | In which of the following process the system and surrounding comes back to its original state after the process is complete? A. Quasi-static Process B. Reversible process c. Both a and ( b ) D. Isobaric process | 11 |

318 | Two different adiabatic parts for the same gas intersect two isothermals at ( T_{1} ) and ( T_{2} ) as shown in P-V diagram Then the ratio of ( frac{V_{a}}{V_{b}} ) will be: A ( cdot frac{V_{c}}{longrightarrow} ) ( overline{V_{d}} ) B. ( underline{V}_{d} ) ( V_{c} ) ( c cdot gamma frac{V_{d}}{V} ) D. ( frac{1}{sim} frac{V_{d}}{V} ) | 11 |

319 | Q Type your question ( A ) ( (A) rightarrow(text { iii }),(B) rightarrow(i),(C) rightarrow(i i),(D) rightarrow(i v) ) ( mathbf{B} cdot(A) rightarrow(i i i),(B) rightarrow(i v),(C) rightarrow(i),(D) rightarrow(i i) ) C ( cdot(A) rightarrow(text { ii }),(B) rightarrow(i),(C) rightarrow(i v),(D) rightarrow( ) iii) D. ( (A) rightarrow(text { iv }),(B) rightarrow(i i),(C) rightarrow(i),(D) rightarrow(text { iii }) ) | 11 |

320 | Q Type your question corresponding to some points in the figure are: ( boldsymbol{P}_{boldsymbol{A}}=mathbf{3} times mathbf{1 0}^{mathbf{4}} boldsymbol{P a} ) ( boldsymbol{V}_{boldsymbol{A}}=boldsymbol{2} times mathbf{1 0}^{-mathbf{3}} boldsymbol{m}^{-3} ) ( boldsymbol{P}_{boldsymbol{B}}=boldsymbol{8} times 10^{4} boldsymbol{P} boldsymbol{a} ) ( V_{C}=5 times 10^{-3} m^{-3} ) In the process ( A B, 600 J ) of heat is added to the system and in process BC, 200 J of heat is added to the system. The change in internal energy of the system in process AC would be A. 560 B. 800J c. 600 J D. 640 | 11 |

321 | The heat of carbon combustion with the ( C O_{2} ) formation, is ( -393.5 K J / m o l ) and the heat of ( C O ) combustion with the formation of ( C O_{2}, ) is ( -283 K J / ) mol calculate the heat of combustion of carbon there in ( C O ) | 11 |

322 | Two moles of a monoatomic gas at 300 Kis kept in a non-conducting container enclosed by a piston. Gas is now compressed to increase the temperature from ( 300 mathrm{K} ) to ( 400 mathrm{K} ). Find work done by the gas ( (boldsymbol{R}= ) ( left.frac{mathbf{2 5}}{mathbf{3}} boldsymbol{J} / boldsymbol{m o l} boldsymbol{K}right) ) | 11 |

323 | The cell in which the following reaction occurs: ( 2 F e_{(a q)}^{3+}+2 I_{(a q)}^{-} rightarrow 2 F e_{(a q)}^{2+}+I_{2(s)} ) has ( E_{c e l l}^{o}=0.236 V ) at ( 298 K ) The equilibrium constant of the cell reaction is: A. ( 6.69 times 10^{-7} ) B . ( 7.69 times 10^{-7} ) c. ( 9.69 times 10^{7} ) D. ( 6.69 times 10^{7} ) | 11 |

324 | For the same mass, which one of the following has the maximum thermal capacity? A. wood B. copper c. water D. Ice | 11 |

325 | A spontaneous process is a process which is instantaneous.lf true enter 1 else o ( A ) | 11 |

326 | Q17. For a reaction at 298 K 2A + BC AH = 400 kJ mol-1 and AS = 0.2 kJ K-1 mol-1 At what temperature will the reaction become spontaneous considering AH and AS to be constant over the temperature range? | 11 |

327 | Water if often used as a coolant, a liquid to remove heat from things like hot engines. One reasons is that water can absorb a lot of heat without changing temperature too much. What property of water allows it to do this? | 11 |

328 | ( (triangle boldsymbol{H}-triangle boldsymbol{E}) ) is maximum at a given temperature in case of: ( mathbf{A} cdot P C l_{5}(g) rightarrow P C l_{3}(g)+C l_{2}(g) ) B. ( C a C O_{3}(s) rightarrow C a O_{3}(s)+C O_{2}(g) ) ( mathbf{c} cdot N H_{4} H S(s) rightarrow N H_{3}(g)+H_{2} S(g) ) D. ( N_{2}(g)+O_{2}(g) rightarrow 2 N O(g) ) | 11 |

329 | (i) ( ln ) a process 10 gm of ice at ( -5^{circ} C ) is converted into steam at ( 100^{circ} mathrm{C} ). If specific heat of water 1 cal ( g^{-1 circ} C^{-1}, ) the heat required to rise the temperature of water 10 g from ( 0^{circ} mathrm{C} ) to ( 100^{circ} mathrm{C} ) A . ( 100 c a l ) в. 1000call ( mathbf{c} cdot 10^{4} ) cal D. ( 10^{5} ) cal | 11 |

330 | A liquid A has specific heat capacity higher than the liquid B. Which liquid can be used as a coolant in car radiators? ( A cdot A ) B. B c. Both can be used D. Data insufficient | 11 |

331 | Using the data given below, establish that the vaporization of ( C C l_{4}(l) ) at 298K to produce ( C C l_{4}(g) ) at 1 atm pressure does not occur spontaneously. Given ( boldsymbol{C C l}_{4}(boldsymbol{l}, mathbf{1 a t m}) rightarrow boldsymbol{C C l}_{4}(boldsymbol{g}, mathbf{1 a t m}) ) ( boldsymbol{Delta} boldsymbol{S}^{o}=boldsymbol{9} boldsymbol{4} . boldsymbol{9} boldsymbol{8} boldsymbol{J} boldsymbol{K}^{-1} boldsymbol{m} boldsymbol{o l}^{-1} ) ( boldsymbol{Delta} boldsymbol{H}_{f}^{o}left(boldsymbol{C} boldsymbol{C l}_{4}, boldsymbol{g}right)=mathbf{1 0 6 . 7} boldsymbol{k} boldsymbol{J} boldsymbol{m o l}^{-1} boldsymbol{z} ) ( Delta H_{f}^{o}left(C C l_{4}, lright)=139.3 k J m o l^{-1} ) A ( cdot Delta G^{o}=4.3 k J / m o l ) в. ( Delta G^{o}=-4.3 k J / ) mol c. ( Delta G^{o}=2.15 k J / ) mol D. None of these | 11 |

332 | A Carnot engine absorbed ( 227^{circ} C ) Calculate works done for the cycle by an engine of its single is maintained at ( 127^{circ} mathrm{C} ) | 11 |

333 | One mole of an ideal gas is compressed from 0.5 lit to 0.25 lit. During the compression, ( 23.04 times 10^{2} J ) of work is done on the gas and heat is removed to keep the temperature of the gas constant at all times. Find the temperature of the gas. (Take universal gas constant ( boldsymbol{R}=mathbf{8 . 3 1} boldsymbol{J} boldsymbol{m o l}^{-1} boldsymbol{K}^{-1} mathbf{)} ) | 11 |

334 | A heat engine operates between ( 2100 mathrm{K} ) and ( 700 mathrm{K} ). Its actual efficiency is ( 40 % ) What percentage of its maximum possible efficiency is this? A. 33.33% B. 66.67% c. ( 60 % ) D. 40% | 11 |

335 | An ideal gas is taken through a cyclic thermo dynamical process through four steps. The amounts of heat involved in steps are ( Q_{1}=5960 J, Q_{2}=-5585 J, Q_{3}= ) ( -2980 J, Q_{4}=3645 J ; ) respectively, the corresponding works involved are ( boldsymbol{W}_{mathbf{1}}=mathbf{2 2 0 0}, boldsymbol{W}_{mathbf{2}}=-mathbf{8 2 5} boldsymbol{J}, boldsymbol{W}_{mathbf{3}}= ) ( -1100 J ) and ( W_{4} ) respectively. Find the value of ( W_{4} ) and efficiency of the cycle A. 1315 J, 10% B. 275 J, 11% C. both of them D. none of these | 11 |

336 | For an ideal gas equation of a process for which the heat capacity of the gas varies with temperature as ( mathrm{C}=frac{alpha}{T}(alpha ) is a constant) is given by A. ( V I n T= ) constant в. ( frac{1}{V T^{(gamma-1)}} e^{frac{alpha}{R T}}= ) constant c. ( frac{1}{V^{(gamma-1)}} T^{frac{alpha}{R T}}= ) constant D. ( V^{gamma-1} T= ) constant | 11 |

337 | For a process to be spontaneous, ( Delta G ) must be: A . negative. B. positive c. zero D. None of these | 11 |

338 | For the reaction; ( F e C O_{3(s)} longrightarrow ) ( boldsymbol{F e O}_{(s)}+boldsymbol{C O}_{2}(boldsymbol{g}), boldsymbol{Delta H}=mathbf{8 2 . 8} boldsymbol{k J} ) at ( 25^{0} C . ) What is ( Delta U ) at ( 25^{0} C ? ) A . ( 82.8 k J ) в. ( 80.32 k J ) c. ( -2394.77 k J ) D. ( 85.28 k J ) | 11 |

339 | For an isomerization ( boldsymbol{X}(boldsymbol{g}) rightleftharpoons boldsymbol{Y}(boldsymbol{g}), ) the temperature dependency of equilibrium constant is given by : ( mathbf{n}=2-frac{mathbf{1 0 0 0}}{mathbf{T}} ) The value of ( Delta_{r} S^{o} ) at ( 300 K ) is : ( mathbf{A} cdot 2 R ) в. ( frac{2}{R} ) c. ( 1000 R ) D. None of these | 11 |

340 | The three thermodynamic states ( P, Q ) and ( R ) of a system are connected by the paths shown in the figure given on the right. The entropy change in the processes ( boldsymbol{P} rightarrow boldsymbol{Q}, boldsymbol{Q} rightarrow boldsymbol{R} ) and ( boldsymbol{P} rightarrow boldsymbol{R} ) along the paths indicated are ( triangle S_{P Q}, triangle S_{Q R} ) and ( triangle S_{P R} ) respectively. If the process ( P rightarrow Q ) is adiabatic and irreversible, while ( P rightarrow R ) is adiabatic and reversible, the correct statement is: A. ( triangle S_{Q R}>0 ) В. ( Delta S_{P R}>0 ) c. ( triangle S_{Q R}0 ) | 11 |

341 | The work done when 2 moles of an ideal gas is compressed from a volume of ( 5 m^{3} ) to ( 1 d m^{3} ) at an initial temperature of ( 300 K, ) under a pressure of ( 100 k P a ) is: A. ( 499.9 k J ) в. ( -499.9 k J ) ( mathbf{c} .-99.5 k J ) D. ( 42495 k J ) | 11 |

342 | Assertion Heat added to a system at lower temperature causes greater randomness than when the same quantity of heat is added to it at higher temperature Reason Entropy is a measure of the degree of randomness or disorder in the system. 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 | 11 |

343 | A gas mixture ( 3.67 L ) in volume contain ( C_{2} H_{4} ) and ( C H_{4} ) is proportion of 2: 1 by moles and is at ( 25^{circ} mathrm{C} ) and 1 atm. If the ( triangle boldsymbol{H}_{C}left(boldsymbol{C}_{2} boldsymbol{H}_{4}right) ) and ( triangle boldsymbol{H}_{C}left(boldsymbol{C H}_{4}right) ) are -1400 and ( -900 k J / ) mol. Find the heat evolved on burning this mixture. A. ( 20.91 k J ) В. ( 50.88 k J ) c. ( 185 k J ) D. 160 k | 11 |

344 | The increase of pressure on ice ( rightleftharpoons ) water system at constant temperature will lead to : A. a decrease in the entropy of the system B. an increase in the Gibbs energy of the system c. no effect on the equilibrium D. a shift of the equilibrium in the forward direction | 11 |

345 | Calculate the volume of ( C O_{2} ) evolved by the combustion of ( 50 mathrm{ml} ) of a mixture contains ( C_{2} H_{4} ) and ( 60 % C H_{4} ) (by volume) | 11 |

346 | The heat capacity at constant volume of a sample of a monoatomic gas is ( mathbf{3 1 . 8 6 7} J / K . ) Find the internal energy at ( 300^{circ} mathrm{C} ) A. ( 8.88 k J ) J в. ( 9.56 k J ) ( c .3 .56 k J ) D. ( 8.96 k J ) | 11 |

347 | Q20. The equilibrium constant for the reaction is 10. Calculate the value of AGO; Given R = 8.314 JK-1 mol-1, T = 300 K. | 11 |

348 | List II تا Q.51 Match the following. List I A. Adiabatic process B. Isolated system Isothermal change D. Path function E. State function F. AU=9 G Law of conservation of energy H Reversible process I Free expansion J. AH = 9 و Heat 2. At constant volume 3 First law of thermodynamics 4. No exchange of energy and matter 5. No transfer of heat Constant temperature Internal energy Pext=o At constant pressure 10. Infinitely slow process which proceeds through a series of equilibrium states 11. Entropy 12. Pressure 13. Specific heat K L Intensive property Extensive property Ane AB | 11 |

349 | Which of the following is/are contributing to the irreversibility of processes? This question has multiple correct options A. Flow of electric current through a resistance B. Unrestrained expansion of fluids c. A quasi-static isothermal expansion of ideal gas D. Spontaneous chemical reactions | 11 |

350 | The volume(V) of a monatomic gas varies with its temperature (T), as shown in the graph. The ratio of work done by the gas, to the heat absorbed by it, when it undergoes a change from state ( A ) to state ( B ), is? A ( cdot frac{1}{3} ) B. 2 ( overline{5} ) ( c cdot 2 ) 7 D. 2 3 | 11 |

351 | The thermodynamical variable temperatures is defined by: A. zeroth law B. I law c. ॥ law D. III law | 11 |

352 | A gas obeys the relation ( V propto frac{1}{T^{2}} . ) The ( frac{C_{p}}{C_{v}} ) value for the gas is A . 1.50 B. 1.30 c. 1.70 D. 2 | 11 |

353 | A gram mole of a gas at ( 127^{circ} mathrm{C} ) expands isothermally until its volume is doubled. find the amount of work done and heat absorbed. A . 238 call ( l ) в. 548 са। ( l ) ( c .548 J ) D. ( 238 J ) | 11 |

354 | Two moles of an ideal monoatomic gas occupies a volume ( V ) at ( 27^{circ} mathrm{C} ). The gas expands adiabatically to a volume ( 2 mathrm{V} ) Calculate (a) the final temperature of the gas and (b) change on its internal energy. B. (a) ( 195 K ) (b) 2.7 k ( c .(a) 189 K(b) 2.7 k J ) D. (a) ( 195 mathrm{k} ) (b) ( -2.7 mathrm{kJ} ) | 11 |

355 | A process is said to be reversible if: A. the system return to their original states B. the surroundings return to their original states C. both the system as well as the surroundings return to their original states D. neither system nor surroundings return to their original states | 11 |

356 | For the change, ( C_{text {diamond}} longrightarrow ) ( C_{g r a p h i t e} ; Delta H=-1.89 k J, ) if ( 6 g ) of diamond and ( 6 g ) of graphite are separately burnt to yield ( C O_{2} ) the heat liberated in first case is: A. Less than in the second case by ( 1.89 k J ) B. Less than in the second case by ( 11.34 k J ) c. Less than in the second case by ( 14.34 k J ) D. More than in the second case by ( 0.945 k J ) | 11 |

357 | Calculate the enthalpy change on freezing of 1.0 mol of water at ( 10.0^{circ} mathrm{C} ) to ice at ( -10.0^{circ} mathrm{C} ) ( triangle_{f u s} H=6.03 K J m o l^{-1} ) at ( 0^{circ} C ) ( boldsymbol{C}_{boldsymbol{p}}left[boldsymbol{H}_{2} boldsymbol{O}(1)right]=mathbf{7 5 . 3} boldsymbol{J} boldsymbol{m o l}^{-1} boldsymbol{K}^{-1} ) ( boldsymbol{C}_{boldsymbol{p}}left[boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s})right]=boldsymbol{3} boldsymbol{6} cdot boldsymbol{8} boldsymbol{J} boldsymbol{m} boldsymbol{o l}^{-1} boldsymbol{K}^{-1} ) | 11 |

358 | Which of the following expressions is true? ( mathbf{A} cdot H_{f}^{o}(C O, g)=frac{1}{2} Delta H_{f}^{o}left(C O_{2}, gright) ) B ( cdot Delta H_{f}^{o}(C O, g)=Delta H_{f}^{o}(C, text { graphite })+frac{1}{2} Delta H_{f}^{o}left(O_{2}, gright) ) C ( cdot Delta H_{f}^{o}(C O, g)=Delta H_{f}^{o}left(C O_{2}, gright)-frac{1}{2} Delta H_{f}^{o}left(O_{2}, gright) ) D. ( Delta H_{f}^{o}(C O, g)=Delta H_{text {comb}}^{o}(C, text { graphite})-Delta H_{text {comb}}^{o}(C O, g) ) | 11 |

359 | According to kinetic theory of gasses at Zero kelvin a) Pressure of ideal gas is zero b) Volume of ideal gas is zero c) Internal energy of ideal gas is zero d) Matter exists in gaseous state only A . a & dare true B. a,b & d are true c. a,b & c are true D. All are true | 11 |

360 | Select the incorrect statements: This question has multiple correct options A. A few combustion process are endothermic B. Heat of combustion may be positive C. Exothermic compounds arc more stable than endothermic compounds D. Hess’s law can he verified experimentally | 11 |

361 | For the reaction ( 2 A l+F e_{2} O_{3} longrightarrow ) ( 2 F e+A l_{2} O_{3}, ) the standard heat enthalpy of ( boldsymbol{F} boldsymbol{e}_{2} boldsymbol{O}_{3} ) and ( boldsymbol{A} boldsymbol{l}_{2} boldsymbol{O}_{3} ) are -196.5 and -399.1 kcal respectively. ( Delta H^{circ} ) for the reaction is: ( mathbf{A} cdot-252.4 k c a l ) в. -135.5 kcal c. ( -202.6 k c a l ) D. none of the above | 11 |

362 | Which of the following is path function? A. Work B. Specific volume c. Pressure D. Temperature | 11 |

363 | If ( I ) is the intensity of absorbed light and ‘C’ is the concentration of AB for the photochemical process, ( A B+h v rightarrow ) ( A B, ) the rate of the formation of ( A B ) is directly proportional to: A. B. ( I ) c. ( I^{2} ) D. ( C, I ) | 11 |

364 | In a reversible process: A. entropy of the system increases. B. entropy of the system decreases. C. entropy of the combined system and surroundings does not change D. entropy of all systems in the universe is constant. | 11 |

365 | Which of the following are examples of endothermic reactions? This question has multiple correct options A. Combustion of methane B. Decomposition of water C. Dehydrogenation of ethane to the ethylene D. Conversion of graphite to diamond | 11 |

366 | ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g})=boldsymbol{2} boldsymbol{H} boldsymbol{C l}(boldsymbol{g}) ) ( Delta H(298 K)=-22.06 mathrm{kcal} . ) For this reaction, ( Delta U ) is equal to: A ( .-22.06+2 times 10^{-3} times 298 times 2 mathrm{kcal} ) В. ( -22.06+2 times 298 ) kcal c. ( -22.06-2 times 298 times 4 ) kcal D. -22.06 kcal | 11 |

367 | Heat of combustion is always: A. positive B. negative C. zero D. may be positive or negative | 11 |

368 | Internal energy of an ideal gas depends on: A. pressure B. temperature c. volume D. none of these | 11 |

369 | A slice of banana weighing 2.502 g was burnt in a bomb calorimeter producing a temperature rise of ( 3.05^{circ} mathrm{C} ). The combustion of ( 0.316 mathrm{g} ) of benzoic acid in the same calorimeter produced a temperature rise of ( 3.24^{circ} mathrm{C} ). The heat of combustion of benzoic acid at constant volume is ( -3227 k J ) mol( ^{-1} . ) If the average banana mass is 125 g, the kilojoules of energy can be obtained from 1 average banana is: (nearest integer value) | 11 |

370 | Standard molar enthalpy of combustion of glucose is ( -2880 k J . ) If only ( 25 % ) of energy is available for muscular work and ( 1.0 k m ) walk consume ( 90 k J ) of energy, what is the maximum distance (in ( mathrm{km} ) ) a person can walk after eating ( 90 g ) of glucose. | 11 |

371 | 11. For the reaction of ammonium carbonate to produce carbon dioxide and ammonia, an experiment was devised and the results were plotted as in the following diagram: AGⓇ vs. temperature 30000 20000 AG° (J/mol) 10000 280 310 320 290 300 Temperature/K Which one of the following is consistent with these results? (a) AH° = 445 kJ mol-1, AS° = 156 J moll K-1 (b) AH° = 156 x 103 J mol-!, AS° = -445 J mol-? K-1 (c) AH° = 156 kJ mol-1, AS° = 445 J mol-1 K-1 (d) AH° = 156 x 103 kJ mol!, AS° = 445 kJ mol K-1 | 11 |

372 | The net heat absorbed by the gas in the path BC | 11 |

373 | A gas is compressed isothermally to half its initial volume. The same gas is compressed separately through an adiabatic process until its volume is again reduced to half. Then. A. compressing the gas isothermally will require more work to be done B. compressing the gas through adiabatic process will require more work to be done c. compressing the gas isothermally or adiabatically will require the same amount of work D. which of the case(whether compression through isothermal or through adiabatic process) requires more work will depend upon the atomicity of the gas | 11 |

374 | A reaction occurs spontaneously if ( mathbf{A} cdot T Delta SDelta H ) and both ( Delta H ) and ( Delta S ) are +ve c. ( T Delta S=Delta H ) and both ( Delta H ) and ( Delta S ) are +ve D. ( T Delta S>Delta H ) and both ( Delta H ) and ( Delta S ) are -ve | 11 |

375 | The standard Gibbs free energy change ( left(Delta G^{o}right) ) at ( 25^{circ} C ) for the dissociation of ( N_{2} O_{4}(g) ) to ( N O_{2}(g) ) is (given, equilibrium constant ( =mathbf{0 . 1 5}, boldsymbol{R}= ) ( 8.314 J K / m o l) ) ( begin{array}{ll}text { A. } 1.1 & k Jend{array} ) B. ( 4.7 k J ) c. ( 8.1 k J ) D. 38.2 k ( J ) | 11 |

376 | If a gas is compressed adiabatically by doing work of ( 150 mathrm{J} ), the change in the internal energy of the gas is: A . 100 J в. 150 c. 200 J D. 250 J | 11 |

377 | Which of the following options is the only correct representation of a process in which ( Delta U=Delta Q-P Delta V ? ) A. ( (I I I)(i i i)(P) ) B. ( (I I)(i i i)(P) ) c. ( (I I)(i i i)(S) ) D. ( (I I)((i v)(R) ) | 11 |

378 | The ratio of the slopes of adiabatic and isothermal curves is A ( cdot frac{1}{gamma} ) в. ( frac{1}{gamma^{3}} ) ( c cdot gamma^{3} ) D. | 11 |

379 | Two moles of helium gas undergo a cyclic process as shown in figure. Assuming the gas to be ideal. The net work done by the gas is: A. 200 R ( ln 2 ) B. 100 R ( ln 2 ) ( c cdot 300 R ln 2 ) D. 400 R ( ln 2 ) | 11 |

380 | For the reaction of one mole zinc dust with one mole sulphuric acid in a bomb calorimeter, ( triangle boldsymbol{U} ) and ( mathbf{w} ) correspond to? A. ( triangle U<0, w=0 ) в. ( triangle U<0, w0, w=0 ) D. ( Delta U>0, w>0 ) | 11 |

381 | What are the most favourable conditions for the reaction; ( boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) leftrightharpoons boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H}^{o}= ) ( – ) ve to occur? A. Low temp and high press B. Low temp and low press c. High temp and low press D. High temp and high press | 11 |

382 | The process is spontaneous at the given temperature, if A. ( Delta H ) is ( +v e ) and ( Delta S ) is ( -v e ) B. ( Delta H ) is ( -v e ) and ( Delta S ) is ( +v e ) ( mathrm{c} . Delta H ) is ( +v e ) and ( Delta S ) is ( +v e ) D. ( Delta H ) is ( +v e ) and ( Delta S ) is equal to zero | 11 |

383 | Steady state is represented by: A. Getting raw materials B. Intake of food and energy. C. Intake of materials and energy, elimination of wastes and dissipation of energy. D. Removal of waste products and intake of raw materials. | 11 |

384 | Using the Gibbs change, ( Delta G^{o}= ) ( +63.3 k J, ) for the following reaction, the ( boldsymbol{K}_{s p} ) of ( boldsymbol{A} boldsymbol{g}_{2} boldsymbol{C} boldsymbol{O}_{3}(s) ) in water at ( boldsymbol{2} boldsymbol{5}^{o} boldsymbol{C} ) is : ( A g_{2} C O_{3}(g) rightleftharpoons 2 A g^{+}(a q)+C O_{3}^{2-}(a q) ) ( left(boldsymbol{R}=mathbf{8 . 3 1 4} boldsymbol{J} boldsymbol{K}^{-1} boldsymbol{m o l}^{-1}right) ) A. ( 3.2 times 10^{-26} ) B. ( 8.0 times 10^{-12} ) c. ( 2.9 times 10^{-3} ) D. ( 7.9 times 10^{-2} ) | 11 |

385 | When an ideal diatomic gas is heated at constant pressure, the fraction of the heat energy supplied which increases the internal energy of the gas is: ( A cdotleft(frac{2}{5}right) ) B. ( left(frac{3}{5}right) ) ( c cdotleft(frac{3}{7}right) ) D. ( left(frac{5}{7}right) ) | 11 |

386 | If ( Delta boldsymbol{H}_{text {vaporisation}} ) of substance ( boldsymbol{X}(l) ) (molar mass ( : 30 g / text { mol }) ) is ( 300 J / g ) at its boiling point ( 300 K ), then molar entropy change for reversible condensation process is: A. ( 30 J / ) mol. ( K ) В ( .-300 J / ) mol. ( K ) c. ( -30 J / ) mol. ( . ) D. None of these | 11 |

387 | Which of the following option are related with the second law of thermodynamics (law of entropy)? A. The heat lost by one object must be gained by another object B. Heat flow naturally from a hotter body to a cooler body C. Celsius degrees and Kelvin degrees are equivalent D. Heat can be transformed into work E. The average kinetic energy of molecules is proportional to temperature | 11 |

388 | The temperature of gas is increased from ( 27^{circ} mathrm{C} ) to ( 127^{circ} mathrm{C} ). The ratio of its mean kinetic energies will be A ( cdot frac{3}{4} ) B. ( frac{4}{3} ) c. ( frac{9}{16} ) D. ( frac{16}{9} ) | 11 |

389 | At what temperature will the hydrogen molecules escape from Earth’s surface? ( A cdot 10^{4} K ) B . ( 10^{3} mathrm{K} ) ( c cdot 10^{2} k ) D. ( 10^{1} mathrm{k} ) | 11 |

390 | You are given a lump of an unknown metal. You perform an experiment and figure out the specific heat is close to ( 0.89 J / g^{o} C . ) What could be the identity of the metal? A. Gold B. Silver c. Iron D. Aluminum E. None of the above | 11 |

391 | HOF is the only known molecule that contains only the elements hydrogen, oxygen and fluorine. Pure ( H F ) is a colourless liquid at ( 273 K ) The liquid contains ( H F ) molecules that have strong hydrogen bonds between them. Draw a fully labelled diagram to suggest how a hydrogen bond can form between two ( H F ) molecules. | 11 |

392 | During what kind of process is there no change in internal energy? A. adiabatic B. isothermal c. isobaric D. cyclic (one cycle) E. Two of the answers are correct | 11 |

393 | A bulb of unknown volume V contains a gas at 1 atm pressure. This bulb was connected to another evacuated bulb of volume ( 0.5 mathrm{L} ) through a stop cock. When the stop cock was opened, the pressure at each bulb becomes ( 7.58 times 10^{4} ) Pa mm while the temperature remained constant. Calculate V in litres. | 11 |

394 | Molar heat capacity of a gas does not depend on A. Its temperature B. Its molecular weight c. Its atomicity D. The conditions under which heat is supplied | 11 |

395 | Calculate the standard internal energy change for the reaction ( boldsymbol{C}_{(text {graphite})}+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightarrow boldsymbol{C O}(boldsymbol{g})+ ) ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) ( Delta_{f}^{o} ) at ( 25^{circ} ; H_{2} O(g)=-241.8 k J m o l^{-1} ) ( boldsymbol{C O}(boldsymbol{g})=-110.5 boldsymbol{k} boldsymbol{J} boldsymbol{m o l}^{-1} ) ( boldsymbol{R}=mathbf{8 . 3 1 4} boldsymbol{J} boldsymbol{K}^{-1} boldsymbol{m o l}^{-1} ) | 11 |

396 | An extensive property is A. a property that changes when the size of the sample changes B. a property that doesn’t change when you take away some of the sample. ( c cdot ) both D. none | 11 |

397 | 5 kilomoles of oxygen is heated at constant pressure. The temperature of the oxygen gas is increased from ( 295 mathrm{K} ) to 305 K. If the molar heat capacity of oxygen at constant pressure is 6.994 kcal/kmole K. The amount of heat absorbed in kcal, A . 249.7 B. 44 c. 349.7 D. 539.7 | 11 |

398 | Calculate the enthalpy of formation of ( operatorname{acetic} operatorname{acid}left(C H_{3} C O O Hright) ) if its enthalpy of combustion is ( -867 k J m o l^{-1} . ) The enthalpies of formation of ( boldsymbol{C O}_{2}(boldsymbol{g}) ) and ( boldsymbol{H}_{2} boldsymbol{O}(l) ) are -393.5 and ( -285.9 k J m o l^{-1} ) respectively. | 11 |

399 | Two moles of a perfect gas undergo the following process: (a) A reversible isobaric expansion from ( (1 operatorname{atm} operatorname{to} 20 L) ) to ( (1 operatorname{atm} operatorname{to~} 40 L) ) (b) A reversible isochoric change of state from ( (1 text { atm to } 40 L) ) to ( (0.5 ) atm to ( 40 L) ) (c) A reversible isothermal compression from ( (0.5 text { at } m text { to } 40 L) ) to ( 1 text { atm to } 20 L) ) (i) Sketch with labels each of the process on the same P-V diagram. (ii) Calculate the total work ( (w) ) and the total change ( (q) ) involved in the above process (iii) What will be the value of ( Delta U, Delta H, Delta S ) for the overall process? | 11 |

400 | A heat engine operating between 227 ( operatorname{deg} mathrm{C} ) and 27 deg ( mathrm{C} ) absorbs 1 kcal of heat from the 227 deg ( C ) reservoir per cycle. Calculate (1) the amount of heat discharged into the low temperature reservoir. (2) the amount of work done per cycle. (3) the efficiency of cycle. A. 0.4 kcal, 0.6 kcal, 40% B. 0.6 kcal, 0.4 kcal, 40% c. 0.4 kcal, 0.6 kcal, ( 60 % ) D. 0.7 kcal, 0.4 kcal, 40% | 11 |

401 | 0.37 Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. What are those conditions? Explain. | 11 |

402 | If an endothermic reaction is non- spontaneous at freezing point of water and becomes feasible at its boiling point, then A. ( Delta H ) is -ve, ( Delta S ) is +ve B. ( Delta H & Delta S ) both are +ve c. ( Delta H & Delta S ) both are -ve D. ( Delta H ) is tve, ( Delta S ) is-ve | 11 |

403 | Gibbs- Helmholtz equation is A ( . Delta G=Delta H-T Delta S ) в. ( Delta G=Delta H+T Delta S ) c. ( Delta G=T Delta H-Delta S ) D. none of these | 11 |

404 | Calculate the approximate speed of sound in oxygen from the following data The mass of 22.4 liter of oxygen at ( boldsymbol{S} boldsymbol{T} boldsymbol{P}(boldsymbol{T}=mathbf{2 7 3} boldsymbol{K} boldsymbol{a n d boldsymbol { p }}=mathbf{1 . 0} times ) ( left.10^{5} N m^{2}right) ) is ( 32 g ) the molar heat capacity of oxygen at constant volume is ( C_{V}=2.5 R ) and that at constant pressure is ( boldsymbol{C}_{boldsymbol{P}}=mathbf{3 . 5} boldsymbol{R} ) | 11 |

405 | Which of the following is a path function? A. internal energy B. enthalpy c. work D. entropy | 11 |

406 | 69. Four curves A, B, C and D are drawn in figure for a given amount of gas. The curves which represent adiabatic and isothermal changes are (a) C and D, respectively (b) D and C. respectively (c) A and B, respectively (d) B and A, respectively | 11 |

407 | A gas is compressed at a constant pressure of ( 50 N / m^{2} ) from a volume of ( 10 m^{3} ) to a volume of ( 4 m^{3} . ) Energy of 100 Jis then added to the gas by heating. Its internal energy is A. increased by 400 B. increased by 200 J c. increased by 100 J D. decreased by 200 | 11 |

408 | The correct relationship between free energy change in a reaction and the corresponding equilibrium constant ( boldsymbol{K}_{c} ) is: A ( cdot Delta G^{o}=R T I n K_{c} ) в. ( -Delta G^{o}=R T I n K_{c} ) c. ( Delta G=R T I n K_{c} ) D. ( -Delta G=R T I n K_{c} ) | 11 |

409 | ( frac{3}{2} O_{2}(g) longrightarrow O_{3}(g) K_{p} ) for this reaction is ( 2.47 times 10^{-29} . ) At ( 298 mathrm{K}, Delta_{r} G^{o} ) for conversion of oxygen to ozone will be: A ( cdot ) 100 ( k ) J mol ( ^{-1} ) – B . 150 kJ mol- c. ( 163 mathrm{kJ} mathrm{mol}^{-1} ) D. 2303 kJ mol-1 | 11 |

410 | In the adjoining graph, possible paths ( A B C ) and ( A C ) for changing a gas from the thermodynamic state ( A ) to the state ( C: ) (i) Along which path greater amount of work will have to be done? (ii) If the internal energy of the gas at the state ( boldsymbol{A} ) be 5 joule, and 100 then calculate the internal energy of the gas at the state ( C ) | 11 |

411 | The basis for measuring thermodynamic property of temperature is given by A. zeroth law of Thermodynamics B. First law of Thermodynamics c. second law of Thermodynamics D. Third law of Thermodynamics | 11 |

412 | What is the amount of work done when 0.5 mole of methane, ( C H_{4(g)}, ) is subjected to combustion at ( 300 mathrm{K} ? ) ( left(operatorname{given}, R=8.314 J K^{-1} mathrm{mol}^{-1}right) ) в. -4988.5 ( mathrm{c} ldots+4988 mathrm{J} ) D. +2494.5 | 11 |

413 | For the reaction at ( 298 mathrm{K}, 2 mathrm{A}+mathrm{B} rightarrow C ) ( triangle H=400 mathrm{KJ} mathrm{mol}^{-1} ) and ( triangle mathrm{S}=0.02 mathrm{KJ} ) ( boldsymbol{K}^{-1} boldsymbol{m} boldsymbol{d}^{-1} ) At what temperature will the reaction become spontaneous considering ( triangle mathrm{H} ) and ( triangle S ) to be constant over the temperature range? | 11 |

414 | A plot of ( ln K ) against ( frac{1}{T}(text { abscissa }) ) is expected to be a straight line with intercept on ordinate axis equal to: A ( cdot frac{Delta S^{o}}{2.303 R^{n}} ) в. ( frac{Delta S^{circ}}{R} ) c. ( -frac{Delta S^{circ}}{R} ) D. ( R times Delta S^{o} ) | 11 |

415 | Latent heat of vapourisation of a liquid at ( 500 K ) and 1 atm pressure is 10 ( k c a l / ) mol. What is the change in internal energy when 3 moles of the liquid is vapourised at the same temperature A . ( 27 k c a l ) B. ( 7 k c a l ) c. ( 33 k c a l ) D. ( 25 k c a l ) | 11 |

416 | A vessel of volume ( 0.2 m^{3} ) contains hydrogen gas at temperature ( 300 K ) and pressure 1 bar. Find the heat required to raise the temperature to ( 400 K . ) The molar heat capacity of hydrogen at constant volume is ( mathbf{5} ) cal / molK. A ( cdot(Delta Q)_{v}=2.1 k c a l ) B . ( (Delta Q)_{v}=4.2 mathrm{kcal} ) C ( cdot(Delta Q)_{v}=2 k c a l ) D. ( (Delta Q)_{v}=4 k c a l ) | 11 |

417 | 10000 Q10. Define the following: (i) First law of thermodynamics. (ii) Standard enthalpy of formation. | 11 |

418 | The molar specific heat of oxygen at constant pressure ( mathrm{C}_{p}=7.03 mathrm{cal} / mathrm{mol}^{o} mathrm{C} ) and ( mathrm{R}=8.31 mathrm{J} / mathrm{mol}^{o} mathrm{C} ). the amount of heat taken by 5 mol of oxygen when heated at constant volume from ( 10^{circ} mathrm{C} ) to ( 20^{circ} mathrm{C} ) will be approximately A ( .25 mathrm{cal} ) B. 50 cal c. ( 250 c a l ) D. 500 call | 11 |

419 | The enthalpy of formation of ( N H_{3}(g) ) is ( -46.2 mathrm{kJ} mathrm{mol}^{-1} . ) The heat of the following reaction is: ( 2 N H_{3}(g) rightarrow N_{2}(g)+3 H_{2}(g) ) B . ( +46.2 mathrm{kJ} ) c. ( -92.4 mathrm{kJ} ) D. ( +92.4 mathrm{kJ} ) | 11 |

420 | A property that must decrease when a gas condense into a liquid: A. Standard voltaic potential B. Entropy c. Enthalpy D. Reaction rate E. Gibbs free energy | 11 |

421 | A certain mass of gas is taken from an initial thermodynamic state ( A ) to another state B by process I and II. In process I the gas does 5 joules of work and absorbs 4 joules of heat energy. In process II, the gas absorbs 5 joules of heat. The work done by the gas in process II (see figure) is A. +6 joules B. – -6 joules c. +4 joules D. – 4 joules | 11 |

422 | Which one from the following is used to measure heat? A. Pipette B. Manometer c. Balance D. Calorimeter | 11 |

423 | The change in internal energy of a system depends on ( A . ) initial and final states of the system B. the path if reversible C. the path if irreversible D. initial, final states and also on the path | 11 |

424 | An ideal refrigerator is working between temperature 27 and ( 127 . ) If it expels 120 calorie of heat in one second then calculate its wattage. | 11 |

425 | Which of the following is not a path function? ( A cdot Delta Q ) B. ( Delta Q+Delta ) W ( c cdot Delta w ) D. ( Delta Q-Delta w ) | 11 |

426 | In an experiment to determine the specific heat capacity of a solid, following observations were made: Mass of calorimeter + stirrer= ( boldsymbol{x} boldsymbol{k} boldsymbol{g} ) Mass of water= ( boldsymbol{y} boldsymbol{k} boldsymbol{g} ) Initial temperature of water ( =t_{1}^{o} C ) Mass of solid ( =boldsymbol{z} boldsymbol{k} boldsymbol{g} ) Temperature of solid= ( t_{2}^{o} boldsymbol{C} ) Temperature of mixture ( =t^{o} C ) Specific heat capacity of calorimeter and water are ( c_{1} ) and ( c_{2} ) respectively. Express the specific heat capacity c of the solid in terms of the above data A ( cdot frac{left(x c_{1}+y c_{2}right)left(t-t_{1}right)}{zleft(t_{2}-tright)} ) B. ( frac{left(x c_{1}+y c_{2}right)left(t-t_{2}right)}{zleft(t_{1}-tright)} ) c. ( frac{left(x c_{1}+y c_{2}right)left(t+t_{2}right)}{zleft(t_{1}+tright)} ) D. ( frac{left(x c_{1}+y c_{2}right)left(t+t_{1}right)}{zleft(t_{2}+tright)} ) | 11 |

427 | 11. A sample containing 2.000 mol of helium gas originally at 298.15 K and 1.000 bar is cooled to its normal boiling temperature of 4 K, condensed to a liquid and then cooled further to 2 K, where it undergoes another phase transition to a second liquid form, called liquid helium II. A beam of laser light suddenly vapourizes this liquid phase, and the helium is brought to a temperature of 298.15 K and a pressure of 0.500 bar. The entropy change for the above process is: (a) 11.5 JK-1 (b) -11.5 JK- (c) 23 KJ-1 (d) Insufficient Information | 11 |

428 | Explain Third law of thermodynamics. | 11 |

429 | The heat change for the following reaction: ( C(s)+2 S(s) rightarrow C S_{2} ) is known as: A. Heat of vaporization B. Heat of solution c. Heat of fusion D. Heat of formation | 11 |

430 | Zeroth law of thermodynamics A. deals with mass and energy B. deals with heat engines C. states that if two systems are both in equilibrium with a third system, they are in thermal equilibrium with each other D. does not exist | 11 |

431 | Which of the following graphs represents an exothermic reaction? ( mathbf{A} ) B. ( mathbf{c} ) D. | 11 |

432 | Q. 58 Derive the relationship between AH and AU for an ideal gas. Explain each term involved in the equation. | 11 |

433 | The oxidation of ( S O_{2} ) by ( O_{2} ) to ( S O_{3} ) is an exothermic reaction. The yield of ( boldsymbol{S O}_{3} ) will be increased for the exothermic reaction if: A. temperature is increases and pressure is kept constant B. temperature is reduced and pressure is increased c. both temperature and pressure are increses D. both temperature and pressure are decreased | 11 |

434 | A pack of cards randomly shuffled has more entropy than a pack of arranged cards.If true enter 1 else 0 ( A ) | 11 |

435 | 015. Define extensive properties. | 11 |

436 | 4 grams of sodium hydroxide pellets were dissolved in ( 100 mathrm{cm}^{3} ) of water. The temperature before adding the sodium hydroxide pellets was 25 degrees ( C ), and after adding the pellets it was 35 degrees C. Calculate the enthalpy change in ( k J / ) mole of the reaction. [Specific heat capacity of water ( = ) ( mathbf{4} . mathbf{2} boldsymbol{J} / boldsymbol{k} / boldsymbol{g}] ) A. ( 42 k J / ) mole в. ( 4.2 k J / ) mole c. ( 4200 k J / ) mole D. None | 11 |

437 | Standard enthalpies of formation of ( boldsymbol{O}_{3} ) ( C O_{2}, N H_{3} ) and ( H I ) are 142.2,-393.2 -46.2 and +25.9 kJ ( m o l^{-1} ) respectively The order of their increasing stabilities will be: A. ( O_{3}, C O_{2}, N H_{3}, H I ) в. ( C O_{2}, N H_{3}, H I, O_{3} ) c. ( O_{3}, H I, N H_{3}, C O_{2} ) D. ( N H_{3}, H I, C O_{2}, O_{3} ) | 11 |

438 | ( boldsymbol{H}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ) ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) longrightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H}=boldsymbol{x}_{4} ) Given ( boldsymbol{E}_{boldsymbol{H}-boldsymbol{H}}=boldsymbol{x}_{boldsymbol{1}} ) ( boldsymbol{E}_{boldsymbol{O}-boldsymbol{O}}=boldsymbol{x}_{boldsymbol{2}} ) ( boldsymbol{E}_{boldsymbol{O}-boldsymbol{H}}=boldsymbol{x}_{boldsymbol{3}} ) ( Delta H_{F} ) of ( H_{2} O ) vapour is: A ( cdot x_{1}+frac{x_{2}}{2}-x_{3}+x_{4} ) B ( cdot 2 x_{3}-x_{1}-frac{x_{2}}{2}-x_{4} ) c. ( _{x_{1}+frac{x_{2}}{2}-2 x_{3}-x_{4}} ) D. ( x_{1}+frac{x_{2}}{2}-2 x_{3}+x_{4} ) | 11 |

439 | Two cylinders ( A ) and ( B ) fitted with pistons contain equal number of moles of an ideal monoatomic gas at ( 400 K ) The piston of ( A ) is free to move while that of B is held fixed Same amount of heat energy is given to the gas in each cylinder. If the rise in temperature of the gas in ( A ) is ( 42 K ), the rise in temperature of the gas in ( mathrm{B} ) is: ( left(gamma=frac{5}{3}right) ) A . 21 в. 35 к ( c cdot 42 k ) D. 7ок | 11 |

440 | Bond dissociation energy of ( boldsymbol{X} boldsymbol{Y}, boldsymbol{X}_{2} ) and ( Y_{2} ) (all diatomic molecules) are in the ratio of 1: 1: 0.5 and ( Delta H_{f} ) of ( X Y ) is ( -100 k J m o l^{-1} . ) The bond dissociation energy of ( X_{2} ) is ( 100 x . ) Find the value of ( x ) ( A cdot 4 ) B. ( c cdot 8 ) D. 10 | 11 |

441 | The heat of combustion of napthalene, ( C_{10} H_{8}, ) at constant volume at ( 25^{circ} mathrm{C} ) was found to be ( -5133 k J ) mol ( ^{-1} ) Calaculate the value of enthalpy change | 11 |

442 | Match list I with list II and select the correct answer using the codes given below the lists: ( begin{array}{ll}text { List I } & text { List II } \ text { A. }left(frac{delta G}{delta P}right)_{T} & text { 1. } mu_{H} \ text { B. }left(frac{delta G}{delta T}right)_{P} & text { 2. } T \ text { C. }left(frac{delta H}{delta S}right)_{P} & text { 3. }-S \ text { D. }left(frac{delta T}{delta P}right)_{H} & text { 4. } P \ & text { 5. } Vend{array} ) A. ( A-5, B-1, C-2, D-4 ) B . ( A-5, B-3, C-2, D-4 ) ( mathbf{c} cdot A-3, B-5, C-2, D-1 ) D . ( A-5, B-3, C-2, D-1 ) | 11 |

443 | Use the given standard enthalpies of formation to determine the heat of reaction of the following reaction: [ begin{array}{c} 2 L i O H+C O_{2}(g) longrightarrow \ L i_{2} C O_{3}(s)+H_{2} O(l) \ Delta H_{f} L i O H(s)=-487.23 k J / text {mole} \ Delta H_{f} L i_{2} C O_{3}(s)=-1215.6 k J / text {mole} \ Delta H_{f} H_{2} O(l)=-285.85 k J / text {mole} \ Delta H_{f} C O_{2}(g)=-393.5 k J / text {mole} end{array} ] A . ( +303 . ) в. -133.5 c. -198.6 D. +198.6 | 11 |

444 | A sample consisting of 1mol of a monoatomic perfect gas ( left(C_{v}=frac{3}{2} Rright) ) is taken through the cycle as shown: Temperature at points (1),(2) and (3) respectively is : A ( .273 K, 546 K, 273 K ) B . ( 546 K, 273 K, 273 K ) C . ( 273 K, 273 K, 273 K ) D. ( 546 K, 546 K, 273 K ) | 11 |

445 | Q Type your question- reaction: ( 4 C O(g)+8 H_{2}(g) longrightarrow 3 C H_{4}(g)+ ) ( boldsymbol{C O}_{2}(boldsymbol{g})+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ) Given that ( boldsymbol{C}(text {graphite})+mathbf{1} / mathbf{2 O}_{2}(boldsymbol{g}) longrightarrow ) ( boldsymbol{C O}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H} / boldsymbol{k} boldsymbol{J}=-110.5 boldsymbol{k} boldsymbol{J} ) ( boldsymbol{C O}(boldsymbol{g})+mathbf{1} / mathbf{2} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow ) ( boldsymbol{C O}_{2}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H} / boldsymbol{k} boldsymbol{J}=-boldsymbol{2} boldsymbol{8} boldsymbol{2} . boldsymbol{9} boldsymbol{k} boldsymbol{J} ) ( boldsymbol{H}_{2}(boldsymbol{g})+mathbf{1} / 2 boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow ) ( boldsymbol{H}_{2} boldsymbol{O}(l) ; boldsymbol{Delta} boldsymbol{H} / boldsymbol{k} boldsymbol{J}=-boldsymbol{2} boldsymbol{8} boldsymbol{5} . boldsymbol{8} boldsymbol{k} boldsymbol{J} ) ( boldsymbol{C}(boldsymbol{g} boldsymbol{r} boldsymbol{a} boldsymbol{p} boldsymbol{h} boldsymbol{i} boldsymbol{e})+boldsymbol{2} boldsymbol{H}_{2}(boldsymbol{g}) longrightarrow ) ( boldsymbol{C H}_{4}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H} / boldsymbol{k} boldsymbol{J}=-mathbf{7 4 . 8 k J} ) A ( .584 .9 mathrm{kJ} mathrm{mol}^{-1} ) в. ( 279.8 mathrm{kJ} mathrm{mol}^{-1} ) c. ( 747.4 mathrm{kJ} mathrm{mol}^{-1} ) D. 925 kJ mol ( ^{-1} ) | 11 |

446 | Q8. State Hess’s law. | 11 |

447 | A balloon contains ( 14.0 L ) of air at 760 torr. What will be the volume of the balloon when it is taken to a depth of 10 ( f t ). in a swimming pool? Assume that the temperature of the air and water are equal (Density: ( boldsymbol{H} boldsymbol{g}=mathbf{1 3 . 6} boldsymbol{g} / boldsymbol{m} boldsymbol{L} .) ) A . 11.0 в. 11.3 c. 10 D. 10.8 | 11 |

448 | The ratio of work done by an ideal diatomic gas to the heat supplied by the gas in an isobaric process is A ( cdot frac{5}{7} ) в. ( frac{3}{5} ) ( c cdot frac{2}{7} ) D. ( frac{5}{3} ) | 11 |

449 | 3. For a cyclic process, the change in internal energy of the system is (a) always +ve (b) equal to zero (c) always -ve (d) none of the above | 11 |

450 | By opening the door of a refrigerator which is inside a room, the temperature of room A. first decreases then increases B. remains unchanged c. increases D. decreases | 11 |

451 | Potential energy is defined as: A. The energy of motion B. Electrical energy C. The energy of heat D. Mechanical energy E. The energy of position and composition | 11 |

452 | A heat engine takes in heat at 750 degrees Celsius and expels heat at 250 degrees Celsius. What is this engine’s theoretically ideal (Carnot) efficiency? A. 33 percent B. 67 percent c. 49 percent D. 300 percent E. 23 percent | 11 |

453 | In the reaction: ( mathbf{2} C O(boldsymbol{g})+boldsymbol{O}_{2}(boldsymbol{g}) rightleftharpoons mathbf{2} boldsymbol{C} boldsymbol{O}(boldsymbol{g}) ) entropy_ – A. decreases B. increases c. constant D. none | 11 |

454 | For a spontaneous process, which of the following is true? A ( cdot Delta S_{s y s} ) is positive B. ( Delta S_{text {surr}} ) is positive ( mathbf{c} cdot Delta S_{t o t a l} ) is positive D. ( Delta S_{text {total }} ) is negative | 11 |

455 | 22. A copper ball of mass 100 g is at a temperature T. It is dropped in a copper calorimeter of mass 100 g, filled with 170 g of water at room temperature. Subsequently, the temperature of the system is found to be 75°C. T is given by (Given: room temperature = 30°C, specific heat of copper = 0.1 cal/g°C) (a) 1250°C (b) 825°C (c) 800°C (d) 885°C (JEE Main 2017) | 11 |

456 | Mention the significance of Zeroth law of Thermodynamics. | 11 |

457 | State whether given statement is True or False Cooling of a cup of coffee is an example of thermal equilibrium. | 11 |

458 | State whether true or false: The thermal capacity of 10 g of a substance is 8 calories then its specific heat is 1.25 cal ( g^{-1 o} C^{-1} ) A. True B. False | 11 |

459 | The standard heats of formation at ( 298 K ) for ( C C l_{4}(g), H_{2} O(g), C O_{2}(g) ) and ( H C l(g) ) are -25.5,-57.8,-94.1 and ( -22.1 k c a l ) mol ( ^{-1} ) respectively Calculate ( Delta H_{298}^{o} ) for the reaction. ( boldsymbol{C C l}_{4}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) longrightarrow boldsymbol{C O}_{2}(boldsymbol{g})+ ) ( 4 H C l(g) ) | 11 |

460 | 13. Select the correct alternate(s). (a) For per mole change d(AH) _d(AE).R & dTdT (b) For an ideal gas, AE = Cv (T2-T) (c) For a real gas, AE = P(V2 – V) in the absence of force of attraction (d) For a real gas, AH = CHR) p(V2 – V) in the absence of force of attraction | 11 |

461 | Calculate the enthalpy of formation of ( Delta H_{f} ) for ( C_{2} H_{5} O H ) from tabulated data and its heat of combustion as represented by the following equations: ( boldsymbol{H}_{2}(boldsymbol{g})+mathbf{1} / mathbf{2} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow ) ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H}^{o}=-boldsymbol{2} mathbf{4} 1.8 boldsymbol{k} boldsymbol{J} boldsymbol{m o l}^{-1} ldots(boldsymbol{i}) ) ( boldsymbol{C}(boldsymbol{s})+boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H}^{o}= ) ( -393.5 k J m o l^{-1} ldots(i i) ) ( boldsymbol{C}_{2} boldsymbol{H}_{5} boldsymbol{O} boldsymbol{H}(boldsymbol{l})+boldsymbol{3} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow ) ( mathbf{3} boldsymbol{H}_{mathbf{2}} boldsymbol{O}(boldsymbol{g})+mathbf{2} boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H}^{o}= ) ( -1234.7 k J ldots(i i i) ) A. ( -2747.1 k J mathrm{mol}^{-1} ) в. ( -277.7 k ) J ( m o l^{-1} ) c. ( -277.7 . k J m o l^{-1} ) D. ( 2747.1 k J ) mol ( ^{-1} ) | 11 |

462 | Which of the following statement is incorrect: A. On addition of catalyst the equilibrium constant value is not affected. B. Equilibrium constant value for negative ( Delta H ) value decreases as the temperature increases C. In equilibrium mixture of ice and water, kept in insulated flask mass of ice and water does not change with time D. The intensity of red colour increases when oxalic acid is added to the solution containing iron nitrate(III) and potassium thiocynate | 11 |

463 | According to law of conservation of energy, the energy can neither be nor A . created, destroyed B. destroyed, suppliedd c. absorbed, emitted D. emitted, absorbed | 11 |

464 | A diatomic ideal gas is compressed adiabatically to ( frac{1}{32} ) of its initial volume. If the initial temperature of the gas is ( mathbf{T}_{mathbf{i}} ) (in Kelvin) and the final temperature is ( a T_{i}, ) the value of a is ( A cdot 4 ) B. 5 ( c cdot 2 ) D. 3 | 11 |

465 | A coffee cup calorimeter initially contains ( 125 g ) of water at a temperature of ( 24.2^{0} C ) After (10.5gm) is added to the water at the same temperature, the final temperature becomes ( 21.1^{0} mathrm{C} ). The heat of solution is: ( A cdot 85 J / g ) B. 110 J/g c. 270 J/g D. 167 J/g | 11 |

466 | The Born Haber cycle below represents the energy changes occurring at ( 298 mathrm{K} ) when ( mathrm{KH} ) is formed from its elements ( mathbf{v}: Delta boldsymbol{H}_{text {atomisation}} mathrm{K}=mathbf{9 0} mathrm{kJ} / mathrm{mol} ) ( mathbf{w}: Delta boldsymbol{H}_{text {ionisation}} mathbf{K}=mathbf{4 1 8} mathbf{k J} / mathrm{mol} ) ( mathbf{x}: boldsymbol{Delta} boldsymbol{H}_{text {dissociation}} mathrm{H}=436 mathrm{kJ} / mathrm{mol} ) ( mathbf{y}: boldsymbol{Delta} boldsymbol{H}_{text {electronaffinity}} mathbf{H}=mathbf{7 8} mathbf{k} mathbf{J} / mathrm{mol} ) ( mathbf{z}: boldsymbol{Delta} boldsymbol{H}_{text {lattice}} mathrm{KH}=710 mathrm{kJ} / mathrm{mol} ) In terms of the letters ( v ) to ( z ) the expression for ( Delta boldsymbol{H}_{i} ) of ( mathrm{K} ) is ( boldsymbol{Delta} boldsymbol{H}_{i}=boldsymbol{w} / 2 ) If true enter 1 , else enter 0 A. 0 B. 1 ( c cdot 2 ) D. 3 | 11 |

467 | Heat of ( 20 mathrm{Kcal} ) is supplied to the system and ( 8400 J ) of external work is done on the system so that its volume decreases at constant pressure. The change in internal energy is ( (J= ) ( 4200 J / k c a l) ) A ( .9 .24 times 10^{4} J ) B. ( 7.56 times 10^{4} J ) c. ( 8.4 times 10^{4} J ) D. ( 10.5 times 10^{4} J ) | 11 |

468 | 12. A person, whose body temperature is 310 K, was sliding with considerable friction, down a mountain whose temperature was 277 K. Which of the following sets of signs of entropy change is correct? AS system ASSurrounding AS Total + + + + Can’t be predicted + + 2 + I + T | 11 |

469 | In an exothermic reaction, ( Delta boldsymbol{H} ) is: A . positive B. negative c. zero D. may be positive or negative | 11 |

470 | Isobaric bulk modules of elasticity is ( A cdot infty ) B. 0 ( c . P ) D. ( frac{C_{p}}{C_{v}} ) | 11 |

471 | The temperature at which the reaction given below is at equilibrium is ( A g_{2} O(s) longrightarrow 2 A g(s)+frac{1}{2} O_{2}(g) ) Given that ( Delta H^{o}=30.5 k J m o l^{-1} ) and ( boldsymbol{Delta} boldsymbol{S}^{o}=mathbf{0 . 0 6 6} boldsymbol{k} boldsymbol{J} boldsymbol{K}^{-1} boldsymbol{m o l}^{-1} ) A. ( T=412.12 K ) в. ( T=432.12 K ) c. ( T=422.12 K ) | 11 |

472 | Assertion An alternative definition of a reversible process is a process that, after it has taken place, can be reversed and, when reversed, causes no change in either the system or its surroundings. Reason By making no changes to system or surrounding we make sure that no no change in entropy has taken place. 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 | 11 |

473 | For a particular reaction ( triangle boldsymbol{H}^{0}= ) ( -76.6 K J ) and ( Delta S^{0}=226 J K^{-1} . ) This reaction is: A. spontaneous at all temperatures B. non-spontaneous at all temperatures C. spontaneous at temperature below ( 66^{circ} mathrm{C} ) D. spontaneous at temperature above ( 66^{circ} mathrm{C} ) | 11 |

474 | Calculate the amount of heat energy required to raise the temperature of ( 100 g ) of copper from ( 20^{circ} C ) to ( 70^{circ} C ) Specific heat capacity of copper: ( mathbf{3 9 0} boldsymbol{J k g}^{-1} boldsymbol{K}^{-1} ) A . ( 195 . J ) в. ( 3900 J ) c. ( 1950 J ) D. ( 390 J ) | 11 |

475 | Therm is the unit of A. heat B. temperature c. thermometry D. work | 11 |

476 | A reaction ( A+B rightarrow C+D ) is found to have a positive entropy change. The reaction will be : A. possible at high temperature B. possible only at low temperature C. not possible at any temperature D. possible at any temperature | 11 |

477 | Which of the following is an energy consuming process? A ( cdot O(g)+e^{-} rightarrow O^{-}(g) ) B . ( N a^{+}(g)+e^{-} rightarrow N a(g) ) ( mathrm{c} cdot O^{-}+e^{-} rightarrow O^{2-}(g) ) D. ( O^{2-}(g) rightarrow O^{-}(g)+e^{-} ) | 11 |

478 | Calculate the work done (in Joules) when 0.2 mole of an ideal gas at 300 K expands isothermally and reversibly from an initial volume of 2.5 liters to the final volume of 25 liters. A .996 B. -1148 c. 11.48 D. 897 | 11 |

479 | Q. 23 The value of AfHⓇ for NH, is-91.8kJ mol-1. Calculate enthalpy change for the following reaction. 2NH3(g) → N2(g)+ 3H2(g) | 11 |

480 | The amount of work done by the gas system in increasing the volume of 10 mols of an ideal gas from one litre to 20 litres at ( 0^{0} ) C will be A . zero B. 3.49 Joule c. ( 3.49 times 10^{4} ) D. 6.79 ( times 10^{4} ) Joule | 11 |

481 | Identify the correct statement from the following in a chemical reaction. A. The entropy always increases B. The change in entropy along with suitable change in enthalpy decides the rate of reaction C. The enthalpy always decreases D. Both the enthalpy and the entropy remains constant | 11 |

482 | The enthalpy of formation of ammonia is ( -46.0 K J ) mol ( ^{-1} . ) The enthalpy change for the reaction ( 2 N H_{3}(g) rightarrow ) ( N_{2}(g)+3 H_{2}(g) ) is: A ( .46 .0 K J ) mol( ^{-1} ) B. ( 92.0 K J ) mol( ^{-1} ) c. ( -23.0 mathrm{KJ} mathrm{mol}^{-1} ) D. ( -92.0 K J ) mol( ^{-1} ) | 11 |

483 | Assertion Water drops take spherical shape when falling freely. Reason Water has minimum surface tension among all liquids. 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 | 11 |

484 | At. N.T.P. ( 28 ~ g ) of Nitrogen occupies 22.4 litres. What is the mass of 5.6 litres of Nitrogen at ( 38 mathrm{cm} ) Hg pressure and ( 273^{0} C ) temperature is then A ( .1 .87 mathrm{g} ) в. 48 g c. ( 1.75 mathrm{g} ) D. ( 1.5 mathrm{g} ) | 11 |

485 | The relation between internal energy U, pressure ( P ) and volume ( V ) of a gas in an adiabatic process is ( U=a+b P V, ) where a and b are positive constants. What is the value of ( gamma ) ? A. ( frac{a}{b} ) B. ( frac{b+1}{b} ) c. ( frac{a+1}{a} ) D. | 11 |

486 | The heat of combustion of ( C, S ) and ( C S_{2} ) are ( -393.3 mathrm{kJ},-293.7 mathrm{kJ} ) and ( -1108.76 mathrm{kJ} ) What will be the heat of formation of ( boldsymbol{C} boldsymbol{S}_{2} ? ) A . -128.02 kJ в. +970 kJ c. ( +1108.7 k J ) D . +12 kJ | 11 |

487 | Assertion Combustion of ( N_{2} ) to give NO is endothermic. Reason Bond energy of ( N_{2} ) is very high. 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 | 11 |

488 | Which of the following is not a state function? A. Temperature B. Density c. work D. volume E . Pressure | 11 |

489 | The compound with negative value of heat of formation is called: A. endothermic compound B. exothermic compound c. heat of formation compound D. none of the above | 11 |

490 | The object under thermodynamical study is called A. system B. Universe c. surrounding D. Boundary | 11 |

491 | Which of the following is technique used to measure the heat of a reaction? A. Gibbs Free Energy B. Entropy c. Enthalpy D. Calorimetry | 11 |

492 | For which one of the following system ( Delta boldsymbol{E}<Delta boldsymbol{H} ? ) A ( cdot 2 S O_{2(g)}+O_{2(g)} rightarrow 2 S O_{3(g)} ) B. ( N_{2(g)}+O_{2(g)} rightarrow 2 N O_{(g)} ) C. ( 2 N H_{3(g)} rightarrow N_{2(g)}+3 H_{2(g)} ) D. ( H_{2(g)}+I_{2(g)} rightarrow 2 H I_{(g)} ) | 11 |

493 | If ( C_{p} ) and ( C_{v} ) are the molar specific heats of a gas at constant pressure and volume respectively then the ratio of adiabatic and isothermal modulii of elasticity will be A. ( frac{C_{p}-C_{v}}{C_{p}} ) B. ( C_{p} C_{v} ) c. ( frac{C_{v}}{C_{p}} ) D. ( frac{C_{p}}{C_{v}} ) | 11 |

494 | Assertion In an adiabatic process change in internal energy of a gas in equal to work done on or by the gas in the process. Reason Temperature of gas remains constant in an adiabatic process. 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 | 11 |

495 | Which of the following is not the component of heat pump? A. Condenser B. Compressor c. cooler D. Expansion valve | 11 |

496 | An stoichiometric mixture of hydrogen gas and the air at ( 25^{circ} mathrm{C} ) and a total pressure of 1 atm, is exploded in a closed rigid vessel. If the process occurs under adiabatic condition then using the given data answer the questions that follow: Given:(i) ( C_{p}=8.3 mathrm{cal} ) deg ( ^{-1} ) mol ( ^{-1} ) ( (mathrm{ii}) C_{p}=11.3 mathrm{cal} mathrm{deg}^{-1} mathrm{mol}^{-1} ) ( Delta boldsymbol{H}_{f}left[boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g})right]=-mathbf{5 7 . 8} boldsymbol{k} boldsymbol{c} boldsymbol{a l} boldsymbol{l} ) [Take air as 80 per ( N_{2}, 20 ) per ( O_{2} ) by volume ( ] ) The value of ( C_{p} ) of ( N_{2} & H_{2} O ) will be: (in cal deg. ( ^{-1} )mol( ^{-1} ) ) A. 8.3,8.3 B. 8.3, 11.3 c. 11.3,11.3 D. 11.3,8.3 | 11 |

497 | ( Delta H ) and ( Delta S ) for the reaction, ( boldsymbol{A} boldsymbol{g}_{2} boldsymbol{O}(boldsymbol{s}) longrightarrow boldsymbol{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) ) are ( 30.56 k J m o l^{-1} ) and ( 66.0 J K^{-1} ) mol ( ^{-1} ) respectively. Calculate the temperature at which free energy change for the reaction will be zero. Predict whether the forward reaction will be forward above or below this temperature. | 11 |

498 | Which are extensive properties? A. ( V ) and ( E ) B. ( V ) and ( T ) c. ( V ) and ( C p ) D. ( P ) and ( T ) | 11 |

499 | Q. 2 For the reaction, H.(q) + L(g) 2 HI(g), the standard free energy is AGⓇ> 0. The equilibrium constant (K) would be (a) K=0 (b) k> 1 on (c) K=1 (d) K <1 | 11 |

500 | An isolated system is one which neither shows an exchange of ( _{–}- ) -nor with surroundings. A. heat, mass B. heat, temperature c. temperature, mass D. None of these | 11 |

501 | Assertion The change in internal energy and change in heat enthalpy does not depend upon the path by which changes are brought in. Reason Both ( Delta U ) and ( Delta H ) are path independent as U and H are state functions. 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 | 11 |

502 | A piece of iron of mass 0.05 kg is heated to a temperature of ( 200^{circ} mathrm{C} ) and dropped into a beaker containing ( 0.4 mathrm{kg} ) of water at ( 20^{circ} mathrm{C} ). If the final temperature of water and iron is ( 22.4^{circ} mathrm{C} ) find the specific heat capacity of iron. A . ( 354.04 J k g^{-1} K^{-1} ) B. ( 454.04 J k g^{-1} K^{-1} ) c. ( 554.04 J k g^{-1} K^{-1} ) D. ( 654.04 J k g^{-1} K^{-1} ) | 11 |

503 | The heat required (in ( c a l ) ) to change 10 g ice at ( 0^{circ} mathrm{C} ) to steam at ( 100^{circ} mathrm{C} ) is: I Heat of fusion and heat of vaporization | 11 |

504 | Assertion During change of state, specific heat of a substance is zero. Reason Specific heat of a substance is directly proportional to change of heat and inversely proportional to change in temperature 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 | 11 |

505 | When we take acetone in a test tube it feels cold. Which reaction occurs in the process? A. endothermic reaction B. exothermic reaction c. reversible process D. adiabatic process | 11 |

506 | For this reaction relate ( Delta boldsymbol{H} ) and ( boldsymbol{Delta} boldsymbol{U} ) ( mathbf{2} N boldsymbol{O}_{2}(boldsymbol{g}) quad longrightarrow boldsymbol{N}_{2} boldsymbol{O}_{4}(boldsymbol{g}) ) A. ( Delta H=Delta U ) в. ( Delta H>Delta U ) ( mathbf{c} cdot Delta H<Delta U ) D. None of these | 11 |

507 | The ( p-V ) diagram of ( 2 g ) of helium gas for a certain process ( A rightarrow B ) is shown in the figure. What is the heat given to the gas during the process ( boldsymbol{A} rightarrow boldsymbol{B} ) ? ( A cdot 4 p_{0} V_{0} ) B. ( 6 p_{0} V_{0} ) ( c cdot 4.5 p_{0} V_{0} ) ( mathbf{D} cdot 2 p_{0} V_{0} ) | 11 |

508 | ( Delta H_{f}=-98.2 mathrm{K} . mathrm{Cal} / mathrm{mole} ) ( boldsymbol{S}_{N a}=36 mathrm{K.Cal} / mathrm{mole} ) ( boldsymbol{I}_{N a}=118.5 mathrm{K} . mathrm{Cal} / mathrm{mole} ) ( frac{1}{2} D_{C l_{2}}=29 mathrm{K} . mathrm{Cal} / mathrm{mole} ) ( boldsymbol{U}_{N a C l}=-184.2 mathrm{K} . mathrm{Cal} / mathrm{mole} ) From the data given below for ( N a C l ) the electron affinity of chlorine ( left[-boldsymbol{E}_{boldsymbol{a}}right] ) is: A . -97.5 K.cal/ mole B. -108 K.cal/mole c. -75 K.cal/mole D. -128 K.cal/mole | 11 |

509 | The van’t Hoff reaction isotherm is: ( mathbf{A} cdot Delta G=R T log _{e} K_{p} ) в. ( -Delta G= ) RТlog( _{e} K_{p} ) ( mathbf{c} cdot Delta G=R T^{2} I n K_{p} ) D. none of these | 11 |

510 | In a thermostat device which parameter remains approximately constant A. Volume B. Pressure c. Temperature D. Mass | 11 |

511 | The standard enthalpy of formation of water liquid is ( 285.76 mathrm{kJ} ) at ( 298 mathrm{K} ) Calculate the value at ( 373 mathrm{K} ). The molar heat capacities at constant pressure ( left(C_{P}right) ) in the given temperature range of ( boldsymbol{H}_{2}(boldsymbol{g}), boldsymbol{O}_{2}(boldsymbol{g}) ) and ( boldsymbol{H}_{2} boldsymbol{O}(l) ) are respectively 38.83,29.16 and 75.312 ( $ $ J K^{wedge}{1} operatorname{mol}^{prime}{1} ) A ( cdot Delta H_{373}^{circ}left(H_{2} O,(l)right)=-284.11 k J ) B. ( Delta H_{3^{prime 3}}left(H_{2} O,(l)right)=+284.11 k J ) C . ( Delta H_{373}^{circ}left(H_{2} O,(l)right)=28.411 k J ) D. None of these | 11 |

512 | A sample consisting of 1 mol of a monoatomic perfect gas ( left(C_{v}=frac{3}{2} Rright) ) is taken through the cycle as shown: ( Delta H ) for the overall cycle is : A ( cdot+5.67 times 10^{3} J ) B ( .-5.67 times 10^{3} J ) c. ( -11.34 times 10^{3} J ) ( D ) | 11 |

513 | Which of the following reactions defines ( Delta H_{f}^{o} ? ) A. ( C_{text {diamond}}+O_{2}(g) rightarrow C O_{2}(g) ) B ( cdot frac{1}{2} H_{2}(g)+frac{1}{2} F_{2}(g) rightarrow H F(g) ) C. ( N_{2}(g)+3 H_{2}(g) rightarrow 2 N H_{3}(g) ) ( ^{mathrm{D}} cdot_{C O(g)}+frac{1}{2} O_{2}(g) rightarrow C O_{2}(g) ) | 11 |

514 | ( 1300 J ) of heat energy is supplied to raise the temperature of ( 0.5 k g ) of lead from ( 20^{circ} mathrm{C} ) to ( 40^{circ} mathrm{C} ). Calculate the specific heat capacity of lead A ( cdot 130 J k g^{-1} K^{-1} ) B . ( 260 J k g^{-1} K^{-1} ) c. ( 650 J k g^{-1} K^{-1} ) D. None of the above | 11 |

515 | In an isothermal change of an ideal gas, ( Delta U=0 . ) The change in the heat energy ( Delta Q ) is equal to ( mathbf{A} cdot 0.5 W ) в. ( W ) c. ( 1.5 W ) D. 2 ( W ) | 11 |

516 | One mole of ideal gas expands freely at ( 310 mathrm{K} ) from five litre volume to 10 litre volume. Then ( Delta E ) and ( Delta H ) of the process are respectively: A . 0 and 5 cal B. 0 and ( (5 times 300) ) cal c. 0 and 0 D. 5 and 0 cal | 11 |

517 | Q17. How is entropy of a substance related to temperature? an | 11 |

518 | For the combustion of benzene to gaseous carbon dioxide and liquid water, ( Delta H ) is more than ( Delta U ) A . True B. False c. Ambiguous D. insufficient data | 11 |

519 | The enthalpies of formation of ( A l_{2} O_{3} ) and ( C r_{2} O_{3} ) are ( -1596 mathrm{kJ} ) and ( -1134 mathrm{kJ} ) respectively. ( Delta H ) for the reaction, ( mathbf{2} boldsymbol{A} boldsymbol{l}+boldsymbol{C r}_{2} boldsymbol{O}_{3} rightarrow boldsymbol{2} boldsymbol{C r}+boldsymbol{A l}_{2} boldsymbol{O}_{3} ) is : B . -462 kJ c. -1365 kJ D. +2730 kJ | 11 |

520 | Two bodies at different temperatures are kept in contact. If the body at higher temperature gets hotter than it violates which law of thermodynamics? A. zeroth law of thermodynamics B. First law of thermodynamics c. second law of thermodynamics D. Third law of thermodynamics | 11 |

521 | Which of the following is an endothermic reaction ( mathbf{A} cdot N_{2}(g)+3 H_{2}(g)-92 k J rightarrow 2 N H_{3}(g) ) B ( cdot N_{2}(g)+O_{2}(g)+180.8 k J rightarrow 2 N O(g) ) ( mathbf{c} cdot H_{2}(g)+C l_{2}(g) rightarrow 2 H C l(g)+184.6 k J ) ( mathbf{D} cdot C(g r)+2 H_{2}(g) rightarrow C H_{4}(g)+74.8 k J ) | 11 |

522 | The standard Gibbs energy change at ( 300 K ) for the reaction ( 2 A leftrightharpoons B+C ) is ( 2494.2 J . ) At a given time, the composition of the reaction mixture is ( [A]=frac{1}{2},[B]=2 ) and ( [C]=frac{1}{2} . ) The reaction proceeds in the ( :[R= ) ( mathbf{8 . 3 1 4 J} / mathbf{K} / mathbf{m o l}, e=mathbf{2 . 7 1 8} ) A . forward direction because ( Q>K_{e} ) B. reverse direction because ( Q>K_{e} ) C. forward direction because ( Q<K_{e} ) D. reverse direction because ( Q<K_{e} ) | 11 |

523 | ( A 60 J ) of heat is added to the system, resulting in 15 J of work being done by the system. The remaining 45 J of heat is released. Find out the efficiency of the system? A. ( 100 % ) B. 75 % c. ( 45 % ) D. 25% E . ( 15 % ) | 11 |

524 | At ( 298 mathrm{K}, Delta_{f} S^{ominus} ) element ( =0 ) A. True B. False | 11 |

525 | ( 146 k J ) work is performed in order to compress 1 kilomole of gas adiabatically and in this process the temperature of the gas increases by ( mathbf{7}^{o} mathbf{C} . ) The gas is: (Take ( left.boldsymbol{R}=mathbf{8 . 3} boldsymbol{J} boldsymbol{m} boldsymbol{o l} boldsymbol{e}^{-1} boldsymbol{K}^{-1}right) ) A. monoatomic B. diatomic c. triatomic D. a mixture of monoatomic and diatomic | 11 |

526 | ( Delta G^{0} ) for the reaction ( 2 N O(g)+ ) ( O_{2}(g) rightarrow N_{2} O_{4}(g) ) at ( 298 mathrm{k} ) and 1 atm pressure, will be [given that the enthalpy of formation of ( mathrm{NO}(mathrm{g}) ) is ( 90.5 k J m o l^{-1} ) The enthalpy of formation of ( N_{2} O_{4}(g) ) is ( 9.7 k J m o l^{-1} ) The standard entropy of ( mathrm{NO}(mathrm{g}) ) is ( 210 J k^{-1}, O_{2}(g) ) is ( 205 J k^{-1} m o l^{-1}, N_{2} O_{4}(g) ) is ( 304 J K^{-1} c ) ( exists: ) B. ( -75.64 k J ) c. ( -64.24 k J ) D . ( -83.27 k J ) | 11 |

527 | ( gamma ) is the ratio of molar specific heat capacity of the given gas at to its specific heat capacity at A. Constant temperature, constant volume B. Constant volume, Constant pressure c. constant pressure, Constant temperature D. constant pressure, constant volume | 11 |

528 | 2.43 The enthalpy of vaporisation of CCL is 30.5 kJ mol-. Calculate the heat required for the vaporisation of 284 g of CCL, at constant pressure. (Molar mass of CCl4 = 154 g mol-?) | 11 |

529 | Boiling point of an organic compound is ( 310 K . ) Its enthalpy of vaporisation per mole ( Delta_{v a p} H ) is ( 27.9 k J m o l^{-1} . ) If the entropy of vaporisation ( Delta_{v a p} S ) of organic compound is ( X ) then find out the value of ( X ) A ( cdot X=0.09 k J K^{-1} m o l^{-1} ) B. ( X=-0.09 k J K^{-1} m o l^{-1} ) c. ( X=0.18 k J K^{-1} m o l^{-1} ) D. None of these | 11 |

530 | Which of the following is true regarding sign of heat and work? A. Heat absorbed by the system has positive sign. Heat released to the surrounding has negative sign. Work done on the system has positive sign. Work done by the system has negative sign. B. Heat absorbed by the system has negative sign. Heat released to the surrounding has positive sign. Work done on the system has positive sign. Work done by the system has negative sign. C. Heat absorbed by the system has negative sign. Heat released to the surrounding has positive sign. Work done on the system has negative sign. Work done by the system has positive sign. D. Heat absorbed by the system has positive sign. Heat released to the surrounding has negative sign. Work done on the system has negative sign. Work done by the system has positive sign. | 11 |

531 | The ratio of the isothermal elasticity of gas to its adiabatic elasticity is : ( A cdot gamma ) B. ( frac{1}{gamma} ) c. ( 1-gamma ) D. ( frac{1}{1-gamma} ) | 11 |

532 | An iron block of mass ( 2 k g ), falls from a height of ( 10 m . ) After colliding with the ground it loses ( 25 % ) energy to surroundings and rest is gained as heat. Then find the temperature rise of the block. (Take sp. heat of iron ( left.470 J / k g^{circ} Cright) ) A. ( 0.53^{circ} ) C C ( C ) ? B. ( 0.053^{circ} mathrm{C} ) c. ( 0.159^{circ} mathrm{C} ) D. ( 0.212^{circ} mathrm{C} ) | 11 |

533 | Which one of the following equations does not correctly represent the first law of thermodynamics for the given process? A. Isothermal process: ( q=-w ) B. Cyclic process: ( q=-w ) C. Isochoric process: ( Delta U=q ) D. Adiabatic process: ( Delta U=-w ) E. Expansion of gas into vacuum: ( Delta U=q ) | 11 |

534 | 5 moles of oxygen are heated at constant volume from ( 10^{0} C ) to ( 20^{0} C . ) The change in internal energy of the gas is: ( C_{p}=7.03 mathrm{cal} mathrm{mol}^{-1} mathrm{K}^{-1} ) and ( R= ) ( 8.31 J mathrm{mol}^{-1} mathrm{K}^{-1} ) A . 125 call ( l ) B. 252 call c. 50 call D. 500 call | 11 |

535 | Which of the following are endothermic processes? This question has multiple correct options A. combustion of glucose B. decomposition of water C. dehydrogenation of ethane to ethene D. conversion of graphite to diamond | 11 |

536 | When the speed of electron increases, its specific charge: A. Increases B. Decreases c. Remains unchanged D. Increases and then decreases | 11 |

537 | An ideal gas undergoes a quasi static, reversible process in which its molar heat capacity ( C ) remains constant. If during this process the relation of pressure ( boldsymbol{P} ) and volume ( boldsymbol{V} ) is given by ( P V^{n}= ) constant, then ( n ) is given by (Here ( C_{P} ) ad ( C_{V} ) are molar specific heat at constant pressure and constant volume, respectively): ( ^{mathrm{A}} cdot_{n}=frac{C-C_{P}}{C-C_{V}} ) B. ( n=frac{C_{P}-C}{C-C_{V}} ) c. ( _{n}=frac{C-C_{V}}{C-C_{P}} ) D. ( _{n}=frac{C_{P}}{C_{V}} ) | 11 |

538 | When ammonium chloride is dissolved in water the solution becomes cold because A. Heat of solution of ammonium chloride is positive B. Heat of solution of ammonium chloride is negative c. Heat of dilution of ammonium chloride is positive D. Heat of formation of ammonium chloride is positive | 11 |

539 | Two moles of helium gas are taken over the cycle ( A B C D A, ) as show in the ( P-T ) diagram. Assuming the gas to be ideal the work done on the gas in taking it from state ( A ) to ( B ) is : ( mathbf{A} cdot 200 R ) B. ( 300 R ) c. ( 400 R ) ( mathbf{D} cdot 500 R ) | 11 |

540 | possible reversible processes performed on a monatomic ideal gas Process ( A ) is isobaris (constant pressure). Pressure ( B ) is isothermal (constant temperature). Process ( C ) is adiabatic. Process ( D ) is isochoric (constant volume). For which process(es) does the temperature of the gas decreases A. Process A only B. Process C only c. only process ( C ) and ( D ) D. Only process ( B, C ) and | 11 |

541 | What is the ratio of the enthalpy yield on combustion of hydrogen atoms to steam to the yield on combustion of an equal mass of hydrogen molecules to steam? Given ( : boldsymbol{H}_{2}(boldsymbol{g})+frac{mathbf{1}}{mathbf{2}} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow ) ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}), boldsymbol{Delta} boldsymbol{H}=-boldsymbol{2} mathbf{4} 2 ) kJ,Bond energy ( (boldsymbol{H}-boldsymbol{H})=mathbf{4 3 6} mathbf{k J} ) A . 0.80: B. 1: 0.80 c. 1.80: 1 D. 2.80: | 11 |

542 | A certain reaction is non-spontaneous at ( 300 mathrm{K} ). The entropy change during the reaction is ( 120 J K^{-1} ). Then the minimum value of ( Delta H ) for the reaction and the nature of the reaction will be: A. 36.0 kj; endothermic B. 36.0 kJ; exothermic c. ( 2.8 mathrm{kJ} ); endothermic D. ( -2.8 mathrm{kJ} ); exothermic | 11 |

543 | 19. A Carnot engine, whose efficiency is 40%, takes in heat from a source maintained at a temperature of 500 K. It is desired to have an engine of efficiency 60%. Then, the intake temperature for the same exhaust (sink) temperature must be (a) efficiency of carnot engine cannot be made larger than 50% (b) 1200 K (c) 750 K (d) 600 K (AIEEE 2012) han D diocrom | 11 |

544 | Based on the following thermochemical equations ( boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{C}(s) longrightarrow boldsymbol{C} boldsymbol{O}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) ) ( Delta boldsymbol{H}=mathbf{1 3 3} boldsymbol{k} boldsymbol{J} boldsymbol{m o l}^{-1} ) ( boldsymbol{C O}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H}= ) ( -282 k J m o l^{-1} ) ( boldsymbol{H}_{2}(boldsymbol{g})+frac{mathbf{1}}{mathbf{2}} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H}= ) ( -242 k J m o l^{-1} ) ( boldsymbol{C}(s)+boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) ; boldsymbol{Delta} boldsymbol{H}= ) ( boldsymbol{x} boldsymbol{k} boldsymbol{J} boldsymbol{m} boldsymbol{o l}^{-1} ) The value of ( x ) will be: A. ( 393.0 mathrm{KJ} ) в. ( 655.0 mathrm{KJ} ) D. ( -655.0 K J ) | 11 |

545 | For the gaseous reaction ( N_{2} O_{4} Leftrightarrow 2 N O_{2} ) ( mathbf{A} cdot Delta H>Delta E ) B. ( Delta H<Delta E ) c. ( Delta H=Delta E ) D. ( Delta H geq Delta E ) | 11 |

546 | For two bodies (which are in contact with each other) to be in thermal equilibrium, they must be separated by A. an insulating wall B. a conducting wall c. both A and B D. none of the above | 11 |

547 | f ( 1.0 k ) cal of heat is added to ( 1.2 L ) of ( O_{2} ) in a cylinder at constant pressure of 1 atm, the volume increase to ( 1.5 L ) Calculate ( Delta U ) and ( Delta H ) of the process ( (1 L-a t m=100 J) ) | 11 |

548 | The enthalpy change for a reaction does not depend upon: A. use of different reactants for the same product B. the nature of intermediate reaction steps C. the differences in initial or final temperatures of involved substances D. the physical states of reactants and products | 11 |

549 | Assertion Statement-I: Enthalpy of atomization is the heat of reaction ( boldsymbol{H}_{2} boldsymbol{O}(mathrm{I}) longrightarrow boldsymbol{H}_{2} boldsymbol{O} ) ( (g) ) Reason Statement-II : Gaseous molecules are far apart of each other due to less attraction. 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 | 11 |

550 | Which among the following are necessary and sufficient conditions for spontaneous reactions. ( A cdot Delta H=- ) ve only B. ( Delta mathrm{S}= ) -ve only c. Both ( Delta mathrm{H}=- ) -ve and ( Delta mathrm{S}=+mathrm{ve} ) D. ( Delta G=+v e ) | 11 |

551 | When 229 J of energy is supplied as heat at constant pressure to 3 mol ( A r(g), ) the temperature of the sample is increased by ( 2.55 mathrm{K} ). Calculate the motor heat capacity at constant volume: A. 30 KJ ( K^{-1} ) mol ( ^{-1} ) – B. 30 J K ( ^{-1} ) mol ( ^{-1} ) C . 21.7 J K ( ^{-1} ) mol ( ^{-1} ) D. 21.7 KJ K ( ^{-1} ) mol ( ^{-1} ) | 11 |

552 | Lan pressure Cp = (5/2) volume 8.3 x 10-3 m3 STRATION 14.6 An ideal gas has a specific heat at constant = (5/2) R. The gas is kept in a closed vessel of 3×10-‘m’ at a temperature of 300 K and a pressure 6 x 106 N/m². An amount of 2.49 X 10^ J of boot energy is supplied to the gas. Calculate the final temperature and pressure of the gas (R = 8.3 J/mol K). colution Asbere volume. | 11 |

553 | The value of ( log _{10} mathrm{K} ) for a reaction ( boldsymbol{A} longrightarrow boldsymbol{B} ) is : ( left(text { Given }: Delta_{mathrm{r}} mathbf{H}_{298 mathrm{K}}^{circ}=right. ) ( -mathbf{5 4 . 0 7 k J m o 1}^{-1}, quad Delta_{mathbf{r}} mathbf{S}_{298 K}^{0}= ) ( 10 mathrm{JK}^{-1} mathrm{mol}^{-1} ) and ( mathbf{R}=mathbf{8 . 3 1 4} mathbf{J K}^{-1} mathbf{m o 1}^{-1} ; quad mathbf{2 . 3 0 3} times ) ( 8.314 times 298=5705) ) A. 5 B. 10 c. 95 D. 100 | 11 |

554 | The enthalpy of dissociation of ( boldsymbol{H}_{3} ) is ( 954 k J / m o l ) and that of ( P_{2} H_{4} ) is ( 1.485 M J ) mol ( ^{-1} . ) What is the bond enthalpy of the ( P-P ) bond? A. ( 213 k J / ) mol в. ( -213 k J / ) тод c. ( 2757 k J / ) mol D. None of these | 11 |

555 | Which of the following is not a correct statement about enthalpy of solution? A. For most ionic compounds, ( Delta H_{s o l}^{0} ) is positive and the dissociation process is endothermic. B. Solubility of most salts increases with increase in temperature C. If the lattice enthalpy is very high, the dissolution of compound becomes very easy. D. Enthalpy of solution is determined by the selective values of the lattice enthalpy and hydration enthalpy. | 11 |

556 | 22. Consider a spherical shell of radius R at temperature T. The black body radiation inside it can be considered as an ideal gas of photons with internal energy per unit volume u = y a 14 and pressure P= . If the shell now undergoes an adiabatic expansion the relation between T and R is (a) Taek h (6) Ta e-R V 31 V (c) T – (d) 1 a 1 (a) R3 (JEE Main 2015) | 11 |

557 | When chlorine gas and hydrogen gas react to form hydrogen chloride, what will be the change of enthalpy of the reaction? (bond energies are at the end of this test) A . ( +245 k J / m o l ) в. +185 k ( J / ) mol c. ( -185 k J / m o l ) D. ( -1105 k J / m o l ) E . ( +1105 ~ k J / m o l ) | 11 |

558 | Which of the following are intensive properties? This question has multiple correct options A. heat capacity B. refractive index c. specific volume D. entropy | 11 |

559 | 27. A gas mixture consists of 2 mol of oxygen and 4 mol of argon at temperature T. Neglecting all vibrational modes, the total internal energy of the system is (a) 4RT (b) 15RT (c) 9RT (d) 11RT . | 11 |

560 | Heat of combustion of ( boldsymbol{C} boldsymbol{H}_{boldsymbol{4}(boldsymbol{g})} ) at constant volume is measured in bomb calorie-meter at ( 298.2 mathrm{K} ) and found to be 885389 find the valve of enthalpy. ( N_{2(g)}+3 H_{2(g)} rightarrow 2 N H_{3(g)} ) | 11 |

561 | a poin is put through a cycle consisting of the following three reversible steps: (CA): Isothermal compression from 2 atm and 10 litres to 20 atm and 1 litre. (AB): Isobaric expansion to return the gas to the original volume of 10 litres with T going from ( boldsymbol{T}_{mathbf{1}} ) to ( boldsymbol{T}_{mathbf{2}} ). (BC): Cooling at constant volume to bring the gas to the original pressure and temperature. The steps are shown schematically in | 11 |

562 | ( K_{P} ) for reaction ( A+B rightleftharpoons C+D ) is 1.34 ( operatorname{at} 60^{circ} mathrm{C} ) and 6.64 at ( 100^{circ} mathrm{C} . ) Determine the free energy change of this reaction at each temperature and ( Delta H^{o} ) for the reaction over this range of temperature? A. 405J/mol ; 5872 J/mol and 41.3 kJ/mol B. 810 J/mol ; 5870 J/mol and 41.3 kJ/mol c. ( 405 J / mathrm{mol} ); ( 5 mathrm{J} / mathrm{mol} ) and ( 20.56 mathrm{kJ} / mathrm{mol} ) D. 810 J/mol; 29362 J/mol and 20.56 kJ/mo | 11 |

563 | One mole of oxygen is allowed to expand isothermally and reversibly from ( 5 m^{3} ) to ( 10 m^{3} ) at 300 K. Calculate the work done in expansion of the gas. | 11 |

564 | ( boldsymbol{C}_{3} boldsymbol{H}_{2}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) rightarrow boldsymbol{C}_{2} boldsymbol{H}_{6}(boldsymbol{g})+ ) ( boldsymbol{C} boldsymbol{H}_{4}(boldsymbol{g}) triangle boldsymbol{H}^{0}=? ) ( begin{array}{ll}C_{2} boldsymbol{H}_{6} & boldsymbol{H}_{2}(boldsymbol{g}) \ (g)end{array} quad boldsymbol{C H}_{4}(boldsymbol{g}) quad ) graphit -1560.1 ( quad ) -225.0 ( quad-090.0 quad ) -393.5 ( triangle H^{0} )combustion( left(K J m o l^{-1}right. ) | 11 |

565 | The heat added to the heat engine is A . 150 B. 100 c. 50 D. 2. E. zero | 11 |

566 | 11 Consider the reactions given below. On the basis of these reactions find out which of the algebraic relationship given in options (a) to (d) is correct? 1. C(g) + 4 H (g) → CH, (g);4, H = x kJ mol-1 2. C (graphite) + 2H, (g) → CH, (g);A,H=ykl molº (a) x=y (b)x= 2y (c) x >Y. (d) x <y | 11 |

567 | In a process 701 J of heat is absorbed by a system and 394 J of work is done by system. What is the change in internal energy for the process? | 11 |

568 | Which one of the following options correctly represents a thermodynamic process that is used as a correction in the determination of the speed of sound in an ideal gas? A ( cdot(I)(i i)(Q) ) c. ( (I V)(i i)(R) ) D. ( (I I I)(i v)(R ) | 11 |

569 | Enthalpy of polymerisation of ethylene, as represented by the reaction, ( boldsymbol{n} boldsymbol{C H}_{2}=boldsymbol{C H}_{2} rightarrowleft(-boldsymbol{C H}_{2}-boldsymbol{C H}_{2}-right) boldsymbol{n} ) is ( -100 mathrm{kJ} ) per mole of ethylene. Given bond enthalpy of ( C=C ) bond is ( 600 mathrm{kJ} ) mol ( ^{-1} ), Determine enthalpy of ( C ) C bond (in ( mathrm{kJ} text { mol }) ) A . 350 в. з23 c. 565 D. 453 | 11 |

570 | Assertion The enthalpy of both graphite and diamond is taken to be zero, being elementry substances. Reason The enthalpy of formation of an elementary substance in any state is taken as zero 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 | 11 |

571 | A fixed amount of dry air at temperature of ( 27^{circ} C ) is compressed to ( frac{1}{9} t h ) of original volume. Its final temperature is ( (gamma=mathbf{1 . 5}) ) ( mathbf{A} cdot 627^{circ} C ) B. ( 600^{circ} mathrm{C} ) ( mathbf{c} cdot 158^{circ} mathrm{C} ) D. ( 527^{circ} mathrm{C} ) | 11 |

572 | The bond energy in ( k c a l m o l^{-1} ) of a ( C- ) ( -C ) single bond is approximately: ( A ) B. 10 ( c cdot 100 ) D. 1000 | 11 |

573 | What is a pure substance? | 11 |

574 | Derive an expression for work done in adiabatic expansion | 11 |

575 | The carnot cycle has maximum efficiency? A. True B. False | 11 |

576 | The molar heat of vaporization of toluene is ( Delta H_{v} . ) If its vapour pressure at ( 315 mathrm{K} ) is 60 torr ( & ) that at ( 355 mathrm{K} ) is 300 torr then ( Delta H_{v}=?(log 2=0.3) ) A . 37.4 kJ/mole B. 3.74 kJ/mole c. 37.4 J/mol D. 3.74 J/mole | 11 |

577 | Which of the following are state property? This question has multiple correct options A. Internal energy (U) B. Volume (V) c. Heat (q) D. Enthalpy (H) | 11 |

578 | Calculate ( Delta S_{r}^{o} ) at ( 298 K ) of (a) ( N a(s)+frac{1}{2} C l_{2}(g) rightarrow N a C l(s) ) ( frac{1}{2} N_{2}(g)+2 H_{2}(g)+frac{1}{2} C l_{2}(g) rightarrow ) ( N H_{4} C l(s) ) (iii) ( C(text { graphite }) rightarrow C ) (Diamond) The values of ( S^{o} ) of ( N a, C l_{2}, N a C l, N H_{4} C l, N_{2}, H_{2} ) diamond and graphite are ( mathbf{5 1}, mathbf{2 2 3}, mathbf{7 2}, mathbf{9 5}, mathbf{1 9 2}, mathbf{1 3 1}, mathbf{2 . 4 3}, mathbf{5}, mathbf{6 9} mathbf{J K} ) and ( m o l^{-1} ) respectively: | 11 |

579 | Pressure is an intensive property. A. True B. False | 11 |

580 | The heat of combustion of carbon (graphite) is not equal to that of carbon(diamond).lf true enter 1 else o ( A ) | 11 |

581 | Q6. A reaction, A + B C+D+q is found to have a positive entropy change. The reaction will be (i) possible at high temperature (ii) possible only at low temperature (iii) not possible at any temperature (iv) possible at any temperature | 11 |

582 | Which of the following is a state function? ( mathbf{A} cdot q times w ) в. ( q+w ) c. ( frac{q^{2}}{w^{2}} ) D. ( sqrt{q w} ) | 11 |

583 | Calculate standard enthalpy of formation for benzene from the following data. ( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{6}(ell)}+frac{mathbf{1 5}}{mathbf{2}} boldsymbol{O}_{mathbf{2}(boldsymbol{g})} longrightarrow boldsymbol{6} boldsymbol{C} boldsymbol{O}_{boldsymbol{2}(boldsymbol{g})}+ ) ( mathbf{3} boldsymbol{H}_{2} boldsymbol{O}_{(ell)} quad boldsymbol{Delta} boldsymbol{H}^{o}=-mathbf{3 2 6 7} boldsymbol{K} boldsymbol{J} ) ( Delta_{f} H^{o}left(C O_{2}right)=-393.5 K J m o l^{-1} ) ( Delta_{f} H^{o}left(C_{2} Oright)=-285.8 K J m o l^{-1} ) | 11 |

584 | What describes a spontaneous reaction? A. Positive ( Delta H ) B. Negative ( Delta H ) c. Positive ( Delta G ) D. Negative ( Delta G ) | 11 |

585 | Molar heat capacity of a gas does not depend on A. Its temperature B. Its molecular weight c. Its atomicity D. The conditions under which heat is supplied | 11 |

586 | For combustion of 1 mole of benzene at ( 25^{0} C, ) the heat of reaction at constant pressure is – 780.9 kcal. What will be the heat of reaction at constant volume? ( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{6}(boldsymbol{I})}+boldsymbol{7} frac{1}{2} boldsymbol{O}_{2(boldsymbol{g})} rightarrow boldsymbol{6} boldsymbol{C} boldsymbol{O}_{2(boldsymbol{g})}+ ) ( mathbf{3} boldsymbol{H}_{2} boldsymbol{O}_{(l)} ) A . -781.8 kcal в. -780.0 kcal c. +781.8 kcal D. +780.0 kcal | 11 |

587 | Heat cannot by itself flow from a body at lower temperature to a body at higher temperature is a statement of consequence of A. second law of thermodynamics B. conservation of momentum c. conservation of mass D. first law of thermodynamics. | 11 |

588 | [ begin{array}{c} text { Given: } S+frac{3}{2} O_{2} longrightarrow S O_{3}+2 x k c a l \ S O_{2}+frac{1}{2} O_{2} longrightarrow S O_{3}+y k c a l end{array} ] With the help of the above reactions, find out the heat of formation of ( boldsymbol{S O}_{2} ) A ( cdot(2 x-y) ) B . ( (x+y) ) ( mathbf{c} cdot(2 x+y) ) D ( cdot(2 x / y) ) | 11 |

589 | Assuming ideal behaviour, calculate the work done when 1.6 mole of water evaporates at ( 373 mathrm{K} ) against the atmospheric pressure of 1 atm. A . 29.67 J B. 48.8 J c. 21.2 J D. none of these | 11 |

590 | Why are exothermic reactions said to have a negative enthalpy? A. Because energy is flowing from the system to the environment B. Because energy is flowing from the environment into a closed system. C. Because endergonic reactions like ( A T P rightarrow A D P ) have a negative change in free energy. D. Because the movement of energy is based on the direction it is flowing. | 11 |

591 | Find work done in the isobaric process. A. ( W=1245 mathrm{J} ) B. ( W=1255 ) J c. ( W=1254 J ) D. ( W=1240 mathrm{J} ) | 11 |

592 | The enthalpy change of a reaction does not depend on A. initial and final enthalpy change of reaction B. state of reactants and products c. different intermediate reactions D. nature of reactants and products | 11 |

593 | Unusually high boiling point of water is result of A. Intermolecular hydrogen bonding B. Intramolecular hydrogen bonding c. Both intra and inter molecular hydrogen bonding D. High specific heat | 11 |

594 | toppr Q Type your question corresponding thermodynamic co- ordinates are given. Here, the ( P ) and ( V ) scales are so chosen that these cycles on ( P-V ) diagram appear to be circular. Analyse these cycles on ( P-V ) diagram and answer the following questions about these processes. What is the net work done in the given process? Cycle on System ( mathbf{A} cdot frac{pi P_{0} V_{0}}{4} ) ( mathbf{B} cdot-frac{pi P_{0} V_{0}}{4} ) ( c ) D. | 11 |

595 | Calculate the amount of heat energy required to raise the temperature of 1 kg of iron from ( 20^{circ} C ) to ( 100^{circ} ) C. ( c= ) ( 483 J k g^{-1} K^{-1} ) A. 35674 B. 48266 J c. ( 38640 mathrm{J} ) D. 56446 J | 11 |

596 | Which of the following is an intensive property? A. temperature B. pressure c. density D. all of the above | 11 |

597 | ( begin{array}{cccc}boldsymbol{H} & boldsymbol{H} & & boldsymbol{H} & boldsymbol{H} \ boldsymbol{C} & = & boldsymbol{C} & +boldsymbol{H}-boldsymbol{H} rightarrow boldsymbol{H}- & boldsymbol{C} & -boldsymbol{C}-boldsymbol{H} \ boldsymbol{H} & boldsymbol{H} & & boldsymbol{H} & boldsymbol{H}end{array} ) From the following bond energies: ( boldsymbol{H}-boldsymbol{H} ) bond energy: ( mathbf{4 3 1 . 3 7 k J} quad boldsymbol{m o l}^{-1} ) ( C=C ) bond energy: 606.10 ( k J quad ) mol ( ^{-1} ) ( boldsymbol{C}-boldsymbol{C} ) bond energy: ( mathbf{3 3 6 . 4 9 k J} quad boldsymbol{m o l}^{-1} ) ( C-H ) bond energy: ( 410.50 k J quad m o l^{-1} ) Enthalpy for the reaction will be: ( begin{array}{ll}text { A } . & 553.0 k Jend{array} quad ) mol ( ^{-1} ) B. 1523.6kJ mol” C . ( -243.6 k J quad ) mol ( ^{-1} ) D. ( -120.0 k J quad ) mol ( ^{-1} ) | 11 |

598 | Total internal energy of a system can never be evaluated but the change in internal energy can be determined by Ist law of thermodynamics. If true enter 1 , else enter 0 . | 11 |

599 | ( C_{P}-C_{V} ) for an ideal gas is R. Explain. | 11 |

600 | Which of the following is correct regarding Ellingham diagram? A ( cdot ) It is plot of ( Delta G_{f} ) per mole of metal versus temperature B. Reduction of a metal oxide is difficult if the metal formed is in liquid state at the temperature of reduction c. Plot is a straight line except when some change in phase. D. Ellingham diagram deals with both the feasibility as well as the rate of the reduction process | 11 |

601 | The relation between ( U, p ) and ( V ) for an ideal gas in an adiabatic process is given by relation ( U=a+b p V ). Find the value of adiabatic exponent ( gamma ) of this gas. A ( frac{b+1}{b} ) в. ( frac{b+1}{a} ) c. ( frac{a+1}{b} ) D. ( frac{a}{a+b} ) | 11 |

602 | Which of the following is the property of a system A. pressure and temperature B. internal energy c. volume and density D. all of the above | 11 |

603 | 0. 27 Given that AH = 0 for mixing of two gases. Explain whether the diffusion of these gases into each other in a closed container is a spontaneous process or not? | 11 |

604 | The rise in temperature of a substance depends on: A. The quality of heat supplied B. The mass of the substance c. The nature of the substance D. All the above | 11 |

605 | During fusion of ice, the entropy of system: A. decreases B. remains constant c. increases D. none of these | 11 |

606 | Warming ammonium chloride with sodium hydroxide in a test tube is an example of: A. closed system B. isolated system D. none of these | 11 |

607 | An ideal gas expands according to the law ( p V^{2}= ) const. The molar heat capacity ( C ) is A. ( C_{v}+ ) R в. ( C_{v}- ) R ( c cdot C_{v}+2 R ) D. ( C_{v}- ) 3R | 11 |

608 | Assertion ( C_{P} ) is always greater than ( C_{V} ) in gases. Reason Work done at constant pressure is more | 11 |

609 | . 32 The standard molar entropy of H.O (l) is 70 JK-1 mol-. Will the standard molar entropy of H20(s) be more, or less than 70 JK molº? | 11 |

610 | Assertion The zeroth law of thermodynamics was known before law I of thermodynamics. Reason The zeroth law concerning thermal equilibrium was appeared after three laws (I, II and III) of termodynamics and thus was named as zeroth law. 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 | 11 |

611 | Which of the following is true in the case of an adiabatic process, where ( gamma=C_{p} / C_{v} ? ) A ( cdot p^{1-gamma} T^{gamma}= ) constant B . ( p^{gamma} T^{1-gamma}= ) constant C ( cdot p T^{y}= ) constant D. ( p^{gamma} T= ) constant | 11 |

612 | Define mixtures. (a) ( boldsymbol{H}_{2}(boldsymbol{g})+frac{mathbf{1}}{mathbf{2}} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{H}_{2} boldsymbol{O}(l) ) [ boldsymbol{Delta} boldsymbol{H}_{298 K}^{o}=-285.9 boldsymbol{k J m o l}^{-1} ] (b) ( boldsymbol{H}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) [ boldsymbol{Delta} boldsymbol{H}_{298 K}^{o}=-241.8 boldsymbol{k J m o l}^{-1} ] The molar enthalpy of vapourisation of water will be: B. 22.0 kJ mol- c. ( 44.1 mathrm{kJ} mathrm{mol}^{-} ) D. ( 527.7 k J ) mol( ^{-} ) | 11 |

613 | Order of heat of combustion is: A. ( 1>3>2>4>5 ) В. ( 4>1>5>3>2 ) c. ( 1>4>2>3>5 ) | 11 |

614 | When a solid is converted into a gas, directly by heating then this process is known as: A. Sublimation B. Vaporization c. condensation D. Boiling | 11 |

615 | Show that the internal energy of the air (treated as an ideal gas) contained in a room remains constant as the temperature changes between day and night. Assume that the atmospheric around remains constant and the air in the room maintains this pressure by communicating with the surrounding through the windows etc. | 11 |

616 | A heat engine absorbs ( Q_{1} ) heat from hot reservoir and work produced by engine is ( W ), then: A ( cdot Q_{1} ) is always ( =W ) B. only in some special cases ( Q_{1}=W ) otherwise ( Q_{1} ) is greater than ( W ) c. ( Q_{1} ) is always less than ( W ) D. ( Q_{1} ) is always greater than ( W ) | 11 |

617 | An ideal gas goes from state ( A ) to state B via three different processes as indicated in the P-V diagram. If ( Q_{1}, Q_{2}, Q_{3} ) indicate the heat absorbed by the gas along the three processes and ( Delta U_{1}, Delta U_{2}, Delta U_{3} ) indicate the change in internal energy along the three processes respectively, then, ( mathbf{A} cdot Q_{3}>Q_{2}>Q_{1} ) and ( Delta U_{1}=Delta U_{2}=Delta U_{3} ) B ( cdot Q_{1}=Q_{2}=Q_{3} ) and ( Delta U_{1}=Delta U_{2}=Delta U_{3} ) ( mathbf{c} cdot Q_{1}>Q_{2}>Q_{3} ) and ( Delta U_{1}=Delta U_{2}=Delta U_{3} ) D ( cdot Q_{3}>Q_{2}>Q_{1} ) and ( Delta U_{1}>Delta U_{2}>Delta U_{3} ) | 11 |

618 | Increasing entropy in the universe means that A. Organisms can use the energy released to break down food products. B. There is increasing amounts of heat energy and small particles of matter becoming disordered C. Reactions cannot occur spontaneously D. The entropy in a system also must increase. | 11 |

619 | Specific heat of one mole of hydrogen at constant pressure and at constant volume are ( 450 J K^{-1} ) and ( 300 J K^{-1} ) respectively. Then what is the density of the gas at S.T.P? ( left(P_{a t m}=1.013 times 10^{5} N m^{-2}right) ) A ( .2 .47 mathrm{kg} / mathrm{m}^{3} ) В. ( 3.0 mathrm{kg} / mathrm{m}^{3} ) c. ( 3.58 mathrm{kg} / mathrm{m}^{3} ) D. ( 4.0 mathrm{kg} / mathrm{m}^{3} ) E. No solution | 11 |

620 | A kettle with ( 2 L ) water at ( 27^{circ} C ) is heated by operating coil heater power ( 1 k W $ . ) The heat is lost to the atmosphere at constant rate ( 160 mathrm{J} / mathrm{s} ) when its lid is open. In how much time will water heated to ( 77^{circ} C ) with the lid open ( ? ) (specific heat of water ( = ) ( left.4.2 k J /^{circ} C-k gright) ) A. 8 min 20 s B. 6 min 2 sec ( c .14 ) min D. 7 min | 11 |

621 | In an adiabatic change, the pressure and temperature of a monoatomic gas are related with relation as ( boldsymbol{P} propto boldsymbol{T}^{C} ) where ( C ) is equal to A ( cdot frac{5}{4} ) B. ( frac{5}{3} ) ( c cdot frac{5}{2} ) D. ( frac{3}{5} ) | 11 |

622 | A cylinder of gas is assumed to contains 14 kg of butane. If a normal family needs ( 20,000 mathrm{kJ} ) of energy per day for cooking, The cylinder will last: (Given : The enthalpy of combustion, ( -Delta H=-2658 mathrm{kJ} / ) mole for butane A. 24.33 days B. 28.44 days. c. 29.33 days D. 32 days. | 11 |

623 | Which of the following property is not a thermodynamic property of the system? A. pressure B. temperature c. specific volume D. heat | 11 |

624 | When two moles of Hydrogen atoms join together to form a mole of hydrogen molecules in closed rigid vessel with diathermic walls: ( boldsymbol{H}(boldsymbol{g})+boldsymbol{H}(boldsymbol{g}) longrightarrow boldsymbol{H}_{2}(boldsymbol{g}) ) A ( . w<0 ) B. ( Delta U= ) negative C ( cdot q_{text {system}}= )positive D. ( q_{text {surrounding}}= )negative | 11 |

625 | Expansion of a perfect gas into vacuum is related with: A. ( Delta H=0 ) в. ( q=0 ) c. ( W=0 ) D. All the above | 11 |

626 | Energy hidden in a definite quantity of substance is: A. Enthalpy B. Internal energy c. Free energy D. Entropy | 11 |

627 | For the decomposition of 1 mole of sodium chlorate, determine ( Delta boldsymbol{H}_{text {reaction}} ) ( left(Delta H_{f}^{0} text { values: } N a C l O_{3}(s)=-85.7right. ) kcal/ mol, ( N a C l(s)=-98.2 mathrm{kcal} / mathrm{mol} ) ( left.boldsymbol{O}_{2}(boldsymbol{g})=mathbf{0} text { kcal } / text { mol }right) ) A . -183.9 kcal B. -91.9 kcal c. +45.3 kcal ( mathbf{D} ldots+22.5 mathrm{kcal} ) E . -12.5 kcal | 11 |

628 | The heat of combustion of ethyne ( C_{2} H_{4} ) gas at ( 298^{circ} ) is ( -1411.3 K J . ) Calculate the heat of reaction at constant value and at ( 298 K . R=8.314 J / k / ) mol | 11 |

629 | Match the following. ( begin{array}{llll}text { I } & text { Isothermal process } & mathbf{1} & boldsymbol{Delta} boldsymbol{Q}=mathbf{0} \ text { II } & text { Isobaric process } & 2 & Delta V=0 \ text { III } & text { Isochoric process } & 3 & Delta P=0 \ text { IV } & text { Adiabatic process } & 4 & Delta T=0end{array} ) ( A ) ( |-4,||-3,|||-2, mid V-1 ) B. ( mid-3, ) । ( -2, ) II ( -1, ) IV- 4 c. ( |-1,| mid-2, ) ।I ( -3, ) ।V -4 D. ( |-4,||-2,| 1|-3,| V-1 ) E . ( |-1,||-4,|||-2, mid v-3 ) | 11 |

630 | Find the enthalpy of ( S-S ) bond from the following data (only magnitude in nearest integer in ( mathrm{kJ} / mathrm{mol} ) ): ( (i) C_{2} H_{5}-S-C_{2} H_{5}(g) Delta H_{f}^{o}= ) ( -147.2 k J / m o l ) ( (i i) C_{2} H_{5}-S-S-C_{2} H_{5}(g) ) ( Delta boldsymbol{H}_{f}^{o}=-mathbf{2 0 1 . 9 k J / m o l} ) ( (i i i) S(g) Delta H_{f}^{o}=222.8 k J / m o l ) | 11 |

631 | For the following reaction: ( boldsymbol{K}_{boldsymbol{p}}=mathbf{1 . 7} times ) ( 10^{7} ) at ( 25^{circ} C ) ( A g^{+}(a q .)+2 N H_{3}(g) rightleftharpoons ) ( left[boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}right]^{+} ) what value of ( Delta G^{o} ) in ( k J ? ) A. -41.2 B. -17.9 ( mathrm{c} cdot+17.9 ) ( mathbf{D} .+41.2 ) | 11 |

632 | Determine ( Delta H ) for the following reaction at ( 500 mathrm{K} ) and constant pressure [ boldsymbol{C O}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightarrow boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) ] use the following data: begin{tabular}{lll} Substance & ( C_{P}(mathrm{J} / ) ( operatorname{mol} mathrm{K}) ) & ( Delta_{f} H(298 mathrm{K})( ) ( mathrm{kJ} / mathrm{mol}) ) \ hline end{tabular} -110.5 begin{tabular}{l|l} со & 29.12 \ & \ ( H_{2} O ) & 33.58 \ & \ ( mathrm{CO}_{2} ) & 37.11 \ ( mathrm{H}_{2} ) & 29.89 end{tabular} -241.8 -393.5 0.0 ( mathbf{A} cdot Delta H=-30.3 mathrm{k} ) B. ( Delta H=-50.3 mathrm{kJ} ) c. ( Delta H=-40.3 mathrm{kJ} ) D. ( Delta H=-20.3 mathrm{kJ} ) | 11 |

633 | The entropy of a gas increases on its expansion. Why? | 11 |

634 | Select the correct option. ( mathbf{A} cdot Delta H_{f}[H(g)] ) is equal to ( Delta H_{text {atomisation}} ) of ( H_{2}(g) ) B. ( Delta H_{B E}[(H-H)] ) is equal to ( Delta H_{f} ) of ( H(g) ) ( mathbf{C} cdot Delta H_{B E}[(H-H)] ) is equal to ( Delta H_{text {atomisation}} ) of ( H_{2}(g) ) D. ( Delta H_{text {combustion}}left[H_{2}(g)right] ) is equal to ( Delta H_{f} ) of ( left[H_{2}(g)right] ) | 11 |

635 | A reversible engine converts one-sixth of the heat supplied into work. When the temperature of the sink is reduced by ( 62^{circ} mathrm{C}, ) the efficiency of the engine is doubled. The temperature of the source and sink are: A ( cdot 99^{circ} mathrm{C}, 37^{circ} mathrm{C} ) в. ( 80^{circ} mathrm{C}, 37^{circ} mathrm{C} ) ( mathbf{c} cdot 95^{circ} C, 37^{circ} C ) D . ( 90^{circ} mathrm{C}, 37^{circ} mathrm{C} ) | 11 |

636 | Calculate the internal energy at ( 298 mathrm{K} ) for the formation of one mole of ammonia, if the enthalpy change at constant pressure is ( -42.0 mathrm{kJ} ) mol( ^{-1} ) ( left[text { Given: } boldsymbol{R}=mathbf{8 . 3 1 4} mathbf{J} boldsymbol{K}^{-mathbf{1}} boldsymbol{m o l}^{-1}right] ) | 11 |

637 | Which of the following conditions make the process non spontaneous at all temperatures. A. ( Delta mathrm{H}=+mathrm{ve} ; Delta mathrm{s}=-mathrm{ve} ) B. ( Delta ) H ( =- ) -ve; ( Delta S=+v e ) c. ( Delta ) H ( =+v e ; Delta s=+v e ) D. ( Delta H=- ) -ve; ( Delta S=-v e ) | 11 |

638 | Explain reversible and irreversible process. Describe the working of Carnot Engine. Obtain an expression for its efficiency. | 11 |

639 | Discuss the change in energy and arrangement of molecules on increasing the temperature of ice from ( -5^{circ} mathrm{C} ) to ( 10^{circ} mathrm{C} ) at 1 atm pressure. | 11 |

640 | Mixing of non-reacting ideal gases at constant pressure is generally accompanied by: A. decrease in entropy B. increase in entropy c. change in enthalpy D. increase in free energy | 11 |

641 | ( 75 g ) of water at ( 10^{circ} C ) is heated by supplying ( 25200 J ) of heat energy. If the specific heat capacity of water is ( 4.2 J / g^{o} C . ) Calculate the final temperature of water ( mathbf{A} cdot 0^{circ} C ) B. ( 10^{circ} mathrm{C} ) c. ( 100^{circ} mathrm{C} ) D. ( 90^{circ} mathrm{C} ) | 11 |

642 | Assertion When ideal gas expand from ( boldsymbol{P}_{1}, boldsymbol{V}_{1}, boldsymbol{T}_{1} ) to ( P_{2}, V_{2}, T_{2} ) in two steps, and work done is high in which number of steps are high Reason Work is path function 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 | 11 |

643 | A box of negligible mass containing 2 moles of an ideal gas of molar mass ( M ) and adiabatic exponent ( gamma ) moves with constant speed ( boldsymbol{v} ) on a smooth horizontal surface. If the box suddenly stops, then change in temperature of gas will be A ( cdot frac{(gamma-1) M v^{2}}{4 R} ) B. ( frac{gamma M v^{2}}{2 R} ) c. ( frac{M v^{2}}{2(gamma-1) R} ) D. ( frac{(gamma-1) M v^{2}}{2 R} ) | 11 |

644 | One gram of water on evaporation at atmospheric pressure forms ( 1671 mathrm{cm}^{3} ) of steam. The heat of vaporisation at this pressure is 540 cal ( / ) gm. The increase in internal energy is A . 250 call в. 500 cal c. 1000 cal D. 1500call | 11 |

645 | Which of the following is a restatement of first law of thermodynamics: A. Guy-Lassac’s Law B. The principle of entropy C. The principle of enthalpy D. conservation of energy E. Avogadro’s hypothesis | 11 |

646 | 9. Two identical containers A and B with frictionless pistons contain the same ideal gas at the same temperature and the same volume V. The mass of the gas in A is ma and that in B is mg. The gas in each cylinder is now allowed to expand isothermally to the same final volume 2V. The changes in the pressure in A and B are found to be AP and 1.5AP, respectively. Then (a) 4mA = 9mB (b) 2mA = 3mp (c) 3mA = 2mB (d) Ima = 3mg | 11 |

647 | The ( Delta H_{t}^{circ} ) for ( C O_{2(g)}, C O_{(g)} ) and ( H_{2} O_{(g)} ) are -393.5,-110.5 and ( -241.8 k J ) mol ( ^{-1} ) respectively the standard enthalpy change (in ( boldsymbol{K} boldsymbol{J} ) ) for the reaction ( C O_{2(g)}+H_{2(g)} rightarrow C O_{(g)}+ ) ( boldsymbol{H}_{2} boldsymbol{O}_{(g)} ) is: ( mathbf{A} cdot 524 cdot 1 ) B. 41.2 c. 262.5 D. -41.2 | 11 |

648 | In the reaction ( q_{(p)=} Delta E+P Delta V ; Delta E ) refers to A. internal energy of the system B. heat content of the system c. change in internal energy D. change in the heat content | 11 |

649 | Equation of first law of thermodynamics for an isochoric process is A ( . Delta U=W ) в. ( Delta Q=W ) c. ( Delta U+W=0 ) D. ( Delta Q=Delta U ) | 11 |

650 | A mass of diatomic gas ( (gamma=1.4) ) at a pressure of 2 atm is compressed adiabatically so that its temperature rise from ( 27^{circ} mathrm{C} ) to ( 927^{circ} mathrm{C} ). The pressure of the gas is final state is A .28 atm B. 68.7 atm c. 256 atm D. 8 atm | 11 |

651 | The volume of a gas is reduced adiabatically to ( frac{1}{4} ) of its volume at ( 27^{circ} C ) If ( gamma=1.4 ) the new temperature is : A ( cdot(300) 2^{0.4} K ) В . (300) ( 2^{1.4} K ) c. ( 300(4)^{text {) }-4} K ) D. ( 300(2)^{0.4} K ) | 11 |

652 | The enthalpy change of which reaction corresponds to ( Delta H_{f}^{o} ) for ( N a_{2} C O_{3} ) at ( 298 K ? ) A ( cdot operatorname{Na(s)}+C(s)+frac{3}{2} O_{2}(g) rightarrow N a_{2} C O_{3}(s) ) в. ( N a_{2} O(s)+C O_{2}(g) rightarrow N a_{2} C O_{3}(s) ) c. ( 2 N a^{+}(a q .)+C O_{3}^{2-}(a q .) rightarrow N a_{2} C O_{3}(s) ) D ( cdot 2 N a^{+}(a q)+2 O H^{-}(a q .)+C O_{2}(a q .) longrightarrow N a_{2} C O_{3}(s)+ ) ( H_{2} O ) | 11 |

653 | Q2. For the process to occur under adiabatic conditions, the correct condition is: (1) AT = 0 (ii) Ap = 0 (iii) q = 0 (iv) w = 0 | 11 |

654 | Variation of ( log _{10} K ) with ( frac{1}{T} ) is shown by the following graph in which straight line is at ( 45^{circ}, ) hence ( Delta H ) is : A ( .+4.606 ) cal B . -4.606 ca ( c .+2 ) cal D. ( -2 mathrm{ca} ) | 11 |

655 | The run of cyanamide ( N H_{2} C N ) with dioxygen was carried out in a bomb calorie meter and ( Delta u ) was found to be ( -742.7 k J / m o l ) Calculate the enthalpy for the reaction at ( 298 mathrm{K} ) ( N H_{2} C N(s)+frac{3}{2} O_{2} rightarrow N_{2}+C O_{2}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ) | 11 |

656 | A system in thermodynamic equilibrium will have the following equilibrium(s):- A. Thermal equilibrium B. Mechanical equilibrium c. chemical equilibrium D. All of these | 11 |

657 | A gas at pressure ( p ) has volume ( V ). It is adiabatically compressed to volume ( V / 32 . ) If ( (32)^{1.4}=128, ) what is the current pressure of the gas? A . ( 128 p ) B. ( 63 p ) c. ( 32 p ) D. ( 16 p ) | 11 |

658 | The molar heat capacity of water at constant pressure ( P, ) is ( 75 mathrm{JK}^{-1} mathrm{mol}^{-1} ) When ( 1.0 mathrm{kJ} ) of heat is supplied to ( 100 mathrm{g} ) of water which is free to expand, the increase in temperature of water is: A . ( 1.2 k ) B. 2.4 K c. ( 4.8 mathrm{k} ) D. 6.6 K | 11 |

659 | Exothermic enthalpy changes are shown as negative values positive values neutral constant ( A ) B. 2 ( c cdot 3 ) D. 4 | 11 |

660 | R. 20 18.0 g of water completely vaporises at 100°C and 1 bar pressure and the enthalpy change in the process is 40.79 kJ molº. What will be the enthalpy change for vaporising two moles of water under the same conditions? What is the standard enthalpy of vaporisation for water? | 11 |

661 | During the phase change, when water freezes, its converted to ice in which molecules is in more structured order. Why doesn’t this contradict the Second Law of Thermodynamics? A. Because the density of the water is decreasing B. Because the water is gaining entropy as it goes from liquid to solid state C. Because the water’s internal energy is decreasing D. Because the surroundings are losing entropy E. Because the surroundings are gaining entropy | 11 |

662 | A gas contained in a cylinder is filled with a frictionless piston expands against a constant pressure 1 atmosphere from a volume of 4 litre to a volume of 14 litre. In doing ( s o, ) it absorbs ( 800 J ) thermal energy from surroundings. Determine ( Delta U ) for the process. | 11 |

663 | Calculate the heat of combustion (kJ) of propane, ( C_{3} H_{8} ) using the listed standard enthalpy of reaction data: [ begin{array}{c} C_{3} H_{8}(g)+mathbf{5} O_{2}(g) longrightarrow \ mathbf{3} C O_{2}(g)+4 H_{2} O(g) \ mathbf{3} C(s)+4 H_{2}(g) longrightarrow \ C_{3} H_{8}(g) Delta H / k J=-103.8 \ C(s)+O_{2}(g) longrightarrow C O_{2}(g) Delta H / k J= \ -393.5 \ H_{2}(g)+1 / 2 O_{2}(g) longrightarrow \ H_{2} O(g) Delta H / k J=-241.8 end{array} ] A . – 2043.9 B. -1532.9 c. -1021.9 D. -739. | 11 |

664 | ( C_{v} ) for helium gas ( (H e) ) is ( left(i n J m o l^{-1} K^{-1}right) ) A . 2.5 B. 10.5 ( c cdot 1.5 ) D. 12.5 | 11 |

665 | Find the product(s) when methane, ( C H_{4}, ) burns in excess of oxygen? A ( cdot C H_{4} O_{2} ) в. ( C O+H_{2} O ) c. ( C O+C H_{2} O H ) D. ( C O_{2}+H_{2} O ) E ( cdot C O_{2}+2 H_{2} ) | 11 |

666 | One litre sample of a mixture of methane gas and ( O_{2} ) measured at ( 25^{circ} C ) and 740 torr was allowed to react at constant pressure in a calorimeter which together with its content has a heat capacity of 1260 cal/degree. The complete combustion of methane to ( C O_{2} ) and ( H_{2} O ) caused a temperature rise in calorimeter of 0.667 K. The percentage of ( C H_{4} ) in original mixture was: Given: ( Delta boldsymbol{H}_{text {combustion}} ) of ( boldsymbol{C} boldsymbol{H}_{4} ) is ( -210.8 k c a l m o l^{-1} ) A . ( 10 % ) в. 20% c. ( 15 % ) D. 30% | 11 |

667 | An open end manometer consists of 0.75 moles of ( X_{g} ) taken in a container of volume 24.63 lit at ( 300 K . ) The level of mercury in the open tube is found to be ( 14 mathrm{cm} ) lower. The height difference when manometer is heated to ( 450 K ) will be: A . ( 14.5 mathrm{cm} ) B. ( 21 mathrm{cm} ) ( mathbf{c} cdot 13 c m ) D. ( 17 mathrm{cm} ) | 11 |

668 | Assertion (A) : Zeroth law of thermodynamics gives us the concept of energy Reason (R) : Internal energy is dependent on temperature A. 1) Both Assertion and Reason are true and reason is correct explanation of Assertion B. 2) Both Assertion and Reason are true but reason is not correct explanation of Assertion C. 3 ) Assertion is true but reason is false D. 4 ) Assertion is false but reason is true | 11 |

669 | 32 gram of oxygen gas at temperature ( 27^{circ} mathrm{C} ) is compressed adiabatically to ( 1 / 3 ) of its change in internal energy. ( gamma=1.5 text { of oxygen }) ) | 11 |

670 | Find out the most efficient engine in the following A. An engine converts ( 80 mathrm{K} ). of heat energy into ( 20 mathrm{KJ} ) of work B. An engine converts 50 KJ of heat energy into 15 KJ of work C. An engine converts 30 KJ of heat energy into 6 KJ of work D. An engine converts 60 KJ of heat energy into 24 KJ of work | 11 |

671 | A gas is taken through the cycle ( A B C A ) as shown. What is the net work done by the gas? ( A cdot 3000 J ) в. ( 1000 J ) c. zer D. 2000J | 11 |

672 | Which of the following equations corresponds to the definition of enthalpy of formation at ( 298 K ? ) A . ( C(text {graphite})+2 H_{2}(g)+1 / 2 O_{2}(l) rightarrow C H_{3} O H(g) ) B. ( C(text { diamond })+2 H_{2}(g)+1 / 2 O_{2}(g) rightarrow C H_{3} O H(l) ) c. ( 2 C(text { graphite })+4 H_{2}(g)+O_{2}(g) quad rightarrow 2 C H_{3} O H(l) ) D. ( C(text {graphite})+2 H_{2}(g)+1 / 2 O_{2}(g) rightarrow C H_{3} O H(l) ) | 11 |

673 | toppr Q Type your question- corresponding ( boldsymbol{P}-boldsymbol{V} ) diagram for the process is (all figures are schematic and not drawn to scale) ( A ) B. ( c ) ( D ) | 11 |

674 | What describes a non-spontaneous reaction? A. Positive ( Delta H ) B. Negative ( Delta H ) c. Positive ( Delta G ) D. Negative ( Delta G ) | 11 |

675 | If water kept in an insulated vessel at ( -10^{circ} C ) suddenly freezes, the entropy change of the system: A. decrease B. increase c. is zero D. equals to that of the surrouding | 11 |

676 | In the following ( V-T ) diagram, what is the relation between ( P_{1} ) and ( P_{2} ? ) ( A cdot P_{2}=P_{1} ) В ( cdot P_{2}>P_{1} ) ( c cdot P_{2}<P_{1} ) D. cannot be predicted | 11 |

677 | An ideal gas is taken around the cycle ABCDA as shown in figure. The net work done during the cycle is equal to: A. zero B. positive c. negative D. we cannot predict | 11 |

678 | Assertion Water in liquid state is more stable than ice at room temperature. Reason Water in liquid form has higher entropy than ice. 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 | 11 |

679 | For a reaction taking place in a container in equilibrium with its surroundings, the effect of temperature on its equilibrium constant ( boldsymbol{K} ) in terms of change in entropy is described by This question has multiple correct options A. With increase in temperature, the value of ( K ) for exothermic reaction decreases because the entropy change of the system is positive B. With increase in temperature, the value of ( K ) for endothermic reaction increases because unfavourable change in entropy of the surroundings decreases c. with increase in temperature, the value of ( K ) for endothermic reaction increases because the entropy change of the system is negative D. With increase in temperature, the value of ( K ) for exothermic reaction decrease because favourable change in entropy of the surroundings decreases | 11 |

680 | ( 0.1 m^{3} ) of water at ( 80^{circ} ) is mixed with ( 0.3 m^{3} ) of water at ( 60^{circ} . ) The final temperature of mixture is : A ( cdot 80^{circ} mathrm{C} ) B . ( 70^{circ} mathrm{C} ) ( mathbf{c} cdot 60^{circ} mathrm{C} ) D. ( 75^{circ} mathrm{C} ) | 11 |

681 | an isochoric reversible process ( mathbf{A} cdot Delta U=19.90 k J, Delta H=24.058 k J ; w=0 ) B . ( Delta U=-19.90 k J, Delta H=24.058 k J ; w=0 ) C ( . Delta U=19.90 k J, Delta H=-24.058 k J ; w=0 ) D. None of these | 11 |

682 | Which of the following is not a characteristic of an irreversible process? A. Spontaneity B. Energy loss C. Slow change in system variables D. All of the above | 11 |

683 | The internal energy of compressed real gas, as compared to that of the ideal gas at the same temperature is A . less B. more c. sometimes less, sometimes more D. maximum | 11 |

684 | For the reaction of one mole of zinc dust with one mole of sulphuric acid in a bomb calorimeter, ( triangle boldsymbol{U} ) and ( boldsymbol{w} ) corresponds to: A. ( triangle U<0, w=0 ) в. ( triangle U<0, w0, w=0 ) D. ( triangle U>0, w>0 ) | 11 |

685 | Dissolution of all gases in water is accompanied by evolution of heat. A. True B. False | 11 |

686 | 0.7 In an adiabatic process, no transfer of heat takes place between system and surroundings. Choose the correct option for free expansion of an ideal gas under adiabatic condition from the following. (a) q =0, AT #0, W=0 (b) q +0,AT =0,W=0 (c) q=0, AT = 0, W=0 (d) q = 0, AT <0,W 70 | 11 |

687 | * 0 The difference between C and Ccan be derived using the empt relation H = U + pv. Calculate the difference between C and C, for 10 moles of an ideal gas. | 11 |

688 | In the following pressure-volume diagram, the isochoric, isothermal and isobaric parts, respectively, are A. ( B A, A D, D C ) в. ( C B, B A, D C ) c. ( A B, B C, C D ) D. ( C D, D A, A B ) | 11 |

689 | On a ship sailing in pacific ocean where temperature is ( 23.4, ) a balloon is filled with ( 2 mathrm{L} ) air. What will be the volume of the balloon when the ship reaches Indian ocean, Where temperature is ( mathbf{2 6 . 1} ? ) | 11 |

690 | If the bond dissociation energies of ( boldsymbol{X} boldsymbol{Y} ) ( X_{2} ) and ( Y_{2} ) (all diatomic molecules) are in the ratio of 1: 1: 0.5 and ( Delta_{1} H ) for the formation of ( X Y ) is ( -200 k J ) mol( ^{-1} . ) The bond dissociates energy of ( X_{2} ) will be: A ( .100 mathrm{kJ} mathrm{mol}^{-1} ) в. 200 kJ mol- c. ( 800 k J ) mol ( ^{-1} ) D. ( 400 mathrm{kJ} mathrm{mol}^{-1} ) | 11 |

691 | Work done in the cyclic process shown in figure is : ( A cdot 4 P_{0} V_{0} ) ( mathbf{B} cdot-4 P_{0} V_{0} ) ( ^{mathbf{C}}-frac{22}{7} P_{0} V_{0} ) ( mathbf{D} cdot-13 P_{0} V_{0} ) | 11 |

692 | Which of the following reactions have same heat of reaction at constant ( boldsymbol{P} ) and constant volume as well? This question has multiple correct options ( mathbf{A} cdot 2 N O(g) longrightarrow N_{2}(g)+O_{2}(g) ) B ( cdot N_{2}(g)+3 H_{2}(g) longrightarrow 2 N H_{3}(g) ) ( mathbf{c} cdot operatorname{Co}_{3} O_{4}(s)+4 C O(g) longrightarrow 3 operatorname{Co}(s)+4 C O_{2}(g) ) D. ( H_{2}(g)+C l_{2}(g) longrightarrow 2 H C l(g) ) | 11 |

693 | A car is moving with a speed of 40 km/hr. If the car engine generated 7 kilowatt power, then the resistive force in the path of the car will be:- A. 360 Netwon B. 630 Newton c. zero D. 280 Newton | 11 |

694 | If the heat absorbed by a heat engine is ( 600 mathrm{kJ} ) per cycle and it releases ( 480 mathrm{kJ} ) of heat each cycle, what is its efficiency? A . 20% B. 80% c. ( 100 % ) D. 30% | 11 |

695 | If the door of a refrigerator is kept open in a room, will it make the room warm or cool? | 11 |

696 | Lets consider a thermodynamic system. If ( Delta U ) represents the increase in its internal energy and ( W ) the work done by the system, which of the following statements is true? A. ( Delta U=-W ) is an adiabatic process B. ( Delta U=W ) in an isothermal process c. ( Delta U=-W ) in an isothermal process D. ( Delta U=W ) in an adiabatic process | 11 |

697 | A reversible process changes the state of a system in such a way that the net change in the combined entropy of the system and its surroundings is : A. zero B. Unity c. Notequal D. More than zero | 11 |

698 | In the process shown in figure, the internal energy of an ideal gas decreases by ( frac{3 P_{0} V_{0}}{2} ) in going point ( C ) to A. Heat transfer along the process CA is A. ( -3 P_{0} V_{0} ) B. ( frac{-5 P_{0} V_{0}}{2} ) ( c cdot frac{-3 P_{0} V_{0}}{2} ) ( D ) | 11 |

699 | Given ( boldsymbol{C}(boldsymbol{s})+boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+ ) ( mathbf{9 4 . 2 K c a l} ) ( boldsymbol{H}_{2}(boldsymbol{g})+frac{1}{2} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{H}_{2} boldsymbol{O}(l)+ ) ( mathbf{6 8 . 3 K c a l} ) ( boldsymbol{C H}_{4}(boldsymbol{g})+mathbf{2} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+ ) ( 2 H_{2} O(l)+210.8 K c a l ) The heat of formation of methane in kcal will be: A . – 45.9 в. -47.8 c. – 20.0 D. -47.3 | 11 |

700 | The heat of formation ( left(Delta H_{f}^{o}right) ) of ( H_{2} O(l) ) is equal to: A. zero B. molar heat of combustion of ( H_{2}(l) ) c. molar heat of combustion of ( H_{2}(g) ) D. sum of heat of formation of ( H_{2} O(g) ) and ( O_{2}(g) ) | 11 |

701 | For a reversible reaction at ( 298 mathrm{K} ), the equilibrium constant K is 200. What is the value of ( triangle G^{0} ) at ( 298 mathrm{K} ? ) A . -13.13 kcal B . -0.13 kcal c. -3.158 kcal D. – 0.413 kcal | 11 |

702 | If the density of a certain gas at ( 30^{circ} mathrm{C} ) and 768 torr is ( 1.35 k g / m^{3}, ) the density at STP would be: A. ( 1.48 mathrm{kg} / mathrm{m}^{3} ) в. 1.58 kg ( / m^{3} ) c. ( 1.25 mathrm{kg} / mathrm{m}^{3} ) D. ( 1.4 mathrm{kg} / mathrm{m}^{3} ) | 11 |

703 | The change in internal energy of the methanol is A ( cdot 9.6 times 10^{5} J ) B . ( 7.14 times 10^{5} mathrm{J} ) c. ( 6.89 times 10^{4} J ) D. ( 6.86 times 10^{5} J ) | 11 |

704 | ( 3000 J ) of heat is given to a gas at a constant pressure of ( 2 times 10^{5} N / m^{2} . ) If its volume increases by 10 litres during the process find the change in the internal energy of the gas. | 11 |

705 | Which of the following quantity decreases when a gas condenses into a liquid? A. Standard voltaic potential B. Entropy c. Enthalpy D. Reaction rate E. Gibbs free energy | 11 |

706 | The heats of formation of ( boldsymbol{C}_{6} boldsymbol{H}_{6}(l), boldsymbol{H}_{2} boldsymbol{O}(l), boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g}) ) are 11.70,-68.4 and ( -94.0 k c a l ) respectively. Calculate the heat of combustion of benzene(l) A . -780.9 kcal-780.9kcal B. -680.9 kcal-780.9kcal c. 580.9 kcal-780.9kcal D. 480.9 kcal-780.9kcal | 11 |

707 | Illustration 2.52 The dissolution of ammonium chloride in water is an endothermic process but still it dissolves in water readily. Why? | 11 |

708 | Assertion Decrease in free energy causes Spontaneous reaction. Reason Spontaneous reactions are invariably exothermic. 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 | 11 |

709 | At the boiling point of water the saturated vapour pressure will be (in mm of ( mathrm{Hg} ) ) A. 750 B. 760 ( c cdot 850 ) D. 860 | 11 |

710 | The heat of combustion of ( boldsymbol{H}_{2}(boldsymbol{g}) ) at constant pressure and ( 300 K ) is ( -280 mathrm{kJ} ) ( operatorname{mol}^{-1} ) What will be the heat of combustion at constant volume and ( 300 K ? ) A. ( Delta U=- ) -276.2587 k B. ( Delta U=+276.2587 mathrm{kJ} ) c. ( Delta U=-27.63 mathrm{kJ} ) D. None of these | 11 |

711 | In carnot cycle to increase efficiency which of the following parameter need to be changed? A. Decrease source temperature B. Decrease sink Temperature C. No effect D. None of these | 11 |

712 | Which of the following statements are correct as per IUPAC sign convention? This question has multiple correct options A. The work done by the system on the surrounding is negative B. The work done by the surrounding on the system is positive C. The heat absorbed by the system from the surrounding is positive D. The heat absorbed by the surrounding from the system is positive | 11 |

713 | R. 55 Assertion (A) Combustion of all organic compounds is an exothermic reaction. Reason (R) The enthalpies of all elements in their standard state are zero. (a) Both A and R are true and R is the correct explanation of A (b) Both A and R are true but R is not the correct explanation of A (c) A is true but R is false (d) A is false but R is true | 11 |

714 | The equilibrium constant for ( boldsymbol{A}(boldsymbol{g})+ ) ( B_{2}(g) rightleftharpoons A B_{2}(g) ) is ( k_{p}=100 a t 522 K ) Structure of ( A B_{2} ) is like ( H_{2} O . ) If bond energy of ( A-B ) bond is ( 200 mathrm{kJ} / mathrm{mol} ) and that of ( B-B ) bond is ( 100 mathrm{kJ} / mathrm{mol} ), then ( Delta S^{o} ) of the above reaction is: A . -0.53 J/mol-K B . – -536 J/mol-K c. – -550 J/mol-K D. – -5.36 J/mol-K | 11 |

715 | In which of the following process the system and surrounding does not comes back to original state after the process is complete? A. Reversible process B. Adiabatic process c. Quasi-static process D. Spontaneous process | 11 |

716 | A monatomic gas is compressed adiabatically to ( frac{1}{4} ) of its original volume, the final pressure of gas in terms of initial pressure P is: A . 7.08 ( mathrm{P} ) B. 8.08 P c. 9.08 p D. 10.08 | 11 |

717 | Assertion Internal energy change in a cyclic process is zero. Reason Internal energy is a state function. 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. | 11 |

718 | Calculate the difference between heat of combustion of carbon monoxide gas at constant pressure and at constant volume at ( 27^{circ} mathrm{C} ?left(mathrm{R}=2 text { cal. } K^{-1} mathrm{mol}^{-1}right. ) ( mathbf{A} cdot 54 mathrm{cal} ) B. 600 call c. -300 cal D. 27 cal | 11 |

719 | When 1 mol gas is heated at constant volume temp. is raised from 298 to 308 K. Heat supplied to the gas is 500 J. Then which statement is correct? ( A cdot q=w=500 mathrm{J}, mathrm{U}=0 ) B. ( q=U=500 ), ( w=0 ) ( c cdot q=w=600,1, U=0 ) D. ( U=0, q=w=400 ) | 11 |

720 | Find the work requires to compress adiabatically ( 1 g ) of air initially at ( N T P ) to half its volume. Density of air at ( N T P=0.001129 g c m^{-3} ) and ( frac{C_{p}}{C_{v}}=1.4 ) A . ( 62.64 J ) в. ( 32.64 J ) c. ( -32.64 J ) D. ( -62.64 J ) | 11 |

721 | In a reaction, if ( Delta H ) and ( Delta S ) both are more than zero, then in which of the following cases, the reaction would not be spontaneous? This question has multiple correct options A ( . Delta H>T Delta S ) в. ( T Delta S>Delta H ) c. ( Delta H=T Delta S ) D. All of the above | 11 |

722 | Which of the following is an intensive property? A. Surface tension and density B. Surface tension and volume c. Enthalpy mass and density D. None of these | 11 |

723 | Find the external work done by the system in kcal, when 20 kcal of heat is supplied to the system the increase in the internal energy is ( 8400 J(J= ) ( 4200 J / k c a l) ) A . ( 16 ~ k c a l l ) B. 18 kcall c. 20 k call ( l ) D. 19 kcall ( l ) | 11 |

724 | For the conversion of liquid into a solid: A. orderliness decreases and entropy decreases B. orderliness increases and entropy increases c. both are not related D. orderliness increases and entropy decreases | 11 |

725 | Assertion For an ideal gas in a cyclic process and in an isothermal process change in internal energy is zero. Reason In both processes there is no change in temperature. 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 | 11 |

726 | Q11. (a) Why is the entropy of a substance taken as zero at OK? (6) Calculate 4G and AG® for the reaction. A+B= C+D at 27°C. Equilibrium constant (K) for this reaction = 102 | 11 |

727 | Gas constant ( (boldsymbol{R}) ) equals to A ( cdot frac{C_{p}}{C_{v}} ) B. c. ( C_{v}-C_{p} ) D. ( C_{p}-C_{v} ) | 11 |

728 | The work done in the given figure is A ( .3 times 10^{5} J ) B ( cdot 2 times 10^{5} J ) ( mathbf{c} cdot 10^{5} J ) D. zero | 11 |

729 | Difference between ( Delta H ) and ( Delta E ) for the combustion of liquid benzene at ( 27^{circ} mathrm{C} ) is: A ( .7 .48 k J ) в. ( 3.47 k J ) c. ( 14.86 k J ) D. ( 5.73 k J ) | 11 |

730 | Which of the following reactions is said to be entropy driven? A. Endothermic reaction with positive entropy change and high temperature B. Endothermic reaction with negative entropy change and low temperature C. Exothermic reaction with positive entropy change and high temperature D. Exothermic reaction with negative entropy change and low temperature | 11 |

731 | Name the apparatus used to measure the heat absorbed or released by a reaction. A. Centrifuge B. Barometer c. Balance D. Calorimeter E. Battery | 11 |

732 | The second law of thermodynamics says that in a cyclic process A. Work cannot be converted into heat B. Heat cannot be converted into work C. Work cannot be completely converted into heat D. Heat cannot be completely converted into work | 11 |

733 | What is the value for ( Delta H ) for the reaction ( N_{2} O_{4} rightarrow 2 N O_{2} ? 2 N O_{2} rightarrow ) ( N_{2}+2 O_{2} quad Delta H=-16.2 k c a l ) ( N_{2}+2 O_{2} rightarrow N_{2} O_{4} quad Delta H= ) ( +2.31 k c a l ) A . +13.89 kcal B . +18.51 kcal c. +37.42 kcal D. -13.89 kcal E . -18.51 kcal | 11 |

734 | When heat is given to gas in an isothermal change, the result will be A. external work done B. rise in temperature c. increase in internal energy D. external work done and also rise in temperature | 11 |

735 | Which physical quantity determines the direction of flow of heat energy? A. Temperature B. Amplitude c. Frequency D. wavelength | 11 |

736 | ( S(s)+O_{2}(g) rightarrow S O_{2}(g) quad Delta H^{circ}= ) ( -297 k J ) ( 2 S O_{2}(g)+O_{2}(g) rightarrow ) ( 2 S O_{3}(g) quad Delta H^{circ}=-198 k J ) Given the above thermochemical reactions, what is the heat of reaction for the formation of ( S O_{3}(g) ) provided below? ( boldsymbol{S}(boldsymbol{s})+boldsymbol{3} / 2 boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{S} boldsymbol{O}_{3}(boldsymbol{g}) ) A ( .-495 mathrm{kJ} ) B . -396 k c. -198 k D . +99 E . +198 k | 11 |

737 | For a spontaneous process, entropy A. Increases B. Decreases c. Unchanged D. Not clear | 11 |

738 | The heat released when the requisite amount of ions in the gaseous state combine to give 1 mol of crystal lattice is known as: A. lattice energy B. hydration energy c. formation energy D. none of the above | 11 |

739 | The standard heat of combustion of solid boron is equal to: A. ( Delta_{f} H^{circ}left(B_{2} O_{3}right) ) (2) B ( cdot frac{1}{2} Delta_{f} H^{circ}left(B_{2} O_{3}right) ) ( mathbf{c} cdot 2 Delta_{f} H^{circ}left(B_{2} O_{3}right) ) ( mathbf{D} cdot-frac{1}{2} Delta_{f} H^{circ}left(B_{2} O_{3}right) ) | 11 |

740 | For a thermodynamics process to be reversible, the temperature difference between hot body and the working substance should be A . zero B. minimunm c. maximum D. infinity | 11 |

741 | A constant valume gas thermometer shows pressure reading of ( 50 mathrm{cm} ) and ( 90 mathrm{cm} ) of mercury at ( 0^{0} mathrm{C} ) and ( 100^{0} mathrm{C} ) respectively. When the pressure reading is ( 60 mathrm{cm} ) of mercury, the temperature is:- ( mathbf{A} cdot 25^{0} C ) в. ( 40^{circ} mathrm{C} ) c. ( ^{circ} mathrm{C} ) D. ( 30^{circ} mathrm{C} ) | 11 |

742 | Neither q nor w is a state function but ( q+w ) is a state function. Why? | 11 |

743 | n changing the state of a gas adiabatically from an equilibrium state A to another equilibrium state ( mathrm{B} ) an amount of work equal to ( 22.3 mathrm{J} ) is done on the system. If the gas is taken from state ( A ) to ( B ) via a process in which the net heat absorbed by the system is 9.35 cal then net work done by the system in the later case is: (Take ( 1 mathrm{cal}=4.2 mathrm{J} ) A . 15 J в. 16 c. 17 D. 18 J | 11 |

744 | The reaction which proceeds with evolution of heat is called: A. exothermic B. endothermic C. may be exothermic or endothermic D. neither endothermic nor exothermic | 11 |

745 | ( K_{c} ) for ( frac{3}{2} H_{2}+frac{1}{2} N_{2} rightleftharpoons N H_{3} ) are 0.0266 and 0.0129 at ( m^{-1} ) respectively at ( 350^{circ} C ) and ( 400^{circ} mathrm{C} . ) Calculate heat of formation of ( boldsymbol{N} boldsymbol{H}_{3} ) A . 12.140 Kcal B. 1.214 Kcal c. ( -12.140 mathrm{Kcal} ) D. -1.214 Kcal | 11 |

746 | If the enthalpy of formation o ( f boldsymbol{H} boldsymbol{C l}(boldsymbol{g}) ) and ( C l^{-}(a q) ) are ( -92 k J / ) mole and ( -167.44 k J / m o l, ) find the enthalpy of solution of hydrogen chloride gas. ( mathbf{A} cdot-75.14 k J / m o l ) B. ( +75.14 k J / ) mol c. ( -260.7 k J / ) mol D. None of these | 11 |

747 | Assertion In a constant pressure process if we neglect the friction between piston then we can definetly say that the process has to be reversible. Reason Since there is always an equilibrium on piston due to constant pressure we can say that it is reversible process. 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 | 11 |

748 | In a cyclic process, which of the following statement is correct? A. Change in internal energy is not zero. B. The system returns to its initial state and it is is is reversible c. The total heat absorbed by the system is not equal to work done by the system D. Change in internal energy is zero. | 11 |

749 | Which of the following statement is false? A. Work is a state function. B. Temperature is a state function. C. Change of state is completely defined when initial and final states are specified. D. Work appears at the boundary of the system. | 11 |

750 | What are the types of thermodynamic equilibrium? A. Thermal equilibrium B. Mechanical equilibrium c. chemical equilibrium D. All above | 11 |

751 | Which is the correct order of bond energy of single, double and triple bonds between carbon atoms? A. ( C-C>C=C>C equiv C ) в. ( C=C>C equiv C>C-C ) c. ( C equiv C>C-C>C=C ) D. ( C equiv C>C=C>C-C ) ( C ) | 11 |

752 | Fill in the blanks. Linear movement of the piston in a heat engine is converted into circular motion by | 11 |

753 | The solubility of ( N a C l(s) ) in water at ( 298 K ) is about 6 moles per litre. Suppose you add 1 mole of ( N a C l(s) ) to a litre of water. For the reaction: | 11 |

754 | A gas has a volume of ( mathrm{V} mathrm{cm}^{3} ) at ( 10^{circ} mathrm{C} ). If the pressure is doubled, at what temperature will the volume still be ( mathbf{V} ) ( c m^{3} ? ) A ( cdot 273^{circ} mathrm{C} ) B. ( 300^{circ} mathrm{C} ) ( mathbf{c} cdot 283^{circ} mathrm{C} ) D. ( 293^{circ} mathrm{C} ) | 11 |

755 | If ( Delta H_{f}^{circ} ) of ( H_{2} S_{(g)} ) and ( H_{2} S_{(a q)} ) are -4.5 and -9.5 kcal. The amount of heat required for the change is [ boldsymbol{H}_{2} boldsymbol{S}_{(a q)} longrightarrow boldsymbol{H}_{2} boldsymbol{S}_{(g)} ] | 11 |

756 | The thermal capacity of 10 g of a substance is ( 8 mathrm{cal}^{0} C^{-1} ) then its specific heat is 1.25 cal ( g^{-1} o C^{-1} ) State whether given statement is True/False A. True B. False | 11 |

757 | The signs of ( Delta mathrm{H}, Delta mathrm{S} ) and ( Delta mathrm{G} ) for a non spontaneous reaction at all temperatures would be: ( A cdot+,+, ) ( B .+. .,+ ) ( c ldots- ) D. ( +,+,+ ) | 11 |

758 | Whether a reaction is endothermic or exothermic can be indicated by: A. enthalpy change. B. entropy change. c. gibbs free energy change D. activation energy E. specific heat capacity | 11 |

759 | . 3 The state of a gas can be described by quoting the relationship between (a) pressure, volume, temperature (b) temperature, amount, pressure (c) amount, volume, temperature (d) pressure, volume, temperature, amount | 11 |

760 | A man of 60 kg gets 1000 cal of heat by eating 5 mangoes. His efficiency is ( 28 % ) To what height he canjump by using this energy A. 2 m B. 20m ( c .28 m ) D. ( 0.2 mathrm{m} ) | 11 |

761 | A piston cylinder device initially contains ( 0.2 m^{3} ) neon (assume ideal) at ( 200 mathrm{kPa} ) inside at ( T_{1}^{0} C . A ) value is now opened and neon is allowed to escape until the volume reduces to half the initial volume. At the same time heat transfer with outside at ( T_{2}^{0} C ) ensures a constant temperature inside. Select the statement(s) for given process: A. ( Delta U ) must be zero B. ( Delta U ) may not be zero c. ( q ) may be ( + ) ve D. q may not be -ve | 11 |

762 | The thermal capacity of ( 40 g ) of aluminium (specific heat = ( 0.2 mathrm{calg}^{-10} mathrm{C}^{-1} ) ) is : A ( cdot 40 ) cal ( ^{circ} C^{-1} ) B . 160 cal ( ^{circ} C^{-} ) c. 200 cal’ ( C^{-1} ) D. 8 cal ( ^{circ} mathrm{C}^{-1} ) | 11 |

763 | The standard enthalpy of combustion at ( 25^{circ} mathrm{C} ) of hydrogen, cyclohexene ( left(C_{6} H_{10}right) ) and cyclohexane ( left(C_{6} H_{12}right) ) are -241,-3800 and ( -3920 k J / ) mole respectively. Calculate the heat of hydrogenation of cyclohexene A. ( -111 k J / ) mole B . ( -121 k J / ) mole c. ( -118 k J / ) mole D. ( -128 k J / ) mole | 11 |

764 | The standard enthalpies of elements in their standard(natural) states are taken as zero. On basis of this statement, we can say that the enthalpy of formation of a compound : A . Is always negative B. Is always positive c. May be positive or negative D. Is never negative | 11 |

765 | Water falls from a height of ( 50 mathrm{cm} ) Calculate the rise in temperature of water when it strikes the bottom. ( (g= ) ( 10 m s^{-2}, ) sp. heat capacity of water ( = ) ( left.4200 J / k g^{o} Cright) ) | 11 |

766 | If we consider molecules of an ideal gas in a box with a frictionless piston and now the box is heated and piston moves slowly outwards then: A. the force on piston is due to molecular collision with piston B. the molecules collide with piston and return back with same speed c. the molecular collision with piston is inelastic D. both (a) and (b) are correct | 11 |

767 | Heat lost by the gas in the process ( B rightarrow ) ( C ) is begin{tabular}{l} ( 4.5312 .5 . ) \ hline end{tabular} 3. 1875 J ( c ) D. ( 8854 J ) | 11 |

768 | ( boldsymbol{H}-boldsymbol{F} ) form stronger bond than ( boldsymbol{H}_{2} boldsymbol{O}[because boldsymbol{E} boldsymbol{N} boldsymbol{o} boldsymbol{f} boldsymbol{F}>boldsymbol{O} & boldsymbol{H} text { bond } boldsymbol{alpha} ) ( boldsymbol{E} boldsymbol{N}] ) still heat of vapourisation of ( boldsymbol{H} boldsymbol{F} ) is lower than that of pure water. Why? | 11 |

769 | Molar heat capacity of water in equilibrium with the ice at constant pressure is A. zero B. Infinity c. ( 40.45 k^{-1} mathrm{mol}^{-1} ) D. None | 11 |

770 | If ( 1.0 mathrm{k} ) cal of heat is added to ( 1.2 mathrm{L} ) of ( mathrm{O}_{2} ) in a cylinder of constant pressure of 1 atm, the volume increases to 1.5 L. Calculate ( Delta H ) and ( Delta U ) of the process. | 11 |

771 | An ideal monatomic gas expands to twice its volume. If the process is isothermal, the magnitude of work done by the gas is ( W_{i} . ) If the process is adiabatic, the magnitude of work done by the gas is ( W_{a} . ) Which of the following is true? A ( . W_{i}=W_{a}>0 ) в. ( W_{i}>W_{a}=0 ) c. ( W_{i}>W_{a}>0 ) D. ( W_{a}=W_{i}=0 ) | 11 |

772 | For a particular reversible reaction at temperature ( mathbf{T}, boldsymbol{Delta} mathbf{H} ) and ( Delta mathbf{S} ) were found to be both +ve. If ( mathbf{T}_{mathbf{e}} ) is the temperature at equilibrium, the reaction would be spontaneous when: A ( cdot mathrm{T}_{mathrm{e}}>mathrm{T} ) в. ( mathrm{T}>mathrm{T}_{mathrm{e}} ) ( mathrm{c} cdot mathrm{T}_{mathrm{e}} ) is 5 times ( mathrm{T} ) D. ( mathrm{T}=mathrm{T}_{mathrm{e}} ) | 11 |

773 | A refrigerator is A. head engine B. an electric motor C. heat engine working in backward direction D. air cooler | 11 |

774 | If ( Delta E ) is the heat of reaction for ( boldsymbol{C}_{2} boldsymbol{H}_{5} boldsymbol{O} boldsymbol{H}(boldsymbol{l})+boldsymbol{3} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow ) ( 2 C O_{2}(g)+3 H_{2} O(l) ) at constant volume, the ( Delta boldsymbol{H} ) (heat of reaction at constant pressure), at constant temperature is: A. ( Delta H=Delta E+R T ) B. ( Delta H=Delta E-R T ) c. ( Delta H=Delta E-2 R T ) D. ( Delta H=Delta E+2 R T ) | 11 |

775 | A diatomic ideal gas is expanded at constant at pressure. If work done by the system is ( 10 J ) then calculate heat absorbed. A . ( 40 J ) в. ( 20 J ) ( c .35 J ) D. ( 15 J ) | 11 |

776 | The difference between ( Delta H ) and ( Delta E ) (on a molar basis) for the combustion of n-octane (I) at 25C would be : A. ( -13.6 mathrm{kJ} ) The ( -13.6 mathrm{c} ). B . – 1.14 k c. – 11.15 k D. ( +11.15 mathrm{kJ} ) | 11 |

777 | What is latent heat of evaporation? | 11 |

778 | An ice cube of mass ( 0.1 mathrm{Kg} ) at ( 0^{circ} mathrm{C} ) is placed in an isolated container which is ( operatorname{at} 227^{circ} mathrm{C} . ) The specific heat ( s ) of the container varies with temperature ( boldsymbol{T} ) according to the empirical relation ( s= ) ( boldsymbol{A}+boldsymbol{B} boldsymbol{T}, ) where ( boldsymbol{A}=mathbf{1 0 0} boldsymbol{c a l} boldsymbol{k} boldsymbol{g}^{-1} boldsymbol{K}^{-1} ) and ( B=2 times 10^{-2} ) cal ( k g^{-1} ) If the final temperature of the container is ( 27^{circ} mathrm{C} ), the mass of the container is (Latent heat of fusion of water ( =8 x ) ( 10^{4} ) cal ( k g-1, ) Specific heat of water ( = ) ( mathbf{1 0}^{mathbf{3}} ) cal ( boldsymbol{k} boldsymbol{g}^{-1} boldsymbol{K}^{-1} ) A . ( 0.495 mathrm{kg} ) в. ( 0.595 mathrm{kg} ) ( c .0 .695 k g ) D. ( 0.795 mathrm{kg} ) | 11 |

779 | 6. Which of the following always has a negative value? (a) heat of reaction (b) heat of solution (c) heat of combustion (d) heat of formation | 11 |

780 | From the thermochemical reactions, ( boldsymbol{C}_{(text {graphite})}+frac{mathbf{1}}{mathbf{2}} boldsymbol{O}_{2} rightarrow boldsymbol{C O} ; boldsymbol{Delta} boldsymbol{H}= ) ( -110.5 k J ) ( boldsymbol{C O}+frac{mathbf{1}}{mathbf{2}} boldsymbol{O}_{2} rightarrow boldsymbol{C O}_{2} ; boldsymbol{Delta} boldsymbol{H}=-mathbf{2 8 3 . 2 k} boldsymbol{J} ) the heat of reaction of ( C_{(g r a p h i t e)}+ ) ( boldsymbol{O}_{2} rightarrow boldsymbol{C} boldsymbol{O}_{2} ) is: ( mathbf{A} cdot+393.7 k J ) B . ( -393.7 k J ) ( mathbf{c} .-172.7 k J ) ( mathbf{D} .+172.7 k J ) | 11 |

781 | Q21. Comment on the thermodynamic stability of NO(g) and NO (9) given:: 1/2N,(8) + 1/20 (8) NOg); AH = 90 kJ mol-1 NO(g) + 1/20 (8) – NO(g); H = – 74 kJ mol-1 | 11 |

782 | Heat of ( 30 k c a l ) is supplied to a system and ( 4200 J ) of external work is done on the system so that its volume decreases at constant pressure. What is the change in its internal energy. ( = ) ( (J=4200 J / k c a l) ) A ( cdot 1.302 times 10^{5} mathrm{J} ) J. ( 1.302 times 10^{2} ) в. ( 2.302 times 10^{5} mathrm{J} ) c. ( 3.302 times 10^{5} J ) D. ( 4.302 times 10^{5} mathrm{J} ) | 11 |

783 | In the given (V T) diagram, what is the relation between pressures ( P_{1} ) and ( P_{2} ? ) ( (2) mathrm{P}_{2}>mathrm{P}_{1} ) (4) cannot be predicted A ( cdot P_{2}=P_{1} ) в. ( P_{2}>P_{1} ) c. ( P_{2}<P_{1} ) D. cannot be predicted | 11 |

784 | Consider the reaction, ( 4 mathrm{NO}_{2}(mathrm{g})+mathrm{O}_{2}(mathrm{g}) rightarrow ) ( mathbf{2} mathbf{N}_{2} mathbf{O}_{5}(mathbf{g}), mathbf{Delta}_{r} boldsymbol{H}=-mathbf{1 1} mathbf{1} mathbf{k} mathbf{J} ) If ( N_{2} O_{5}(s) ) is formed instead of ( N_{2} O_{5}(g) ) in the above reaction, the ( Delta_{r} H ) value will be (Given, ( Delta H ) of sublimation for ( N_{2} O_{5} ) is ( left.54 k J m o l^{-1}right) ) A. ( -165 k J ) в. ( +54 k J ) ( mathrm{c} ldots+219 k J ) D. ( -219 k J ) | 11 |

785 | The Born Haber cycle below represents the energy changes occurring at ( 298 mathrm{K} ) when ( mathrm{KH} ) is formed from its elements ( mathbf{v}: Delta boldsymbol{H}_{text {atomisation}} mathbf{K}=mathbf{9 0} mathbf{k J} / mathrm{mol} ) ( mathbf{w}: mathbf{Delta} boldsymbol{H}_{text {ionisation}} mathbf{K}=mathbf{4 1 8} mathbf{k} mathbf{J} / mathrm{mol} ) ( mathbf{x}: boldsymbol{Delta} boldsymbol{H}_{text {dissociation}} mathrm{H}=mathbf{4 3 6} mathrm{kJ} / mathrm{mol} ) ( mathbf{y}: boldsymbol{Delta} boldsymbol{H}_{text {electronaffinity}} mathbf{H}=mathbf{7 8} mathbf{k J} / mathrm{mol} ) ( mathbf{z}: boldsymbol{Delta} boldsymbol{H}_{text {lattice}} mathrm{KH}=710 mathrm{kJ} / mathrm{mol} ) In terms of the letters ( v ) to ( z ) the expression for ( boldsymbol{Delta} boldsymbol{H}_{text {electronaffinity}} ) of H is ( boldsymbol{Delta} boldsymbol{H}_{text {electronaffinity}} ) is ( _{–} ) A . ( y ) в. ( y / 2 ) ( c cdot 2 y ) D. ( y / 3 ) | 11 |

786 | Which of the following is an implication of the zeroth law of thermodynamics? A. Energy in the universe can neither be created nor destroyed B. A pure crystal kept at ( -273.15^{circ} mathrm{C} ) has a very low entropy C. If systems A and B are in thermal equilibrium with system C , then systems A, B,C are in thermal equilibrium with each other D. Entropy of the universe is always increasing | 11 |

787 | A closed system shows exchange of mass and not energy with surroundings A. True B. False | 11 |

788 | Vant Hoff’s equation is A ( cdot log frac{K_{2}}{K_{1}}=frac{-Delta H^{0}}{2.303 R}left[frac{T_{2}-T_{1}}{T_{2} T_{1}}right] ) B. ( log frac{K_{2}}{K_{1}}=frac{Delta H^{0}}{2.303 R}left[frac{T_{2}-T_{1}}{T_{2}+T_{1}}right] ) C. ( log frac{K_{2}}{K_{1}}=frac{Delta H^{0}}{2.303 R}left[frac{T_{2}-T_{1}}{T_{2} T_{1}}right] ) D. ( log _{frac{K_{1}}{L}=frac{Delta H^{0}}{2.203 R}}left[frac{T_{3}+T_{1}}{T_{1} 2_{1}}right] ) | 11 |

789 | ( triangle U^{theta} ) of combustion of methane is ( -x ) k mol ( ^{-1} ). The value of ( triangle boldsymbol{H}^{boldsymbol{theta}} ) is: ( mathbf{A} cdot=Delta U^{theta} ) в. ( Delta U^{theta} ) | 11 |

790 | When ( C a C O_{3} ) is heated to a high temperature, it undergoes decomposition into ( C a C O ) and ( C O_{2} ) whereas it is quite stable at room temperature. The most likely explanation of it is: A. The enthalpy of reaction ( (Delta H) ) overweight the term ( T Delta S ) at high temperature B. The term ( T Delta S ) overweight the enthalpy of reaction at high temperature c. At high temperature, both enthalpy of reaction and entropy change become negative D. None of these | 11 |

791 | Which of the following statements is/are true? This question has multiple correct options A. The standard molar enthalpy of formation of ( C O_{2} ) is equal to the standard molar enthalpy of combustion of carbon (graphite). B. Molar heat capacity of water in equilibrium with ice at constant pressure is infinity. C. A reaction is impossible at any temperature if ( Delta H> ) ( 0, Delta S<0 ) D. The heat of neutralization of strong acid and strong base in solution is equal to the ( Delta H ) of the reaction ( H_{2} O+H^{+} rightleftharpoons H_{3} O^{+} ) | 11 |

792 | Specific heat of a substance depends on its. A. Mass B. Volume c. Temperature D. colour | 11 |

793 | Which of the following are correct for the given diagram? This question has multiple correct options A. ( Delta H_{3}=Delta H_{1}+Delta H_{2} ) В. ( Delta H_{1}=0 ) C. ( Delta H_{2}=left(C_{text {calorimeter}}+C_{text {produt} t}right) timesleft(T_{1}-T_{2}right) ) D. ( Delta H_{2}=left(C_{text {clorimeter}}+C_{text {produc} t}right) timesleft(T_{2}-T_{1}right) ) | 11 |

794 | In which pair, 1st compound having more heat of combustion as compared to 2nd compound ( A ) ( = ) в. ( c ) D. | 11 |

795 | Actual flame temperature is always lower than the adiabatic flame temperature, because there is A. no possibility of obtaining complete combustion at high temperature B. always loss of heat from the flame c. both (a) and (b). D. neither (a) nor (b) | 11 |

796 | as 15 The P-V yrapli ol an ideal gas cycle is shown below. The adiabatic process is described by (a) AB and BC (b) AB and CD (c) BC and DA (d) BC and CD AD and BGrenresent adiabatic need | 11 |

797 | The figure shows the variation of internal energy (U) with the pressure (P) of 2.0 mole gas in cyclic process abcda. The temperature of the gas at ( c ) and ( d ) are ( 300 mathrm{K} ) and ( 500 mathrm{K} ). Calculate the heat absorbed by the gas during the process. ( A cdot 400 mathrm{R} ln 2 ) B. 200 R ( ln 2 ) ( c cdot 100 mathrm{R} ln 2 ) D. 300 R In 2 | 11 |

798 | An experiment needs to heat a small sample to temperature ( 900 K, ) but the only available large object has maximum temperature of 600 ( K . ) Could the experimenter heat the sample to ( 900 K ) by using a large lens to concentrate the radiation from the large object onto the sample as shown below? A. Yes, if the front area of the large object is at least 1.5 times the area of the front of the sample B. Yes, if the sample is placed at the focal point of the lens c. It is not possible D. Yes, if the volume of the large object is atleast 1.5 times the volume of the sample | 11 |

799 | If ( Delta Q ) and ( Delta W ) represents the heat supplied to the system and the work done on the system respectively, then the first law of thermodynamics can be written as A. ( Delta Q=Delta U+Delta W ) в. ( Delta Q=Delta U-Delta W ) c. ( Delta Q=Delta W-Delta U ) D. ( Delta Q=-Delta W-Delta U ) | 11 |

800 | Match the following from Table ( A, ) in the case of gases, with those in Table B. Table – A Table – B (a) Work done in isobaric [ n R T log _{e}left(frac{V_{2}}{V_{1}}right) ] process (b) Wok done in isothermal (e) ( Pleft(V_{2}-V_{1}right) ) process ( T ) (c) Work done in adiabatic process ( frac{n R Tleft(T_{1}-T_{2}right)}{gamma-1} ) (g) Zero ( mathbf{A} cdot a rightarrow h, b rightarrow g, c rightarrow e ) В . ( a rightarrow e, b rightarrow d, c rightarrow g ) ( mathbf{c} cdot a rightarrow g, b rightarrow h, c rightarrow e ) D ( . a rightarrow e, b rightarrow d, c rightarrow f ) | 11 |

801 | A reversible engine operates between temperatures ( 900 mathrm{K} & T_{2}left(T_{2}400 mathrm{K}right) ) in series. What is the value of ( T_{2} ) if work outputs of both the engines are equal? ( A cdot 600 K ) B. 625K ( c .650 k ) D. 675K | 11 |

802 | A gas cylinder contains ( 14.2 mathrm{Kg} ) butane gas. it is consumption of energy in a family is ( 10000 mathrm{KJ} ) for cooking purposes how long this cylinder will be sufficient to supply. If the enthalpy of combustion of butane is ( 2658 mathrm{KJ} ) mol | 11 |

803 | Endothermic reactions, having ( Delta S= ) + ( boldsymbol{v} e ) may be spontaneous if: This question has multiple correct options A ( . Delta H>T Delta S ) в. ( Delta H<T Delta S ) c. ( Delta H=T Delta S ) D. ( T ) is very high | 11 |

804 | When 2 moles of ( C_{2} H_{6} ) are completely burnt, ( 3120 k J ) of heat is liberated. Calculate the heat of formation ( Delta boldsymbol{H}_{f}^{o} ) for ( boldsymbol{C}_{2} boldsymbol{H}_{mathbf{6}} ) Given: ( Delta H_{f}^{o} ) for ( C O_{2}(g) ) and ( H_{2} O(l) ) are -395 and ( -286 k J ) respectively. A . ( -88 k J / m o l ) в. ( +88 k J / m o l ) c. ( -58 k J / m o l ) D. None of the above | 11 |

805 | Draw the pressure-temperature and volume-temperature diagrams of an isochoric process of ( n ) moles of an ideal gas from pressure ( P_{0}, ) volume ( V_{0} ) to pressure ( 4 P_{0}, ) indicating the pressures and temperatures of the gas in the initial and the final states. | 11 |

806 | In a reavrsible process, ( Delta S_{s y s}+Delta S_{s u r r} ) is ( A cdot>0 ) B. < ( c cdot geq 0 ) ( D_{1}=0 ) | 11 |

807 | At ( 300 mathrm{K} ) the standard enthalpies of formation of ( C_{6} H_{5} C O O H_{(s)}, C O_{2(g)} ) and ( H_{2} O_{(l)} ) are -408,-393 and -286 kJ ( m o l^{-1} ) respectively. Calculate the heat of combustion of benzoic acid at constant volume. B. +3199.75 kJ D. -3199.75 k | 11 |

808 | 10. An ideal gas expands isothermally from a volume V to V2 and then compressed to original volume V, adiabatically. Initial pressure is P, and final pressure is P3. The total work done is W. Then (a) Pz > P, W> 0 (b) P; <P, WP, W<0 (d) P = P, W=0 EV) DV) | 11 |

809 | The temperature of 5 mol of a gas which was held at constant volume was changed from ( 100^{circ} mathrm{C} ) to ( 120^{circ} mathrm{C} ). The change in internal energy was found to be 80 . ( J ). The total heat capacity of the gas at constant volume will be equal to ( mathbf{A} cdot 8 J / K ) в. ( 0.8 mathrm{J} / mathrm{K} ) c. ( 4 J / K ) D. ( 0.4 J / K ) | 11 |

810 | The standard absolute entropy of a substance, ( left(S^{ominus}right) ) is the entropy of the substance in its standard state at 1 atm, temperature being (in K) | 11 |

811 | Some heat is provided to a body to raise its temperature by ( 25^{circ} mathrm{C} ). What will be the corresponding rise in temperature of the body as shown on the kelvin scale? | 11 |

812 | An ideal diatomic gas ( left(gamma=frac{7}{5}right) ) undergoes a process in which its internal energy relates to the volume as ( U=alpha sqrt{V}, ) where ( alpha ) is a constant. Find the molar specific heat of the gas. | 11 |

813 | Figure below shows pressure (P) versus volume(V) graphs for a certain mass of a gas at two constant temperatures ( T_{1} ) and ( T_{2} . ) Which of the inferences given below is correct? ( A cdot T_{1}=T_{2} ) в. ( T_{1}>T_{2} ) ( c cdot T_{1}<T_{2} ) D. none of the above | 11 |

814 | Which one of the following statement(s) is/are true? This question has multiple correct options ( mathbf{A} cdot Delta E=0 ) for combustion of ( C_{2} H_{6}(g) ) in a sealed rigid adiabatic container ( mathbf{B} cdot Delta_{f} H^{o}(S, text { monolithic}) neq 0 ) C . If dissociation energy of ( C H_{4}(g) ) is ( 1656 k J / ) mol and ( C_{2} H_{6}(g) ) is ( 2812 k J / m o l, ) then value of ( C-C ) bond energy will be ( 328 k J / m o l ) D. If ( Delta H_{f}left(H_{2} O, gright)=-242 k J / m o l ; Delta H_{v a p}left(H_{2} O, lright)= ) ( 44 k J / m o l ) then ( Delta_{f} H^{o}left(O H^{-}, a qright) ) will be ( -142 k J / m o l ) | 11 |

815 | Which of the following is not a state function? A . B. ( c cdot v ) ( D ) | 11 |

816 | For the gaseous reaction involving the complete combustion of isobutane: ( mathbf{A} cdot Delta H=Delta E ) B. ( Delta H>Delta E ) c. ( Delta H=Delta E=0 ) D. ( Delta H<Delta E ) | 11 |

817 | If ( x ) and ( y ) are two intensive variables then: This question has multiple correct options A. ( x y ) is an intensive variable B. ( frac{x}{y} ) is an intensive variable c. ( (x+y) ) is an intensive variable D ( cdot frac{d x}{d y} ) is an extensive property | 11 |

818 | Which of the following relation is incorrect? A ( . Delta S=Delta H+T Delta G ) B . ( Delta S=frac{Delta H-Delta G}{T} ) c. ( -Delta G=-W_{text {non exp}} ) D. ( W_{P V}=-P Delta V ) | 11 |

819 | The laws of thermodynamics speak about A. rates of chemical changes B. feasibility and energy transformations of a process C. Both the rate and energy changes of a process D. Energy changes in chemical reactions only | 11 |

820 | What would be the efficiency of a Carnot engine operating with boiling water as one reservoir and a freezing mixture of ice and water as the other reservoir? A . ( 27 % ) B. 77 % c. ( 20 % ) D. 67 % | 11 |

821 | A system or a group of systems, in which there is no net macroscopic flow of energy or matter either within the system or in between systems is known as? A. Chemical equilibrium B. Thermal equilibrium c. Thermodynamic equilibrium D. Radiative equilibrium | 11 |

822 | The spontaneity of a reaction is indicated by: A. enthalpy change B. entropy change c. gibbs free energy change D. activation energy E. specific heat capacity | 11 |

823 | For a reaction involving condensed phases, ( Delta boldsymbol{H}=boldsymbol{Delta} boldsymbol{U} ) A. true B. false c. insufficient data D. none | 11 |

824 | Work is function. A . path B. state c. both path and state D. none of these | 11 |

825 | Four curves ( A, B, C ) and ( D ) are drawn in figure for a given amount of gas. The curves which represent adiabatic and isothermal changes are. A. ( C ) and ( D ), respectively B. ( D ) and ( C ), respectively c. ( A ) and ( B ), respectively D. ( B ) and ( A ), respectively | 11 |

826 | An ideal gas at a pressure of 1 atmosphere and temperature of ( 27^{circ} mathrm{C} ) is compressed adiabatically until its pressure becomes 8 times the initial pressure, then the final temperature is ( (gamma=3 / 2) ) ( mathbf{A} cdot 627^{0} C ) В. ( 527^{circ} mathrm{C} ) c. ( 427^{circ} mathrm{C} ) D. ( 327^{circ} mathrm{C} ) | 11 |

827 | What is the relation between ( T ) and ( V ) of gas in this process? A ( cdot T cdot V^{2(gamma-1)}= ) constant B. ( T cdot V^{gamma-1}= )constant c. ( T cdot V^{gamma-1 v^{2}}= ) constant D. ( T cdot V^{gamma}= ) constant | 11 |

828 | Explain why (a) Two bodies at different temperatures ( T_{1} ) and ( T_{2} ) if brought in thermal contact do not necessarily settle to the mean temperature ( left(T_{1}+T_{2}right. ) 12 (b) The coolant in a chemical or a nuclear plant (i.e. the liquid used to prevent the different parts of a plant from getting too hot) should have high specific heat (c) Air pressure in a car tyre increases during driving (d) The climate of a harbour town is more temperate than that of a town in a desert at the same latitude | 11 |

829 | ( 1^{s t} ) law of thermodynamics is not adequate in presenting the direction of process. A. True B. False | 11 |

830 | For the same mass, which one of the following has the maximum thermal capacity? A. wood B. copper c. water D. Ice | 11 |

831 | In the given graph an ideal gas change its state from A to state ( C ) by two paths ABC and AC. The internal energy of gas at ( A ) is ( 10 mathrm{J} ) and the amount of heat supplied in path AC is 200 J. The internal energy (in J) of gas at ( mathrm{C} ) is ( 6 k^{2} ) What is the value of ( k ? ) | 11 |

832 | A heat engine is ( 20 % ) efficient. If the engine does ( 500 J ) of work every second, how much heat does the engine exhaust every second? A . ( 2000 J ) в. 2500 J c. ( 400 J ) D. ( 500 J ) | 11 |

833 | The disachharide ( alpha ) – maltose can be hydrolysed to glucose according to the equation (only magnitude in nearest integer in ( mathrm{kj} / mathrm{mol} ) ) ( boldsymbol{C}_{12} boldsymbol{H}_{22} boldsymbol{O}_{11}(boldsymbol{a} boldsymbol{q})+boldsymbol{H}_{2} boldsymbol{O}(l) longrightarrow ) ( mathbf{2} C_{6} boldsymbol{H}_{12} boldsymbol{O}_{6}(boldsymbol{a} boldsymbol{q}) ) Using the following values, calculate the standard enthalpy change in this reaction: ( Delta_{f} H^{o}left(H_{2} O, lright)=-285.85 k J m o l^{-1} ) ( Delta_{f} H^{o}left(C_{6} H_{12} O_{6}, a qright)=-1263.1 k J ) ( m o l^{-1} ) ( Delta_{f} H^{o}left(C_{12} H_{22} O_{11}, a qright)=-2238.3 .1 k J ) ( m o l^{-1} ) | 11 |

834 | Hot water in an ideal thermos flask is an example for (This question may have one or more correct answers) This question has multiple correct options A. Isolated system c. closed system D. Adiabatic system | 11 |

835 | A system is taken along paths ( A ) and ( B ) as shown. If amounts of heat given in these processes are respectively ( Q A ) and ( mathrm{QB}, ) then: A ( cdot mathrm{QA}=mathrm{Q} ) B. QA>QB c. ( Q B<Q A ) D. none of these | 11 |

836 | In which of the following pairs, both properties are intensive? A. Pressure, temperature B. Density, volume c. Temperature, density D. Pressure, volume | 11 |

837 | In the Born-Haber cycle for the formation of solid common salt (Nacl) the largest contribution comes from A. the low ionization potential of ( N a ) B. the high electron affinity of ( C l ) C. the low ( Delta H_{v a p} ) of ( N a(s) ) D. the lattice energy | 11 |

838 | When hydrochloric acid is added to cobalt nitrate solution at room temperature, the following reaction takes place and the reaction mixture becomes blue. On cooling the mixture, it becomes pink. On the basis of this information mark the correct answer. ( left[boldsymbol{C o}left(boldsymbol{H}_{2} boldsymbol{O}right)_{6}right]_{(a q)}^{3+}+boldsymbol{4} boldsymbol{C l}_{(a q)}^{-} rightleftharpoons ) ( left[boldsymbol{C o C l}_{4}right]_{(a q)}^{2-}+boldsymbol{6} boldsymbol{H}_{2} boldsymbol{O}_{(l)} ) A. ( triangle H>0 ) for the reaction B. ( triangle H<0 ) for the reaction c. ( triangle H=0 ) for the reaction D. The sign of ( triangle H ) cannot be predicted on the basis of this information | 11 |

839 | If ( Delta G^{circ}>0 ) for a reaction, then: A ( cdot K_{p}>1 ) в. ( K_{p}<1 ) c. The products predominate in the equilibrium mixture D. None of the above | 11 |

840 | The temperature at the bottom of a high water fall is higher than that at the top because A. by itself heat flows from higher to lower temperature B. the difference in height causes a difference in pressure c. thermal energy is transformed into mechanical energy D. mechanical energy is transformed into thermal energy | 11 |

841 | The statement “lt is impossible to construct a heat engine which can convert heat directly to work completely” was given by A. Clausius B. Carnot c. Plank D. Kelvin & Plank | 11 |

842 | The change in free energy accompanied by the isothermal reversible expansion of 1 mole of an ideal gas when it doubles its volume is ( Delta G_{1} ). The change in free energy accompanied by sudden isothermal irreversible doubling volume of 1 mole of the same gas is ( Delta G_{2} ). Ratio of ( Delta G_{1} ) and ( Delta G_{2} ) is: ( A ) B. ( c cdot-1 ) D. ( frac{-1}{2} ) | 11 |

843 | In thermodynamics process pressure of a fixed mass of gas is changed in such a manner that the gas releases ( 30 J ) of heat and ( 18 J ) of work was done on the gas. If the initial energy of the gas was ( 60 J ) then, the final internal energy will be: в. 48 Л ( c .72 J ) D. 965 | 11 |

844 | Which of the following equations corresponds to the definition of enthalpy of formation at ( 298 K ? ) A ( cdot C(text { graphite })+2 H_{2}(g)+frac{1}{2} O_{2}(g) longrightarrow C H_{3} O H(l) ) B ( cdot 2 C(text { graphite })+4 H_{2}(g)+O_{2}(g) longrightarrow 2 C H_{3} O H(l) ) c. ( C(text { diamond })+2 H_{2}(g)+frac{1}{2} O_{2}(g) longrightarrow C H_{3} O H(l) ) D. ( C(text { graphite })+2 H_{2}(g)+frac{1}{2} O_{2}(l) longrightarrow C H_{3} O H(g) ) | 11 |

845 | Regarding a thermochemical equation a Wrong statement is A. It tells about the physical states of reactants and products B. It tells whether the reaction is exothermic or endothermic C. It tells about the allotropic form (if any) of the reactant D. It tells whether the reaction is possible or not | 11 |

846 | What amount of heat energy (kJ) is released in the combustion of 12.0 g of [ begin{array}{l} C_{3} H_{4} ? \ C_{3} H_{4}(g)+4 O_{2}(g) rightarrow 3 C O_{2}(g)+ end{array} ] ( mathbf{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) quad boldsymbol{Delta} boldsymbol{H}^{circ}=-mathbf{1} mathbf{9} mathbf{3} mathbf{9} . mathbf{1} boldsymbol{k} boldsymbol{J} ) [Atomic weights: ( C=12.01, H=1.008,0= ) 16.00] A. 725 B. 504 c. 783 D. 581 | 11 |

847 | An Ideal gas undergoes an isobaric process. If its heat capacity is ( C_{v} ) at constant volume and number of mole ( n ) then the ratio of work done by gas to heat given to gas when temperature of gas changes by ( Delta boldsymbol{T} ) is: ( ^{A} cdotleft(frac{n R}{c_{v}+R}right) ) в. ( left(frac{R}{c_{v}+R}right) ) ( ^{mathrm{c}} cdotleft(frac{n R}{c_{v}-R}right) ) ( ^{D cdot}left(frac{R}{c_{v}-R}right) ) | 11 |

848 | For a chemical reaction, ( Delta G ) will always be negative if A. ( Delta H ) and ( T Delta S ) both are positive B. ( Delta H ) and ( T Delta S ) both are negative c. ( Delta H ) is negative and ( T Delta S ) is positive D. ( Delta H ) is positive and ( T Delta S ) is negative | 11 |

849 | For the reversible process, the value of ( Delta S ) is given by the expression A. ( Delta H / Delta T ) в. ( T / q(r e v) ) ( mathbf{c} cdot q(r e v) times T ) D. ( q(r e v) / T ) | 11 |

850 | What is the Enthalpy change? A. the amount of energy as heat that is lost or made by a system B. the total amount of energy in a system C . a chemical reaction D. when energy is neither created nor destroyed E. when one or more substances are changed into one or more different substances. | 11 |

851 | Assuming that water vapour is an ideal gas, the internal energy change ( (Delta U) ) when 1 mol of water is vaporised at 1 bar pressure and ( 100^{circ} mathrm{C} ) will be: (Given: Molar enthalpy of vapourisation of water at 1 bar and ( 373 K= ) ( 41 k J . m o l^{-1} ) and ( R=8.3 J m o l^{-1} K^{-1} ) A ( cdot 4.100 k J ) mol ( ^{-1} ) В. 3.7904 k J ( mathrm{mol}^{-1} ) c. ( 37.904 k J ) mol ( ^{-1} ) D. ( 41.00 mathrm{kJ} mathrm{mol}^{-1} ) | 11 |

852 | Find out the temperature at which half of the air escapes out. | 11 |

853 | The conversion of ozone into oxygen is exothermic. Under what conditions is ozone the most stable? ( mathbf{2} boldsymbol{O}_{3}(boldsymbol{g}) rightleftharpoons mathbf{3} boldsymbol{O}_{2}(boldsymbol{g}) ) A. At low pressure and low temperature B. At high pressure and high temperature C. At high pressure and low temperature D. At low pressure and high temperature | 11 |

854 | Which of the following is an example of a closed system? A . a cup of tea B. an air-tight container c. a jug of water D. all of the above | 11 |

855 | The efficiency of a heat engine: A. is independent of the temperature of the source and the sink B. is independent of the working substance c. can be ( 100 % ) D. is not affected by the thermal capacity of the source or the sink | 11 |

856 | Heat of formation of ( boldsymbol{H}_{2} boldsymbol{O}(g) ) at ( boldsymbol{2} boldsymbol{5}^{0} boldsymbol{C} ) is ( -243 mathrm{KJ} . Delta U ) for the reaction ( boldsymbol{H}_{2}(boldsymbol{g})+ ) ( frac{1}{2} O_{2}(g) rightarrow H_{2} O(g) ) at ( 25^{0} C ) is: A. 241.8 KJ B . -241.8 KJ c. -243 к D. 243 KJ | 11 |

857 | CuUULUU LUIS uut to be POSitive. Q8. 19 of graphite is burnt in a bomb calorimeter in excess of oxygen at 298 K and I atmospheric pressure according to the equation C(graphite) + 0.(g) → CO, (g) During the reaction, temperature rises from 298 K to 299 K. If the heat capacity of the bomb calorimeter is 20.7K/K, what is the enthalpy change for the above reaction at 298 K and I am: Ans Sunni 1.11 | 11 |

858 | An ideal monoatomic gas undergoes expansion according to ( boldsymbol{P}=boldsymbol{b} boldsymbol{V}, ) Where b’ is a constant.Molar heat capacity of gas in the process is A ( cdot frac{3 R}{2} ) в. ( 2 R ) c. ( frac{5 R}{2} ) D. 3R | 11 |

859 | Q13. What is an adiabatic process? | 11 |

860 | Cell reaction is spontaneous when : A. G is negative B. G is positive c. E is positive D. E is negative | 11 |

861 | The internal energy of an isolated system A. keeps on changing B. remains constant c. zero D. none of these | 11 |

862 | The work done by a weightless piston in causing an expansion ( Delta V ) (at constant temperature), when the opposing pressure ( boldsymbol{P} ) is variable. What will be the final expression of the work? | 11 |

863 | Bond energies of H – H and Cl – Cl are ( 430 k J m o l^{-1} ) and ( 242 k J m o l^{-1} ) respectively. ( Delta boldsymbol{H}_{f} ) for HCl is ( 91 k J m o l^{-1} . ) What will be the bond energy of H – Cl bond (per mole value)? A . 672 kJ B. 182 kJ c. 245 kJ D. 88 kJ | 11 |

864 | Assertion For a reaction, ( mathbf{2} boldsymbol{N} boldsymbol{H}_{mathbf{3}}(boldsymbol{g}) longrightarrow boldsymbol{N}_{mathbf{2}}(boldsymbol{g})+ ) ( mathbf{3} boldsymbol{H}_{mathbf{2}}(boldsymbol{g}) ) ( triangle boldsymbol{H}>triangle boldsymbol{E} ) Reason Enthalpy change is always greater than internal energy 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. Both Assertion and Reason are incorrect | 11 |

865 | The specific latent heat of fusion of water is : A. 80 cal ( g^{-1} ) В. ( 2260 mathrm{J} g^{-1} ) c. ( 80 J g^{-1} ) D. ( 3366 J g^{-1} ) | 11 |

866 | In which case reaction is spontaneous? ( mathbf{A} cdot Delta H:-v e, Delta S:+v e ) B. ( Delta H:+v e, Delta S:-v e ) c. Both (a) and (b) D. None of these | 11 |

867 | [ begin{array}{c} boldsymbol{M} boldsymbol{X}(mathbf{s o l i d})+boldsymbol{E}_{1} rightarrow boldsymbol{M}^{+}+boldsymbol{X}^{-} ; \ boldsymbol{M}^{+}+boldsymbol{n} boldsymbol{H}_{2} boldsymbol{O} rightarrowleft[boldsymbol{M}left(boldsymbol{H}_{2} boldsymbol{O}right)_{n}right]^{+}+boldsymbol{E}_{2} \ boldsymbol{X}^{-}+boldsymbol{m} boldsymbol{H}_{2} boldsymbol{O} rightarrowleft[boldsymbol{X}left(boldsymbol{H}_{2} boldsymbol{O}right)_{m}right]^{-}+boldsymbol{E}_{3} end{array} ] ( E_{1}, E_{2} ) and ( E_{3} ) are energies, then correct statement is : A. Compound ( (M X) ) soluble in water if ( E_{3}-E_{2}>E_{1} ) B. compound soluble in water ( E_{3}+E_{2}E_{3} ) D. compound soluble in water if ( E_{2}+E_{3}>E_{1} ) | 11 |

868 | The earthen pots prepared by using clay only are generally A. Porous B. Non-porous c. conductors of electricity D. Transparent | 11 |

869 | Q19. What is Gibbs Helmholtz equation? | 11 |

870 | Five moles of Hydrogen initially at STP is compressed adiabatically so that its temperature becomes 673 K. The increase in internal energy of the gas, in ( boldsymbol{k} boldsymbol{J} ) is: ( [R=8.3 J / m o l e-K ; gamma=1.4 ) for diatomic gas A . 80.5 B. 21.55 c. 41.50 D. 65.55 | 11 |

871 | Rate of disappearance of the reactant ( boldsymbol{A} ) at two different temperature is given by ( boldsymbol{A} rightleftharpoons boldsymbol{B} ) ( frac{-boldsymbol{d}[boldsymbol{A}]}{boldsymbol{d t}}=left(boldsymbol{2} times mathbf{1 0}^{-2} boldsymbol{S}^{-1}right)[boldsymbol{A}]-boldsymbol{4} times ) ( mathbf{1 0}^{-3} boldsymbol{S}^{-mathbf{1}}[boldsymbol{B}], boldsymbol{T}=mathbf{3 0 0} boldsymbol{K} ) ( frac{-boldsymbol{d}[boldsymbol{A}]}{boldsymbol{d t}}=left(boldsymbol{4} times mathbf{1 0}^{-2} boldsymbol{S}^{-1}right)[boldsymbol{A}]-mathbf{1 6} times ) ( mathbf{1 0}^{-mathbf{4}}[boldsymbol{B}], boldsymbol{T}=mathbf{4 0 0} boldsymbol{K} ) Calculate heat of reaction in the given temperature range, when equilibrium is ( operatorname{set} ) up. A. ( 16.06 k J ) в. ( 23.04 k J ) c. ( 26.78 k J ) D. ( 29.34 k J ) | 11 |

872 | Explain System and Boundary | 11 |

873 | Q. 24 Enthalpy is an extensive property. In general, if enthalpy of an overall reaction A B along one route is A, H and A, H, A, H2, A, Hz… represent enthalpies of intermediate reactions leading to product B. What will be the relation between A, H overall reaction and 4,H1,4,H… etc for intermediate reactions. | 11 |

874 | The specific heat of ( I_{2} ) in vapour and solid state are 0.031 and 0.055 cal/g respectively. The heat of sublimation of iodine at 200 is 6.096 kcal ( ^{-1} ). The heat of sublimation of iodine at 250 will be: ( begin{array}{lll}text { A } cdot 3.8 & text { kal }-1end{array} ) ( begin{array}{ll}text { B. } 4.8 & text { kal }-1 \ -1end{array} ) ( begin{array}{lll}text { C. } 2.28 & text { kcal } & -1end{array} ) | 11 |

875 | toppr Q Type your question_ ( mathbf{A} ) ( B ) ( c ) D. | 11 |

876 | Which of the following is correct for the efficiency of a heat engine: A ( cdot eta=frac{W}{Q_{1}} ) в. ( eta=frac{W}{Q_{2}-Q_{1}} ) c. ( _{eta}=frac{W}{Q_{2}} ) D. ( eta=frac{Q_{2}}{Q_{1}} ) | 11 |

877 | Which of the reactions defines ( Delta boldsymbol{H}_{boldsymbol{f}}^{o} ) ? A. ( C_{text {diamond}}+O_{2}(g) longrightarrow C O_{2}(g) ) B ( cdot frac{1}{2} H_{2}(g)+frac{1}{2} F_{2}(g) rightarrow H F(g) ) C. ( N_{2}(l)+3 H_{2}(g) longrightarrow 2 N H_{3}(g) ) ( ^{mathrm{D}} cdot operatorname{CO}(g)+frac{1}{2} O_{2}(g) rightarrow C O_{2}(g) ) | 11 |

878 | Which of the following cycloalkanes has lowest heat of combustion per- ( C H_{2} ) group per mole? ( A ) в. ( c ) D. | 11 |

879 | Bond energies can be obtained by using the following relation: ( Delta H(text { reaction })=sum ) Bond energy of bonds, broken in the reactants ( -sum ) Bond energy of bonds, formed in the products Bond energy depends on three factors: a. greater is the bond length, lesser is the bond energy b. bond energy increases with the bond multiplicity c. bond energy increases with the electronegativity difference between the bonding atoms. Arrange ( N-H, O-H ) and ( F-H ) bonds in the decreasing order of bond energy: ( mathbf{A} cdot F-H>O-H>N-H ) B ( . N-H>O-H>F-H ) ( mathbf{c} cdot O-H>N-H>F-H ) D . ( F-H>N-H>O-H ) | 11 |

880 | ( Delta mathrm{SOH} 2(g)=130.6 mathrm{JK}-1 mathrm{mol}-1 Delta mathrm{SH} 2(mathrm{g}) 0=130 ) 6JK-1mol-1 is: A . ( -163.2 mathrm{Jmol}^{-1} mathrm{K}^{-1} ) B. +163.2Jmol-1K-1+163.2Jmol-1K-1 c. ( -303 J ) mol ( ^{-1} K^{-1} ) D. ( +303 J ) mol ( ^{-1} ) K ( ^{-1} ) | 11 |

881 | Q6. From thermodynamic point of view, to which system the animals and plants belong? | 11 |

882 | In which case, a spontaneous reaction is possible at any temperature? A. ( Delta H-v e, Delta S+v e ) в. ( Delta H-v e, Delta S-v e ) c. ( Delta H+v e, Delta S+v e ) D. none of these | 11 |

883 | The important considerations in deciding if a reaction will be spontaneous are : A. stability & state of reactants B. energy gained & heat evolved c. exothermic energy & randomness of the products D. endothermic energy & randomness of the products E. endothermic energy & structure of the products | 11 |

884 | The enthalpy of formation of water from hydrogen and oxygen is ( -286.0 k J ) mol ( ^{-1} ). The enthalpy of decomposition of water into hydrogen and oxygen is ( k J m o l^{-1}: ) A . -286.0 в. -143.0 c. 286.0 D. 143.0 | 11 |

885 | At constant pressure and at ( 290 K, ) the heatnof combustion of glucose (s) was found to be ( -2723.78 k J . ) Calculate the heat of combustion of glucose at constant volume. (Assume water to be in gaseous state) | 11 |

886 | A gas is expanded from volume ( V_{0} ) to ( 2 V_{0} ) under three different processes. Process 1 is isobaric process, process 2 is isothermal and process 3 is adiabasic. Let ( triangle boldsymbol{U}_{1}, triangle boldsymbol{U}_{2} ) and ( triangle boldsymbol{U}_{3} ) be the change in internal energy of the gas in these three processes. Then A. ( triangle U_{1}>triangle U_{2}>triangle U_{3} ) В. ( triangle U_{1}<Delta U_{2}<triangle U_{3} ) c. ( triangle U_{2}<triangle U_{1}<Delta U_{3} ) D. ( triangle U_{2}<Delta U_{3}<triangle U_{1} ) | 11 |

887 | Which of the following laws of thermodynamics leads to the inference that it is difficult to convert whole of heat into work: A. zeroth B. second ( c . ) first D. third | 11 |

888 | State whether true or false: In carnot cycle heat removal takes place at constant pressure? A. True B. False | 11 |

889 | At the vicinity of absolute zero: A. ( C_{p}+C_{v}=0 ) B. ( C_{p}C_{v} ) | 11 |

890 | The relation between the slope of isothermal curve and slope of adiabatic Curve: A. Slope of adiabatic curve ( =gamma ) times slope of isothermal curve B. Slope of isothermal curve ( =gamma ) times slope of adiabatic curve C. Slope of adiabatic curve ( =gamma^{2} ) times slope of isothermal curve D. Slope of isothermal curve ( =gamma^{2} ) times slope of adiabatic curve | 11 |

891 | A reaction attains equilibrium, when the free energy change is A . B. ( c cdot 3 ) ( D ) | 11 |

892 | The temperature of 5 mol of a gas which was held at constant volume was changed from ( 100^{circ} mathrm{C} ) to ( 120^{circ} mathrm{C} ). The change in internal energy was found to be 80 . ( J ). The total heat capacity of the gas at constant volume will be equal to ( mathbf{A} cdot 8 J K^{-1} ) B . ( 0.8 mathrm{JK}^{-1} ) ( mathbf{c} cdot 4 J K^{-1} ) D. ( 0.4 mathrm{JK}^{-1} ) | 11 |

893 | In which case mean free path is not affected? A ( cdot H_{2} ) gas at ( 100^{circ} mathrm{C} ) and 1 atm is transferred into a vessel at ( 50^{circ} mathrm{C} ) and 0.5 atm B. ( O_{2} ) gas at ( 200 K ) and ( 2 a t m ) is transferred into a vessel at ( 400 K ) and 1 atm c. ( O_{2} ) gas is replaced by ( H_{2} ) gas keeping other variables constant D. Medium is made more viscous | 11 |

894 | Assertion In free expansion of a gas inside an adiabatic chamber ( Q, W ) and ( Delta U ) all are zero. Reason In such an expansion ( boldsymbol{P} boldsymbol{alpha} frac{mathbf{1}}{boldsymbol{V}} ) 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 | 11 |

895 | Calculate ( C-C l ) bond enthalpy from following reaction: ( boldsymbol{C H}_{3} boldsymbol{C l}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) longrightarrow ) ( boldsymbol{C H}_{2} boldsymbol{C l}_{2}(boldsymbol{g})+boldsymbol{H} boldsymbol{C l}(boldsymbol{g}) boldsymbol{Delta} boldsymbol{H}^{o}= ) ( -104 k J . ) If ( C-H, C l-C l ) and ( H-C l ) bond enthalpies are 414,243 and ( 431 k J m o l^{-1} ) respectively | 11 |

896 | Heat is absorbed by a body but its temperature does not rise. Which of the following statements explains the phenomena? A. No increase in internal energy takes place B. Only kinetic energy of vibration increases c. Increase in kinetic energy in balanced by decrease in potential energy D. Only potential energy of intermolecular force field increases | 11 |

897 | Give the characteristics of free energy. | 11 |

898 | 10. Which one is the correct unit for entropy? (a) KJ mol (1) JK mol (C) JK-mol-1 (d) KJ mol-1 | 11 |

899 | The Zeroth law of thermodynamics leads to the concept of A. internal energy B. heat content c. pressure D. temperature | 11 |

900 | 1.0 g magnesium atoms in vapour phase absorbs ( 50.0 mathrm{kJ} ) of energy to convert all Mg into Mg ions. The energy absorbed is needed for the following changes: [ boldsymbol{M} boldsymbol{g}(boldsymbol{g}) longrightarrow boldsymbol{M} boldsymbol{g}^{+}(boldsymbol{g})+boldsymbol{e} ; boldsymbol{Delta} boldsymbol{H}= ] ( 740 k J m o l^{-1} ) [ begin{array}{c} boldsymbol{M} boldsymbol{g}^{+}(boldsymbol{g}) longrightarrow boldsymbol{M} boldsymbol{g}^{2+}(boldsymbol{g})+boldsymbol{e} ; boldsymbol{Delta} boldsymbol{H}= \ mathbf{1 4 5 0} boldsymbol{k} boldsymbol{J} boldsymbol{m o l}^{-1} end{array} ] Find out the ( % ) of ( M g^{+} ) and ( M g^{2+} ) in the final mixture A . % ( M g^{+}=68.28 % ), % of ( M g^{2+}=31.72 % ) B . % ( M g^{+}=58.28 % ), % of ( M g^{2+}=41.72 % ) c. % ( M g^{+}=78.28 % ), % ( o f M g^{2+}=21.72 % ) D. None of these | 11 |

901 | Which solid dissolve exothermically in water? A. ( N a C l ) в. ( C a O ) ( mathbf{c} cdot N H_{4} N O_{3} ) D. ( C u S O_{4} ) | 11 |

902 | The amount of heat required to increase the temperature of 1 mol of ( a ) triatomatic gas (non-linear) at constant volume is ( n ) times the amount of heat required for 1 mol of monatomic gas. The value of ( n ) will be A . 1 в. 1.3 c. 2 D. 2.5 | 11 |

903 | The specific heat of a metal is 0.16 cal/g approximate atomic weight would be: A . 40 B. 16 ( c .32 ) D. 64 | 11 |

904 | The standard Gibbs free energy change, ( Delta G^{0} ) is related to equilibrium constant, ( K_{p} ) as: A ( . K_{p}=-R T ln Delta G^{0} ) B. ( quad K_{p}=left[frac{e}{R T}right]^{Delta G^{0}} ) ( c cdot_{K_{p}}=-frac{Delta G}{R T} ) D. ( K_{p}=e^{-Delta G^{0} / R T} ) | 11 |

905 | The symbols ( F . H . S . V_{m} ) and ( E^{o} ) denote Helmholtz free energy, enthalpy, entropy, molar volume and standard electrode potential, respectively. The correct classification of the properties is: A. ( F . H . S ) are intensive; ( V_{m} ) and ( E^{o} ) are extensive B. F.H.S are extensive; ( V_{m} ) and ( E^{circ} ) are intensive c. ( F . H . S ) and ( V_{m} ) are intensive; ( E^{o} ) are extensive D. ( F . H . S ) and ( E^{o} ) are extensive; ( V_{m} ) are intensive | 11 |

906 | Bond dissociation enthalpies of ( boldsymbol{H}_{mathbf{2}(boldsymbol{g})} ) and ( N_{2(g)} ) are ( 436.0 K J ) mol ( ^{-1} ) and 941.8 ( K J ) mol ( ^{-1}, ) respectively and enthalpy of formation of ( boldsymbol{N} boldsymbol{H}_{mathbf{3}(boldsymbol{g})} ) is ( -mathbf{4 6} boldsymbol{K} boldsymbol{J} boldsymbol{m o l}^{-1} ) What is the enthalpy of atomization of ( N H_{3}_{(g)} ) and the average bond enthalpy of ( N-H ) bond respectively ( (text { in } K J ) ( left.m o l^{-1}right) ? ) A. 1170.9,390.3 B. 117,300 c. 300,200 D. 2000, 1975 | 11 |

907 | Diborane is a potential rocket fuel which undergoes combustion according to the reaction ( B_{2} H_{6(g)}+3 O_{2(g)} rightarrow ) ( B_{2} O_{3(s)}+3 H_{2} O(g) ) Form the following dada, calculation the enthalpy change for the combustion of diborane. ( 2 B(s)+(3 / 2) O_{2(g)} rightarrow B_{2} O_{3(s)} ) ( boldsymbol{Delta} boldsymbol{H}=-mathbf{1 2 7 3} boldsymbol{k J} boldsymbol{m o l}^{-1} boldsymbol{H}_{2(g)}+ ) ( (1 / 2) O_{2(g)} rightarrow H_{2} O(1) quad Delta H= ) ( -286 k J m o l^{-1} H_{2} O_{(1)} rightarrow H_{2} O_{(g)} ) ( Delta H=44 k J m o l^{-1} ) ( 2 B(s)+3 H_{2(g)} rightarrow B_{2} H_{6(g)} ) ( Delta boldsymbol{H}=mathbf{3 6 K J m o l}^{-1} ) | 11 |

908 | Internal energy of ( n_{1} ) moles of hydrogen at temperature ( T ) is equal to the internal energy of ( n_{2} ) moles of helium at temperature 2T. Then the ratio ( n_{1} / n_{2} ) is: A B. ( frac{2}{3} ) ( c cdot frac{6}{5} ) D. ( frac{3}{7} ) | 11 |

909 | In the ( ln boldsymbol{K} boldsymbol{v} boldsymbol{s} cdot frac{boldsymbol{1}}{boldsymbol{T}} ) plot of chemical process having ( Delta S^{circ}>0 ) and ( Delta H^{circ}<0 ) the slope is proportional to (where Kis equilibrium constant) A . ( -left|Delta H^{circ}right| ) в . ( left|Delta H^{circ}right| ) ( mathrm{c} cdot-Delta S^{circ} ) D. ( Delta G^{circ} ) | 11 |

910 | Assertion Mass, volume and pressure are extensive properties. Reason Extensive properties depend upon the amount of the substance. 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 | 11 |

911 | Combustion of carbon studies in a bomb calorimeter to obtain heat of reaction. Which of the following options are correct? This question has multiple correct options A. The value obtained shows change in heat enthalpy B. The value obtained shows change in internal energy. c. The volume remains constant D. The pressure remains constant | 11 |

912 | A steam engine delivers ( 5.4 times 10^{8} ) Jof work per minute and services ( 3.6 times 10^{9} ) Jof heat per minute from its boiler What is the efficiency of the engine? How much heat is wasted per minute? | 11 |

913 | ( boldsymbol{Delta} boldsymbol{H}^{0} ) for the raection ( boldsymbol{X}_{(boldsymbol{g})}+boldsymbol{Y}_{(boldsymbol{g})} rightleftharpoons ) ( Z_{(g)} ) is ( -4.6 mathrm{Kcal} ), the value of ( Delta U^{0} ) of the reaction at ( 227^{circ} mathrm{C} ) is ( R= ) ( 2 c a l m o l^{-1} K^{-1} ) A. – -3.6kcal B . – -5.6kcal c. -4.6kcal D. – -2.6kcal | 11 |

914 | ( A B, A_{2} ) and ( B_{2} ) are diatomic molecules If the bond enthalpies of ( A_{2}, A B & B_{2} ) are in the ratio 1: 1: 0.5 and enthalpy of formation of ( A B ) from ( A_{2} ) and ( B_{2} ) is -100 kJ/mol ( ^{-1} ). What is the bond enthalpy of ( boldsymbol{A}_{2} ) A. ( 400 mathrm{kJ} / mathrm{mol} ) B. 300 kJ/mole c. ( 500 mathrm{kJ} / mathrm{mole} ) D. 900 kJ/mole | 11 |

915 | Thermodynamically, in which form of carbon is the most stable? A. coal B. Fullerenes c. Diamond D. Graphite | 11 |

916 | Consider the reaction at ( 300 K ) ( boldsymbol{C}_{6} boldsymbol{H}_{6}(ell)+frac{mathbf{1 5}}{mathbf{2}} boldsymbol{O}_{2}(boldsymbol{g}) longrightarrow mathbf{6} boldsymbol{C O}_{2}(boldsymbol{g})+ ) ( mathbf{3} boldsymbol{H}_{2} boldsymbol{O}(ell) ; boldsymbol{Delta} boldsymbol{H}=-mathbf{3 2 7 1} boldsymbol{k} boldsymbol{J} ) What is ( Delta U ) for the combustion of 1.5 mole of benzene at ( 27^{circ} mathrm{C} ) ? A. ( -3267.25 k J ) ( J ) в. ( -4900.88 k J ) c. ( -4906.5 k J ) D. ( -327.754 k J ) | 11 |

917 | For the process, ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l})(mathbf{1} boldsymbol{b} boldsymbol{a} boldsymbol{r}, boldsymbol{3} boldsymbol{7} boldsymbol{3} boldsymbol{K}) rightarrow ) ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g})(boldsymbol{1} boldsymbol{b} boldsymbol{a} boldsymbol{r} ; boldsymbol{3} boldsymbol{7} boldsymbol{3} boldsymbol{K}) ) The correct set of thermodynamics parameters is: A. ( Delta G=0, Delta S=+v e ) в. ( Delta G=0, Delta S=-v e ) c. ( Delta G=+v e, Delta S=0 ) D. ( Delta G=-v e, Delta S=+v e ) | 11 |

918 | If ( x ) is the temperature ( left(text { in }^{circ} Cright) ) at which liquid ( H_{2} O ) will be in equilibrium with its vapours ( (Delta H quad text { and } quad Delta S ) for vaporization are ( 40.7 k J m o l^{-1} ) and ( left.0.11 k J m o l^{-1} K^{-1} text {respectively }right), ) then ( x ) is: | 11 |

919 | Enthalpy of sublimation of iodine is ( 24 operatorname{cal} g^{-1} ) at ( 200^{circ} mathrm{C} . ) If specific heat of ( I_{2}(s) ) and ( I_{2}(text { vap ) are } 0.055 ) and ( 0.031 mathrm{cal} mathrm{g}^{-1} mathrm{K}^{-1} ) respectively, then enthalpy of sublimation of iodine at ( 250^{circ} mathrm{C} ) in ( operatorname{cal} g^{-1} ) is : A . 2.85 B. 11.4 ( c .5 .7 ) D . 22.8 | 11 |

920 | Carefully observe the given diagrams which indicates standard enthalpy of formation of different states of one mole Mg and 2 mole Cl atom and match the entries in column I and II provided. Energy (k) ( quad ) state of Mg and ( C l_{2} ) Energy (k.) States of Mg and C Columnı | 11 |

921 | The density of an equilibrium mixture of ( N_{2} O_{4} ) and ( N O_{2} ) at ( 101.32 K P_{a} ) is 3.62 ( g d m^{3} ) at ( 288 mathrm{K} ) and ( 1.84 mathrm{g} d m^{3} ) at ( 348 mathrm{K} ) What is the heat of the reaction for the following reaction? ( N_{2} O_{4} rightleftharpoons 2 N O_{2}(g) ) B. ( Delta_{r} H=75.68 ) kJ ( mathrm{mol}^{-1} ) C . ( Delta_{r} H=95.7 ) kJ ( mathrm{mol}^{-1} ) D. ( Delta_{r} H=151.3 ) kJ ( mathrm{mol}^{-1} ) | 11 |

922 | How does the internal energy of the system change? A. Increases B. Decreases c. Remains Same D. cannot be predicted | 11 |

923 | Among the following, the state function(s) is(are): This question has multiple correct options | 11 |

924 | ( A B, A_{2}, ) and ( B_{2} ) are diatomic molecules. If the bond enthalpies of ( A_{2}, A B, ) and ( B_{2} ) are in the ratio 2: 2: 1 and ethalpy of formation ( A B ) from ( A_{2} ) and ( B_{2} ) is ( -100 k J ) mol ( ^{-1} . ) What is the bond energy of ( boldsymbol{A}_{2} ? ) В. ( 100 k J ) mol( ^{-1} ) c. ( 300 k J ) mol( ^{-1} ) D. ( 400 mathrm{kJ} mathrm{mol}^{-1} ) | 11 |

925 | Five moles of Hydrogen initially at STP compressed acrobatically so that its temperature becomes ( 73 mathrm{K} ). The increase in internal of the gas in Kilo joules is: ( (boldsymbol{R}-mathbf{8 . 3} boldsymbol{j} / boldsymbol{m o l} boldsymbol{e}-boldsymbol{K}: boldsymbol{gamma}=mathbf{1 . 4} ) for A . 80.5 B. 21.55 c. 41.50 D. 65.55 | 11 |

926 | Match the List-II ans List-II and List III: ( begin{array}{lll}text { List-I } & text { List-II } & text { List-III } \ text { A. } Delta G>0 & begin{array}{l}text { X. } Delta S> \ 0end{array} & begin{array}{l}text { 1. Non- } \ text { spontaneous }end{array} \ begin{array}{l}text { B. } Delta G< \ 0end{array} & text { Y. } Delta S<0 & text { 2. Spontaneous } \ begin{array}{l}text { C. } Delta G= \ 0end{array} & text { Z. } Delta S=0 & text { 3. Equilibrium }end{array} ) select the correct answering from the following codes: ( A cdot A-(Y, 1) B-(X, Y) C-(Z, 3) ) B. ( A-(X, 2) B-(Y, 3) C-(Z, 1) ) C. ( A-(X, 3) B-(Y, 1) C-(Z, 2) ) D. ( A-(Y, 1) B-(X, 3) C-(Z, 2) ) | 11 |

927 | Two bars of same length and same cross -sectional area but of different thermal conductivities ( K_{1} ) and ( K_{2} ) are joined end to end as shown in the figure One end of the compound bar is at temperature ( T_{1} ) and the opposite end at temperature ( T_{2}left(w h e r e T_{1}>T_{2}right) ) The temperature of the junction is ( mathbf{A} ) [ frac{K_{1} T_{1}+K_{2} T_{2}}{K_{1}+K_{2}} ] B. [ frac{K_{1} T_{2}+K_{2} T_{1}}{K_{1}+K_{2}} ] c. ( frac{K_{1}left(T_{1}+T_{2}right)}{K_{2}} ) D. [ frac{K_{2}left(T_{1}+T_{2}right)}{K_{1}} ] | 11 |

928 | Draw V-T curve | 11 |

929 | ( 34.05 mathrm{mL} ) of phosphorus vapour weighs ( 0.0625 mathrm{g} ) at ( 546^{circ} mathrm{C} ) and 1.0 bar pressure. What is the molar mass of phosphorus? | 11 |

930 | Two identical calorimeter ( boldsymbol{A} ) and ( boldsymbol{B} ) contain equal quantity of water at ( 20^{circ} C ) A ( 5 g m ) piece of metal ( X ) of specific heat 0.2 cal ( g^{-1}left(C^{circ}right)^{-1} ) is dropped into ( A ) and a ( 5 g m ) piece of metal ( Y ) into ( B ) The equilibrium temperature in ( A ) is ( 22^{circ} mathrm{C} ) and in ( B 23^{circ} mathrm{C} . ) The initial temperature of both the metals is ( 40^{circ} mathrm{C} ) Find the specific heat of metal ( Y ) in cal ( boldsymbol{g}^{-1}left(boldsymbol{C}^{circ}right)^{-1} ) | 11 |

931 | Which of the following processes produces a decrease of the entropy of the system? A. Dissolving sodium chloride in water B. Sublimation of naphthalene c. Dissolving oxygen in water D. All of these | 11 |

932 | Equal masses of hydrogen gas and oxygen gas are placed in a closed container at a pressure of ( 3.4 a t m . ) The contribution of hydrogen gas to the total pressure is: A . ( 1.7 a t m ) B. ( 0.2 a t m ) c. ( 3.2 a t m ) D. 3.02atm | 11 |

933 | The integral enthalpy of solution in ( mathrm{kJ} ) of one mole of ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) dissolved in ( boldsymbol{n} ) mole of water is given by: ( Delta boldsymbol{H}_{s}=frac{mathbf{7 5 . 6} times boldsymbol{n}}{boldsymbol{n}+mathbf{1 . 8}} ) Calculate ( Delta H ) for ( H_{2} S O_{4} ) dissolved in 2 mole of ( boldsymbol{H}_{2} boldsymbol{O} ) ( A cdot-48.54 mathrm{kJ} ) B. 39.79 kJ c. 48.54 k] D. ( 75.60 mathrm{kJ} ) | 11 |

934 | Temperature of 2 moles of a monoatomic gas is increased from T to 2T. Match the following two columns. | 11 |

935 | Heat of reaction for; ( boldsymbol{C O}(boldsymbol{g})+ ) ( frac{1}{2} O_{2}(g) rightarrow C O_{2}(g) ) at constant ( V ) is -67.71 cal ( 17^{circ} C . ) The heat of reaction at constant ( P ) at ( 17^{circ} C ) A. ( -68.0 K ) cal в. +68.0 Кса c. -67.42 К ( c a l ) D. None of these | 11 |

936 | 0.59 Extensive properties depend on the quantity of matter but intensive properties do not. Explain whether the following properties are extensive or intensive. Mass, internal energy, pressure, heat capacity, molar heat capacity, density, mole fraction, specific heat, temperature and molarity. | 11 |

937 | The quantity of heat needed to raise the temperature of ‘M’ g of water from ( t_{1}^{o} C ) ( operatorname{to} t_{2}^{o} C ) is ( M Cleft(t_{2}-t_{1}right) ) A. True B. False | 11 |

938 | As shown in the figure three ( p-v ) diagrams .In which case the work done is minimum. ( A ) B. I c. III D. cannot say | 11 |

939 | Q Type your question to X). Assume that ( Y ) and ( Z ) are on the same horizontal line, and ( z ) and ( X ) are on the same vertical line. The area inside the shape ( boldsymbol{X}-boldsymbol{Y}-boldsymbol{Z}-boldsymbol{X} ) is ( mathbf{1 0 0 0} boldsymbol{J} ) If the heat absorbed by the gas during process ( X-Y ) is ( 2000 J ) and the heat released by the gas during process ( Y ) ( Z ) is ( 3000 J ), how much heat is lost or gained during process ( Z-X ? ) A ( .2000 J ) is gained B. ( 2000 mathrm{J} ) is lost c. ( 1000 J ) is gained D. ( 1000 mathrm{J} ) is lost E. ( 5000 mathrm{J} ) is gainec | 11 |

940 | When an ideal gas expands isothermally, its internal energy will A. increases B. decreases c. remains constant D. becomes zero | 11 |

941 | What is the heat of formation of ( C_{6} H_{6} ) give that the heat of combustion of Benzene, carbon and Hydrogen are -782,-94 and ( -68 K ) respectvely A. +14 K.Cal в. -14 К.Са c. +28 K.Cal D . -28 K.Cal | 11 |

942 | ( boldsymbol{H}_{2(g)}+frac{1}{2} boldsymbol{O}_{2(g)} rightarrow boldsymbol{H}_{2} boldsymbol{O}_{(l)} ; boldsymbol{Delta} boldsymbol{H}= ) ( -286.2 k J ; H_{2} O_{(l)} rightarrow H_{(a q)}^{+}+O H_{(a q)}^{-} ) ( Delta H=+57.3 k J . ) Enthalpy of ionisation of ( O H^{-} ) in aqueous solution is: B . ( +228.5 k J ) c. ( -343.5 k J ) D. zero | 11 |

943 | A parallel plate condenser with a dielectric constant ( K ) between the plates has a capacity ( C ) and is charged to a potential ( V ) volt. The dielectric slab is slowly removed from, between the plates and then reinserted. The net work done by the system in this process is A. zero в. ( frac{1}{2}(K-1) C V^{2} ) c. ( frac{C V^{2}(K-1)}{K} ) D ( cdot(K-1) C V^{2} ) | 11 |

944 | Discuss the relation between free energy and EMF. | 11 |

945 | Energy flow and energy transformations of a living system follow: A. Law of limiting factors B. Law of thermodynamics c. Leibig’s law of minimum D. Biogenetic law | 11 |

946 | Which selection applies to the process shown below? ( boldsymbol{C H}_{3} boldsymbol{O H}(l) rightarrow boldsymbol{C H}_{3} boldsymbol{O H}(boldsymbol{g}) ) A. ( Delta H_{f u s} ) в. ( Delta H_{c} ) c. ( Delta H_{s o l n} ) D. ( Delta H_{v a p} ) | 11 |

947 | Which of the following is not a thermodynamic property of a system? ( mathbf{A} cdot H ) в. ( P ) ( c . E ) D. ( W ) | 11 |

948 | The lattice energy of ( N a C l(s) ) is ( -790 k J . m o l^{-1} ) and enthalpy of hydration is ( -785 k J . m o l^{-1} . ) Calculate the enthalpy of the solution of ( N a C l(s) ) | 11 |

949 | Q18. For the reaction; 2Cl(g) – Ce); what will be the signs of AH and AS? | 11 |

950 | Express 60.1 cal of energy in units of joules. A. 251 J в. 251.5 J c. 14.4 J D. 14.36 J E. 251.4 | 11 |

951 | In which process volume increases? ( A cdot A B, C D ) B. АВ, ВС c. ( operatorname{co}, ) DA D. BC, CD | 11 |

952 | The heat of combustion of ethanal determined in a bomb calorimeter is ( -670.48 K ) Cals mole( ^{-1} ) at ( 25^{circ} ) C.What is ( Delta H ) at ( 25^{circ} C ) for the reaction: A . ( -335.24 K ) Cals В. -671.08 КСа( l s ) c. ( -670.48 K ) Cals. D. +670.48 KCals. | 11 |

953 | The specific heat of copper is ( 0.385 mathrm{J} / mathrm{g} ) ( ^{o} C ) ). If 34.2 g of copper, initially at ( 25^{circ} mathrm{C} ) absorbs ( 4.689 mathrm{kJ} ), what will be the final temperature of the copper? A . ( 25.4^{circ} mathrm{C} ) B . ( 27.8^{circ} mathrm{C} ) ( mathbf{c} cdot 356^{circ} mathrm{C} ) D. ( 381^{circ} mathrm{C} ) | 11 |

954 | The temperature at which two bodies appear equally hot or cold when touched by a person is: A ( cdot 0^{0} C ) B . ( 37^{0} C ) ( mathbf{c} cdot 25^{0} C ) D. ( 4^{0} C ) | 11 |

955 | Assertion In a gas any rapid change must be adiabatic whereas a slow change may be adiabatic. Reason In a P-V diagram, the magnitude of the slope is greater for an adiabatic process than for an isothermal process. A. Both statements 1 and 2 are true and statement 2 is the correct explanation of statement 1 B. Both statements 1 and 2 are true but statement 2 is not the correct explanation of statement 1 c. statement 1 is true but statement 2 is false D. Statement 1 is false but statement 2 is true | 11 |

956 | A vessel of volume of ( 0.2 m^{3} ) contains hydrogen gas at temperature ( 300 K ) and pressure 1 bar. Find the heat required to raise the temperature to ( 400 K . ) The molar heat capacity of hydrogen at constant volume is 5 cal ( / ) mol ( K ) ( mathbf{A} cdot 4 k c a l ) B. 5 kcall c. ( 6 k c a l ) D. ( 2 k c a l ) | 11 |

957 | The standard heat of formation of sodium ions in aqueous solution from the following data: Heat of formation of ( N a O H(a q .) ) at ( 25^{circ} C=-470.7 k J ) Heat of formation of ( boldsymbol{O} boldsymbol{H}^{-}(boldsymbol{a} boldsymbol{q} .) ) at ( mathbf{2 5}^{circ} boldsymbol{C}=-mathbf{2 2 8 . 8 k J} mathbf{i s} ) ( mathbf{A} cdot-251.9 k J ) в. 241.9k. ( mathbf{c} .-241.9 k J ) D. ( 251.9 k J ) | 11 |

958 | Boiling does not occur in a closed vessel. Give reason. | 11 |

959 | Q2. Predict in which of the following, entropy increases/decreases. (1) A liquid crystallizes into a solid (11) Temperature of a crystallize solid is raised from OK to 115 K (iii) 2NaHCO3(s) – Na, CO2 (s) + CO, () + H2O (8) (iv) H.(8) 2H(g) dored state an | 11 |

960 | LS LLLCCLLLS UIVAUGULINI Q4. (a) What is bond energy? Why is it called enthalpy of atomisation : (6) Calculate the bond energy of C-H bond, given that the heat of formation of CH4, heat of sublimation of carbon and heat of dissociation of H, are – 74.8, + 719.6, 435.4 kJ mol-1 respectively. no mole of bonde | 11 |

961 | Consider a new system of units in which ( c( ) speed of light in vacuum), h(Planck’s constant) and G (gravitational constant) are taken as fundamental units. Which of the following would correctly represent mass in this new system? ( ^{mathrm{A}} cdot sqrt{frac{h c}{G}} ) B. ( sqrt{frac{G c}{h}} ) c. ( sqrt{frac{h G}{c}} ) D. ( sqrt{h G c} ) | 11 |

962 | Two moles of an ideal monoatomic gas, initially at pressure ( P_{1} ) and volume ( V_{1} ) undergo an adiabatic compression until its volume is ( V_{2} . ) Then the gas is given heat ( Q ) at constant volume ( V_{2} ) Find the total work done by the gas, the total change in its internal energy and the final temperature of the gas.[Give your answers in terms of ( boldsymbol{P}_{1}, boldsymbol{V}_{1}, boldsymbol{V}_{2} mathrm{Q} ) and ( mathrm{R}] ) A. ( frac{P_{1} V_{1}^{5 / 3} V_{2}^{-2 / 3}}{2 R}+frac{Q}{3 R} ) в. (ii) ( frac{P_{1} V_{1}^{5 / 3} V_{2}^{-2 / 3}}{2 R}+frac{Q}{4 R} ) ( ^{mathrm{C}} cdot frac{P_{1} V_{1}^{5 / 3} V_{2}^{-2 / 3}}{2 R}+frac{Q}{5 R} ) D. ( frac{P_{1} V_{1}^{5 / 3} v_{2}^{-2 / 3}}{5 R}+frac{Q}{3 R} ) | 11 |

963 | Monatomic 70. If 50 cal of heat is supplied to the system containing 2 mol of an ideal monatomic gas, the rise in temperature is (R = 2 cal/mol-K) (a) 50K (b) 5 K (c) 10K (d) 20 K gas | 11 |

964 | ( 2.8 times 10^{-2} mathrm{kg} ) of nitrogen is expanded isothermally and reversibly at ( 300 K ) from ( 15.15 times 10^{5} N m^{-2} ) when the work done is found to be ( -17.33 mathrm{kJ} ). Find the final pressure. | 11 |

965 | Which of the following is the set of products formed when propanol ( C_{2} H_{2} O H, ) undergoes a combustion reaction? A ( cdot C O_{2(g)} ) and ( H_{2} O_{(l)} ) B. ( C O_{2(g)} ) and ( H_{2} O_{(g)} ) ( mathbf{c} cdot C_{(a)}, O_{2(g)} ) and ( H_{2} O_{(g)} ) D. ( C_{(a)}, H_{2(g)} ) and ( H_{2} O_{(g)} ) E ( cdot C O_{2(g)}, H_{2} O_{(g)} ) and ( O_{2(g)} ) | 11 |

966 | ( P-V ) diagram of an ideal gas for a process ( A B C ) is as shown in the figure. If the total heat absorbed or released by the gas during the process ( A B C ) is ( operatorname{given} operatorname{by} boldsymbol{H}=-boldsymbol{x} boldsymbol{P}_{0} boldsymbol{V}_{0}, ) what is the value of ( x ) ? | 11 |

967 | Find the net amount of heat absorbed by the system for the cyclic process. | 11 |

968 | Dissolution of ammonium chloride in water is an endothermic reaction, yet it is a spontaneous process. This is due to the fact that: A. ( Delta H ) is ( +v e, Delta s ) is -ve B. ( Delta H ) is -ve, ( Delta ) s is tve c. ( Delta ) H is ( + ) ve, ( Delta ) s is ( + ) ve and ( Delta ) H ( ) T ( Delta ) ss | 11 |

969 | The most efficient engine is? A . Petrol B. Electric c. Steam D. Diesel | 11 |

970 | Determine enthalpy change for, [ boldsymbol{C}_{3} boldsymbol{H}_{8}(boldsymbol{g})+boldsymbol{H}_{2}(boldsymbol{g}) longrightarrow boldsymbol{C}_{2} boldsymbol{H}_{6}(boldsymbol{g})+ ] ( boldsymbol{C H}_{4}(boldsymbol{g}) ) at ( 25^{circ} boldsymbol{C} ). using heat of combustion values under standard conditions. [ begin{array}{llll} text { Compounds } & boldsymbol{H}_{2}(boldsymbol{g}) & boldsymbol{C H}_{4}(boldsymbol{g}) & boldsymbol{C}_{2} boldsymbol{H}_{mathbf{6}} \ boldsymbol{Delta H}^{mathrm{o}} text { in } & -285.8 & -890.0 & -1560.0 end{array} ] kJ/mol The standard heat of formation of [ C_{3} H_{8}(g) text { is }-103.8 k J m o l^{-1} ] A. ( -55.7 k J ) B . ( -75.5 k J ) c. -55.7 D. None of these | 11 |

971 | A body cools from ( 60^{circ} mathrm{C} ) to ( 50^{circ} mathrm{C} ) in 2 min when it is placed in a room maintained at ( 30^{circ} mathrm{C} ). The time taken by the same body in the same room to cool further from ( 50^{circ} mathrm{C} ) to ( 40^{circ} mathrm{C} ) will be A. Less than 2 min B. Approximately 2 min c. Greater than 2 min D. 2 min | 11 |

972 | An electric heater supplies heat to a system at a rate of 120 W. If system performs work at a rate of ( 80 mathrm{J} s^{-1} ), the rate of increase in internal energy is : A. 30 J ( s^{-1} ) B. 40 J ( s^{-1} ) c. 50 jmath ( s^{-1} ) D. 60 J ( s^{-1} ) | 11 |

973 | As the temperature of liquid is increased, mass & volume will A. both change B. mass change & volume is fixed c. Mass remains same ( & ) volume increases D. both remain same | 11 |

974 | For a process, entropy change of a system is expressed as: A. ( H-T S ) B. ( frac{q_{r e v}}{T} ) c. ( frac{T}{q_{r e v}} ) D. ( q_{r e v} times T ) | 11 |

975 | 24. The value of C. – C = 1.00 R for a gas in state A and p y =1.06 R in another state. If P. and P, denote the pressure and TA and T, denote the temperatures in the two states, then (a) PA = PB, TA > TB A PB TA > TB (b) PA > PB, TA = TB (c) PA TR (d) PA = Pb, TA < TB 25 I mola af dine: 11. fonotomicas | 11 |

976 | An open system can exchange: A. matter with surroundings B. energy with surroundings C. both ( A ) and ( B ) D. none of the above | 11 |

977 | The standard enthalpy of combustion of sucrose is-5645 kJ mol ( ^{-1} ).What is the advantage (in kJ ( m o l^{-1} ) of energy released as heat) of complete aerobic oxidation compared to anaerobic hydrolysis of sucrose to lactic acid? ( triangle H_{int}^{circ} ) for lactic acid,CO_ {2} and ( H_{2} O ) is -694,-395 and -286.0 respectively A . advantage=4356 k..mol ( ^{-1} ) B. advantage=5396 k..mol- c. advantage=4756 kJ.mol- D. advantage=5657 kJ.mol- | 11 |

978 | When a liquid in a heat insulated closed vessel is stirred using a peddle then the temperature of the liquid: A. Increases B. Decreases c. Remains constant D. Becomes ( 0^{circ} mathrm{C} ) | 11 |

979 | A good fuel has high calorific values. A. True B. False | 11 |

980 | ( boldsymbol{C}+boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{C} boldsymbol{O}_{2}(mathrm{i}) ; quad boldsymbol{Delta} boldsymbol{H}=-boldsymbol{3} boldsymbol{9} boldsymbol{3} mathbf{k} ) ( m o l^{-1} ) ( boldsymbol{H}_{2}+mathbf{1} / mathbf{2} boldsymbol{O}_{2} rightarrow boldsymbol{H}_{2} boldsymbol{O},(mathbf{i} mathbf{i}) ; quad boldsymbol{Delta} boldsymbol{H}= ) ( -287.3 mathrm{kJ} ) mole( ^{-1} ) ( 2 C O_{2}+3 H_{2} O rightarrow C_{2} H_{5} O H+3 O_{2} ) (iii); ( Delta boldsymbol{H}=mathbf{1 3 6 6 . 8} ) kJ ( boldsymbol{m o l}^{-1} ) Find the standard enthalpy of formation of ( C_{2} H_{5} O H(l) ) A ( cdot 281.1 ) kJ ( m o l^{-1} ) в. ( -281.1 mathrm{kJ} ) тог ( mathrm{c} cdot_{562.2 mathrm{kJ}} mathrm{mol}^{-1} ) D. ( -562.2 mathrm{k} ) s ( mathrm{mol}^{-1} ) | 11 |

981 | What amount of heat (in ( mathrm{kJ} ) ) is released in forming ( 31.2 g ) of ( A s H_{3} ) by the following reaction? (Given : At. wt. As = 75, H = 1) Given ( : 2 A s(s)+3 H 2(g) rightarrow 2 A s H 3(g) ) ( Delta H=-780 k J ) A. 312 B. 390 ( c cdot ) १५ D. 780 | 11 |

982 | Answer the following by appropriately matching the lists based on the information given in the paragraph. If the process on one mole of monatomic ideal gas is as shown in the TV-diagram with ( P_{0} V_{0}=frac{1}{3} R T_{0} ), the correct match is, A. ( I rightarrow P, I I rightarrow R, I I I rightarrow T, I V rightarrow S ) в. ( I rightarrow P, I I rightarrow T, I I I rightarrow Q, I V rightarrow T ) c ( . I rightarrow S, I I rightarrow T, I I I rightarrow Q, I V rightarrow U ) D. ( I rightarrow P, I I rightarrow R, I I I rightarrow T, I V rightarrow P ) | 11 |

983 | ( 540 g ) ice at ( 0^{circ} mathrm{C} ) is mixed with ( 540 g ) of water at ( 80^{circ} mathrm{C} ). The final temperature of mixture is ( mathbf{A} cdot 0^{circ} C ) B . ( 40^{circ} mathrm{C} ) ( mathbf{c} cdot 80^{circ} mathrm{C} ) D. less than ( 0^{circ} mathrm{C} ) | 11 |

984 | Under which of the following conditions is the relation, ( triangle boldsymbol{H}=triangle boldsymbol{U}+boldsymbol{P} triangle boldsymbol{V} ) valid for a closed system? A. constant pressure B. Constant temperature c. constant temperature and pressure D. constant temperature, pressure and composition | 11 |

985 | ( 50 L t r ) of a certain liquid is confined in a piston system at the external pressure 100atm. This pressure is suddenly released and liquid is expanded against the constant atmospheric pressure, volume of the liquid increases by 1 Lt ( r ) and the final pressure of the liquid is 100 atm. Find the work done. A. 1 L. ( a+m ) B. 5 Latm c. 500 Latm D. 50 L.atm | 11 |

986 | Bond energies can be obtained by using the following relation: ( Delta H(text {reaction})=sum ) Bond energy of bonds, broken in the reactants ( -Sigma ) Bond energy of bonds, formed in the products. Bond energy depends on three factors: | 11 |

987 | Ethylene on combustion gives carbon dioxide and water. Its heat of combustion is ( 1410.0 mathrm{kJ} ). ( mathrm{mol}^{-1} ). If the heat of formation of ( C O_{2} ) and ( H_{2} O ) are ( 393.3 k J ) and ( 286.2 k J, ) respectively Calculate the heat of formation of ethylene. ( mathbf{A} cdot Delta_{f} H=51.0 k J m o l^{-1} ) B . ( Delta_{f} H=102.0 k J m o l^{-1} ) C ( . Delta_{f} H=25.0 k J m o l^{-1} ) D. None of these | 11 |

988 | Q. 35 Which quantity out of A, G and A,GⓇ will be zero at equilibrium? | 11 |

989 | Evaporation of the solution of copper sulfate solution helps in: A. making the solution concentrated B. crystallization of copper sulfate c. both A and B D. none of these | 11 |

990 | What is the amount of heat given off by ( 100 g ) of ( O_{2} ) when it is used to burn an excess of sulfur according to the following reaction? ( S(s)+O_{2} rightarrow S O_{2}(g) Delta H= ) ( -296 k J / ) mole A. ( 925,000 mathrm{J} ) B. 29,000 J c. 1,850 J D . 296 J E. 100 | 11 |

991 | Which of the following is true in the case of a reversible process: A. There will be energy loss due to friction B. System and surroundings will not be in thermodynamic equilibrium c. Both system and surroundings retain their initial states D. Both A and C | 11 |

992 | Assertion In the refrigerator, the evaporator is located in the freezer section. Reason In the heat pump, the evaporator is located outside the room which is to be heated. 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 | 11 |

993 | For the reaction ( boldsymbol{S O C l}_{2}+boldsymbol{H}_{2} boldsymbol{O} longrightarrow boldsymbol{S O}_{2}+2 boldsymbol{H C l} ) the enthalpy of reaction is ( 49.4 k J ) and the entropy of reaction is ( 336 J K^{-1} ) Calculate ( Delta G ) at ( 300 K ) and predict the nature of the reaction. | 11 |

994 | If the specific heat capacity of iron is 0.108 cal/g’C. Then how much heat is sufficient to raise the temperature of 1 g of iron through ( 1^{prime} mathrm{C} ? ) A. 0.108 calories B. 108 calories c. 0.0108 calories D. 10.8 calories | 11 |

995 | Enthalpy change during a reaction does not depend upon A. conditions of a reaction B. initial and final concentration C . physical states of reactants and products D. number of steps in the reaction | 11 |

996 | Heat of combustion of glucose at constant pressure at ( 17^{circ} mathrm{C} ) was found to be ( -651,000 c a l . ) Calculate the heat of combustion of glucose at constant volume considering water to be in the gaseous state. | 11 |

997 | If for a reaction ( k_{c}=1 ) then ( Delta G^{circ} ) ( = ) A . 1.987 B. 4.184 ( c cdot 0 ) D. | 11 |

998 | Given the reaction: ( N_{2}(g)+3 H_{2}(g) rightleftharpoons ) ( 2 N H_{3}(g)+22 k c a l ) When 6 moles of ( N H_{3} ) are consumed to produce nitrogen gas and hydrogen gas, determine the value of ( Delta H ) for the reverse reaction? ( mathbf{A} cdot+22 k c a l ) B . +66 kcal c. -22 kcal D. – 66 kcal E . +33 kcal | 11 |

999 | Calculate the temperature of a hydrogen-oxygen flame assuming that the gases at ( 25^{circ} mathrm{C} ) are mixed in stoichiometric proportion and react completely to give ( H_{2} O(g) . Delta H_{298}^{circ} ) of combustion of ( boldsymbol{H}_{2} ) is ( -mathbf{5 8} ) kcal ( boldsymbol{m o l}^{-1} ) The reaction is at constant pressure and the ( C_{p} ) values are ( (7 / 2) R ) for each gas. ( (boldsymbol{R}=mathbf{2} boldsymbol{c} boldsymbol{a} boldsymbol{l}) ) A. ( 8583.71 K ) B . ( 9583.71 K ) c. ( 4283.71 mathrm{K} ) D. None of the above | 11 |

1000 | ( 6.24 g ) of ethanol are vaporized by supplying ( 5.89 k j ) of heat energy. What is enthalpy of vaporisation of ethanol? | 11 |

1001 | 5 mol of liquid water is compressed from 1 bar to 10 bar at constant temperature. Change in Gibb’s energy ( (Delta G) ) in Joule is: (Density of water ( = ) ( left.1000 k g / m^{3}right) ) A . 18 B. 225 ( c cdot 450 ) D. 900 | 11 |

1002 | Which portion of the heating curve for water shown would there be ONLY liquid water present? ( mathbf{A} cdot A-B ) ( mathbf{B}, quad B-C ) ( mathbf{c} cdot C-D ) ( mathbf{D}, quad D-E ) | 11 |

1003 | In a heat engine, heat energy is converted into mechanical energy. A. True B. False | 11 |

1004 | In which of the following pair of reactions first reaction is spontaneous while second reaction is non spontaneous? ( mathbf{A} cdot(mathbf{i})-S H+H_{2} O rightarrow H_{2} S+O H^{-} ) (ii) ( N H_{2}^{-}+H_{2} O rightarrow N H_{3}+O H^{-} ) B. (i) – ( O R+H_{2} S O_{4} rightarrow R O H+H S O_{4}^{-} ) (ii) ( R^{-}+N H_{3} rightarrow R H+N H_{2}^{-} ) C . (i) ( C l^{-}+H F rightarrow H C l+F^{-} ) (ii) ( -O H+H C l rightarrow H_{2} O+C l^{-} ) D. ( left(text { i) }-O H+H B r rightarrow H_{2} O+B r^{-}right. ) (ii) ( R O^{-}+N H_{3} rightarrow R O H+N H_{2}^{-} ) | 11 |

1005 | For the gas phase exothermic reaction, ( A_{2}+B_{2} rightleftharpoons C_{2}, ) carried out in a closed vessel, the equilibrium moles of ( A_{2}, ) can be increased by: A. increasing the temperature B. decreasing the pressure c. adding inert gas at constant pressure D. removing some ( C_{2} ) | 11 |

1006 | If a maximum cube carved out from a gold sphere has thermal capacity of ‘K’ units, what would be the thermal capacity of the sphere? | 11 |

1007 | An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If ( T_{i} ) is the initial temperature and ( T_{f} ) is the final temperature, which of the following is correct? ( mathbf{A} cdot T_{f}>T_{i} ) for reversible process but ( T_{f}=T_{i} ) for irreversible process B . ( left(T_{f}right) ) rev ( =left(T_{f}right) ) irrev C. ( T_{f}=T_{i} ) for both reversible and irreversible process D. ( left(T_{i}right) ) irrev ( >left(T_{f}right) ) rev | 11 |

1008 | Assertion (A): The enthalpy of formation of gaseous oxygen molecules at ( 298 mathrm{K} ) and under a pressure of 1 atm is zero. Reason (R): The entropy of formation of gaseous oxygen molecules under the same condition is zero. A. Both assertion and reason are correct, reason is the correct explanation of the assertion B. Both assertion and reason are correct, reason is the not correct explanation of the assertion c. Assertion is correct, reason is incorrect D. Assertion is incorrect, reason is correct | 11 |

1009 | We can drive any themodynamically forbidden reaction in the desired direction by coupling with: A. highly exothermic reaction B. highly endothermic reaction C. highly exergonic reaction D. highly endergonic reaction E. reaction with large positive ( Delta S ) values | 11 |

1010 | A gas for which ( gamma=1.5 ) is suddenly compressed to ( frac{1}{4} ) th of its initial value then the ratio of the final to initia pressure is A . 1: 16 B. 1:8 ( c cdot 1: 4 ) D. 8: | 11 |

1011 | Calculate the total entropy change for the transition at ( 368 mathrm{K} ) of 1 mol of sulphur from the monoclinic to the rhombic solid state. Given ( Delta boldsymbol{H}= ) ( -401.7 J m o l^{-1} ) for the transition Assume the surroundings to be an ice- water. Both at ( mathbf{0}^{o} boldsymbol{C} ) ? A. ( -1.09 J K^{-1} ) B . ( 1.47 J K^{-1} ) c. ( 0.38 J K^{-1} ) D. ( 0.76 J K^{-1} ) | 11 |

1012 | A gas is compressed from a volume of ( 2 m^{3} ) to a volume of ( 1 m^{3} ) at a constant pressure of ( 100 N / m^{2} . ) Then it is heated at constant volume by supplying ( 150 J ) of energy. As a result, the internal energy of the gas: A. Increases by ( 250 mathrm{J} ) B. Decreases by 250 J c. Increases by ( 50 mathrm{J} ) D. Decreases by ( 50 mathrm{J} ) | 11 |

1013 | To which portion of the heating curve for water does ( Delta H_{f u s} ) apply? ( A cdot A-B ) B. ( B-C ) ( c cdot C-D ) D. ( D-E ) | 11 |

1014 | Calculate the average bond enthalpy of the ( boldsymbol{O}-boldsymbol{H} ) bond in water at ( 298 mathrm{K} ) using the data / information given below : ( Delta_{f} boldsymbol{H}^{0}[boldsymbol{H}(boldsymbol{g})]=mathbf{2} mathbf{1} mathbf{8} mathbf{k} mathbf{J} / mathrm{mol} ) 2. ( Delta_{f} H^{0}[O(g)]=249.2 mathrm{kJ} / mathrm{mol} ) 3. ( Delta_{f} H^{0}left[H_{2} O(g)right]=-241.8 mathrm{kJ} / mathrm{mol} ) The average bond enthalpy of the ( – ) bond in water is defined as one – half of the enthalpy change for the reaction ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightarrow boldsymbol{2} boldsymbol{H}(boldsymbol{g})+boldsymbol{O}(boldsymbol{g}) ) Also, determine the ( Delta U ) of the ( O-H ) bond in water at 298 K. Assume ideal gas behaviour. A ( cdot E(O-H)=462 ) kJ/mol; ( Delta U=461 ) kJ/mol B . ( E(O-H)=463.5 ) kJ/mol; ( Delta U=463.5 ) kJ/mol C ( cdot E(O-H)=461 mathrm{kJ} / mathrm{mol} ; Delta U=461 mathrm{kJ} / mathrm{mol} ) D – ( E(O-H)=463.5 mathrm{kJ} / mathrm{mol} ; Delta U=461 mathrm{kJ} / mathrm{mol} ) | 11 |

1015 | Q16. For an isolated system AU = 0; what will be AS? | 11 |

1016 | Which of the following does not result in an increase in entropy? A. Rusting of iron B. Conversion of ice to water c. crystallisation of sucrose from solution D. Sublimation of camphor | 11 |

1017 | The process on an ideal gas, shown in figure is : A. isothermal B. isobaric C. isochoric D. none of the above | 11 |

1018 | The P-V diagram of path followed by one mole of perfect gas in a cylindrical container is shown in figure, the work done when the gas is taken from state ( A ) to state B is: ( ^{mathrm{A}} cdot_{2 P_{2} V_{1}left[1-frac{sqrt{V}}{sqrt{V}_{1}}right]} ) в. ( 2 P_{1} V_{1}left[1-frac{sqrt{V}_{1}}{sqrt{V}_{2}}right] ) ( c cdot_{2 P_{2} V_{2}left[1-frac{sqrt{V}}{sqrt{V}_{2}}right]} ) D. ( 2 P_{1} V_{2}left[1-frac{sqrt{V}_{1}}{sqrt{V}_{2}}right] ) | 11 |

1019 | Bond energy of ( A B, A_{2} ) and ( B_{2} ) are in the ratio 1: 1: 0.5 and the enthalpy of formation of ( A B ) from ( A_{2} ) and ( B_{2} ) is ( -100 mathrm{kJ} mathrm{mol}^{-1} . ) Then the bond enthalpy of ( boldsymbol{A}_{2} ) is: begin{tabular}{l} A. ( 400 mathrm{kJ} mathrm{mol}^{-1} ) \ hline end{tabular} B. 200 kJ mol- c. ( 100 mathrm{kJ} mathrm{mol}^{-1} ) D. 300 kJ mol- | 11 |

1020 | A partition divides a container having insulated walls into two compartments and II. The same gas is filled in the two compartments whose initial parameters are given in figure. The partition is a conducting wall which can move freely without friction. Which of the following statements is/are correct with reference to teh final equilibrium position? begin{tabular}{|c|c|} hline( P, V, T ) & ( 2 P, 2 V, T ) \ ( I ) & ( I I ) \ hline end{tabular} This question has multiple correct options A. The pressure in the two compartments are equal B. Volume of the compartment I is ( frac{3 V}{5} ) C. volume of the compartment II is ( frac{12 V}{5} ) D. Final pressure I in compartment I is ( frac{5 P}{3} ) | 11 |

1021 | A mixture contains 1 mole of helium ( left.C_{p}=2.5 R, C_{v}=1.5 Rright) ) and 1 mole of hydrogen ( left(C_{p}=3.6 R, C_{v}=2.5 Rright) ) Calculate the volue of ( C_{p}, C_{v} ) and ( gamma ) for the mixture. | 11 |

1022 | Study the given figure and label ( X, Y ) and Z. A. ( x ) – Backward reaction; Y – Forward reaction; ( z ) Products B. ( x ) – Forward reaction; ( Y ) – Backward reaction; ( z ) Equilibrium C. ( x ) – Reversible reaction; Y – – Irreversible reaction; ( z ) – Equilibrium D. ( x ) – Forward reaction; Y – Forward reaction; ( z ) – Backward reaction | 11 |

1023 | In a reaction, ( Delta H ) and ( Delta S ) both are more than zero. In which of the following cases, the reaction would not be spontaneous? This question has multiple correct options ( mathbf{A} cdot Delta H>T Delta S ) в. ( T Delta S>Delta H ) c. ( Delta H=T Delta S ) D. ( Delta G<0 ) | 11 |

1024 | Which of the following system exchanges only energy but not matter? B. close system c. Isolated system D. None of the above | 11 |

1025 | Assertion Stirring the liquid in thermal contact with the reservoir will convert the work done into heat, is an irreversible process. Reason If it is the reversible process it will violate the second law of thermodynamics. 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 | 11 |

1026 | A thermodynamic system undergoes a cyclic process as shown in the figure. In each of the loops 1 and 2 , does the heat flow into or out of the system? A. into loop 1 and out of loop 2 B. into loop 2 and out of loop 1 ( c . ) into loop 1 and into loop 2 D. out of loop 1 and loop 2 both | 11 |

1027 | An isolated box, equally partitioned contains two ideal gases ( A ) and ( B ) as shown When the partition is removed, the gases mix. The changes in enthalpy ( (Delta H) ) and entropy ( (Delta S) ) in the process, respectively, are:ositive, zero | 11 |

1028 | In an isobaric process, the work done by a di-atomic gas is ( 10 mathrm{J} ), the heat given to the gas will be? A . ( 35 J ) в. ( 30 J ) c. ( 45 J ) D. ( 60 J ) | 11 |

1029 | The spontaneous nature of a reaction is impossible only if: A. ( Delta H=+v e, Delta S=+v e ) B. ( Delta H=-v e, Delta S=-v e ) c. ( Delta H=-v e, Delta S=+v e ) D. ( Delta H=+v e, Delta S=-v e ) | 11 |

1030 | Consider the following reaction: ( mathbf{2} boldsymbol{A}_{(boldsymbol{g})}+boldsymbol{B}_{(boldsymbol{g})} longrightarrow boldsymbol{C}_{(boldsymbol{g})}+boldsymbol{D}_{(boldsymbol{g})}+boldsymbol{q} ) If ( q ) is ( -v e, ) then which of the following is correct? A. Reaction is possible only at low temperature B. Reaction is possible only at high temperature c. Reaction is never possible D. Reaction is possible at all temperatures | 11 |

1031 | The work done in adiabatic compression of 2 mole of an ideal monoatomic gas by constant external pressure of 2 atm starting from initia pressure of 1 atm and initial temperature of ( 300 K(R=2 mathrm{cal} / mathrm{mol}- ) degree celsius) is : A . 360 cal B. 720 call c. 800 cal D. 1000 call | 11 |

1032 | The internal energy of 1 mol of an ideal gas depends on A. only volume B. only temperature c. only pressure D. temperature and pressure | 11 |

1033 | The equilibrium constant for the reaction ( boldsymbol{A} boldsymbol{g} boldsymbol{C l}_{s} rightleftharpoons boldsymbol{A} boldsymbol{g}_{(a q)}^{+}+boldsymbol{C l}_{(a q)}^{-} ) is ( x times 10^{-10} . ) Then, the value of ( x ) is : (Given ( : Delta G_{f(A g C l)}^{0}=-109.7 k J ) ( Delta G_{fleft(A g^{+}right)}^{0}=mathbf{7 7 . 1 k J} ; Delta G_{fleft(C l^{-}right)}^{0}= ) ( -131.2 k J) ) | 11 |

1034 | Among the following the irreversible process is A. free expansion of gas B. extension or compression of spring C. motion of an object on a perfectly frictionless surface D. all of them | 11 |

1035 | 1 mole of an ideal gas is taken through a cyclic process. The minimum temperature during the cycle is ( 300 K ) Then net exchange of heat for complete cycle is: Note ( :left(boldsymbol{T}_{boldsymbol{A}}=boldsymbol{6 0 0} boldsymbol{K} ; quad boldsymbol{T}_{boldsymbol{B}}=right. ) ( left.mathbf{1 2 0 0} boldsymbol{K} ; quad boldsymbol{T}_{c}=mathbf{6 0 0} boldsymbol{K}right) ) ( mathbf{A} cdot 600 R ln 2 ) в. ( 300 R ln 2 ) c. ( -300 R ln 2 ) D. ( 900 R ln 2 ) | 11 |

1036 | Temperature on the internal energy? | 11 |

1037 | The pressure of a given mass of gas at constant volume varies with temperature ( a S ) A ( cdot frac{1}{T^{2}} ) в. ( frac{1}{T} ) c. ( frac{1}{T^{3}} ) D. ( T ) | 11 |

1038 | If a system left over a period of time, What happens to the amount of its usable energy? A . increases B. decreases c. remains constant D. increases until the heat of friction equal the original potential energy in the system E. decreases until no heat is left in the system | 11 |

1039 | Assertion: Specific heat of a body is always more than its thermal capacity Reason : Thermal capacity is the heat required for raising temperature of unit mass of the body through unit degree. A. Both assertion and reason are correct and reason is the correct explanation of the assertion. B. Both assertion and reason are correct, but reason is not the correct explanation of the assertion. c. Assertion is correct but reason is incorrect D. Assertion is incorrect but Reason is correct E. Both assertion and reason is incorrect | 11 |

1040 | Which of the following relationship is incorrect? A ( cdot frac{Delta H-Delta E}{Delta n T}= ) constant B. ( Delta G=Delta H-T Delta S ) c. ( q=Delta U+W ) D. ( Delta G^{o}=-R T ln K ) | 11 |

1041 | An ideal gas occupying a volume of 2 ( d m^{3} ) and pressure of 5 bar undergoes isothermal and irreversible expansion against an external pressure of 1 bar Find the work done in the process? | 11 |

1042 | If the temperature scale is changed from ( ^{0} mathrm{C} ) to ( ^{0} mathrm{F} ). the numerical value of specific heat will ( A ). increase B. decrease c. remain unchanged D. nothing can be said | 11 |

1043 | Spot the statement which is true for temperature of gas and every kinetic model of gas: A. Temperature ( propto ) Average kinetic energy of the gas molecule B. temperature ( propto frac{1}{K . E_{text {of gas molecule}}} ) C. Temperature has no effect on kinetic energy of gas not D. All true according to condition | 11 |

1044 | At thermal equilibrium: A ( . Delta P=0 ) в. ( Delta T=0 ) c. ( Delta V=0 ) D. ( Delta n=0 ) | 11 |

1045 | The equilibrium constant is 10 at ( 100 K ) Hence, ( Delta G ) will be negative. A. True B. False | 11 |

1046 | The average translational energy and the rms speed of molecules in a sample of oxygen gas at ( 300 mathrm{K} ) are ( 6.21 times 10^{-21} mathrm{J} ) and ( 484 mathrm{m} / mathrm{s} ) respectively. The corresponding values at ( 600 mathrm{K} ) are nearly (assume ideal gas behaviours) A ( .12 .42 times 10^{-21} mathrm{J}, 968 mathrm{m} / mathrm{s} ) B. ( 8.78 times 10^{-21} ) J, ( 684 mathrm{m} / mathrm{s} ) c. ( 6.21 times 10^{-21} ) J, ( 968 mathrm{m} / mathrm{s} ) D. ( 12.42 times 10^{-21} ) 」, ( 684 mathrm{m} / mathrm{s} ) | 11 |

1047 | The enthalpies of formation of ( N_{2} O ) and ( N O ) are 28 and ( 90 k J m o l^{-1} ) respectively. The enthalpy of the reaction, ( 2 N_{2} O(g)+O_{2}(g) longrightarrow ) ( 4 N O(g) ) is equal to : ( A cdot 8 k J ) B. 88 kJ c. ( -16 k J ) D. 304 kJ | 11 |

1048 | For which of the following cases, ( Delta S= ) ( frac{Delta H}{T} ? ) A. Process of which ( Delta C_{P}=0, ) but ( Delta C_{V}=0 ) B. An isothermal process C. An isobaric process D. An isothermal reversible phase transition process | 11 |

1049 | A monoatomic ideal gas undergoes a process ABC. The heat given to the gas is A . 7.5 PV B. 12.5 PV ( c .16 .5 mathrm{Pv} ) D. 20.5 PV | 11 |

1050 | Blowing air with open mouth is an example of : A. isobaric process B. isochoric process c. isothermal process D. adiabatic process | 11 |

1051 | Q.1 Thermodynamics is not concerned about (a) energy changes involved in a chemical reaction (b) the extent to which a chemical reaction proceeds (c) the rate at which a reaction proceeds (d) the feasibility of a chemical reaction | 11 |

1052 | When the reaction is at equilibrium,the value of ( Delta G ) is ( A ) B. ( c cdot 3 ) D. ( 1 / 2 ) | 11 |

1053 | Which of the following drives spontaneous reactions? A. Low enthalpy values and high entropy values. B. Low enthalpy values and low entropy values. C. High enthalpy values and low entropy values. D. High enthalpy values and high entropy values E. High temperatures and low pressures. | 11 |

1054 | Q15. Calculate the enthalpy change for the process CCI(g) – C (g) + 4 Cl (g) and calculate bond enthalpy of C-Cl in CCI (3) 4Jap HⓇ (CCI) = 30.5 kJ mol-I; AH® (CC1.) = – 135.5 kJ mol-1 4 HP (C) = 715.0 kJ mol-1 where A H® is enthalpy of atomisation 4, H® (C12) = 242 kJ mol-1. Given: | 11 |

1055 | 70 cal of heat is required to raise the temperature of a diatomic gas at constant pressure from 30 to ( 35^{circ} ) C. The amount of heat required (in cal) to raise the temperature of the same gas through the same range ( left(30 text { to } 35^{circ} Cright) ) at constant volume is: A . 30 B. 60 c. 50 D. 70 | 11 |

1056 | A thermodynamic system is taken from an original state to an intermediate state by the linear process shown in the figure. Its volume is then reduced to the original value from ( boldsymbol{E} ) to ( boldsymbol{F} ) by an isobaric process. Calculate the total work done by the gas from ( D ) to ( E ) to ( F ) A .225 J D. 600 | 11 |

1057 | The minimum work which must be done to compress ( 16 g ) of oxygen isothermally, at ( 300 K ) from pressure of ( 1.01325 times ) ( mathbf{1 0}^{3} boldsymbol{N} / boldsymbol{m}^{2} ) to ( mathbf{1 . 0 1 3 2 5} times mathbf{1 0}^{mathbf{5}} boldsymbol{N} / boldsymbol{m}^{mathbf{2}} ) is ( mathbf{n} mathbf{1 0 0}=mathbf{4 . 6}, boldsymbol{R}=mathbf{8 . 3} boldsymbol{J} / boldsymbol{K}-boldsymbol{m o l} ) ( mathbf{A} cdot 5727 J ) в. ( 11.454 k J ) c. ( 123.255 k J ) D. ( 1232.55 J ) | 11 |

1058 | Among the following, the state functions are: This question has multiple correct options | 11 |

1059 | A diatomic ideal gas initially at 273 k is given 100 cal heat due to which system did ( 209 mathrm{J} ) work Molar heat capacity ( left(C_{m}right) ) of gas for the process is : A ( cdot frac{3}{2} ) R B ( cdot frac{5}{2} ) R ( c cdot frac{5}{4} R ) D. 5 R | 11 |

1060 | At ( 27 C ) latent heat of fusion of a compound is 2930 J/mol. Entropy change is : A. 9.77 J/molk B. 10.77 J/molk c. 9.07 J/molk D. 0.977 J/molk | 11 |

1061 | If the pressure in a closed vessle is reduced by drawing out some gas the mean-free path of molecules A. losing their kinetic energy B. sticking to the walls c. changing their momenta due to collision with the walls D. getting accelerated towards the wall | 11 |

1062 | Which of the following is true for the reaction? ( boldsymbol{H}_{2} boldsymbol{O}(l) rightleftharpoons boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) at ( mathbf{1 0 0}^{circ} mathbf{C} ) and ( mathbf{1} ) atm pressure. A ( . Delta S=0 ) в. ( Delta H=T Delta S ) c. ( Delta H=Delta U ) D. ( Delta H=0 ) | 11 |

1063 | Body A is in contact with body B, which is in contact with body C. The temperature of A is more than B which is more than C. Which of the following is the correct direction of flow in accordance with the zeroth law of thermodynamics. ( A cdot A ) to ( B ) to ( c ) B. A to B and C to B ( c cdot c ) to ( B ) to ( A ) D. B to A and B to C | 11 |

1064 | Transit of work takes place when any property other than differs A. Temperature B. Pressure c. volume D. All the above | 11 |

1065 | ( mathbf{A} cdot-62.7 k J m o l^{-1} ) ( mathbf{B} cdot-31.4 k J m o l^{-1} ) ( mathbf{c} cdot-15.7 k J m o l^{-1} ) D. ( -3.14 k J ) mol( ^{-1} ) | 11 |

1066 | 2. 25 The enthalpy of atomisation for the reaction CH, (g) → C(g)+ 4H (g) is 1665 kJ mol-1. What is the bond energy of C-H bond? | 11 |

1067 | Two bodies at different temperatures are mixed in a calorimeter. Which of the following quantities remains conserved? A. sum of the temperatures of the two bodies B. total heat of the two bodies c. total internal energy of the two bodies D. internal energy of each body | 11 |

1068 | The terms bond enthalpy and bond dissociation enthalpy stand for one and the same thing.If true enter 1 else o ( A ) | 11 |

1069 | Considering ( triangle G=triangle H-T triangle S, ) a spontaneous reaction will occur when : A. ( triangle G ) is positive and ( triangle S ) is positive B. ( triangle G ) is positive and ( triangle S ) is negative c. ( triangle H ) is negative and ( triangle S ) is positive D. ( triangle H ) is negative and ( triangle S ) is negative E. ( triangle H ) is positive and ( triangle T ) is negative | 11 |

1070 | A Carnot engine used first an ideal monoatomic gas and then an ideal diatomic gas. If the source and sink temperature are ( 411^{circ} mathrm{C} ) and ( 69^{circ} mathrm{C} ) respectively and the engine extracts ( 1000 mathrm{J} ) of heat in each cycle, then area enclosed by ( p V ) diagram is A . 100 J B. 300 J c. 500 D. 700 J | 11 |

1071 | If we place a solid hot metal in a cool liquid the metal and the liquid come to some final temperature together. The specific heat of the liquid is five times as great as the specific heat of the metal. The temperature change for the metal is twenty times as much as that for the liquid. How does the mass of the liquid compare to the mass of the solid metal? Assume no heat is lost from the system. A. The mass of the liquid is 100 times as much as the mass of the metal. B. The mass of the liquid is 5 times as much as the mass of the metal. c. The mass of the liquid is 20 times as much as the mass of the metal. D. The mass of the liquid is ( 1 / 4 ) times as much as the mass of the metal. E. The mass of the liquid is 4 times as much as the mass of the metal. | 11 |

1072 | Assertion Thermodynamic process in nature are irreversible. Reason Dissipative effect cannot be eliminated. 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 | 11 |

1073 | At ( 373 mathrm{K}, ) a gaseous reaction ( boldsymbol{A} rightarrow ) ( 2 B+C ) is found to be of first order. Starting with pure ( A ), the total pressure at the end of 10 min. was ( 176 mathrm{mm} ) and after a long time when A was completely dissociated, it was ( 270 mathrm{mm} ). The pressure of ( A ) at the end of 10 minutes was? A. ( 94 mathrm{mm} ) B. 47mm c. ( 43 mathrm{mm} ) D. 90mm | 11 |

1074 | Which of the following process is/are irreversible? This question has multiple correct options A. Combustion reaction of a mixture of petrol and air ignited by a spark B. Diffusion of cooking gas in air c. Temperature change in atmosphere D. None of these | 11 |

1075 | If the heat of formation of ( N O_{2} ) is ‘x’ ( left[1 / 2 N_{2(g)}+O_{2(g)} rightarrow N O_{2(g)}right] ) the heat of reaction ( N_{2(g)}+O_{2(g)} rightarrow 2 N O_{(g)} ) is y and the heat of reaction ( 2 N O_{(g)}+ ) ( O_{2(g)} rightarrow 2 N O_{2(g)} ) is z, then: A. ( 2 x+z=y ) в. ( 2 y+z=x ) c. ( 2 x-z=y ) D. ( 2 z+x=y ) | 11 |

1076 | The pressure at point ( C ) is given by A ( cdot frac{3 P_{0}}{2^{0.4}} ) в. ( frac{3 P_{0}}{2^{1.4}} ) c. ( 3 P_{0} times 2^{0.4} ) D. ( 3 P_{0} times 2^{1.4} ) | 11 |

1077 | ( 100 m l ) of ( 0.2 M H_{2} S O_{4} ) is reacted with ( 100 m l ) of ( 0.5 M N a O H ) solution. what is the normality of the solution A . 0.3N B. 0.8N c. ( 0.1 mathrm{N} ) D. 1N | 11 |

1078 | Q4. The bond enthalpy of H.() is 436 kJ mol-1 and that of N. (g) is 941.3 kJ mol. Calculate the average bond enthalpy of an N-H bond in ammonia. Given: A H® (NH3) = -46 kJ mol-1 | 11 |

1079 | The enthalpy of neutralisation of a strong acid by a strong base is ( -57.32 k J ) mol ( ^{-1} . ) The enthalpy of formation of water is ( -285.84 k J ) mol( ^{-1} . ) The enthalpy of formation of hydroxy ion is: A ( .+228.52 k J ) mol ( ^{-1} ) B. ( -114.26 k J ) mol( ^{-} ) c. ( -228.52 k J ) mol ( ^{-1} ) D. ( +114.2 mathrm{kJ} mathrm{mol}^{-1} ) | 11 |

1080 | Assertion Internal energy change in a cyclic process is zero. Reason Internal energy is a state function. 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 | 11 |

1081 | An automobile engine absorbs ( 1600 J ) of heat from a hot reservoir and expel ( 1000 J ) to a cold reservoir in each cycle.Find the efficiency of the cycle? A . ( 37.5 % ) B . ( 47.5 % ) % c. ( 40 % ) D. 30 % | 11 |

1082 | During the cycle A. work done by the gas is about ( 55 J ) and heat absorbed by the gas is also about ( 55 J ) B. work done by the gas is about ( 42 J ) and heat rejected by the gas is ( 60 J ) C. work done on the gas is ( 60 J ) and heat rejected by the ( operatorname{gas} ) is also ( 60 J ) D. work done on the gas is ( 60 J ) and heat absorbed by the gas is also about ( 60 J ) | 11 |

1083 | What is approximately its increase in internal energy in ( J ) | 11 |

1084 | One mole of an ideal monoatomic gas is heated at a constant pressure of one atmosphere from ( 0^{circ} mathrm{C} ) to ( 100^{circ} mathrm{C} ). Then the change in the internal energy is : A ( .20 .80 times 10^{2} J ) ( J ) B . ( 12.48 times 10^{2} J ) c. ( 832 times 10^{2} J ) D. ( 6.25 times 10^{2} J ) | 11 |

1085 | Internal energy change in a cyclic process is zero. A. True B. False | 11 |

1086 | The equilibrium constant ( boldsymbol{K}_{boldsymbol{p}} ) for the reaction ( boldsymbol{A}(boldsymbol{g}) rightleftharpoons boldsymbol{B}(boldsymbol{g})+boldsymbol{C}(boldsymbol{g}) ) is 1 at ( 27^{circ} mathrm{C} ) and 4 at ( 47^{circ} mathrm{C} . ) Calculate enthalpy change for: ( boldsymbol{B}(boldsymbol{g})+boldsymbol{C}(boldsymbol{g}) rightleftharpoons boldsymbol{A}(boldsymbol{g}) ) (Given ( boldsymbol{R}=mathbf{2} ) cal / mol. ( boldsymbol{K} ) ). A ( .-13.31 mathrm{kcal} / mathrm{mol} ) B. ( 13.31 mathrm{kcal} / mathrm{mol} ) c. ( -19.2 mathrm{kcal} / mathrm{mol} ) D. ( 55.63 mathrm{kcal} / mathrm{mol} ) | 11 |

1087 | Assertion ( C_{P}-C_{V}=R ) for ideal gas. Reason ( R ) is the work done when temperature of one mole of an ideal gas is increased by ( mathbf{1}^{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. Both Assertion and Reason are incorrect | 11 |

1088 | The work done in an adiabatic change in a particular gas depends only upon A. change in volume B. change in temprature c. change in pressure D. none of these | 11 |

1089 | Calculate the work done injoules when 3 moles of an ideal gas at ( 27^{circ} C ) expands isothermally and reversibly from 10 atm to 1 atm ( (1 a t m=1.013 x ) ( 10^{5} N m^{-2} ) ). What will be the work done if the expansion is against the constant pressure of 1 atm? | 11 |

1090 | Which is not true for Second Law of Thermodynamics? A. The second law of thermodynamics states that the total entropy of an isolated system always increases over time, or remains constant in ideal cases where the system is in a steady state or undergoing a reversible process. B. It is impossible, by means of inanimate material agency, to derive mechanical effect from any portion of matter by cooling it below the temperature of the coldest of the surrounding objects C. It is impossible to construct an engine which will work in a complete cycle, and produce no effect except the raising of a weight and cooling of a heat reservoir. D. The second law of thermodynamics states that the total energy of an isolated system is constant. | 11 |

1091 | At ( 320 K, ) a gas ( A_{2} ) is ( 20 % ) dissociated to ( A(g) ). The standard free energy change at ( 320 K ) and 1 atm in ( J ) mol ( ^{-1} ) is approximately: ( left[boldsymbol{R}=mathbf{8 . 3 1 4} boldsymbol{J} boldsymbol{K}^{-1} boldsymbol{m o l}^{-1} ; ln mathbf{2}=mathbf{0 . 6 9 3}right. ) A. 4763 B. 2068 c. 4281 D. 1844 | 11 |

1092 | When the volume of a gas is decreased at constant temperature the pressure increases because the molecules A. strike unit area of the walls of the container more often B. strike the unit area of the walls of the container with higher speed C. strike the unit area of the wall of the container with lesser speed D. move with more kinetic energy | 11 |

1093 | An isolated system can exchange: A. matter with the surroundings B. energy with the surroundings C. both ( A ) and ( B ) D. none of the above | 11 |

1094 | Which of the following equations corresponds to the enthalpy of combustion at ( 298 K ? ) ( mathbf{A} cdot C_{2} H_{6}(g)+7 / 2 O_{2}(g) longrightarrow 2 C O_{2}(g)+3 H_{2} O(g) ) B ( cdot 2 C_{2} H_{6}(g)+7 O_{2}(g) longrightarrow 4 C O_{2}(g)+6 H_{2} O(g) ) ( mathbf{c} cdot C_{2} H_{6}(g)+7 / 2 O_{2}(g) longrightarrow 2 C O_{2}(g)+3 H_{2} O(l) ) D. ( 2 C_{2} H_{6}(g)+7 O_{2}(g) longrightarrow 4 C O_{2}(g)+6 H_{2} O(l) ) | 11 |

1095 | In a particular experiment, a gas undergoes adiabatic expansion satisfying the equation ( V T^{3} ) =constant. The ration of specific heats, ( boldsymbol{Y} ) is: A . 4 B. 3 ( c cdot frac{5}{3} ) D. | 11 |

1096 | Differentiate between heat capacity and specific heat capacity | 11 |

1097 | mole of a gas with ( gamma=7 / 5 ) is mixed with 1 mole of a gas with ( gamma=5 / 3 ) then the value of ( gamma ) for resulting mixture is A . ( 7 / 5 ) в. ( 2 / 5 ) c. ( 24 / 16 ) D. ( 12 / 7 ) | 11 |

1098 | For which of the following processes, total entropy of universe increases. This question has multiple correct options A. Melting one mole of ice to water at ( 0^{circ} mathrm{C} ) B. Freezing one mole of water to ice at ( 0^{circ} mathrm{C} ) C. Freezing one mole of water to ice at ( -10^{circ} mathrm{C} ) D. Melting one mole of ice at ( 10^{circ} mathrm{C} ) into water | 11 |

1099 | When ( 229 J ) of energy is supplied as heat as constant pressure to 3 mol ( boldsymbol{A} boldsymbol{r}(boldsymbol{g}), ) the temperature of the sample is increased by ( 2.55 K . ) Calculate the molar heat capacity at constant volume A ( cdot 40 J K^{-1} m o l^{-1} ) B. ( 30 J K^{-1} ) mol ( ^{-1} ) c. ( 21.7 J K^{-1} ) mol ( ^{-1} ) D. ( 81.7 J K^{-1} mathrm{mol}^{-1} ) | 11 |

1100 | Assertion In free expansion of an ideal gas, the entropy increases. Reason Entropy increases in all natural processes. 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 | 11 |

1101 | Q1. Choose the correct answer: A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii) used to determine pressure volume work (iv) whose value depends on temperature only. | 11 |

1102 | A gas is enclosed in a vessel of volume ( 1000 mathrm{cc} ) at a pressure of ( 72.6 mathrm{cm} ) of Hg. It is being evacuated with the help of a piston pump, which expels ( 10 % ) gas in each stroke. The pressure after the second stroke will be nearest to ( A cdot 60 mathrm{cm} ) B. 55 ( mathrm{cm} ) ( c cdot 66 mathrm{cm} ) D. 50 cm | 11 |

1103 | Calculate the heat of combustion (in KJ) of methane from the following data i) ( mathrm{C}(text { graphite })+2 mathrm{H}_{2}(mathrm{g}) rightarrow mathrm{CH}_{4}(mathrm{g}), Delta mathrm{H}= ) ( -74.8 k J ) ii) ( C(text { graphite })+O_{2}(g) rightarrow C O_{2}(g), Delta H= ) ( -393.5 mathrm{kJ} ) iii) ( mathrm{H}_{2}(mathrm{g})+1 / 2 mathrm{O}_{2}(mathrm{g}) rightarrow mathrm{H}_{2} mathrm{O}(l), Delta mathrm{H}=-286.2 ) KJ. A. – 891.1 B . -816.3 c. -965.9 D. -1040.7 | 11 |

1104 | A closed system can exchange: A. matter with the surroundings B. energy with the surroundings C. both ( A ) and ( B ) D. none of the above | 11 |

1105 | ( N X ) is produced by the following step of reactions: ( boldsymbol{M}+boldsymbol{X}_{2} longrightarrow boldsymbol{M} boldsymbol{X}_{2} ) ( mathbf{3} boldsymbol{M} boldsymbol{X}_{mathbf{2}}+boldsymbol{X}_{mathbf{2}} longrightarrow boldsymbol{M}_{mathbf{3}} boldsymbol{X}_{mathbf{8}} ) ( M_{3} X_{8}+N_{2} C O_{3} longrightarrow N X+C O_{2}+ ) ( boldsymbol{M}_{3} boldsymbol{O}_{4} ) How much ( M ) (metal) is consumed to produce ( 206 g m ) of ( N X ? ) (Take atomic weight of ( boldsymbol{M}=mathbf{5 6}, boldsymbol{N}= ) ( mathbf{2 3}, mathbf{X}=mathbf{8 0}) ) ( mathbf{A} cdot 42 g m ) в. ( 336 g m ) c. ( frac{14}{3} g m ) D ( cdot frac{7}{4}^{g m} ) | 11 |

1106 | A system where there is exchange of energy but not of mass is called system. A. insulated B. isolated c. open D. closed | 11 |

1107 | Assertion Work and internal energy are not state functions. Reason The sum of ( boldsymbol{q}+boldsymbol{w} ) is state function 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 | 11 |

1108 | The heat of combustion of carbon to ( C O_{2} ) is ( -393.5 mathrm{kJ} / mathrm{mol} ). What is the heat released upon formation of 35.2 g of ( C O_{2} ) from carbon and oxygen gas? | 11 |

1109 | If an ideal gas, at constant temperature and pressure, expands, then its A. entropy increases and then decrease B. internal energy increases C. internal energy remains the same D. internal energy decreases | 11 |

1110 | When two bodies at different temperatures are placed in thermal contact with each other, heat flows from the body at a higher temperature until they both acquire the same temperature. Assuming that there is no loss of heat to the surroundings, then: A. The heat gained by the hotter body will be equal to the heat lost by the colder body B. The heat gained by the hotter body will be less than the heat lost by the colder body c. The heat gained by the hotter body will be greater than the heat lost by the colder body D. The heat lost by the hotter body will be equal to the heat gained by the colder body | 11 |

1111 | Conversion of sulphur to ( boldsymbol{S O}_{3} ) has ( triangle H=2 x K c a l ) and conversion of ( S O_{2} ) to ( S O_{3} ) involves ( triangle H=-y k c a l ). The correct thermochemical equation for formation of ( boldsymbol{S} boldsymbol{O}_{2} ) is: A ( . S+O_{2} rightarrow S O_{2} triangle H=(y-2 x) ) B. ( S+O_{2} rightarrow S O_{2} triangle H=-(y-2 x) ) c. ( S+O_{2} rightarrow S O_{2} triangle H=(x+y) ) D. ( S+O_{2} rightarrow S O_{2} triangle H=2 y-3 x ) | 11 |

1112 | During one cycle of a heat engine 2000 calories of heat is supplied and 1500 calories rejected. The amount of work done equals: A .2093 J B. ( 4186 J ) c. ( 1042 J ) D. 0 | 11 |

1113 | Find out the efficiency of the heat engine if it produces ( 100 J ) of heat, does ( 30 J ) of work, and emits ( 70 J ) into a cold reservoir. ( mathbf{A} cdot 100 % ) B. ( 70 % ) c. ( 42 % ) D. 40% E . ( 30 % ) | 11 |

1114 | Q12. Calculate the enthalpy of the reaction: 1,04(8) + 3CO(g) — >N20(g) + 3C0 (8) Given that; 1, HCO(g) = – 110 kJ mol-1, A,HCO,(g) = – 393 kg mol- 4HN,O(g) = 81 kJ mol I, 4, HN,O2(g) = 9.7 kJ mol- | 11 |

1115 | Which one of the following bonds has the highest average bond energy? A. ( S=O ) в. ( C equiv C ) ( mathbf{c} cdot C equiv N ) D. ( N equiv N ) | 11 |

1116 | The volume of one mole of an ideal gas with the adiabatic exponent ( gamma ) is changed according to the relation ( V= ) ( frac{a}{T} ) where a is a constant. Find the amount of heat absorbed by the gas in the process, if the temperature is increased by ( Delta T ) | 11 |

1117 | List I and List II contains four entries each. Entries of Column I are to be matched some entries of List II. One or more than one entries of List I may match with the same entry of List II. List I lists the partial derivatives and List II lists the thermodynamic variable. | 11 |

1118 | The efficiency of the heat engine is A . 75% B. 33% c. 50% D. 25% E . ( 100 % ) | 11 |

1119 | In a gamma decay process, the internal energy of a nucleus of mass ( M ) decreases, a gamma photon of energy ( boldsymbol{E} ) and linear momentum ( boldsymbol{E} / boldsymbol{c} ) is emitted and the nucleus recoils. Find the decrease in internal energy. | 11 |

1120 | Calculate ( Delta H_{f}^{o} ) for chloride ion from the following data: [ begin{array}{l} frac{1}{2} H_{2}(g)+frac{1}{2} C l_{2}(g longrightarrow H C l(g) ; Delta H= \ -92.4 k J quad m o l^{-1} \ H C l(g)+n H_{2} O longrightarrow H^{+}(a q .)+ \ C l^{-}(a q .) ; Delta H=-74.8 k J quad m o l^{-1} \ quad Delta H_{fleft(H^{+}(a q .)right.}^{o}=0.0 k J quad m o l^{-1} end{array} ] A ( .-167 k J mathrm{mol}^{-} ) в. 267 k ( J ) mol ( ^{-1} ) ( mathbf{c} cdot 167 k J operatorname{mol}^{-1} ) D. ( -267 k J mathrm{mol}^{-1} ) | 11 |

1121 | GRUN ANSWER TYPE QUESTIONS Q1. When liquid benzene is oxidised at constant pressure at 300 K, the change in enthalpy is -3728 kJ. What is the change in internal energy at the same temperature? | 11 |

1122 | Assertion Work done during free expansion of an ideal gas whether reversible or irreversible is positive. Reason During free expansion, external pressure is always less than the pressure of the system. 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 | 11 |

1123 | For the equilibrium, ( Delta G=-R T l n K ) If true enter 1 else 0 A . | 11 |

1124 | What is meant by Thermochemical Equation? | 11 |

1125 | For a reversible spontaneous change ( triangle s ) is: ( A cdot frac{Delta E}{T} ) в. ( frac{P Delta V}{T} ) c. ( frac{q}{T} ) D. ( R T l o g K ) | 11 |

1126 | Which has maximum internal energy at 298 K? A. Helium gas B. Oxygen gas c. Ozone gas D. All are equal | 11 |

1127 | Predict which of the following reaction (s) has a positive entropy change? ।. ( boldsymbol{A} boldsymbol{g}(boldsymbol{a} boldsymbol{q})+boldsymbol{C l}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{A} boldsymbol{g} boldsymbol{C l}(boldsymbol{s}) ) II. ( boldsymbol{N} boldsymbol{H}_{boldsymbol{4}} boldsymbol{C l}(boldsymbol{s}) rightarrow boldsymbol{N} boldsymbol{H}_{boldsymbol{3}}(boldsymbol{g})+boldsymbol{H} boldsymbol{C l}(boldsymbol{g}) ) III. ( 2 N H_{3}(g) rightarrow N_{2}(g)+3 H_{2}(g) ) A . I and II в. ॥ c. ॥ and III D. I | 11 |

1128 | A constant pressure calorimeter consists of an insulated beaker of mass ( 82 g ) made up of glass with heat capacity ( 0.75 J K^{-1} g^{-1} . ) The beaker contains ( 100 mathrm{m} L ) of ( 1 mathrm{M} ) HCl at ( mathbf{2 2 . 6}^{circ} boldsymbol{C} ) to which ( mathbf{1 0 0} boldsymbol{m} boldsymbol{L} ) of ( mathbf{1} boldsymbol{M} ) NaOH at ( 23.4^{circ} C ) is added. The final temperature after the reaction is complete at ( 29.3^{circ} mathrm{C} ). What is ( Delta H ) per mole for this neutralisation reaction? Assume tha the heat capacities of all solutions are equal to that of same volumes of water | 11 |

1129 | The relation between internal energy U, pressure ( P ) and volume ( V ) of a gas in an adiabatic process is ( U=a+b P V, ) where a and b are positive constants. What is the value of ( gamma ) ? A. ( frac{a}{b} ) B. ( frac{b+1}{b} ) c. ( frac{a+1}{a} ) D. | 11 |

1130 | Latent heat of vaporization of liquid at ( mathbf{5 0 0} boldsymbol{K} ) and ( mathbf{1} ) atm pressure is ( 10 mathrm{kcal} / ) mol. What is the change in internal energy when 3 moles of the liquid is vaporized at the same temperature? A . ( 27 mathrm{kcal} ) B. ( 7 k c a l ) c. 33 k call ( l ) | 11 |

1131 | mole of an ideal gas at initial temperature T was cooled is ochorically till the gas pressure decreased n times. Then by an isobaric process, the gas was restored to the initial temperature T. Find the net heat absorbed by the gas in the whole process. | 11 |

1132 | Compare rates of loss heat by the body at temperatures ( 527^{circ} C ) and ( 127^{circ} C ) Temperature of surrounding is ( 27^{circ} C ) | 11 |

1133 | Calorific value of ( boldsymbol{H}_{2} ) gas is ( mathbf{x} ) kJ ( / mathrm{g} ) m. What is heat of formation of ( boldsymbol{H}_{2} boldsymbol{O} ) ? ( A . x k J ) B. ( 2 x k J ) c. ( x / 2 k J ) D. ( 18 x k J ) | 11 |

1134 | The coefficient of performance of a carnot refrigerator working between ( 30^{circ} mathrm{C} ) and ( 0^{C} ) is A . 10 B. ( c cdot 9 ) D. | 11 |

1135 | Calculate change in internal energy if ( triangle H=-92.2 k J, P=40 a t m ) and ( triangle V=-1 L ) A . -42 kJ B. -88kJ ( c cdot+88 k J ) D. +42 kJ | 11 |

1136 | An ideal heat engine working between temperatures ( T_{1} ) and ( T_{2} ) has an efficiency ( eta ). The new efficiency if the temperatures of both th |