We provide redox reactions practice exercises, instructions, and a learning material that allows learners to study outside of the classroom. We focus on redox reactions skills mastery so, below you will get all questions that are also asking in the competition exam beside that classroom.
List of redox reactions Questions
| Question No | Questions | Class |
|---|---|---|
| 1 | The oxidation number of Fe in ( boldsymbol{K}_{4} boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6} ) is? ( A cdot+6 ) B. +4 ( c cdot+3 ) D. +2 | 11 |
| 2 | Out of ( F e O_{4}^{2-}, F e C l_{3}, F e C l_{2} ) and ( F e ) This question has multiple correct options A. best reducing agent is ( F e ) B. best oxidising agent is ( F e O_{4}^{2} ) c. best oxidising agent is ( F e C l_{3} ) D. best reducing agent is ( F e O_{4}^{2} ) | 11 |
| 3 | In three test tubes ( P, Q ) and ( R ) iron nails water, oil and anhydrous calcium chloride is taken. Among these test tubes, in which test tubes corrosion of nails will not take place? ( A cdot P, Q ) and ( R ) B. P and R c. P and ( Q ) D. Q and | 11 |
| 4 | . 31 Assertion (A) The decomposition of hydrogen peroxide to form water and oxygen is an example of disproportionation reaction. Reason (R) The oxygen of peroxide is in -1 oxidation state and it is converted to zero oxidation state in 0, and -2 oxidation state in H20. (a) Both A and Rare true and R is the correct explanation of A (b) Both A and Rare true but R is not the correct explanation of A (c) A is true but R is false (d) Both A and Rare false | 11 |
| 5 | Which of the following has been arranged in order of increasing oxidation number of nitrogen? A. ( N H_{3}<N_{2} O_{5}<N O<N_{2} ) B . ( N O_{2}^{+}<N O_{3}^{-}<N O_{2}^{-}<N_{3}^{-} ) C . ( N H_{4}^{+}<N_{2} H_{4}<N H_{2} O H<N_{2} O ) D. ( N O_{2}<N a N_{3}<N H_{4}^{+}<N_{2} O ) | 11 |
| 6 | Balance the following equation by oxidation number method ¡) ( K_{2} C r_{2} O_{7}+K I+H_{2} S O_{4} rightarrow ) ( boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{C r}_{2}left(boldsymbol{S O}_{4}right)_{3}+boldsymbol{I}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) ii) ( K M n O_{4}+N a_{2} S O_{3} rightarrow M n O_{2}+ ) ( N a_{2} S O_{4}+K O H ) iii) ( boldsymbol{C u}+boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} rightarrow boldsymbol{C u}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}+ ) ( N O_{2}+H_{2} O ) iv) ( K M n O_{4}+H_{2} C_{2} O_{4}+H_{2} S O_{4} rightarrow ) ( boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{M} boldsymbol{n} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{C} boldsymbol{O}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 7 | The oxidation number of iodine in ( I F_{5} ) is | 11 |
| 8 | When Carbon monoxide is passed over heated copper oxide it gives: A. ( C O_{2} ) в. ( C O ) ( c cdot O_{2} ) D. all of these | 11 |
| 9 | Examples of few compounds in a particular oxidation state are given Mark the example which is not correct. A. Phosphorus in + 1 oxidation state – ( H_{3} P O_{2} ) B. Chlorine in +7 oxidation state – ( H C l O ) c. Chromium in +6 oxidation state ( -C r O_{2} C l_{2} ) D. Carbon in 0 oxidation state ( -C_{12} H_{22} O_{1} ) | 11 |
| 10 | Which equation is correctly labeled oxidation or reduction? ( mathbf{A} cdot H_{2} S=S+2 e^{-}+2 H^{+} ) oxidation B ( cdot S O_{2}+4 e^{-}+2 H_{2} O=S+4 O H^{-} ) oxidation ( mathbf{C} cdot N H_{3}+H C l=N H_{4}++C l_{2}^{-} ) oxidation D. ( N a C l+A g N O_{3}=A g C l+N a N O_{3} ) reduction ( mathrm{E} cdot M n^{2+}=M n O_{4} ) reduction | 11 |
| 11 | State the characteristic of chemical reaction which takes place when 1) Lead reacts with KI 2) Zinc reacts with HCl 3) Reaction of candle wax | 11 |
| 12 | After balancing and reducing the coefficients to lowest whole number terms, What is the coefficient of ( boldsymbol{H}_{2} boldsymbol{O} ) ? ( boldsymbol{H} boldsymbol{C l}+boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} rightarrow boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{K} boldsymbol{C l}+ ) ( M n C l_{2}+C l_{2} ) ( A cdot 1 ) B. 2 ( c .5 ) D. 8 E . 16 | 11 |
| 13 | Balance the following redox reactions by the ion-electron method in basis medium ( M n O_{4}^{-}(a q)+I^{-}(a q) rightarrow M n O_{2}(s)+ ) ( boldsymbol{I}_{2}(boldsymbol{s}) ) | 11 |
| 14 | ( boldsymbol{H} boldsymbol{C l}(boldsymbol{a q})+boldsymbol{Z n}(boldsymbol{s}) rightarrow boldsymbol{Z n l}_{2}(boldsymbol{a q})+ ) ( boldsymbol{H}_{2}(boldsymbol{g}) ) In the above reaction ( boldsymbol{H} boldsymbol{C l} ) (aq) play a role as: A. bronsted acid B. oxidizing agent c. reducing agemt D. precipitate E. cathode | 11 |
| 15 | 20. Which is the poorest reducing agent? (a) Atomic hydrogen (b) Nascent hydrogen (c) Dihydrogen (d) All have same reducing strength | 11 |
| 16 | The total number of ( boldsymbol{H}_{2} boldsymbol{O} ) molecules present in the balanced chemical reaction is : ( M n O_{4}^{ominus}+F e^{2+} longrightarrow M n^{2+}+F e^{3+}( ) in alkaline medium) | 11 |
| 17 | Hydrogen sulphide ( left(boldsymbol{H}_{2} boldsymbol{S}right) ) is a strong reducing agent. Which of the following reactions shows its reducing action? A ( cdot C dleft(N O_{3}right)_{2}+H_{2} S rightarrow C d S+2 H N O_{3} ) B. ( C u S O_{4}+H_{2} S rightarrow C u S+H_{2} S O_{4} ) c. ( 2 mathrm{FeCl}_{3}+mathrm{H}_{2} mathrm{S} rightarrow 2 mathrm{Fe} mathrm{Cl}_{2}+2 mathrm{HCI}+mathrm{S} ) D. ( P bleft(N O_{3}right)_{2}+H_{2} S rightarrow P b S+2 C H_{3} C O O H ) | 11 |
| 18 | A redox reaction is shown in the diagrams. Identify the reaction. ( left.mathbf{A} cdot Z n(s)+C u_{(a q)}^{2+} rightarrow Z n_{(a q)}^{2+}+C u_{(} sright) ) B. ( left.C u(s)+2 A g_{a q}^{+} rightarrow C u_{(a q)}^{2+}+2 A g_{(} sright) ) C ( cdot 2 A g(s)+C u_{(a q)}^{2+} rightarrow 2 A g_{(a q)}^{+}+C u(s) ) ( left.mathbf{D} cdot C u_{(} sright)+Z n_{(a q)}^{2+} rightarrow C u_{(a q)}^{2+}+Z n(s) ) | 11 |
| 19 | Assertion Combining equal volumes of ( 0.2 M ) ( A g N O_{3}, ) and ( 0.2 M H C l ) does not produce a precipitate of ( boldsymbol{A} boldsymbol{g} boldsymbol{C l} ) Reason The silver ion is rapidly reduced to silver metal, producing chlorine 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 |
| 20 | The oxidation number of ( C ) atom in ( C H_{2} C l_{2} ) and ( C C l_{4} ) are respectively ( A cdot-2 ) and -4 B. 0 and -4 ( c .0 ) and 4 D. 2 and 4 | 11 |
| 21 | ( H_{3} P O_{4} ) is a tri basic acid and one of its salt is ( N a H_{2} P O_{4} . ) What volume in ml of 1M NaOH solution should be added to ( 12 g ) of ( N a H_{2} P O_{4} ) to convert it into ( N a_{3} P O_{4} ? ) | 11 |
| 22 | Complete and balance the following compound ( boldsymbol{A l} boldsymbol{B} boldsymbol{r}_{3}+boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7}+ ) [ boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} rightarrow boldsymbol{K}_{3} boldsymbol{P} boldsymbol{O}_{4}+boldsymbol{A} boldsymbol{l} boldsymbol{P} boldsymbol{O}_{4}+ ] | 11 |
| 23 | Assign oxidation number to the underlined element in ( boldsymbol{H}_{2} underline{S}_{2} boldsymbol{O}_{7} ) | 11 |
| 24 | What is redox reaction? In the reaction ( Z n O+C rightarrow Z n+C O ) which substance gets oxidised and which gets reduced? | 11 |
| 25 | The oxidation number of ‘N’ in NOCIO: ( A cdot+3 ) B. +1 ( c cdot+2 ) ( D cdot+7 ) | 11 |
| 26 | What is the number of moles of ( K M n O_{4} ) that will be needed to react completely with one mole of ferrous oxalate in an acidic medium? | 11 |
| 27 | Calculate the oxidation number of ( M n ) in the product formed on strongly heating ( M n_{2} O_{7} ) (write absolute value of an answer) | 11 |
| 28 | The oxidation states of ( P ) atom in ( boldsymbol{P O C l}_{3}, boldsymbol{H}_{2} boldsymbol{P O}_{3} ) and ( boldsymbol{H}_{4} boldsymbol{P}_{2} boldsymbol{O}_{6} ) respectively are: ( mathbf{A} cdot+5,+4,+4 ) B. +5,+5,+4 ( mathbf{c} cdot+4,+4,+5 ) ( mathbf{D} cdot+3,+4,+5 ) | 11 |
| 29 | Balance the following reaction. ( boldsymbol{Z} boldsymbol{n}(boldsymbol{s})+boldsymbol{P b C l}_{2}(boldsymbol{a q}) longrightarrow boldsymbol{P b}(boldsymbol{s})+ ) ( Z n C l_{2}(a q) ) ( mathbf{A} cdot Z n(s)+P b C l_{2}(a q) longrightarrow P b(s)+Z n C l_{2}(a q) ) B ( cdot 2 Z n(s)+P b C l_{2}(a q) longrightarrow P b(s)+2 Z n C l_{2}(a q) ) ( mathbf{c} cdot Z n(s)+2 P b C l_{2}(a q) longrightarrow P b(s)+Z n C l_{2}(a q) ) D ( cdot Z n(s)+2 P b C l_{2}(a q) longrightarrow P b(s)+2 Z n C l_{2}(a q) ) | 11 |
| 30 | In which of the following reactions, ( H_{2} O_{2} ) acts as a reducing reagent? A ( cdot P b O_{2(s)}+H_{2} O_{2(a g)} rightarrow P b O_{(s)}+H_{2} O_{(i)}+O_{2(g)} ) B. ( N a_{2} S O_{3(a g)}+H_{2} O_{2(a g)} rightarrow N a_{2} S O_{4(a g)}+H_{2} O_{(i)} ) C ( cdot 2 K I_{(a)}+H_{2} O_{2(a)} rightarrow 2 K O H_{(a q)}+I_{2(s)} ) D. All the above | 11 |
| 31 | Number of moles of ( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7} ) reduced by one mole of iodide ions is : A . 3 B. ( frac{1}{3} ) ( c .6 ) D. | 11 |
| 32 | The sum of the oxidation numbers of all the carbons in ( C_{6} H_{5} C H O ) is : ( A cdot O ) ( B cdot+2 ) ( c cdot+4 ) D. – – | 11 |
| 33 | Which equation represents charge balanced equation for a solution of ( boldsymbol{H}_{2} boldsymbol{S} ) in water? ( mathbf{A} cdotleft[H^{+}right]=2left[S^{2-}right]+left[H S^{-}right]+left[O H^{-}right] ) B ( cdotleft[H^{+}right]=left[O H^{-}right] ) C ( cdotleft[H^{+}right]=left[S^{2-}right]+left[H S^{-}right]+left[H^{+}right] ) D. ( left[H^{+}right]=left[S^{2-}right]+left[H S^{-}right]+left[O H^{-}right] ) | 11 |
| 34 | Which of the following reactions involves oxidation and reduction? ( mathbf{A} cdot N a B r+H C l rightarrow N a C l+H B r ) B. ( H B r+A g N O_{3} rightarrow A g B r+H N O_{3} ) ( mathbf{c} cdot H_{2}+B r_{2} rightarrow 2 H B r ) D. ( N a_{2} O+H_{2} S O_{4} rightarrow N a_{2} S O_{4}+H_{2} O ) | 11 |
| 35 | Hydrolysis of ( X e F_{6} ) in strongly alkaline solution is an auto-redox process. If true enter 1 , else enter 0 ( A ) | 11 |
| 36 | What will be the octane number of best fuel? A. 80 B. 81 ( c cdot 82 ) D. 83 | 11 |
| 37 | Balance the following equation. ( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{H}^{+} rightarrow boldsymbol{C r}_{2} boldsymbol{O}_{3}+ ) ( boldsymbol{S}_{8}+boldsymbol{H}_{2} boldsymbol{O} ) ( mathbf{A} cdot 24 H_{2} S+8 C r_{2} O_{7}^{2-}+16 H^{+} rightarrow 8 C r_{2} O_{3}+3 S_{8}+32 H_{2} O ) B ( cdot 24 H_{2} S+3 C r_{2} O_{7}^{2-}+6 H^{+} rightarrow 7 C r_{2} O_{3}+3 S_{8}+32 H_{2} O ) ( mathbf{c} cdot 24 H_{2} S+8 C r_{2} O_{7}^{2-}+5 H^{+} rightarrow 6 C r_{2} O_{3}+4 S_{8}+32 H_{2} O ) D. None of these | 11 |
| 38 | A student places a strip of solid magnesium metal into a beaker full of ( 100 . m L ) of ( 3.0 mathrm{M} ) hydrochloric acid solution. The student observes bubbling and the disappearance of the magnesium metal. Which species is being oxidized and which species is being reduced in this reaction? A. Magnesium being oxidized and the chloride ion is being reduced. B. Magnesium being oxidized and the hydrogen ion is being reduced. c. Magnesium being reduced and the chloride ion is being oxidized. D. Magnesium being reduced and the hydrogen ion is being oxidized. | 11 |
| 39 | Which statement(s) is/are not correct about the reaction? ( boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow ) ( boldsymbol{I}_{2}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}(l) boldsymbol{I}_{2}(boldsymbol{a} boldsymbol{q})+ ) ( mathbf{2} N a_{2} S_{2} O_{3} rightarrow N a_{2} S_{4} O_{6}+2 N a I ? ) This question has multiple correct options A. The ( I_{2} ) formed is consumed completely in the second state is confirmed by addition of starch just before its complete consumption B. The reaction process is called clock reaction because the appearance of blue colour on addition of starch is like an alarm given by clock c. Sulphur is oxidised whereas iodine is oxidised and reduced during whole process D. ( H_{2} O_{2} ) acts as reducing agent | 11 |
| 40 | It is a chemical reaction where two reactants, each containing the same element but with a different oxidation number, will form a product in which the elements involved reach the same oxidation number. This reaction is called: A. Comproportionation reaction B. Disproportionation reaction c. Reduction D. Double displacement reaction | 11 |
| 41 | Write the type of reaction. Ethene is burnt in the presence of oxygen to form carbon dioxide, water and releases heat and light. A. Endothermic reaction B. Combustion reaction c. Redox reaction D. Esterificaton reaction | 11 |
| 42 | Assertion Fluorine always exhibits an oxidation state of -1 in its compounds. Reason Fluorine has maximum electronegativity and it contain seven electrons in its valence shell. 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 |
| 43 | Balance the following redox reactions in basc medium: [ M n O_{4}^{-}+I^{-} longrightarrow M n O_{2}+I O_{3}^{-} ] A ( cdot 2 M n O_{4}^{-}+I^{-}+H_{2} O longrightarrow 2 M n O_{2}+I O_{3}^{-}+2 O H^{-} ) B. ( 3 M n O_{4}^{-}+I^{-}+H_{2} O longrightarrow 4 M n O_{2}+I O_{3}^{-}+2 O H^{-} ) ( mathrm{c} cdot 3 mathrm{Mn} mathrm{O}_{4}^{-}+I^{-}+mathrm{H}_{2} mathrm{O} longrightarrow 5 mathrm{MnO}_{2}+mathrm{IO}_{3}^{-}+2 mathrm{OH}^{-} ) D. None of these | 11 |
| 44 | Although ( C u^{+} ) disproportionates in aqueous solution as ( 2 C u^{+}(a q) rightarrow ) ( boldsymbol{C u}(boldsymbol{s})+boldsymbol{C u}^{2+}(boldsymbol{a q}) . ) Write down a reaction in which disproportionation is reversed. A ( cdot C u(s)+C u^{2+}(a q)+2 C l^{-} rightarrow C u C l(s) ) в. ( C u(l)+C u^{2+}(a q)+2 C l^{-} rightarrow C u C l(l) ) c. ( C u(s)+C u^{+}(a q)+C l^{-} rightarrow C u C l(s) ) D. None of these | 11 |
| 45 | Which of the following species will not exhibit disproportionation reaction? A ( cdot C l O^{-} ) B. ( C l O_{2}^{-} ) ( mathrm{c} cdot mathrm{ClO}_{3}^{-} ) D. ( C l O_{4}^{-} ) | 11 |
| 46 | Which of the following statement is correct? A. Oxidation involves gain of electron B. Substance which is reduced is reducing agent C. Exothermic process involves absorption of heat D. Oxidation involves loss of electrons | 11 |
| 47 | Q7. Write the cell reactions: Zn Zn2+(1M) / Cd2+(1M) Cd E° Zn + Zn = -0.76 V, E° Cd2+/Cd = 0.40 V 72+ Coolt | 11 |
| 48 | ( Delta_{r} H ) of which of the following reaction is zero? ( mathbf{A} cdot H_{2(g)} rightarrow 2 H_{(g)}^{+}+2 e^{-} ) B. ( 2 H_{(g)}+a q rightarrow 2 H_{(a q)}^{+}+2 e^{-} ) ( mathbf{c} cdot 2 H_{(g)} rightarrow 2 H_{(g)}^{+}+2 e^{-} ) D. ( H_{2(g)}+a q rightarrow 2 H_{(a q)}^{+}+2 e^{-} ) | 11 |
| 49 | Q4. Find out the oxidation state of sodium in Na,O in Mo | 11 |
| 50 | The ( M n^{3+} ) ion is unstable in solution and undergoes disproportionation to ( operatorname{give} M n^{2+}, M n O_{2} ) and ( H^{+} ) ion. Write a balanced ionic equation for the reaction. | 11 |
| 51 | The complete balanced equation is: ( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{K}_{2} boldsymbol{C r} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow ) A ( cdot 3 mathrm{H}_{2} S+2 mathrm{K}_{2} mathrm{CrO}_{4}+5 mathrm{H}_{2} mathrm{SO}_{4} rightarrow mathrm{Cr}_{2}left(mathrm{SO}_{4}right)_{3}+ ) ( 2 K_{2} S O_{4}+8 H_{2} O+3 S ) B. ( 3 H_{2} S+K_{2} C r O_{4}+5 H_{2} S O_{4} rightarrow C r_{2}left(S O_{4}right)_{3}+ ) ( K_{2} S O_{4}+8 H_{2} O+3 S ) c. ( H_{2} S+2 K_{2} C r O_{4}+3 H_{2} S O_{4} rightarrow C r_{2}left(S O_{4}right)_{3}+ ) ( 2 K_{2} S O_{4}+8 H_{2} O+3 S ) D. none of these | 11 |
| 52 | Which is not redox change? ( mathbf{A} cdot C a C O_{3} rightarrow C a O+C O_{2} ) ( mathbf{B} cdot 2 H_{2}+O_{2} rightarrow 2 H_{2} O ) ( mathrm{c} cdot_{N a}+H_{2} O rightarrow N a O H+frac{1}{2} H_{2} ) D. ( M n C I_{3} rightarrow M n C I_{2}+frac{1}{2} C I_{2} ) | 11 |
| 53 | The balanced molecular equation is : A. ( C l_{2}+H_{2} O+N a_{2} S_{2} O_{3} rightarrow N a_{2} S O_{4}+S+2 H C l ) в. ( C l_{2}+N a_{2} S_{2} O_{3} rightarrow 2 N a C l+N a_{2} S O_{4} ) c. ( quad C l_{2}+S_{2} O_{3}^{2-} rightarrow S O_{4}^{2-}+S+C l ) D. none of these | 11 |
| 54 | Amongst the following, identify the species with an atom in +6 oxidation state. ( mathbf{A} cdotleft[M n O_{4}right]^{-} ) B . ( left[operatorname{Cr}(C N)_{6}right]^{3-} ) ( mathrm{c} cdot mathrm{Cr}_{2} mathrm{O}_{3} ) D. ( operatorname{Cr} mathrm{O}_{2} mathrm{Cl}_{2} ) | 11 |
| 55 | An amount of 0.2 mole of ( A O_{3}^{-} ) gains 1.2 mole of electron in a process. Assuming that there is no change in oxidation state of oxygen, determine the oxidation state of ‘A’ in product: ( A cdot+1 ) B. – ( c cdot 0 ) ( D cdot+6 ) | 11 |
| 56 | Mixture of ( boldsymbol{N a I}(boldsymbol{s})+boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7}(boldsymbol{s})+ ) conc. ( H_{2} S O_{4} ) when heated in a test tube dark vapours evolve A. ( I_{2} ) в. ( N a_{2} ) ( mathrm{c} cdot H_{2} ) D. All the above | 11 |
| 57 | ( boldsymbol{A}^{+} boldsymbol{B}^{-}+boldsymbol{C}^{+} boldsymbol{D}^{-} longrightarrow boldsymbol{A}^{+} boldsymbol{D}^{-}+boldsymbol{C}^{+} boldsymbol{B}^{-} ) Identify the above generalized type of reaction: A. Chemical replacement reaction B. Chemical double decomposition reaction c. Chemical displacement reaction D. Chemical combination reaction | 11 |
| 58 | Reduction of the metal centre in aqueous permanganate ion involves: This question has multiple correct options A. 3 electrons in neutral medium B. 5 electrons in neutral medium c. 1 electron in alkaline medium D. 5 electrons in acidic medium | 11 |
| 59 | Which of the following statements is not correct about the given reaction? ( boldsymbol{K}_{4}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6} frac{text {Oxidation}}{boldsymbol{leftrightarrow}} boldsymbol{F} boldsymbol{e}^{3+}+boldsymbol{C O}_{2}+right. ) ( mathbf{N} boldsymbol{O}_{mathbf{3}}^{-} ) A. Fe is oxidised from ( F e^{2+} ) to ( F e^{3 text { – }} ) B. Carbon is oxidised from ( C^{2+} ) to ( C^{4+} ). c. ( mathrm{N} ) is oxidised from ( N^{3} ) – to ( N^{5+} ) D. Carbon is not oxidised | 11 |
| 60 | A redox reaction is one in which: A. both the substances are reduced B. both the substances are oxidized c. an acid is neutralized by the base D. one substance is oxidized, while the other is reduced | 11 |
| 61 | The reaction, ( A B rightarrow A+B ) is a: This question has multiple correct options A. Decombination reaction B. Combination reaction c. chemical composition D. Decomposition reaction | 11 |
| 62 | Which of the following is true about the reaction ( boldsymbol{F} boldsymbol{e}+boldsymbol{S} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{S} ? ) This question has multiple correct options A ( cdot F e+2 e^{-} rightarrow F e^{2+} ) B. ( F e rightarrow F e^{2+}+2 e^{-} ) C ( cdot F e^{2+} rightarrow F e+2 e^{-} ) D. ( S rightarrow S^{2-}+2 e^{-} ) E ( . S+2 e^{-} rightarrow S ) | 11 |
| 63 | 0.16 Which of the following electrodes will act as anodes, which connected to Standard Hydrogen Electrode ? (a) AI/AP+ E = -1.66 (6) Fe/Fe2+ = -0.44 (c) Cu/Cu2+ E = +0.34 (d) F2 (g)/2F- (aq) E=0287 | 11 |
| 64 | Assertion ( H_{3} P O_{2} ) can act as strong reducing agent and gives disproportionation reaction on heating. Reason Due to presence of one ( -O H ) group and ( boldsymbol{P}-boldsymbol{H} ) group, ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{2} ) is a monobasic bronsted acid. 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 |
| 65 | Calculate the oxidation number of ( F e ) in ( boldsymbol{K}_{mathbf{4}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right] ) | 11 |
| 66 | Which of the following substances undergo(s) disproportionation reactions under basic medium? This question has multiple correct options A. ( F_{2} ) в. ( P_{4} ) ( mathrm{c} cdot S_{8} ) D. ( B r_{2} ) | 11 |
| 67 | The number of moles of ( K M n O_{4} ) that will be needed to react completely with one mole of ferrour oxalate ( F eleft(C_{2} O_{4}right) ) in acidic solution is : ( mathbf{A} cdot mathbf{1} ) B. ( frac{2}{5} ) ( c cdot frac{3}{5} ) D. | 11 |
| 68 | Balance the following equation: ( boldsymbol{C u}(boldsymbol{s})+boldsymbol{A} boldsymbol{u}^{oplus} longrightarrow boldsymbol{A u}(boldsymbol{s})+boldsymbol{C u}^{2+} ) ( mathbf{A} cdot C u(s)+2 A u^{oplus} longrightarrow A u(s)+C u^{2+} ) B ( cdot C u(s)+2 A u^{oplus} longrightarrow 2 A u(s)+C u^{2+} ) ( mathbf{c} cdot 2 C u(s)+A u^{oplus} longrightarrow 2 A u(s)+2 C u^{2+} ) D ( cdot 2 C u(s)+A u^{oplus} longrightarrow 2 A u(s)+C u^{2+} ) | 11 |
| 69 | Match the Column-I with Column-II. | 11 |
| 70 | Balance the following redox reaction ( left(boldsymbol{C r}_{2} boldsymbol{O}_{7}right)_{(a q)}^{2-}+boldsymbol{F} boldsymbol{e}_{(a q)}^{2+} rightarrow boldsymbol{C r}_{(a q)}^{3+}+boldsymbol{F} boldsymbol{e}_{(a q)}^{3+} ) (acidic medium) | 11 |
| 71 | In double decomposition reaction are exchanged | 11 |
| 72 | Assertion In the titration of ( N a_{2} C O_{3} ) with ( H C l ) using methyl orange indicator, the volume required at the equivalence point is twice that of the acid required using phenolphthalein indicator. Reason Two mole of ( H C l ) are required for the complete neutralization of one mole of ( N a_{2} C O_{3} ) 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 incorrect but Reason is correct D. Both Assertion and Reason are correct | 11 |
| 73 | Balance the following equation and find the values of ( a, b, c, d ) ( boldsymbol{a} boldsymbol{P b O}_{2}+boldsymbol{b C l}^{ominus} longrightarrow boldsymbol{c} boldsymbol{C l O}^{ominus}+ ) ( boldsymbol{d}left[boldsymbol{P b}(boldsymbol{O H})_{3}right]^{ominus}(text { in basic solution }) ) В. ( a=1, b=1, c=1, d=1 ) c. ( a=2, b=1, c=1, d=2 ) D. ( a=1, b=1, c=2, d=2 ) | 11 |
| 74 | Hydrogen atom in the basic medium is balanced by which of the following species? A ( cdot O H^{-} ) в. ( H^{+} ) c. ( H_{3} O^{+} ) D. ( H_{2} ) | 11 |
| 75 | Give the oxidation state of underlined. ( boldsymbol{C a O C l}_{2} ) | 11 |
| 76 | Which one of the following leads to redox reaction? A. ( A g N O_{3}+H C l ) в. ( K O H+H C l ) c. ( K I+C l_{2} ) D. ( N H_{3}+H C l ) | 11 |
| 77 | Find the oxidation number of ( mathrm{P} ) in ( boldsymbol{P} boldsymbol{H}_{4}^{+} ) | 11 |
| 78 | When the gases; sulphur dioxide and hydrogen sulphide mix in the presence of water, the reaction ( S O_{2}+2 H_{2} S rightarrow ) ( 2 H_{2} O+3 S ) occurs Here hydrogen sulphide is acting as: A. an oxidizing agent B. a reducing agent c. a dehydrating agent D. a catalyst | 11 |
| 79 | Above diagram represents an atom ( X ) Atom ‘X’ is a reducing agent. A . True B. False | 11 |
| 80 | What is the oxidation state of central ( operatorname{atom} operatorname{in} C aleft[P t C l_{4}right] ? ) ( mathbf{A} cdot mathbf{1} ) B . 2 ( c .3 ) D. 4 | 11 |
| 81 | The sum of the oxidation numbers of all the atoms in a neutral molecule is equal to: A. zero B. one c. three D. four | 11 |
| 82 | The other name of comproportionation is: A. disproportionation B. proportionation c. symproportionation D. antiproportionation | 11 |
| 83 | The compound(s) which generate(s) ( N_{2} ) gas upon thermal decomposition below ( 300^{circ} mathrm{C} ) is/are: This question has multiple correct options A. ( N H_{4} N O_{3} ) B. ( left(N H_{4}right)_{2} C r_{2} O_{7} ) c. ( B aleft(N_{3}right)_{2} ) D. ( M g_{3} N_{2} ) | 11 |
| 84 | 8. Consider the following reaction, (NH2)2Cr2O, –> N2 + Cr,O, +4H,0 (a) it is an example of intramolecular redox reaction (b) it is an example of intermolecular redox reaction (C) NH4 ion is a reducing agent and Cr,04 is an oxidizing agent (d) it is an example of disproportionation reaction | 11 |
| 85 | Balance the following equation: ( boldsymbol{C u O}+boldsymbol{N H}_{3} rightarrow boldsymbol{N}_{2}+boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C u} ) | 11 |
| 86 | Write balanced chemical equations for the conversion of ( C r O_{4}^{2-} ) to ( C r_{2} O_{7}^{2-} ) in acidic medium and ( C r_{2} O_{7}^{2-} ) to ( C r O_{4}^{2-} ) in basic medium. | 11 |
| 87 | ( boldsymbol{C l O}^{-} rightleftarrows boldsymbol{C l O}_{3}^{-}+boldsymbol{C l}^{-} ) When the equation for the reaction represented above is balanced with coefficients reduced to the lowest whole-umber terms, correct statements include which of the following? I. The coefficient for ( C l^{-} ) is 4 II. The coefficient for ( C l O_{3}^{-} ) is 2 III. The coefficient for ( C l O^{-} ) is 3 A. I only B. II only C. III only D. I and II only E . I, II and III only | 11 |
| 88 | Assertion Statement ( 1: H g C l_{2} ) and ( S n C l_{2} ) exist together in an aqueous solution. Reason Statement ( 2: S n C l_{2} ) is a strong | 11 |
| 89 | 4 mol of a solution containing ( boldsymbol{A}^{boldsymbol{n}} ) requires 1.6 mol of ( M n O_{4}^{ominus} ) for the oxidation of ( A^{n+} ) to ( A O_{3}^{ominus} ) in acidic medium. The value of ( n ) is : A . 1 B . 2 ( c .3 ) D. | 11 |
| 90 | 0.1M of ( boldsymbol{H} boldsymbol{A} ) is titrated with ( mathbf{0 . 1} boldsymbol{M} ) ( N a O H, ) calculate ( p H ) at end point ( operatorname{Given} K(H A)=5 times 10^{-6} ) and ( alpha ll 1 ) | 11 |
| 91 | Find the oxidation number of ( N & C l ) in ( N O C l_{4} ) respectively is: ( A cdot+3,+6 ) B. +2,+6 ( mathrm{c} cdot+3,+7 ) ( mathrm{D} cdot+2,+7 ) | 11 |
| 92 | When the equation: ( C_{2} H_{6}+O_{2} rightarrow ) ( boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) is completely balanced using the lowest whole number coefficients, the sum of the coefficients will be : A . 4 B. 9. c. 19 D. 15.5 E. 1 | 11 |
| 93 | In the reaction: ( 3 C l_{2}+6 N a O H longrightarrow ) ( mathbf{5} N a C l+N a C l O_{3}+3 H_{2} O, C l_{2} ) acts purely as an oxidizing agent. If true enter 1 , else enter 0 . A. | 11 |
| 94 | Identify ( M ) and ( N ) in the following reaction. Copper glance controlledheating in presence ( boldsymbol{M}+boldsymbol{S O}_{2} uparrow ) ( boldsymbol{M} stackrel{N}{longrightarrow} boldsymbol{C} boldsymbol{u}+boldsymbol{S} boldsymbol{O}_{2} uparrow ) ( boldsymbol{M} stackrel{N}{longrightarrow} boldsymbol{C} boldsymbol{u}+boldsymbol{S} boldsymbol{O}_{2} uparrow ) A . ( M=C u_{2} O ; N= ) self reduction B. ( M=C u_{2} O+C u_{2} S ; N= ) self reduction c. ( M=C u_{2} O ; N= ) carbon reduction D. ( M=C u_{2} O ; N= ) electrolytic reduction | 11 |
| 95 | In the reaction ( 2 N a_{2} S_{2} O_{3}+I_{2} rightarrow ) ( N a_{2} S_{4} O_{6}+2 N a I, ) the oxidation state of sulphur is : A. decreased B. increased c. unchanged D. none of these | 11 |
| 96 | ( 100 mathrm{mL} ) solution of ( 0.1 mathrm{M} H C l ) was titrated with 0.2 ( N a O H ) solution. The titration was discontinued after the addition of ( 30 mathrm{mL} ) of ( mathrm{NaOH.} ) The remaining titration was completed with the addition of 0.5 M ( K O H . ) The volume of ( K O H ) required for completing the titration is: ( A cdot 8 m L ) в. ( 16 m L ) c. ( 32 m L ) D. ( 64 m L ) | 11 |
| 97 | Which of the following is not a disproportionation reaction? ( mathbf{A} cdot stackrel{ominus}{O} H+B r_{2} longrightarrow B r^{ominus}+B r O_{3}^{mathbf{j}} ) в. ( C u_{2} O+2 H^{oplus} rightarrow C u+C u^{2+}+H_{2} O ) ( mathrm{c} cdot(C N)^{ominus} rightarrow C O_{3}^{2-}+N O_{3}^{circ} ) D ( cdot(C N)_{2}+2 hat{O} H rightarrow C N^{ominus}+C N O^{ominus}+H_{2} O ) | 11 |
| 98 | ( boldsymbol{B} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{4} boldsymbol{C} rightarrow boldsymbol{B} boldsymbol{a} boldsymbol{S}+boldsymbol{4} boldsymbol{C} boldsymbol{O} ) In above reaction, write for each reactant that undergoes oxidation or reduction and identify the type of reaction. | 11 |
| 99 | The reaction of ( K M n O_{4} ) and ( mathrm{HCl} ) results in A. Oxidation of ( mathrm{Mn} ) in ( mathrm{KMnO}_{4} ) and production of ( mathrm{Cl}_{2} ) B. Reduction of Mn in ( K M n O_{4} ) and production of ( H_{2} ) C. Oxidation of ( mathrm{Mn} ) in ( mathrm{KMnO}_{4} ) and production of ( mathrm{H}_{2} ) D. Reduction of Mn in ( K M n O_{4} ) and production of ( C l_{2} ) | 11 |
| 100 | Balance the following equation by oxidation number method. ( A l+K M n O_{4}+H_{2} S O_{4} rightarrow ) ( boldsymbol{A l}_{2}left(boldsymbol{S O}_{4}right)_{3}+boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{M} boldsymbol{n} boldsymbol{S} boldsymbol{O}_{4}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 101 | Determine the oxidation state of Cr in ( left[boldsymbol{C r}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4} boldsymbol{C l}_{2}right] boldsymbol{C l} ) ( A cdot+3 ) B . – – ( c cdot+2 ) ( D cdot+4 ) | 11 |
| 102 | The oxidation number of ( mathrm{N} ) and ( C l ) in ( N O C l O_{4} ) respectively are : ( A cdot+2 ) and +7 B. +3 and +7 ( c cdot-3 ) and +5 D. +2 and -7 | 11 |
| 103 | Oxidation number of ( ^{prime} boldsymbol{N}^{prime} ) in ( boldsymbol{N}_{3} boldsymbol{H} ) (hydrazoic acid) is: ( ^{A} cdot-frac{1}{3} ) B. +3 c. 0 D. – | 11 |
| 104 | ( K M n O_{4} ) reacts with oxalic acid according to the equation ( 2 M n O_{4}^{-}+5 C_{2} O_{4}^{2-}+16 H^{+} rightarrow ) ( mathbf{2} M n^{2+}+mathbf{1 0} C O_{2}+mathbf{8} H_{2} O ) Here ( , 20 m L ) of ( 0.1 mathrm{M} K M n O_{4} ) is This question has multiple correct options | 11 |
| 105 | n ( N i(C O)_{4}, ) the oxidation state of Ni is: ( A cdot 4 ) B. ( c cdot 2 ) D. 8 | 11 |
| 106 | What would be the stoichiometric coefficient of hydrochloric acid in the following equation? ( boldsymbol{C l}_{2}+_{–} boldsymbol{H}_{2} boldsymbol{O} rightarrow_{–} boldsymbol{H} boldsymbol{C l}+_{-} ) ( boldsymbol{H} boldsymbol{C l O}_{3} ) ( A ) B. 3 ( c cdot 5 ) D. 10 | 11 |
| 107 | Balance the following equations by ion electron method. ( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} rightarrow boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{N} boldsymbol{O}_{2}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 108 | Electrolysis of water to form hydrogen and oxygen gases is : A. precipitation B. oxidation-reduction c. distillation D. hydration E. condensation | 11 |
| 109 | The species undergoin disproportionation is: ( mathbf{A} cdot B r O_{4}^{-} ) B. ( B r O_{3}^{-} ) ( mathbf{c} cdot H B r O ) ( mathbf{D} cdot B r ) | 11 |
| 110 | Which of the following is an example of a disproportionation reaction? A. ( C a C O_{3} rightarrow C a O+C O_{2} ) в. ( 2 H C u C l_{2} rightarrow C u+C u^{2+}+4 C l^{-}+2 H^{+} ) c. ( P C l_{5} rightarrow P C l_{3}+C l_{2} ) D. ( 2 H_{2} S+S O_{2} rightarrow 2 H_{2} O+3 S ) | 11 |
| 111 | Sodium chloride and sodium iodide react with concentrated sulfuric acid Which statements are correct? 1. Sodium chloride is not oxidised by concentrated sulfuric acid. 2. No colour change is seen when concentrated sulfuric acid is added to sodium chloride 3. Sodium iodide is oxidised by concentrated sulfuric acid. A. 1,2 and 3 are correct B. 1 and 2 only are correct c. 2 and 3 only are correct D. 1 only is correct | 11 |
| 112 | For decolourisation of 1 mole of acidified ( K M n O_{4} ) the moles of ( H_{2} O_{2} ) required are: A ( cdot 1 / 2 ) B. 3/2 ( c cdot 5 / 2 ) D. 7/2 | 11 |
| 113 | 1 mol of ferric oxalate is oxidised completely by ( x ) mol of ( M n O_{4}^{-} ) in acidic medium. Then, ( x ) is : A . 1.2 в. 1.6 c. 1.8 D. 1.5 | 11 |
| 114 | Balance the following ionic equations (i) ( boldsymbol{C} boldsymbol{r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+boldsymbol{H}^{+}+boldsymbol{I}^{-} rightarrow boldsymbol{C} boldsymbol{r}^{boldsymbol{3}+}+ ) ( boldsymbol{I}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) (ii) ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+boldsymbol{F} boldsymbol{e}_{2}^{+}+boldsymbol{H}^{+} rightarrow boldsymbol{C r}^{3+}+ ) ( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{H}_{2} boldsymbol{O} ) (iii) ( M n O^{4-}+S O_{3}^{2-}+H^{+} rightarrow ) ( M n^{2+}+S O_{4}^{2-}+H_{2} O ) (iv) ( M n O^{4-}+H^{+}+B r^{-} rightarrow M n^{2+}+ ) ( boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 115 | Which of the following will act as anodes when connected to standard hydrogen electrode? This question has multiple correct options ( mathbf{A} cdot A l / A l^{3+} ; quad E^{-}=-1.66 ) ( mathbf{B} cdot F e / F e^{2+} ; quad E^{-}=-0.44 ) ( mathbf{c} cdot C u / C u^{2+} ; quad E^{-}=+0.34 ) D ( cdot F_{2}(g) / 2 F^{-}(a q) ; quad E^{-}=+2.87 ) | 11 |
| 116 | Which of the following is a non-redox process? This question has multiple correct options A ( cdot S O_{4}^{2-} rightarrow S O_{3} ) B. ( C r_{2} O_{7}^{2-} rightarrow C r O_{4}^{2} ) ( mathbf{c} cdot P O_{4}^{3-} rightarrow P_{2} O_{7}^{4} ) ( mathrm{D} cdot C_{2} O_{4}^{-2} rightarrow C O_{2} ) | 11 |
| 117 | When benzaldehyde is oxidised to give benzoic acid then the oxidation state of carbon of aldehydic group is changed from: ( mathbf{A} cdot+2 ) to +3 B. +1 to +3 c. zero to +2 D. No change | 11 |
| 118 | The reaction, ( 3 C l O^{-}(a q) rightarrow C l O_{3}^{-}(a q)+2 C l^{-} ) A. Oxidation reaction B. Reduction reaction c. Disproportionation reaction D. neutralisation reaction | 11 |
| 119 | The number of moles of ( K M n O_{4} ) that will be needed to react completely with one mole of sulphite ion in acidic solution is: A . ( 3 / 5 ) B. 2/5 c. ( 4 / 5 ) ( D ) | 11 |
| 120 | State whether the given statement is true or false. ( X^{2+}+2 e^{-} rightarrow X ) is an example of oxidation. A. True B. False | 11 |
| 121 | Assertion Decomposition of hydrogen peroxide is an example of disproportionation reaction. Reason In a disproportionation reaction, an element in one oxidation state is simultaneously oxidised and reduced. 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 |
| 122 | 2.1 Which of the following is not an example of redox reactions (a) CuO+ H Cu+ H,O (b) Fe,, + 3C0 2 Fe + 300, (c) 2K+F, 2KF (d) BaCl, HSO Baso, + 2HCI | 11 |
| 123 | In the electrochemical series, metals are arranged in order of their tendency to A. release halogens from their salts B. become reduced c. react with water D. lose electrons | 11 |
| 124 | Match the reactions in Column I with nature of the reactions/type of the products in Column II. | 11 |
| 125 | Q. 35 Why does fluorine not show disproportionation reaction? | 11 |
| 126 | Which of the following shows highest oxidation number in combined state? A. ( O s ) в. ( R u ) c. Both (1) & (2) D. None | 11 |
| 127 | In which of the following reactions does ( O_{2} ) acts as an oxidant? This question has multiple correct options ( mathbf{A} cdot 3 O_{2} rightarrow 2 O_{3} ) B. ( 2 F_{2}+O_{2} rightarrow 2 F_{2} ) O c. ( N_{2}+O_{2} rightarrow 2 N O ) D. ( C+O_{2} rightarrow C O_{2} ) | 11 |
| 128 | Which one of the following compounds involve in disproportionation reaction with water? A. ( X e F_{2} ) в. ( X e F_{4} ) c. ( X e F_{6} ) D. ( X e O_{2} F_{2} ) | 11 |
| 129 | The ratio of number of moles of ( K M n O_{4} ) and ( K_{2} C r_{2} O_{7} ) required to oxidise ( 0.1 mathrm{mol} mathrm{Sn}^{+4} ) in acidic medium: A .6: 5 B. 5: 6 c. 1: 2 D. 2: 1 | 11 |
| 130 | Identify from the reaction the reactants that undergo oxidation and reduction ( F e+S rightarrow F e S ) | 11 |
| 131 | Which of the following is a redox reaction? A ( cdot C a C O_{3} rightarrow C a O+C O_{2} ) в. ( H_{2}+C l_{2} rightarrow 2 H C l ) ( mathrm{c} cdot mathrm{CaO}+2 mathrm{HCl} rightarrow mathrm{CaCl}_{2}+mathrm{H}_{2} mathrm{O} ) D. ( N a O H+H C l rightarrow N a C l+H_{2} O ) | 11 |
| 132 | Assertion All the stoichiometric calculations are based on law of conservation of mass. Reason In redox reactions, both oxidation and | 11 |
| 133 | The redox reaction among the following is : ( mathbf{A} cdot ) reaction of ( left[mathrm{Co}left(mathrm{H}_{2} mathrm{O}right)_{6}right] mathrm{Cl}_{3} ) with ( mathrm{AgNO}_{3} ) B. formation of ozone from atmospheric oxygen in the presence of sunlight C. combination of dinitrogen with dioxygen at ( 2000 K ) D. reaction of ( H_{2} S O_{4} ) with ( N a O H ) | 11 |
| 134 | The coefficient of ( boldsymbol{I}^{-}, boldsymbol{I} boldsymbol{O}_{3}^{-} ) and ( boldsymbol{H}^{+} ) in the redox reaction, ( boldsymbol{I}^{-}+boldsymbol{I} boldsymbol{O}_{3}^{-}+boldsymbol{H}^{+} rightarrow ) ( I_{2}+H_{2} O, ) in the balanced form respectively are: ( mathbf{A} cdot 5,1,6 ) в. 1,5,6 c. 6,1,5 D. 5,6,1 | 11 |
| 135 | What is the oxidation number of ( boldsymbol{H} ) and ( C l ) in ( H C l O_{4} ) respectively? ( A cdot+1,+7 ) B. +2,+6 ( mathrm{c} cdot+3,+7 ) ( mathrm{D} cdot+2,+7 ) | 11 |
| 136 | Which of the following show non-zero multiple oxidation state? A . ( S ) B. ( O ) ( c cdot Z n ) D. ( H ) | 11 |
| 137 | Assertion The oxidation state of Cr in ( A l_{2}left(C r_{2} O_{7}right)_{3} ) is +3 Reason As a neutral compound, the sum of the oxidation numbers of all the atoms must equal 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 |
| 138 | Which of the following cell representations is/are correct? This question has multiple correct options ( left.mathbf{A} cdot P l, H_{2}(1 b a r)|H C I(a q)| C l_{2}(1 b a r)right) P t ) B . ( H gleft|H g_{2} C l_{2}(S)right| H C l(a q) mid H_{2}(1 b a r), P t ) ( mathbf{c} cdot A t|A g C l(s)| K C I(a q)left|H g_{2}(s)right| H g ) D ( cdot P t_{3} H_{2}(1 b a r)|H l| A u l(s) mid A mu ) | 11 |
| 139 | Balanced chemical equation imply which of the following? A. Numbers of atoms are conserved in a chemica change B. Numbers of molecules are conserved in a chemica change c. volume is conserved in a chemical change D. ‘A’ and ‘B’ E . ‘B’ and ‘C’ | 11 |
| 140 | Give the oxidation state of underlined. ( N H 4 N O_{3} ) | 11 |
| 141 | The values of coefficients to balance the following reaction are: ( boldsymbol{C r}(boldsymbol{O H})_{3}+boldsymbol{C l O}^{-}+boldsymbol{O H}^{-} rightarrow ) ( boldsymbol{C r} boldsymbol{O}_{4}^{2-}+boldsymbol{C l}^{-}+boldsymbol{H}_{2} boldsymbol{O} ? ) A ( cdot operatorname{Cr}(O H)_{3}-(2), C l O^{-}-(3), C r O_{4}^{2-}-(3), C l^{-}-(3) ) B. ( operatorname{Cr}(O H)_{3}-(2), C l O^{-}-(4), C r O_{4}^{2-}-(3), C l^{-}-(2) ) c. ( operatorname{Cr}(O H)_{3}-(2), operatorname{ClO}^{-}-(4), operatorname{Cr} O_{4}^{2-}-(4), C l^{-}-(2) ) D. ( operatorname{Cr}(O H)_{3}-(2), C l O^{-}-(3), C r O_{4}^{2-}-(2), C l^{-}-(3) ) | 11 |
| 142 | Calculate oxidation number of central ( operatorname{atom} operatorname{in}left[boldsymbol{K}_{4}left[boldsymbol{F} e(boldsymbol{C} boldsymbol{N})_{6}right]right. ) | 11 |
| 143 | When ( S O_{2} ) is passed in acidified potassium dichromate solution, the oxidation number of ( S ) is changed from: ( A cdot+4 ) to zero B. +4 to +2 ( mathbf{c} cdot+4 ) to +6 D. +6 to +4 | 11 |
| 144 | State True or False. The following reaction is a disproportionation reaction. ( N H_{4} N O_{3} stackrel{Delta}{longrightarrow} N_{2} O+2 H_{2} O ) | 11 |
| 145 | Which of the following is redox reaction? ( mathbf{A} cdot N a O H+H C I rightarrow N a C l+H_{2} O ) B. ( A g N O_{3}+K l rightarrow A g l+K N O_{3} ) ( mathbf{c} cdot B a O_{2}+H_{2} S O_{4} rightarrow B a S O_{4}+H_{2} O_{2} ) ( mathbf{D} cdot operatorname{Sn} C l_{2}+H g C l_{2} rightarrow S n C l_{4}+H g ) | 11 |
| 146 | Q. 32 Assertion (A) Redox couple is the combination of oxidised and reduced form of a substance involved in an oxidation or reduction half cell. Reason (R) In the representation 3+ 2+ and Eo2+ Fe / Fe and Cu²+ / Cu are redox couples. (a) Both A and R are true and R is the correct explanation of A T (b) Both A and Rare true but Ris not the correct explanation of A (c) A is true but R is false (d) Both A and Rare false anh MOMA (A) not | 11 |
| 147 | Select Redox reaction from the following: A ( . Z n+C u S O_{4} rightarrow Z n S O_{4}+C u ) в. ( C a O+2 H C l rightarrow C a C l_{2}+H_{2} O ) c. ( N a O H+2 H C l rightarrow N a C l+H_{2} O ) D. ( C a C O_{3} rightarrow C a O+C O_{2} ) | 11 |
| 148 | Which of the following reactions is not a redox reaction? A ( cdot A g^{+}+C l^{-} rightarrow A g C l ) B. ( Z n(s)+C u^{2+}(a q .) rightarrow Z n^{2+}(a q .)+C u(s) ) ( mathrm{c} cdot 2 M g(s)+O_{2}(g) rightarrow 2 M g O ) D. ( F e O+C rightarrow F e+C O ) | 11 |
| 149 | Which is the best description of the behaviour of bromine in the reaction given below? ( boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{B} boldsymbol{r}_{2} rightarrow boldsymbol{H} boldsymbol{O} boldsymbol{B} boldsymbol{r}+boldsymbol{H} boldsymbol{B} boldsymbol{r} ) A. Proton acceptor only B. Both oxidised and reduced c. oxidised only D. Reduced only | 11 |
| 150 | Which of the following statement is TRUE for the electrochemical Daniel cell A. Electron flow from Zinc electrode to copper electrode. B. Current flows from zinc electrode to copper electrode c. cation moves towards copper electrode. D. cation moves towards zinc electrode | 11 |
| 151 | Q. 23 Calculate the oxidation number of each sulphur atom in the following compounds. (a) Na,s,o (b) Na 5.0 (c) Na,SO (d) Na SOA TER | 11 |
| 152 | Complete and balance the following compound ( boldsymbol{S n}+mathbf{2 K O H}+mathbf{4 H}_{mathbf{2}} boldsymbol{O} rightarrow ) ( t ) | 11 |
| 153 | Q14. Define Oxidation and Reduction in terms of oxidation number. | 11 |
| 154 | Q. 36 Write redox couples involved in the reactions (a) to (d) given in question 34. | 11 |
| 155 | What is the oxidation state of ( boldsymbol{T} boldsymbol{h} ) in organometallic compound ( left[T h H O Rleft(C_{5} M e_{5}right)_{2}right] ? ) A ( .+1 ) B. +2 ( c cdot+4 ) D. +3 | 11 |
| 156 | State True or False. In a galvanic cell, reduction occurs at cathode. A. True B. False | 11 |
| 157 | What is the oxidation number for As in the chemical formula for arsenic acid, ( boldsymbol{H}_{3} boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4} ? ) ( A cdot+1 ) ( B .+2 ) ( c cdot+3 ) ( D cdot+4 ) ( E cdot+5 ) | 11 |
| 158 | Which gas is evolved when ( P b O_{2} ) is treated with conc ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ? ) A ( . N O_{2} ) в. ( O_{2} ) c. ( N_{2} ) D. ( N_{2} ) O | 11 |
| 159 | 3. (d) is Consi oxidis Which one of the following is a combination reaction? (a) Formation of a mixture of carbon monoxide and hydrogen. When steam is passed over red hot iron. (b) Reaction of water with sodium metal to form sodium hydroxide and hydrogen. © Ca(OH)2 + Na CO2 — 2NaOH+CaCO3 (d) Preparation of stannic chloride (Tin (iv) chloride) by passing chlorine gas into molten tin (Sn). (a) s (0) 10. Cuo Abo (a) | 11 |
| 160 | Number of peroxy linkage in ( boldsymbol{K}_{3} boldsymbol{C r}left(boldsymbol{O}_{2}right)_{x} ) having oxidation number of ( C r ) as +5 is : | 11 |
| 161 | The oxidation number of iron in ( boldsymbol{F} boldsymbol{e}_{3} boldsymbol{O}_{4} ) is: ( A cdot+2 ) B. +3 ( c cdot frac{8}{3} ) D. ( frac{2}{3} ) | 11 |
| 162 | Reaction of iron filings with powdered sulfur is a ( _{–}- ) – process. A. precipitation B. oxidation-reduction C. distillation D. hydration E. condensation | 11 |
| 163 | f the balanced reaction is as given below, find the value of ( x, y ) and ( z ) ( boldsymbol{C u}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4}^{2+}(boldsymbol{a q})+boldsymbol{S}_{2} boldsymbol{O}_{4}^{2-}(boldsymbol{a q})+ ) ( boldsymbol{x} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{y} boldsymbol{S} boldsymbol{O}_{3}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{C} boldsymbol{u}(boldsymbol{s}) ) ( +z N H_{3}(a q)+2 H_{2} O ) A. ( x=4, y=2, z=4 ) в. ( x=3, y=2, z=3 ) c. ( x=4, y=3, z=4 ) D. None of the above | 11 |
| 164 | ( boldsymbol{S} boldsymbol{i} boldsymbol{O}_{2}(boldsymbol{s})+boldsymbol{N} boldsymbol{a} boldsymbol{O} boldsymbol{H}(boldsymbol{l}) rightarrow boldsymbol{N} boldsymbol{a}_{2} boldsymbol{S} boldsymbol{i} boldsymbol{O}_{3}(boldsymbol{a} boldsymbol{q}) ) ( +? ) A ( cdot H_{2} O(l) ) в. ( H_{2}(g) ) c. ( H_{3} O^{+} ) D. ( O H^{-} ) | 11 |
| 165 | How many moles of electrons are involved in the conversion of 1 mole ( C r_{2} O_{7}^{2-} ) into ( C r^{3+} ) ion? | 11 |
| 166 | Balance the following equation by oxidation number method. ( M n O_{4}^{2-}+H^{+} rightarrow M n O_{2}+ ) ( M n O_{4}^{-}+H_{2} O ) | 11 |
| 167 | Choose the correct statements – This question has multiple correct options ( mathbf{A} cdot C_{2} H_{6}+O_{2} rightarrow C O_{2}+H_{2} O ) is an unbalanced combustion reaction. B. ( 2 H_{2} O_{2} rightarrow 2 H_{2} O+O_{2} ) is a balanced combustion reaction. C ( . A+B C rightarrow A C+B ) represents a single replacement reactions. D. ( H N O_{3}+C a(O H)_{2} rightarrow C aleft(N O_{3}right)_{2}+2 H_{2} O ) is an unbalanced neutralization reaction. | 11 |
| 168 | Which of the following arrangements represent increasing oxidation number of the central atom? A ( cdot C r O_{2}^{-}, C l O_{3}^{-}, C r O_{4}^{2-}, M n O_{4} ) B . ( C l O_{3}^{-}, C r O_{4}^{2-}, M n O_{4}^{-}, C r O_{2}^{-} ) c. ( C r O_{2}^{-}, C l O_{3}^{-}, M n O_{4}^{-}, C r O_{4}^{2} ) D. ( C r O_{4}^{2-}, M n O_{4}^{-}, C r O_{2}^{-}, C l O_{3} ) | 11 |
| 169 | Assertion ( N H_{4} N O_{3} ) undergoes a redox reaction to give ( N_{2} O ) and ( H_{2} O ) Reason It is a disproportionation reaction. 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 |
| 170 | Which of the following statements is correct for oxidation reaction? A. Loss or removal of electron. B. Removal of hydrogen atom. C. Removal or loss of electropositive radical or element D. All the above statements are correct | 11 |
| 171 | The oxidant which cannot act as a reducing agent is : ( A cdot S O_{2} ) в. ( N O_{2} ) ( c cdot C O_{2} ) D. ( C l O_{2} ) | 11 |
| 172 | For the reaction, ( boldsymbol{N} boldsymbol{H}_{3}+boldsymbol{O C l}^{-} rightarrow ) ( N_{2} H_{4}+C l^{-} ) occurring in basic medium, the coefficient of ( N_{2} H_{4} ) in the balanced equation will be : ( mathbf{A} cdot mathbf{1} ) B. 2 ( c cdot 3 ) D. 4 | 11 |
| 173 | ( boldsymbol{C u} boldsymbol{O}+boldsymbol{H}_{2} longrightarrow boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C u}, ) reaction is an example of : A. redox reaction B. synthesis reaction c. neutralisation D. analysis reaction | 11 |
| 174 | What is the oxidation number of ( C l ) in the ( C l O_{3}^{-} ) ion? ( A cdot-1 ) B. +5 ( c cdot-5 ) ( D cdot+7 ) | 11 |
| 175 | Which of the following is a redox reaction? ( mathbf{A} cdot 2 C r O_{4}^{2-}+2 H^{+} rightarrow C r_{2} O_{7}^{2-}+H_{2} O ) В ( cdot quad C u S O_{4}+4 N H_{3} rightarrowleft[C uleft(N H_{3}right)_{4}right] S O_{4} ) ( mathbf{c} cdot N a_{2} S_{2} O_{3}+I_{2} rightarrow N a_{2} S_{4} O_{6}+N a I ) D. ( C r_{2} O_{7}^{2-}+2 O H^{-} rightarrow 2 C r O_{4}^{2-}+H_{2} O ) | 11 |
| 176 | During the oxidation of ( M n^{2+} ) to ( M n O_{4}^{-} ) by ( P b O_{2} ) in acid medium, the number of moles of acid consumed per mole of ( M n^{2+} ) ion is A .4 B. 1/2 ( c cdot 2 ) D. 1/4 | 11 |
| 177 | When ( 6 times 10^{22} ) electrons are used in the electrolysis of a metalic salt, ( 1.9 mathrm{gm} ) of the metal is deposited at the cathode The atomic weight of that metal Is 57 So oxidation state of the metal in the salt is: ( A cdot+2 ) ( B cdot+3 ) ( c cdot+1 ) ( D cdot+4 ) | 11 |
| 178 | In the reaction ( M g+C l_{2} rightarrow M g C l_{2} ) Chlorine may be regarded as: A. an oxidising agent B. a reducing agent c. a catalyst D. providing an inert medium | 11 |
| 179 | Which one of the following reactions is not a redox reaction? A ( cdot I_{2}+2 F e^{2+} rightarrow 2 I^{-}+2 F e^{3+} ) в. ( H C l+N a O H rightarrow N a C l+H_{2} O ) c. ( 2 M g+O_{2} rightarrow 2 M g O ) D. ( Z n+C u^{2+} rightarrow Z n^{2+}+C u ) | 11 |
| 180 | A list of reactions are given below. (a) ( boldsymbol{F e}+mathbf{2 H C l} rightarrow boldsymbol{F e C l}_{2}+boldsymbol{H}_{2} ) (b) ( boldsymbol{F e} boldsymbol{S}+boldsymbol{2} boldsymbol{H} boldsymbol{C l} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{C l}_{2}+boldsymbol{H}_{2} boldsymbol{S} ) (c) ( boldsymbol{F} boldsymbol{e}+boldsymbol{S} stackrel{boldsymbol{Delta}}{longrightarrow} boldsymbol{F} boldsymbol{e} boldsymbol{S} ) (d) ( boldsymbol{N a C l}+boldsymbol{H}_{2} boldsymbol{S O}_{4} stackrel{<200^{circ} boldsymbol{C}}{longrightarrow} ) ( N a H S O_{4}+H C l ) ( (e) C u S O_{4}+H_{2} S rightarrow C u S+H_{2} S O_{4} ) ( (f) S+H_{2} S O_{4} rightarrow 3 S O_{2}+H_{2} O ) Identify redox reactions. ( A cdot a, c ) and ( f ) B. d and f ( c cdot c ) and ( d ) D. c, d and f | 11 |
| 181 | 5. Assertion : A redox reaction involves both oxidation and reduction. Reason: SO, +2H, S — → 2H 0+3S is an example of redox reaction. | 11 |
| 182 | Q4. What is the source of electrical energy in a galvanic cell? | 11 |
| 183 | Which of the followings are correct regarding complexometric titration? A. A titration in which colour is changed due to formation of complex B. Usually occur when d-block elements are involved c. Usually happen when chelating ligands are involved D. All of the above | 11 |
| 184 | Oxidation state of ‘S’ in sodium tetrathionate is : ( mathbf{A} cdot+5,0,0,+5 ) в. +6,+6,0 ( mathbf{c} cdot+4,+2,+5 ) D. +2,0,+2,+3 | 11 |
| 185 | A student prepares for an experiment involving a voltaic cell. Which of the following is needed the least to perform the experiment? A. Burette B. Salt bridge c. Strip of zinc metal D. copper wire E. Solution of zinc sulfate | 11 |
| 186 | Q. 24 Balance the following equations by following equations by the oxidation number method. (a) Fet + H + Cr,0,2 Cr3+ + Fe** + H20 (b) 12 + NO; NO, +10; (c) I, +,0 – +50% (d) MnO2 +0,0% → Mn2+ + CO2 | 11 |
| 187 | In volcanic eruptions, Sulphur undergoes following reaction: ( mathbf{2} boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g})+boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{3} boldsymbol{S}(boldsymbol{s})+mathbf{2} boldsymbol{H}_{2} boldsymbol{O} ) A. Disproportionation B. Comproportionation c. Neutralisation D. Displacement | 11 |
| 188 | How many moles of electrons are needed in the balanced equation for the oxidation of ethanol (1 mol) to acetic ( operatorname{acid} ?left(C_{2} H_{5} O H rightarrow C H_{3} C O O Hright) ) ( mathbf{A} cdot mathbf{1} ) B . 2 ( c .3 ) D. 4 | 11 |
| 189 | An example of oxidation-reduction reaction is: ( mathbf{A} cdot B C l_{3}+C l^{-} rightarrow B C l_{4} ) B. ( H C N+H_{2} O rightarrow H_{3} O^{+}+C N^{-} ) ( mathbf{c} cdot H_{2} O_{2}+2 B r^{-}+2 H^{+} rightarrow 2 H_{2} O+B r_{2} ) D. ( 2 N H_{3}(g) rightarrow N_{2}(g)+3 H_{2}(g) ) | 11 |
| 190 | For the Daniel cell involving the cell reaction ( Z n_{(s)}+C u_{(a q)}^{+2} rightleftharpoons ) ( Z n^{+2}_{(a q)}+C u_{(s)} ) the standard free energies of formation of ( Z n_{(s)}, C u_{(s)} ) ( C u_{(a q)}^{+2} ) and ( Z n_{(a q)}^{+2} ) are 0,0,64.4 KJ/Mole and -154.0 KJ/Mole, respectively. Calculate the standard EMF of the cell? A. 2.13 Volts B. 1.13 Volts c. ( 2.26 mathrm{Volts} ) D. 3.42Volts | 11 |
| 191 | Oxidation state of ( boldsymbol{C r} ) in ( boldsymbol{K}_{3}left[boldsymbol{C r}left(boldsymbol{C}_{2} boldsymbol{O}_{4}right)_{3}right] ) is : | 11 |
| 192 | ( boldsymbol{C H}_{2}=boldsymbol{C H}_{2}+boldsymbol{H}_{2} stackrel{N i}{rightarrow} boldsymbol{C H}_{3}-boldsymbol{C H}_{3} ) is an addition reaction. ( boldsymbol{C H} equiv boldsymbol{C H}+boldsymbol{H}_{2} stackrel{N i}{rightarrow} ? ) Predict and write the products. | 11 |
| 193 | . 12 Which of the following statement(s) is/are not true about the following decomposition reaction? 2KCLO, – 2KCL + 302 (a) Potassium is undergoing oxidation (b) Chlorine is undergoing oxidation S 0591910 (c) Oxygen is reduced (d) None of the species are undergoing oxidation or reduction | 11 |
| 194 | Balance the following equation by ion electron method: ( boldsymbol{A} boldsymbol{s}_{2} boldsymbol{S}_{3}+boldsymbol{N} boldsymbol{O}_{3}^{-}+boldsymbol{H}^{+}+boldsymbol{H}_{2} boldsymbol{O} rightarrow ) ( boldsymbol{H}_{3} boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}+boldsymbol{N} boldsymbol{O}+boldsymbol{S} ) | 11 |
| 195 | Oxygen can show positive oxidation state in its compounds with: A. Fluorine B. Nitrogen c. Hydrogen D. Sulphur | 11 |
| 196 | In the reaction ( boldsymbol{P b O}+boldsymbol{C} rightarrow boldsymbol{P b}+boldsymbol{C O} ) A. ( P b O ) is oxidised B. c acts as oxidising agentt ( c cdot c ) acts as a reducing agent D. This reaction does not represent a redox reaction | 11 |
| 197 | Write the chemical equations to represent the following reactions. The disproportionation of ( mathrm{SnO} ) to ( mathrm{Sn} ) and ( operatorname{Sn} O_{2} ) is ( 2 S n O rightarrow S n+S n O_{2} ) If true enter 1 , else enter 0 | 11 |
| 198 | Assertion For the reaction, ( N a_{2} C O_{3}+H C l rightarrow ) ( N a C l+N a H C O_{3}, ) the suitable indicator is phenolphthalein. Reason Phenolphthalein provides its colour in acidic medium. 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 |
| 199 | The reaction ( boldsymbol{A} boldsymbol{g}^{2+}(boldsymbol{a} boldsymbol{q})+boldsymbol{A} boldsymbol{g}(s) rightarrow ) ( 2 A g^{+}(a q) ) is an example of This question has multiple correct options A. disproportionation B. proportionation c. comproportionation D. symproportionation | 11 |
| 200 | Consider the following reaction: ( boldsymbol{C l}_{2}+boldsymbol{S}^{2-} longrightarrow boldsymbol{S}+boldsymbol{C l}^{-} ) The above reaction is a disproportionation reaction. Is it True or False? Explain why? | 11 |
| 201 | Balance the following equation by oxidation number method. ( Z n+H N O_{3} rightarrow Z nleft(N O_{3}right)_{2}+ ) ( N H_{4} N O_{3}+H_{2} O ) | 11 |
| 202 | Balance the following equation by ion electron method. ( boldsymbol{C o}^{2+}+boldsymbol{N} boldsymbol{O}_{2}^{-}+boldsymbol{H}^{+} rightarrow boldsymbol{C} boldsymbol{o}^{3+}+ ) ( N O+H_{2} O ) | 11 |
| 203 | Fill the blank. ( $ $ 2{text { Ca }}_{-}{3}left{text { lleft }left(P{0}_{-}{4} mid text { right }right)right. ) 3. ( {2}+6 operatorname{si}{0}_{-}{2}+10 C ) lrightarrow ( {P ) ( -{4}+mid ) text ( {-} operatorname{casi}{0}_{-}{3 ) ( 3+10 cos $ ) ( A cdot 2 ) B. 4 ( c .5 ) D. 6 E . 8 | 11 |
| 204 | The oxidation number of ( sin H_{2} S_{2} O_{8} ) is: ( A cdot+2 ) ( B cdot+4 ) ( c cdot+6 ) ( D cdot+7 ) | 11 |
| 205 | In balancing the following half-reaction: ( boldsymbol{C N}^{-} longrightarrow boldsymbol{C N O}^{-}(boldsymbol{s k e l e t a l}), ) the number of electrons that must be added on the right is : | 11 |
| 206 | The oxidation state of the most electronegative element in the products of the reaction between ( B a O_{2} ) and ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) is: A. 0 and -1 B. – – 1 and – 2 c. – – a and o D. – 2 and +1 | 11 |
| 207 | Which of the following is/are autoredox reactions? This question has multiple correct options A ( cdot P_{4}+O H longrightarrow H_{2} P O_{2}^{ominus}+P H_{3} ) B . ( S_{2} O_{3}^{2-} rightarrow S O_{4}^{2-}+S ) ( mathrm{c} cdot mathrm{H}_{2} mathrm{O}_{2} longrightarrow mathrm{H}_{2} mathrm{O}+mathrm{O}_{2} ) D. ( _{A g C l}+N H_{3} rightarrowleft[A gleft(N H_{3}right)_{2}right] C l ) | 11 |
| 208 | Which among the following are intramolecular redox reactions? This question has multiple correct options A. ( P C l_{5} rightarrow P C l_{3}+C l_{2} ) в. ( C H O-C H O+O H^{-} rightarrow C O O^{-}-C H_{2} O H ) c. ( 2 K C l O_{3} rightarrow 2 K C l+3 O_{2} ) D. ( N H_{4} N O_{2} longrightarrow N_{2}+2 H_{2} O ) | 11 |
| 209 | Balance the following below equation. ( boldsymbol{A u}+boldsymbol{N O}_{3}^{-}+boldsymbol{C l}^{-}+boldsymbol{H}^{+} rightarrow boldsymbol{A u} boldsymbol{C l}_{4}^{-}+ ) ( N O_{2}+H_{2} O ) A ( cdot A u+3 N O_{3}^{-}+4 C l^{-}+6 H^{+} rightarrow A u C l_{4}^{-}+3 N O_{2}+ ) ( 3 H_{2} O ) B . ( A u+2 N O_{3}^{-}+5 C l^{-}+8 H^{+} rightarrow A u C l_{4}^{-}+6 N O_{2}+ ) ( 3 H_{2} O ) c. ( A u+4 N O_{3}^{-}+2 C l^{-}+6 H^{+} rightarrow A u C l_{4}^{-}+5 N O_{2}+ ) ( 3 H_{2} O ) D. None of these | 11 |
| 210 | A certain amount of a reducing agent reduces x mole of ( K M n O_{4} ) and y mole of ( K_{2} C r_{2} O_{7} ) in different experiments in acidic medium. If the change in oxidation state in reducing agent is same in both experiments, ( boldsymbol{x}: boldsymbol{y} ) A . 5: 3 B. 3: 5 ( c .5: 6 ) D. 6: 5 | 11 |
| 211 | In which of the following reactions there is a change in the oxidation number of nitrogen atom? A ( .2 N O_{2} rightarrow N_{2} O_{4} ) B. ( N H_{3}+4 N H_{3} rightarrowleft[C uleft(N H_{3}right)_{4}right] S O_{4} ) c. ( 2 N a_{2} S_{2} O_{3}+I_{2} rightarrow N a_{2} S_{4} O_{6}+2 N a I ) D. None of these | 11 |
| 212 | Which of the following involves reduction? A. conversion of an anion to atom B. conversion of a cation to atom c. both these D. none of these | 11 |
| 213 | Balance the following equation by ion electron method. ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{H}^{+}+boldsymbol{C}_{2} boldsymbol{O}_{4}^{2-} rightarrow boldsymbol{C r}^{3+}+ ) ( boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 214 | In which compound among the following, carbon has a zero oxidation state? A ( . C H_{4} ) в. ( C H_{3} C l ) c. ( C H_{2} C l_{2} ) D. ( C C l_{4} ) | 11 |
| 215 | Find the sum of the coefficients when given equation is balanced. ( boldsymbol{A l}_{2}left(boldsymbol{S O}_{4}right)_{3}+boldsymbol{C a}(boldsymbol{O H})_{2} rightarrow boldsymbol{A l}(boldsymbol{O H})_{3}+ ) ( boldsymbol{C} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4} ) A . 5 B. 6 ( c cdot 7 ) D. 8 E . 9 | 11 |
| 216 | 0.29 Assertion (A) Among halogens fluorine is the best oxidant. Reason (R) Fluorine is the most electronegative atom. (a) Both A and Rare 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) Both A and Rare false h otanden otru but recon is not the corrent oynlanation of | 11 |
| 217 | When ( K M n O_{4} ) act as an oxidising agent and ultimately form ( M n O_{4}^{2-}, M n O_{2}, M n_{2} O_{3} ) and ( M n^{2+} ) then the numbers of electrons transferred in each case, respectively, are : A .4,3,1,5 B. 1, 5, 3, 7 ( c cdot 1,3,4,5 ) D. 3, 5, 7, | 11 |
| 218 | The oxidation state of the underlined element in the given compound is: ( B a_{2} X e O_{2} ) ( A cdot+2 ) ( B cdot+3 ) ( c cdot+4 ) D. | 11 |
| 219 | On the basis of the following ( E^{o} ) values, the strongest oxidising agent is: ( left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right]^{4-} longrightarrowleft[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right]^{boldsymbol{3}+}+ ) ( boldsymbol{e}^{-}, boldsymbol{E}^{o}=-mathbf{0 . 3 5} boldsymbol{V} ) ( boldsymbol{F} boldsymbol{e}^{2+} rightarrow boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{e}^{-1} ) ( boldsymbol{F} boldsymbol{e}^{2+} rightarrow boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{e}^{-1} ; boldsymbol{E}^{boldsymbol{o}}=-boldsymbol{0 . 7 7} boldsymbol{V} ) A ( cdot F e^{3} ) в. ( left[F e(C N)_{6}right]^{3-} ) ( mathrm{c} cdotleft[mathrm{Fe}(mathrm{CN})_{6}right]^{4} ) D. ( F e^{2} ) | 11 |
| 220 | Total number of electrons involved per molecule in the oxidation of ( F e C_{2} O_{4} ) to ( F e^{3+} ) and ( C O_{2} ) is : ( mathbf{A} cdot mathbf{3} ) B. 2 ( c cdot 4 ) D. none of these | 11 |
| 221 | The following reaction is an example of ( a: ) ( mathbf{4} boldsymbol{N} boldsymbol{H}_{3}(boldsymbol{g})+mathbf{5} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{4} boldsymbol{N} boldsymbol{O}(boldsymbol{g})+ ) ( mathbf{6} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ) (i) displacement reaction (ii) combination reaction (iii) redox reaction (iv) neutralisation reaction ( A ). (i) and (iv) B. (ii) and (iii) c. (i) and (iii) D. (iii) and (iv) | 11 |
| 222 | “In moist air, copper corrodes to produce a green layer on the surface”. For this, the reaction is : ( boldsymbol{C u}+boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C O}_{2}+boldsymbol{O}_{2} rightarrow boldsymbol{C u} boldsymbol{C O}_{3} ) ( boldsymbol{C u}(boldsymbol{O} boldsymbol{H})_{2} ) If the statement is true enter 1 else enter 0 | 11 |
| 223 | Redox reactions are reactions during which electron transfer takes place. Here magnesium atom transfers two electrons one each to the two chlorine atoms i) What are the products of this reaction? ii) Write the balanced equation for the complete reaction. iii) Which element is being oxidized? iv) Which element is being reduced? v) Write the reduction part of the reaction? | 11 |
| 224 | Write balanced net ionic equation for the following reaction in acidic solution ( boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4}(boldsymbol{a} boldsymbol{q})+boldsymbol{A} boldsymbol{s}_{4}(boldsymbol{s})+boldsymbol{P} boldsymbol{b}_{3} boldsymbol{O}_{4}(boldsymbol{s}) rightarrow ) ( boldsymbol{P b S O}_{4}(boldsymbol{s})+boldsymbol{H}_{2} boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}^{-}(boldsymbol{a} boldsymbol{q}) ) | 11 |
| 225 | The tendency of two species to disproportionate can be determined by examining the: A. Phase diagram B. Volume vs Temperature graph c. Frost diagram D. Heat capacity vsTemperature graph | 11 |
| 226 | Chlorine is in +1 oxidation state in: A. нс B. ( mathrm{HClO}_{4} ) c. ( A & B ) both D. none of these | 11 |
| 227 | Q. 11 Which of the following elements does not show disproportionation tendency? (a) CI (b) Br (d) I teagency. (b) B (c) F | 11 |
| 228 | Balance the following equation: ( N H_{3}+O_{2} rightarrow N O+H_{2} O ) | 11 |
| 229 | When ( H_{2} S ) is passed into aqueous ( S O_{2} ) ( mathbf{A} cdot H_{2} S ) is converted to yellow precipitate of sulphur. B. ( S O_{2} ) is converted to yellow precipitate of sulphur. C . a clear solution of ( H_{2} S O_{4} ) is formed. D. ( S O_{2} ) as well as ( H_{2} S ) are converted into a yellow precipitate of sulphur | 11 |
| 230 | Balance the following equation. ( boldsymbol{P}_{2} boldsymbol{H}_{4} rightarrow boldsymbol{P} boldsymbol{H}_{3}+boldsymbol{P}_{4} boldsymbol{H}_{2} ) | 11 |
| 231 | . 6 The oxidation number of an element in a compound is evaluated on the basis of certain rules. Which of the following is incorrect in this respect? (a) The oxidation number of hydrogen is always +1 (b) The algebraic sum of all the oxidation numbers in a compound is zero (c) An element in the free or the uncombined state bears oxidation number zero (d) In all its compounds, the oxidation number of fluorine is -1 | 11 |
| 232 | Which of the following reaction shows reduction of water? A ( cdot 2 H_{2} O+2 N a rightarrow 2 N a O H+H_{2} ) B ( cdot 6 C O_{2}+12 H_{2} O rightarrow C_{6} H_{1} 2 O_{6}+6 H_{2} O+6 O_{2} ) ( mathbf{c} cdot 2 F_{2}+2 H_{2} O rightarrow 4 H^{+}+4 F^{-}+O_{2} ) D. ( P_{4} O_{1} 0+6 H_{2} O rightarrow 4 H_{3} P O_{4} ) | 11 |
| 233 | Reaction of iron filings with powered sulfur is known as: A. precipitation B. oxidation-reduction c. distillation D. hydration E. condensation | 11 |
| 234 | Which of the following species are oxidised and reduced in the following (unbalanced) reaction? ( boldsymbol{C}+boldsymbol{Z} boldsymbol{n} boldsymbol{O} longrightarrow boldsymbol{Z} boldsymbol{n}+boldsymbol{C O} ) A. zno Reduced ; c Oxidizedd B. c Reduced ; zno Oxidizedd c. Neither of them reduced or oxidized D. None of the above | 11 |
| 235 | What product is formed when cyclohexanone is oxidised? A. НООС( cdotleft(C H_{2}right)_{4} cdot )СООН в. ( C H_{3} C H_{2} C O O H ) c. ( C H_{3}left(C H_{2}right)_{4} cdot C O O H ) D. None of the above | 11 |
| 236 | The reaction ( : Z n^{2+}(a q)+ ) ( mathbf{2} e^{-} rightarrow boldsymbol{Z} boldsymbol{n} ) ( (s) ) has a electrode potential of ( 0.76 V ) This means: | 11 |
| 237 | In the reaction: ( 2 F e C l_{2}+C l_{2} rightarrow 2 F e C l_{3} ) Chlorine may be regarded as: A. an oxidising agent B. a reducing agent c. a catalyst D. providing an inert medium | 11 |
| 238 | Which of these reactions are redox reactions? ( 16 N O(g)+4 N H_{3}(g) rightarrow 5 N_{2}(g)+ ) ( mathbf{6} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) ( 22 S O_{2}(g)+O_{2}(g) rightarrow 2 S O_{3}(g) ) 3. ( boldsymbol{S O}_{3}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightarrow boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}(boldsymbol{g}) ) A .1,2 and 3 are correct B. 1 and 2 only are correct c. 2 and 3 only are correct D. 1 only is correct | 11 |
| 239 | Balance the given below reaction ( boldsymbol{x} boldsymbol{A} boldsymbol{s}_{2} boldsymbol{S}_{3}+boldsymbol{y} boldsymbol{N} boldsymbol{a} boldsymbol{O} boldsymbol{H}+boldsymbol{z} boldsymbol{N} boldsymbol{a} boldsymbol{C l} boldsymbol{O}_{3} rightarrow ) ( boldsymbol{a} boldsymbol{N} boldsymbol{a}_{3} boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}+boldsymbol{b} boldsymbol{N} boldsymbol{a}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{c} boldsymbol{N} boldsymbol{a} boldsymbol{C l O}+ ) ( d H_{2} O ) Calculate the value of ( (x-y+z+a) ) b+c), when the molar coefficient are in simplest whole number ratio. | 11 |
| 240 | TEL is a compound used as: ( A ). antibiotic B. antiswptic c. antiknocking D. antioxidant | 11 |
| 241 | Which of the following is an example of oxidation? A ( cdot S n^{+2}-2 e^{-} rightarrow S n^{+} ) B. ( F e^{+3}+e^{-} rightarrow F e^{+} ) c. ( C l_{2}+2 e^{-} rightarrow 2 C l ) D. None of the above | 11 |
| 242 | Which of the following statement is correct for a galvanic cell? A. Reduction occurs at cathode B. Oxidation occurs at anode c. Electrons flow anode to cathode D. All the statements are correct | 11 |
| 243 | Balance the following redox reaction ( M n O_{4}^{ominus}(a q)+I^{ominus}(a q) rightarrow M n O_{2}(s)+ ) ( boldsymbol{I}_{2}(boldsymbol{s}) ) What is the coefficient of ( boldsymbol{I}^{-} ) ? | 11 |
| 244 | Oxidation number of sodium in sodium amalgam is: ( A cdot+2 ) B. +1 ( c cdot-2 ) D. zero | 11 |
| 245 | Sodium forms an oxide containing one oxygen atom for every two atoms of sodium. What is the coefficient of sodium in the balanced equation for the reaction of sodium with oxygen to form this oxide? ( mathbf{A} cdot mathbf{0} ) B. 1 c. 2 D. 3 ( E .4 ) | 11 |
| 246 | Consider the reaction: ( C l_{2}+2 K I rightarrow ) ( boldsymbol{I}_{2}+2 boldsymbol{K} boldsymbol{C l} ) Which species will be reduced at the cathode? A ( cdot C l_{2} ) В. ( I_{2} ) c. ( I^{-} ) D. ( C l ) | 11 |
| 247 | Balance the following equations by oxidation number method. ( boldsymbol{K} boldsymbol{I}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{I}_{2}+boldsymbol{S} boldsymbol{O}_{2}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 248 | ( F e^{2+} ) is oxidised by ( M n O_{4}^{-} ) or ( C r_{2} O_{7}^{2-} ) in acidic medium. What is new oxidation number of Fe? ( A cdot+3 ) B. +1 ( c cdot+2 ) D. +4 | 11 |
| 249 | Which of the following is a redox reaction? ( mathbf{A} cdot N a C l+K N O_{3} rightarrow N a N O_{3}+K C l ) B ( cdot C a C_{2} O_{4}+2 H C l rightarrow C a C l_{2}+H_{2} C_{2} O_{4} ) ( mathbf{c} cdot M g(O H)_{2}+2 N H_{4} C l rightarrow M g C l_{2}+2 N H_{4} O H ) ( mathbf{D} cdot Z n+2 A g C N rightarrow 2 A g+Z n(C N)_{2} ) | 11 |
| 250 | In the redox reaction: ( boldsymbol{x} boldsymbol{M} boldsymbol{n} boldsymbol{O}+ ) ( boldsymbol{y} boldsymbol{P} boldsymbol{b} boldsymbol{O}_{2}+boldsymbol{z} boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} rightarrow boldsymbol{H} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}+ ) ( boldsymbol{P b}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}+boldsymbol{H}_{2} boldsymbol{O} ) A. ( x=2, y=5, z=10 ) в. ( x=2, y=7, z=8 ) c. ( x=2, y=5, z=8 ) D. ( x=2, y=5, z=5 ) | 11 |
| 251 | What would be the stoichiometric coefficient of hydrochloric acid in the following equation? ( -C l_{2}+_{-} H_{2} O rightarrow_{-} H C l+_{-} H C l O_{3} ) A . 1 B. 3 c. 5 D. 10 | 11 |
| 252 | 0.37 Find out the oxidation number of chlorine in the following compounds and arrange them in increasing order of oxidation number of chlorine. NaClO4, NaClO3, NaClO, KCLO, C120,, CLO3, C120, NaCl, Cl2, CLO2. Which oxidation state is not present in any of the above compounds? | 11 |
| 253 | Consider the following reaction: ( boldsymbol{x} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-}+boldsymbol{y} boldsymbol{C}_{2} boldsymbol{O}_{4}^{2-}+boldsymbol{z} boldsymbol{H}^{+} rightarrow ) ( boldsymbol{x} boldsymbol{M} boldsymbol{n}^{2+}+mathbf{2} boldsymbol{y} boldsymbol{C} boldsymbol{O}_{2}+frac{boldsymbol{z}}{2} boldsymbol{H}_{2} boldsymbol{O} . ) The values of ( x, y ) and ( z ) in the reaction are, respectively: A .2,5 and 16 B. 5,2 and 8 c. 5,2 and 16 D. 2,5 and 8 | 11 |
| 254 | In the electrochemical cell: ( Z nleft|Z n S O_{4}(0.01 M)right|left|C u S O_{4}(1.0 M)right| C ) the emf of this Daniel cell is ( E_{1} . ) When the concentration of ( Z n S O_{4} ) is changed to ( 1.0 M ) and that of ( C u S O_{4} ) changed to ( mathbf{0 . 0 1} boldsymbol{M}, ) the emf changes to ( boldsymbol{E}_{2} . ) From the followings, which one is the relationship between ( boldsymbol{E}_{1} ) and ( boldsymbol{E}_{2} ? ) (Given, ( left.frac{boldsymbol{R T}}{boldsymbol{F}}=mathbf{0 . 0 5 9}right) ) A ( . E_{2}=0 neq E_{1} ) B ( . E_{1}=E_{2} ) c. ( E_{1}E_{2} ) | 11 |
| 255 | Which of the following does not exist? This question has multiple correct options ( A cdot H S_{6} ) B. ( mathrm{HPO}_{4} ) ( mathbf{c} cdot ) Fel ( _{3} ) D. ( mathrm{HClO}_{4} ) | 11 |
| 256 | The process of reduction involves: A. removal of hydrogen B. gain of electrons C. addition of oxygen D. loss of electrons | 11 |
| 257 | One of the fuel cells uses the reaction of hydrogen and oxygen to form water. Write down the cell reaction taking place in the anode and cathode of that fuel cell. | 11 |
| 258 | Find the oxidation and reduction process for the following reaction: ( boldsymbol{C H}_{2}=boldsymbol{C H}_{2}+boldsymbol{H}_{2} rightarrow boldsymbol{C H}_{3}-boldsymbol{C H}_{3} ) | 11 |
| 259 | Change of orange color of chromium(VI) to green color of chromium(III) indicates presence of a: A. reducing agent B. oxidizing agent c. reagent D. drying agent | 11 |
| 260 | The oxidation number of underlined element in ( underline{M} boldsymbol{n}_{3} boldsymbol{O}_{4} ) compound is : ( A cdot frac{8}{3} ) B. ( frac{7}{3} ) ( c cdot frac{8}{5} ) D. none of these | 11 |
| 261 | True statements for the chemical reaction of the formation of lithium oxide is: ( 4 L i(s)+O_{2}(g) rightarrow 2 L i_{2} O(s) ) A. lithium metal is the oxidizing agent B. oxygen gas is the reducing agent c. lithium is oxidized D. oxygen is oxidized E. oxygen loses two electrons to become ( O^{-2} ) ion | 11 |
| 262 | In the reaction ( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{C l}_{2} rightarrow boldsymbol{2} boldsymbol{H} boldsymbol{C l}+ ) ( S, ) the oxidizing agent is : A ( . H_{2} ) в. ( C l_{2} ) c. ( H C l ) D. ( S ) | 11 |
| 263 | In the reaction of ( H I ) with ( H_{2} S O_{4} ) the oxidation state of sulphur is changed to -2. Identify the correct balanced equation A ( cdot H_{2} S O_{4}+2 H I rightarrow S O_{2}+2 H_{2} O+I_{2} ) в. ( H_{2} S O_{4}+6 H I rightarrow S+4 H_{2} O+3 I_{2} ) c. ( H_{2} S O_{4}+8 H I rightarrow H_{2} S+4 H_{2} O+4 I_{2} ) D. All of the above | 11 |
| 264 | Give two examples for oxidation reduction reaction | 11 |
| 265 | Photographic paper is developed with alkaline hydroquinone Select correct statement A. Hydroquinone is the oxidant B. ( A g^{+} ) is the oxidant ( mathrm{c} cdot B r^{-} ) is the oxidant D. ( A g^{+} ) is the reductant | 11 |
| 266 | Two elements combine to form one compound in a displacement reaction. A. True B. False | 11 |
| 267 | If true enter 1 , else enter 0 . ( H C H O ) disproportionates in presence of ( boldsymbol{O} boldsymbol{H}^{-} ) ( A ) | 11 |
| 268 | In Ostwald’s process for the manufacture of nitric acid, the first step involves the oxidation of ammonia gas by oxygen gas to give nitric oxide gas and steam. What is the maximum weight of nitric oxide that can be obtained starting only with 10.00 g. of ammonia and 20.00 g of oxygen? | 11 |
| 269 | When ferrous oxalte is titrated against ( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7} ) m eq. of ( boldsymbol{F} boldsymbol{e}^{2+}, boldsymbol{C}_{2} boldsymbol{O}_{4}^{2-} ) and ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-} ) in the redox reaction are ( boldsymbol{X}, boldsymbol{Y} ) and ( Z ) respectively, then:- A ( . X=Y ) в. ( X+Y=Z ) c. ( X+2 Y=Z ) D. ( 2 X+6 Y+6 Z ) | 11 |
| 270 | 32. Browning of paper in books is caused by (1) frequent use (2) lack of aeration (3) collection of dust (4) oxidation of cellulose | 11 |
| 271 | (a) Give one example of redox reaction. (b) Draw the labelled diagram of electrolytic decomposition of water | 11 |
| 272 | What occurs most often in nature: oxidation or reduction? A. Oxidation. B. Reduction. c. Both occur equally D. Depends on the scenario | 11 |
| 273 | Which of the following oxoacid of phosphorous does not disproportionate? A ( . H_{3} P O_{2} ) в. ( H_{3} P O_{4} ) c. ( H_{3} P O_{3} ) D. All of these | 11 |
| 274 | An element, which never as a positive oxidation state in any of its compounds is: A. boron B. oxygen c. chlorine D. fluorine | 11 |
| 275 | If the balanced reaction is as given below, find the value of ( x, y ) and ( z ) ( boldsymbol{T} boldsymbol{i}_{2} boldsymbol{O}_{3}(boldsymbol{s})+boldsymbol{x} boldsymbol{N} boldsymbol{H}_{2} boldsymbol{O} boldsymbol{H}(boldsymbol{a} boldsymbol{q}) rightarrow ) ( 2 T i O H(s)+y N_{2}(g)+z H_{2} O ) A. ( x=4, y=2, z=5 ) в. ( x=3, y=2, z=5 ) c. ( x=4, y=2, z=4 ) D. None of the above | 11 |
| 276 | The oxidation number of phosphorus in ( boldsymbol{B} boldsymbol{a}left(boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{2}right)_{2} ) is: ( A cdot+3 ) B. +2 ( c cdot+1 ) D. – | 11 |
| 277 | Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction. ( boldsymbol{H} boldsymbol{C H O}_{(l)}+mathbf{2}left[boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}right]_{(a q)}^{+}+ ) ( mathbf{3} boldsymbol{O} boldsymbol{H}_{(boldsymbol{a q})}^{-} rightarrow mathbf{2} boldsymbol{A} boldsymbol{g}_{(s)}+boldsymbol{H} boldsymbol{C O O}_{(boldsymbol{a q})}^{-}+ ) ( mathbf{4} boldsymbol{N} boldsymbol{H}_{3(a q)}+mathbf{2} boldsymbol{H}_{2} boldsymbol{O}_{(l)} ) | 11 |
| 278 | Write half-reactions using electrons. ( boldsymbol{C r}_{2} boldsymbol{O}_{2}^{boldsymbol{7}-}+boldsymbol{6} boldsymbol{F} boldsymbol{e}^{boldsymbol{2}+}+mathbf{1 4} boldsymbol{H}^{+} longrightarrow ) ( 2 C r^{3+}+6 F e^{3+}+7 H_{2} O ) A. Oxidation : ( F e^{2+} longrightarrow F e^{3+}+e^{-} ); Reduction: [ C r_{2} O_{2}^{7-}+14 H^{+}+6 e^{-} longrightarrow 2 C r^{2+}+7 H_{2} O ] B. Oxidation: ( 3 F e^{2+} longrightarrow 3 F e^{3+}+e^{-} ); Reduction: ( mathrm{Cr}_{2} mathrm{O}_{2}^{7-}+14 mathrm{H}^{+}+6 e^{-} longrightarrow 2 mathrm{Cr}^{2+}+7 mathrm{H}_{2} mathrm{O} ) C. Oxidation : ( 2 F e^{2+} longrightarrow 2 F e^{3+}+e^{-} ); Reduction: ( mathrm{Cr}_{2} mathrm{O}_{2}^{7-}+14 mathrm{H}^{+}+6 e^{-} longrightarrow 2 mathrm{Cr}^{2+}+7 mathrm{H}_{2} mathrm{O} ) D. Oxidation: ( 3 F e^{2+} longrightarrow F e^{3+}+3 e^{-} ; ) Reduction : ( C r_{2} O_{2}^{7-}+14 H^{+}+3 e^{-} longrightarrow 2 C r^{2+}+7 H_{2} O ) | 11 |
| 279 | Select the oxidant in the given reactions. ( boldsymbol{K} boldsymbol{I} boldsymbol{O}_{3}+boldsymbol{5} boldsymbol{K} boldsymbol{I}+boldsymbol{6} boldsymbol{H} boldsymbol{C l} rightarrow boldsymbol{3} boldsymbol{I}_{2}+ ) ( 6 K C l+3 H_{2} O ) | 11 |
| 280 | Which element among the following will not have an oxidation number of ( -1 ? ) A. ( F ) in ( H F ) B. ( C l ) in ( N a C l ) ( c cdot O operatorname{in} H_{2} O_{2} ) D. ( F ) in ( N a F ) E ( . H ) in ( N a_{2} H P O_{4} ) | 11 |
| 281 | Which of the following is a decomposition reaction? ( mathbf{A} cdot 3 N a(s)+F e B r_{3}(a q) rightarrow 3 N a B r(a q)+F e(s) ) B. ( N a O H(a q)+H N O_{3}(a q) rightarrow N a N O_{3}(a q)+H_{2} O(l) ) ( mathbf{c} cdot 2 N a H C O_{3}(s) rightarrow N a_{2} C O_{3}(s)+C O_{2}(g)+H_{2} O(l) ) D. ( 3 H_{2}(g)+N_{2}(g) rightarrow 2 N H_{3}(g) ) | 11 |
| 282 | When ( mathrm{K}_{2} mathrm{Cr}_{2} mathrm{O}_{7} ) is converted into ( mathrm{K}_{2} mathrm{Cr} mathrm{O}_{4}, ) the change in oxidation number of Cr is A . B. 6 ( c cdot 4 ) D. 3 | 11 |
| 283 | State the type of chemical reaction involved in given reaction, a] Calcium + oxygen ( rightarrow ) Calcium oxide A. Displacement Reactions B. Decomposition Reactions c. combination Reactions D. Neutralization Reactions | 11 |
| 284 | 1 9. Consider the following reaction and tell which one is the oxidising reagent. SO2 +2H2S → 2H 0+3S (a) SOM (b) HAS (c) H2O (d) S So, *211,5 2,0 | 11 |
| 285 | The elements undergoing reduction and oxidation during the reaction, ( left(N H_{4}right)_{2} C r_{2} O_{7} rightarrow N_{2}+C r_{2} O_{3}+ ) ( 4 H_{2} O ) are respectively: ( A cdot N ) and ( C r ) B. Crand N c. ( mathrm{N} ) and 0 D. Crand 0 | 11 |
| 286 | The reaction, ( 2 H_{2} O(l) rightarrow 4 H^{+}(a q .)+ ) ( O_{2}(g)+4 e^{-} ) is? A. A oxidation reaction B. A hydrolysis reaction C. A solvolysis reaction D. An oscillatory reaction E. An acid catalyst reaction | 11 |
| 287 | The missing term in the following equation is ( 2 F e^{3+}+S n^{2+} rightarrow 2 F e^{2+}+ ) ( ldots . ? ) ( A cdot S n^{4} ) в. ( S n^{3} ) ( c cdot s n^{2} ) D. ( S n^{+} ) | 11 |
| 288 | Q. 27 Match Column I with Column II for the oxidation states of the central atoms. Column 1 Column II CrO B. Mno 2 4 C VO D. Fef- А. +3 | 11 |
| 289 | ( A l+M n O_{4}^{-} rightarrow A l(O H)_{4}^{-}+M n O_{2} ) For this reaction the oxidation state of ( A l ) and ( M n ) in the product are respectively: ( mathbf{A} cdot+3 a n d+4 ) B. +4 and +4 c. +3 and +7 D. +2 and +4 | 11 |
| 290 | Write the name of the cell which is generally used in transistors. Write the reactions taking place at the anode and the cathode of this cell. | 11 |
| 291 | Oxidation state of oxygen in hydrogen peroxide is? A . – B. +1 ( c cdot 0 ) ( D cdot-2 ) | 11 |
| 292 | Q21. The Mn+ ion is unstable in solution and undergoes disproportionation to give Mn2+, MnO2 and H ion. Write a balanced ionic equation for the reaction. 1 1 1 | 11 |
| 293 | A dilute Ferrous sulphate solution was gradually added to the beaker containing acidified permanganate solution. The light purple colour of the solution fades and finally disappears. Which of the following is the correct explanation for the observation? A. ( K M n O_{4} ) is an oxidizing agent, it oxidizes ( F e S O_{4} ) B. ( F e S O_{4} ) acts as an oxidizing agent and oxidizes ( K M n O_{4} ) c. The colour disappears due to dilution: no reaction is involved D. ( K M n O_{4} ) is an unstable compound and decompose presence of ( F e S O_{4} ) to a colourless compound | 11 |
| 294 | In the ethylene molecule the two carbon atoms have the oxidation numbers. A . -1,-1 в. -2,-2 c. -1,-2 D. +2,-2 | 11 |
| 295 | Reducing agents does not include: A. chlorine B. carbon c. potassium iodide D. carbon monoxide | 11 |
| 296 | Which of the following reactions is/are disproportionation reaction(s)? This question has multiple correct options A ( cdot C l_{2}+2 stackrel{ominus}{O} H rightarrow C l^{ominus}+C l O^{ominus}+H_{2} O ) в. ( 2 H C u C l_{2} rightarrow C u+C u^{2+}+4 C l^{ominus}+2 H^{oplus} ) c. ( _{H C H O}+stackrel{ominus}{O H} longrightarrow C H_{3} O H+H C O O^{circ} ) D. ( M g C O_{3} rightarrow M g O+C O_{2} ) | 11 |
| 297 | Complete and balance the following compound. Acidic solution of ( F e^{2+} ) ion gives a brown ring when it comes in contact with ( N O^{-} 3 ) ion. Complete the following reaction of this process. [ begin{array}{l} {left[boldsymbol{F e}left(boldsymbol{H}_{2} boldsymbol{O}right)_{6}right]^{2+}+boldsymbol{N} boldsymbol{O}_{3}^{-}+boldsymbol{H}^{+} rightarrow} \ ——+left[boldsymbol{F} eleft(boldsymbol{H}_{2} boldsymbol{O}right)_{6}right]^{3+}+boldsymbol{H}_{2} boldsymbol{O} end{array} ] | 11 |
| 298 | What are the oxidation number of the underlined elements in ( underline{C} boldsymbol{H}_{3} underline{boldsymbol{C}} boldsymbol{O} boldsymbol{O} boldsymbol{H} ) | 11 |
| 299 | Which of the following is true of oxidation-reduction reactions? A. The reducing agent is reduced at the cathode. B. The oxidizing agent is oxidized at the anode. C. The oxidizing agent is reduced at the cathode. D. The reducing agent is oxidized at the cathode. | 11 |
| 300 | Hydrogen gas will reduce: A. hot cupric oxide B. hot ferric oxide c. hot stanic oxide D. hot aluminium oxide | 11 |
| 301 | In the reaction, ( boldsymbol{C u}(boldsymbol{s})+boldsymbol{2} boldsymbol{A} boldsymbol{g}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow ) ( boldsymbol{C u}^{2+}+mathbf{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s}) ) A ( cdot ) cu(s) is oxidised to ( C u^{2} ) B. ( operatorname{Cu}(mathrm{s}) ) reduced to ( C u^{2+}(a q) ) c. ( operatorname{Ag} ) (aq) is oxidised to ( mathrm{Ag} ) (s) D. Both Cu(s) and ( A g^{+} ) (aq) are oxidised | 11 |
| 302 | Calculate the oxidation no. of sulphur in ( boldsymbol{H}_{2} underline{boldsymbol{S}}_{4} boldsymbol{O}_{boldsymbol{6}} ) | 11 |
| 303 | What is the oxidation number of carbon in carbon suboxide ( left(C_{3} O_{2}right) ? ) | 11 |
| 304 | Q Type your question appropriate choice. Column I 11 ( (A) ) [ begin{array}{l} left.3 M g_{(} sright)+ \ N_{2(g)} stackrel{Delta}{longrightarrow} quad(i) quad text { Displacement } end{array} ] ( N_{2}(g) longrightarrow ) ( M g_{3} N_{2(s)} ) [ begin{array}{l} left.N a H_{(} sright)+ \ left.H_{2} O_{(} lright) rightarrow end{array} ] ( (B) ) [ N a O H_{(a q)}+ ] ( (i i) ) Decomposition ( H_{2(g)} ) [ 3 C l O_{(a q)}^{-} rightarrow ] ( (C) ) ( 2 C l_{(a q)}^{-}+ ) ( (i i i) ) Combination ( mathrm{ClO}^{-}_{(a q)} ) [ 2 K C l O_{3(s)} rightarrow ] ( (D) ) ( left.2 K C l_{(} sright)+ ) ( (i v) ) Disproportiona ( 3 O_{2(g)} ) ( mathbf{A} cdot(A) rightarrow(i),(B) rightarrow(i i i),(C) rightarrow(i i), D rightarrow(i v) ) B ( .(A) rightarrow(i v),(B) rightarrow(i i i),(C) rightarrow(i i), D rightarrow(i) ) ( mathbf{c} cdot(A) rightarrow(i i),(B) rightarrow(i),(C) rightarrow(i i i), D rightarrow(i v) ) ( mathbf{D} cdot(A) rightarrow(i i i),(B) rightarrow(i),(C) rightarrow(i v), D rightarrow(i i) ) | 11 |
| 305 | State whether the given statement is true or false: Combination is the reverse of decomposition reaction A. True B. False | 11 |
| 306 | What do you mean by oxidation and reduction? | 11 |
| 307 | ( mathrm{Cu}(s)+mathrm{NO}_{3}^{-}(a q)+mathrm{H}^{+}(a q) rightarrow mathrm{Cu}^{2+}(a q) ) ( +mathrm{NO}_{2}(g)+mathrm{H}_{2} mathrm{O}(1) ) If the above equation is balanced with lowest whole number coefficients, find the coefficient for ( mathrm{H}+(mathrm{aq}) ) A B. 2 ( c cdot 3 ) D. 4 E. 5 | 11 |
| 308 | The yellow coloured solution of chromate salt changes to orange colour on acidification due to the formation of : A ( cdot C r^{3} ) B. ( C r_{2} O_{7}^{2} ) ( mathrm{c} cdot mathrm{Cr} mathrm{O}_{4} ) ( mathrm{D} cdot mathrm{Cr}_{2} mathrm{O}_{3} ) | 11 |
| 309 | Balance the following equation, when it occurs in basic medium. [ boldsymbol{C l O}_{boldsymbol{3}}^{-} longrightarrow boldsymbol{C l}^{-} ] A ( cdot C l O_{3}^{-}+3 H_{2} O+6 e rightarrow C l^{-}+6 O H^{-} ) B . ( C l O_{3}^{-}+3 H_{2} O+5 e rightarrow C l^{-}+6 O H^{-} ) c. ( 3 C l O_{3}^{-}+3 H_{2} O+3 e rightarrow C l^{-}+3 O H ) D. None of these | 11 |
| 310 | The oxidation number of ( C r ) in ( C r O_{5} ) which has the following structure is: ( A cdot+4 ) B. +5 ( c cdot+6 ) ( D ) | 11 |
| 311 | Balance the following redox reactions: ( boldsymbol{S}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{I}_{2}(boldsymbol{s}) longrightarrow boldsymbol{S} boldsymbol{O}_{4}^{2-}(boldsymbol{a} boldsymbol{q})+ ) ( boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q}) ) A ( cdot S^{2-}(a q)+4 I_{2}(s)+4 H_{2} O(l) rightarrow 8 I^{-}(a q)+S O_{4}^{2-}(a q)+ ) ( 8 H^{+}(a q) ) B . ( S^{2-}(a q)+6 I_{2}(s)+4 H_{2} O(l) longrightarrow 8 I^{-}(a q)+4 S O_{4}^{2-}(a q)+ ) ( 8 H^{+}(a q) ) ( mathbf{c} cdot 3 S^{2-}(a q)+4 I_{2}(s)+4 H_{2} O(l) longrightarrow ) ( 8 I^{-}(a q)+5 S O_{4}^{2-}(a q)+8 H^{+}(a q) ) D ( cdot 2 S^{2-}(a q)+4 I_{2}(s)+H_{2} O(l) rightarrow 8 I^{-}(a q)+S O_{4}^{2-}(a q)+ ) ( 8 H^{+}(a q) ) | 11 |
| 312 | Which of the following reactions do not involve oxidation or reduction: A ( cdot 2 R b+2 H_{2} O rightarrow 2 R b O H+H_{2} ) в. ( 2 C u I_{2} rightarrow 2 C u+I_{2} ) c. ( N H_{4} C l+N a O H rightarrow N a C l+N H_{3}+H_{2} O ) D. None of these. | 11 |
| 313 | The balanced chemical reaction with ( boldsymbol{C l}_{2} ) is A ( cdot C l_{2}+2 N a_{2} S_{2} O_{3} rightarrow 2 N a C l+N a_{2} S_{4} O_{6} ) в. ( C l_{2}+H_{2} O+N a_{2} S_{2} O_{3} rightarrow N a_{2} S O_{4}+2 H C l+S ) c. ( C l_{2}(g)+S_{2} O_{3}^{2-} rightarrow S O_{4}^{2-}+S+C l ) D. None of the above | 11 |
| 314 | Q. 17 The reaction Cl, (g) + 20H(aq) → CLO- (aq) + Cl(aq) + H20(1) represents the process of bleaching. Identify and name the species that bleaches the substances due to its oxidising action. Thinking Process Write the oxidation number of each element above its symbol, and then identify the bleaching reagent by observing the change in oxidation number. | 11 |
| 315 | Which of the following is the strongest reducing agent in aqueous medium? ( mathbf{A} cdot M g ) в. ( N a ) ( c cdot L i ) D. ( C a ) | 11 |
| 316 | Balance the following equation. ( boldsymbol{I} boldsymbol{O}_{4}^{-}+boldsymbol{I}^{-}+boldsymbol{H}^{+} rightarrow boldsymbol{I}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) A ( cdot 2 I O_{4}^{-}+14 I^{-}+16 H^{+} rightarrow 8 I_{2}+8 H_{2} O ) B . ( 2 I O_{4}^{-}+14 I^{-}+4 H^{+} rightarrow 3 I_{2}+8 H_{2} O ) c. ( I O_{4}^{-}+7 I^{-}+8 H^{+} rightarrow 4 I_{2}+4 H_{2} O ) D. None of these | 11 |
| 317 | Which of the following is disproposination reaction? A ( cdot C a C O_{3}+2 H^{+} rightarrow C a^{2+}+H_{2} O+C O_{2} ) B . ( 2 mathrm{CrO}_{4}^{2-}+2 mathrm{H}^{+} rightarrow mathrm{Cr}_{2} mathrm{O}_{7}^{2-}+mathrm{H}_{2} mathrm{O} ) c. ( C r_{2} O_{7}^{2-}+2 O H^{-} rightarrow 2 C r O_{4}^{2-}+H_{2} O ) D. ( C u_{2} O+2 H^{+} rightarrow C u+C u^{2+}+H_{2} O ) | 11 |
| 318 | The oxidation state of the underlined element in the given compound is: ( C_{12} H_{22} O_{11} ) A ( .+5 ) ( B cdot+4 ) ( c cdot 0 ) D. none of these | 11 |
| 319 | Match the reaction in list 1 with their type in list 2 | 11 |
| 320 | The reaction ( Z n O+C rightarrow Z n+C O ) is an example of a A. Combination reaction B. Reduction-oxidation reaction c. Displacement reaction D. Decomposition Reaction | 11 |
| 321 | ( a C u^{2+}(a q)+b I^{-}(a q) rightarrow c C u I(s)+d I_{2}(s) ) When the equation above is balanced and all coefficients are reduced to lowest whole-number terms, what will be the coefficient for ( I^{-} ) ? ( mathbf{A} cdot mathbf{1} ) B. 2 ( c cdot 3 ) ( D cdot 4 ) ( E cdot 5 ) | 11 |
| 322 | The number of moles of ( C r_{2} O_{7}^{2-} ) needed to oxidize 0.136 equivalent of ( N_{2} H_{5}^{+} ) through the reaction ( N_{2} H_{5}^{+}+ ) ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-} rightarrow boldsymbol{N}_{2}+boldsymbol{C r}^{3+}+boldsymbol{H}_{2} boldsymbol{O}, ) is : A . 0.236 B. 0.087 c. 0.136 D. 0.488 | 11 |
| 323 | The oxidation state of oxygen of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) in the final products when it reacts with ( boldsymbol{A} boldsymbol{s}_{2} boldsymbol{O}_{3} ) is : ( mathbf{A} cdot mathbf{0} ) B. ( c cdot-1 ) D. – – | 11 |
| 324 | Which of the following is not a redox reaction? A ( cdot C a C O_{3} rightarrow C a O+C O_{2} ) в. ( O_{2}+2 H_{2} longrightarrow 2 H_{2} O ) c. ( N a+H_{2} O longrightarrow N a O H+frac{1}{2} H_{2} ) D. ( M n C l_{3} longrightarrow M n C l_{2}+frac{1}{2} C l_{2} ) | 11 |
| 325 | What is the oxidation number of Cl in ( H C l O ) and ( H C l O_{2} ? ) | 11 |
| 326 | ( boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{O} boldsymbol{H}^{-}(boldsymbol{H} boldsymbol{o} boldsymbol{t}) rightarrow(boldsymbol{P})+ ) ( (Q) ;(P)+(Q)+H^{+} rightarrow B r_{2} ) ( (P) ) gives yellow precipitate with ( A g N O_{3},(P) ) and ( (Q) ) are: A. ( B r^{-}, B r O^{-} ) B. ( B r^{-}, B r O_{3} ) c. ( B r O^{-}, B r O_{3}^{-} ) D. ( B r O^{-}, B r O 4 ) | 11 |
| 327 | The oxidation state of the most electronegative element in the products of the reaction between ( B a O_{2} ) and ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) are A. 0 and -1 B. -1 and -2 c. -2 and 0 D. -2 and +1 | 11 |
| 328 | Balance the following redox reactions in acidic medium : [ Z n+N O_{3}^{-} longrightarrow Z n^{2+}+N_{2} ] A ( cdot 5 Z n+2 N O_{3}^{-}+12 H^{+} rightarrow 5 Z n^{2+}+N_{2}+3 H_{2} O ) B . ( 5 Z n+2 N O_{3}^{-}+12 H^{+} rightarrow 5 Z n^{2+}+N_{2}+6 H_{2} O ) ( mathrm{c} cdot 5 Z n+2 N O_{3}^{-}+6 H^{+} rightarrow 3 Z n^{2+}+N_{2}+6 H_{2} O ) D. None of these | 11 |
| 329 | In the redox reaction given below: ( boldsymbol{x} boldsymbol{N} boldsymbol{O}_{3}^{-}+boldsymbol{y} boldsymbol{A} boldsymbol{s}_{2} boldsymbol{S}_{3}+boldsymbol{z} boldsymbol{H}_{2} boldsymbol{O} rightarrow ) ( boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}^{3-}+boldsymbol{N} boldsymbol{O}+boldsymbol{S} boldsymbol{O}_{4}^{2-}+boldsymbol{H}^{+} ) What is the value of ( frac{x}{z} ? ) | 11 |
| 330 | 11. A double salt KHC204.H_C204.2H20 is 0.2 N acid. Thus, it is (a) 0.267 N as reducing agent (b) 0.6 M as an acid (c) 0.067 M as a reducing agent (d) 0.067 M as an acid | 11 |
| 331 | In which of the following, sulphur has the highest oxidation state? This question has multiple correct options ( A cdot S O_{2} ) в. ( S O_{3} ) c. ( H_{2} S O_{4} ) D. ( H_{2} S_{S} ) | 11 |
| 332 | Balance the following reaction. ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{C}_{2} boldsymbol{H}_{4} boldsymbol{O}+boldsymbol{H}^{+} rightarrow ) ( boldsymbol{C}_{2} boldsymbol{H}_{4} boldsymbol{O}_{2}+boldsymbol{C} boldsymbol{r}^{3+} ) A ( cdot C r_{2} O_{7}^{2-}+3 C_{2} H_{4} O+8 H^{+} rightarrow 3 C_{2} H_{4} O_{2}+2 C r^{3+}+ ) ( 4 H_{2} O ) B . ( C r_{2} O_{7}^{2-}+C_{2} H_{4} O+8 H^{+} rightarrow 3 C_{2} H_{4} O_{2}+5 C r^{3+}+H_{2} O ) C. ( C r_{2} O_{7}^{2-}+4 C_{2} H_{4} O+4 H^{+} rightarrow C_{2} H_{4} O_{2}+2 C r^{3+}+ ) ( 4 H_{2} O ) D. None of these | 11 |
| 333 | ( C u^{+} ) undergoes disproportionation to ( C u ) and ( C u^{2+} ) If true enter 1 , else enter 0 . ( A ) | 11 |
| 334 | The balanced equation in basic medium is : ( boldsymbol{S}_{2} boldsymbol{O}_{4}^{2-}+boldsymbol{A} boldsymbol{g}_{2} boldsymbol{O} stackrel{O H^{-}}{rightarrow} boldsymbol{A} boldsymbol{g}+boldsymbol{S} boldsymbol{O}_{3}^{2-} ) A ( cdot S_{2} O_{4}^{2-}+A g_{2} O+2 O H^{-} rightarrow 2 A g+2 S O_{3}^{2-}+H_{2} O ) B. ( S_{2} O_{4}^{2-}+2 A g_{2} O+2 O H^{-} rightarrow 2 A g+S O_{3}^{2-}+H_{2} O ) ( mathbf{c} cdot 2 S_{2} O_{4}^{2-}+3 A g_{2} O+2 O H^{-} rightarrow 2 A g+2 S O_{3}^{2-}+H_{2} O ) D. none of these | 11 |
| 335 | The species reduce in the following reaction is : ( boldsymbol{F} boldsymbol{e}_{2} boldsymbol{O}_{3}+boldsymbol{3} boldsymbol{C} boldsymbol{O} rightarrow boldsymbol{2} boldsymbol{F} boldsymbol{e}+boldsymbol{3} boldsymbol{C} boldsymbol{O}_{2} ) A . ( F e ) в. ( C O ) ( c cdot C O_{2} ) D. ( F e_{2} O_{3} ) | 11 |
| 336 | Find the sum of average oxidation number of ( S ) in ( H_{2} S O_{5} ) (peroxy monosulphuric acid) and ( N a_{2} S_{2} O_{3} ) (sodium thiosulphate) | 11 |
| 337 | In the following reaction ( : boldsymbol{C r}(boldsymbol{O H})_{3}+ ) ( boldsymbol{O H}^{-}+boldsymbol{I O}_{3}^{-} rightarrow boldsymbol{C r} boldsymbol{O}_{4}^{2-}+boldsymbol{H}_{2} boldsymbol{O}+ ) ( boldsymbol{I}^{-}: ) A ( cdot I O_{3} ) – is oxidising agent B. ( C r(O H)_{3} ) is oxidised C. ( 6 e^{-} ) are being taken per iodine atom D. all of these | 11 |
| 338 | Q19. Identify the oxidant and the reductant in the following reaction. N,H.(g) + Clo, (aq) → NO(g) + Cl(aq) | 11 |
| 339 | Out of the halogens, which one is the most powerful oxidizing agent? A. bromine B. fluorine c. iodine D. chlorine | 11 |
| 340 | Estimate the cell potential of a Daniel cell having ( 1.0 M Z n^{++} ) and originally having ( 1.0 M C u^{++} ) after sufficient ( N H_{3} ) has been added to the cathode compartment to make ( N H_{3} ) concentration ( 2.0 M ) at equilibrium. ( operatorname{Given} boldsymbol{K}_{f} ) for ( left[boldsymbol{C u}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4}right]^{2+}=mathbf{1} times ) ( 10^{12}, E^{o} ) for the reaction, ( Z n+ ) ( boldsymbol{C u}^{2+} longrightarrow Z boldsymbol{n}^{2+}+boldsymbol{C u} quad mathbf{1 . 1} boldsymbol{V} ) (Take ( frac{mathbf{2 . 3 0 3} boldsymbol{R} boldsymbol{T}}{boldsymbol{F}}=mathbf{0 . 0 6} log mathbf{6 . 2 5}=mathbf{0 . 8} mathbf{)} ) | 11 |
| 341 | 0.5 Thiosulphate reacts differently with iodine ate reacts differently with iodine and bromine in the reactions given below 250 + Iz 50% + 25 S203 + 2Br2 + 5H20 – 2503 + 2Br + 10H* Which of the following statements justifies the above dual behaviour of thiosulphate? (a) Bromine is a stronger oxidant than iodine (b) Bromine is a weaker oxidant than iodine (c) Thiosulphate undergoes oxidation by bromine and reduction by iodine in these reactions (d) Bromine undergoes oxidation and iodine undergoes reduction in these reactions | 11 |
| 342 | Choose the redox reaction from the following. ( mathbf{A} cdot C u+2 H_{2} S O_{4} rightarrow C u S O_{4}+S O_{2}+2 H_{2} O ) B ( cdot B a C l_{2}+H_{2} S O_{4} rightarrow B a S O_{4}+2 H C l ) ( mathbf{c} cdot 2 N a O H+H_{2} S O_{4} rightarrow N a_{2} S O_{4}+2 H_{2} O ) ( mathbf{D} cdot K N O_{2}+H_{2} S O_{4} rightarrow 2 H N O_{2}+K_{2} S O_{4} ) | 11 |
| 343 | The oxidation state of phoshorus varies from A. -1 to +1 B . -3 to +3 ( mathbf{c} cdot-3 ) to +5 D. -5 to +1 | 11 |
| 344 | The reaction is balanced if ( 5 H_{2} O_{2}+ ) ( boldsymbol{x} boldsymbol{C l} boldsymbol{O}_{2}+mathbf{2} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{x} boldsymbol{C l}^{-}+boldsymbol{y} boldsymbol{O}_{2}+ ) ( 6 H_{2} O ) The value of ( y ) is : | 11 |
| 345 | Write formulas for the following compounds. Tin (IV) oxide | 11 |
| 346 | Identify the pair of binary corresponds in which nitrogen exhibits the lowest and the highest oxidation state. A. ( N H_{3}, N O_{2} ) в. ( N_{3} H, N_{2} O_{5} ) c. ( N_{2}, H N O_{3} ) D. ( N_{2} O, N_{2} O_{5} ) | 11 |
| 347 | Explain Displacement reaction with examples | 11 |
| 348 | What coefficients are required to balance the following equation? ( boldsymbol{F} boldsymbol{e}+boldsymbol{O}_{2} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{O} ) ( mathbf{A} cdot 2,1,2 ) B. 1,1,1 c. 4,2,4 D. 2,1,1 | 11 |
| 349 | Corrosion of iron is : ( A cdot ) redox process B. neutrilization process C . precipitation process D. none of the above | 11 |
| 350 | ( Z n+H_{2} S O_{4} rightarrow ) a gas If we bring a burning splinter near the gas produced in the given reaction, it burns with a pop sound. The gas is: ( A cdot O_{2} ) в. ( N_{2} ) ( mathrm{c} cdot mathrm{H}_{2} ) D. ( C O_{2} ) | 11 |
| 351 | Match the reactions in column I with the molar ratio of their respective oxidants and reductant in column II. | 11 |
| 352 | How many substances have underlined atoms of different nature? ( N a_{2} S_{4} O_{6}, N a_{2} S_{2} O_{3}, C a O C l_{2}, N_{2} H_{4} O_{3} ) A. 7 B. 5 ( c cdot 4 ) D. 8 | 11 |
| 353 | In the formation of electrovalent compound ( M g C l_{2} ) name the substance that is oxidized and is reduced. | 11 |
| 354 | The redox process involves the complete transfer of electrons in the formation in ionic bonds or partial transfer or shift of electrons in the formation of covalent bonds. If true enter 1 , else enter 0 . ( A ) | 11 |
| 355 | An element forms two oxides containing respectively 53.33 and 36.36 percent of oxygen. These figures illustrate the law of A. Conservation of mass B. Constant proportions c. Reciprocal proportions D. Multiple proportions | 11 |
| 356 | Which of the following compounds have zero oxidation state at carbon? This question has multiple correct options A. ( C_{6} H_{12} O_{6} ) в. нсоон c. нсно D. ( C H_{4} ) | 11 |
| 357 | ( N a O H+H_{2} S O_{4} rightarrow N a_{2} S O_{4}+H_{2} O ) Balance the given chemical equation | 11 |
| 358 | Which of the following represents a correctly balanced half-reaction? A ( cdot C l_{2}+2 e^{-} rightarrow C l^{-} ) B ( cdot 2 e+F e rightarrow F e^{2+} ) c. ( O_{2} rightarrow 2 e^{-}+2 O^{2} ) D. ( A l^{3+} rightarrow A l+3 e^{-} ) E ( cdot 2 H^{+}+2 e^{-} rightarrow H_{2} ) | 11 |
| 359 | Identify redox reaction among the following: A. acid-base neutralization B. precipitation reaction c. metal displacement reaction D. all the above | 11 |
| 360 | Volume of ( 0.1 mathrm{M} K M n O_{4}, ) required to oxidise completely ( 50 mathrm{ml} ) of ( 0.5 mathrm{M} ) ferrous oxalate solution in acidic medium will be: A . ( 100 mathrm{mL} ) B . ( 120 mathrm{mL} ) ( c .150 mathrm{mL} ) D. ( 200 mathrm{mL} ) | 11 |
| 361 | Q2. What is a redox couple? | 11 |
| 362 | In the reaction ( 2 A g+2 H_{2} S O_{4} rightarrow ) ( A g_{2} S O_{4}+2 H_{2} O+S O_{2} ) sulphuric acid acts as: A. an oxidising agent B. a reducing agent c. a catalyst D. an acid as well as oxidant | 11 |
| 363 | When ( S O_{2} ) is passed in a solution of potassium iodate, the oxidation state of iodine changes from: A . +5 to 0 B. +5 to -1 c. -5 to 0 D. -7 to -1 | 11 |
| 364 | In the following reaction which element is oxidized? ( boldsymbol{M} boldsymbol{g}(boldsymbol{s})+boldsymbol{C l}_{2}(boldsymbol{g}) longrightarrow boldsymbol{M} boldsymbol{g} boldsymbol{C l}_{2}(boldsymbol{s}) ) ( mathbf{A} cdot M g ) в. ( C l_{2} ) ( mathrm{c} cdot M g^{+} ) D. ( C l^{-} ) | 11 |
| 365 | ( B r_{2} rightarrow B r O_{3}^{-}+B r^{-}(text {acidic }) ) is a balanced equation. If true enter 1 , else enter 0 . ( A ) | 11 |
| 366 | What is incorrectly matched? ( mathbf{A} cdot C s B r_{3} rightleftharpoons C s^{oplus}+B r_{3}^{ominus} rightleftharpoons C s^{oplus}+B r^{ominus}+B r_{2} ) B ( cdot I_{4} O_{9} rightleftharpoons I^{3}+3left(I O_{3}right)^{ominus} ) ( mathbf{c} cdot A g B r O_{3} rightleftharpoons A g^{oplus} B r_{3}^{ominus} ) ( mathbf{D} cdot I_{2} O_{4} rightleftharpoons I O_{2}^{oplus}+I O_{2}^{ominus} ) | 11 |
| 367 | Q6. (a) Arrange the following in order of increasing O.N of iodine: 1,, HI, HIO, KIO, ICI. (b) Identify the oxidant and reductant in the following redox reaction: 2KMnO4 + Cl2KCl + 2KMnO ta TL | 11 |
| 368 | Q. 22 Calculate the oxidation number of phosphorus in the following species. (a) HPO- (6) PO3- | 11 |
| 369 | Which of the following oxidation numbers is not correctly matched? A ( cdot P ) in ( N a H_{2} P O_{4}=+5 ) B. ( N i ) in ( left[N i(C N)_{6}right]^{4-}=+2 ) ( mathbf{c} cdot P ) in ( M g_{2} P_{2} O_{7}=+6 ) D. ( C r ) in ( left(N H_{4}right)_{2} C r_{2} O_{7}=+6 ) | 11 |
| 370 | Q.10 Identify disproportionation reaction (a) CH4 + 202 → CO2 + 2H,0 (b) CH4 + 4Cl2 → CCIA + 4HCI (c) 2F + 20H2F+OF+ HO (d) 2NO, + 2OH- NO2 + NO3 + H2O | 11 |
| 371 | Consider the reaction: ( boldsymbol{F e}+boldsymbol{H}_{2} boldsymbol{O} rightarrow ) ( boldsymbol{F} boldsymbol{e}_{3} boldsymbol{O}_{4}+boldsymbol{H}_{2} ) If the number of electrons lost or gained during the changes is ( x ). Then, the value of ( x ) is : | 11 |
| 372 | A qualitative analysis test for ( M n^{2+} ) involves its oxidation to ( M n O_{4}^{-} ) in acidic solution by sodium bismuthate, ( N a B i O_{3} . ) The bisulphate ion is reduced to ( B i^{3 i} . ) What is a balanced equation for this test? A ( cdot B i O_{3}^{-2}+M n^{2+}+H^{+} rightarrow M n O_{4}^{-}+B i^{3+}+H_{2} O ) B. ( 5 B i O_{3}^{-}+2 M n^{2+}+7 H^{+} rightarrow 2 M n O_{4}^{-}+5 B i^{3+}+7 O H ) C. ( 5 B i O_{3}^{-}+2 M n^{2+}+14 H^{+} rightarrow 2 M n O_{4}^{-}+5 B i^{3+}+7 H_{2} O ) D. None of these | 11 |
| 373 | Which of the following examples does not represent disproportionation? A ( cdot M n O_{2}+4 H C l rightarrow M n C l_{2}+C l_{2}+2 H_{2} O ) в. ( 2 H_{2} O_{2} rightarrow 2 H_{2} O+O_{2} ) c. ( 4 K C l O_{3} rightarrow 3 K C l O_{4}+K C l ) D. ( 3 C l_{2}+6 N a O H longrightarrow 5 N a C l+N a C l O_{3}+3 H_{2} O ) | 11 |
| 374 | In an experiment, 20 g of vanadium ( (V) ) oxide (molar mass ( =182 ) g/mol) was reduced by excess of zinc dust in acidic solution to vanadium (II) ions. If the required number of moles of iodine to reoxidise vanadium (II) to ( V O^{2+} ) is ( 22 times 10^{-x}, ) then what is the value of ( x ? ) | 11 |
| 375 | Consider the following reaction, ( mathbf{5} boldsymbol{H}_{mathbf{2}} boldsymbol{O}_{mathbf{2}}+boldsymbol{x} boldsymbol{C l} boldsymbol{O}_{mathbf{2}}+mathbf{2} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{x} boldsymbol{C l}^{-}+ ) ( boldsymbol{y} boldsymbol{O}_{2}+boldsymbol{6} boldsymbol{H}_{2} boldsymbol{O} . ) The reaction is balanced if A ( . x=5, y=2 ) в. ( x=2, y=5 ) c. ( x=4, y=10 ) D. ( x=5, y=5 ) | 11 |
| 376 | Which compound amongst the following has the highest oxidation number of ( M n ? ) A. ( K M n O_{4} ) в. ( K_{2} M n O_{4} ) ( mathrm{c} cdot M n O_{2} ) D. ( M n_{2} O_{3} ) | 11 |
| 377 | Which of the following is not a redox reaction? A. ( M g+N_{2} rightarrow M g_{3} N_{2} ) B . ( M n O_{4}^{-}+C_{2} O_{4}^{2-} rightarrow M n^{2+}+C O_{2} ) c. ( C u S O_{4}+K I rightarrow 2 C u I+I_{2}+K_{2} S O_{4} ) D. ( A g C l+N H_{3} rightarrowleft[A gleft(N H_{3}right)_{2}right] C l ) | 11 |
| 378 | Balance the following in basic medium: ( boldsymbol{A s O}_{3}^{3+}+boldsymbol{M n O}_{4}^{-} rightarrow boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}^{3-}+boldsymbol{M n O}_{2} ) A ( cdot 3 A s O_{3}^{3+}+2 M n O_{4}^{-}+H_{2} O rightarrow 3 A s O_{4}^{3-}+2 M n O_{2}+ ) ( 2 O H^{-} ) B. ( 3 A s O_{3}^{3+}+2 M n O_{4}^{-}+4 H_{2} O rightarrow 3 A s O_{4}^{3-}+3 M n O_{2}+ ) ( 2 O H^{-} ) ( mathrm{c} cdot 3 A s O_{3}^{3+}+4 M n O_{4}^{-}+3 H_{2} O rightarrow 3 A s O_{4}^{3-}+2 M n O_{2}+ ) ( 4 O H^{-} ) D. None of these | 11 |
| 379 | ( 2 P b O+C rightarrow 2 P b+C O_{2} ) is an example of A. oxiation reaction B. reduction reaction c. redox reaction D. none | 11 |
| 380 | Q. 9 The largest oxidation number exhibited by an element depends on its outer electronic configuration. With which of the following outer electronic configurations the element will exhibit largest oxidation number? (a) 3d 452 (b) 3d 452 (c) 3d 4s’ (d) 3d 4s | 11 |
| 381 | Which of the followings are redox titration? A. Complexometric titration B. Iodometric titration c. Acid-base titration D. Back titration E. All of these | 11 |
| 382 | What coefficient is needed for fluorine to balance the following equation? ( boldsymbol{L} boldsymbol{i}+boldsymbol{F}_{2} rightarrow boldsymbol{L} boldsymbol{i} boldsymbol{F} ) ( mathbf{A} cdot mathbf{0} ) B. ( c cdot 2 ) D. 3 | 11 |
| 383 | For the reaction between ( M n O_{4}^{-} ) and ( C_{2} O_{4}^{-} ) in basic solution, the unbalanced equation is as follows: ( M n O_{4}^{-}+C_{2} O_{4}^{2-} longrightarrow M n O_{2}(s)+ ) ( boldsymbol{C O}_{3}^{2-} ) In a balanced equation, the number of ( O H^{-} ) ions on the right is : | 11 |
| 384 | In which of the following, the oxidation number of oxygen has been arranged in increasing order? A. ( B a O_{2}<K O_{2}<O_{3}<O F_{2} ) в. ( O F_{2}<K O_{2}<B a O_{2}<O_{3} ) c. ( B a O_{2}<O_{3}<O F_{2}<K O_{2} ) D. ( K O_{2}<O F_{2}<O_{3}<B a O_{2} ) | 11 |
| 385 | ( A l+M n O_{4}^{-} rightarrow A l(O H)_{4}^{-}+M n O_{2} ) For this reaction, element ( X ) is reduced and element Y is oxidised. Then ( X ) and ( Y ) are respectively: A. ( A l ) and ( M n ) B. ( M n ) and ( A l ) c. ( A l ) and ( A l ) D. Mn and ( M n ) | 11 |
| 386 | Write the overall reaction taking place in Daniel Cell. | 11 |
| 387 | The cell reaction ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2+}(boldsymbol{a q})+ ) ( mathbf{1 4} boldsymbol{H}^{+}(boldsymbol{a q})+boldsymbol{6} boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{a q}) rightarrow ) ( mathbf{6} F e^{3+}(boldsymbol{a} boldsymbol{q})+mathbf{2} boldsymbol{C} boldsymbol{r}^{3+}(boldsymbol{a} boldsymbol{q})+mathbf{7} boldsymbol{H}_{2} boldsymbol{O}(l) ) best represented by: A ( cdot P t(s)left|F e^{2+}(a q), F e^{3+}(a q) | C r_{2} O_{7}^{2+}(a q), C r^{3+}(a q)right| P t(s) ) B . ( P t(s)left|C r_{2} O_{7}^{2+}(a q), C r^{3+}(a q) | F e^{3+}(a q), F e^{2+}(a q)right| P t(s) ) C. ( F e^{2+}(a q)left|F e^{3+}(a q) | C r_{2} O_{7}^{2+}(a q)right| C r^{3+}(a q) ) D. ( C r_{2} O_{7}^{2+}(a q)left|C r^{3+}(a q) | F e^{3+}(a q)right| F e^{2+}(a q) ) | 11 |
| 388 | Select the correct alternative. In the reaction of ( Z n+F e S O_{4} rightarrow ) ( Z n S O_{4}+F e ) A. zn gets oxidized B. Fe gets oxidized c. zn is oxidized in agent D. zn and Fe both get oxidized | 11 |
| 389 | The oxidation number of chlorine is maximum in A . ( H O C l ) в. ( C l_{2} O_{6} ) c. ( K C l O_{4} ) D. ( N a C l O_{3} ) | 11 |
| 390 | Which type of reaction produces heat and light? A. Endothermic B. Phytochemical c. Reduction D. Exothermic | 11 |
| 391 | The reaction: ( 3 C l O^{-} rightarrow C l O_{3}^{-}+2 C l^{-} ) is an example of A. Oxidation reaction B. Reduction reaction c. Disproportionation reaction D. Decomposition reaction | 11 |
| 392 | How many mL of ( 0.3 mathrm{M} K_{2} C r_{2} O_{7}(text { acidic }) ) is required for complete oxidation of 5 ( mathrm{mL} ) of ( 0.2 mathrm{M} ) Sn ( C_{2} mathrm{O}_{4} ) solution. (Round off to 1 decimal place) | 11 |
| 393 | 07. What is salt bridge? | 11 |
| 394 | What is the reaction called when oxidation and reduction take place simultaneously? Explain with one example. | 11 |
| 395 | State whether the given statement is true or false: Neutralisation is a double displacement reaction A. True B. False | 11 |
| 396 | Which indicator we prefer to use in iodometric titration? A. Starch B. Phenolphthalein c. 1,10 phenathroline D. All of the above | 11 |
| 397 | Number of peroxide bonds in ( K_{3} C r O_{8} ) is 4 If true enter 1 , else enter 0 . ( A ) | 11 |
| 398 | Which of the following reactions is/ are not intermolecular redox reaction? This question has multiple correct options ( mathbf{A} cdot P b O_{2}+H_{2} O rightarrow P b O+H_{2} O_{2} ) B ( cdot 2 K C l O_{3} rightarrow 2 K C l+3 O_{2} ) ( mathbf{C} cdotleft(N H_{4}right)_{2} C r_{2} O_{7} rightarrow N_{2}+C r_{2} O_{3}+4 H_{2} O ) D. ( N H_{4} N O_{2} rightarrow N_{2}+2 H_{2} O ) | 11 |
| 399 | Balance the following redox reactions: [ boldsymbol{I}_{2}(boldsymbol{s})+boldsymbol{O} boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q}) longrightarrow boldsymbol{I} boldsymbol{O}_{3}^{-}(boldsymbol{a} boldsymbol{q})+ ] ( boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q}) ) ( mathbf{A} cdot I_{2}(s)+5 O C l^{-}(a q)+H_{2} O(l) longrightarrow 2 I O_{3}^{-}(a q)+ ) [ 5 C l^{-}(a q)+2 H^{+}(a q) ] B ( cdot I_{2}(s)+5 O C l^{-}(a q)+2 H_{2} O(l) longrightarrow I O_{3}^{-}(a q)+ ) [ 4 C l^{-}(a q)+2 H^{+}(a q) ] ( mathbf{c} cdot I_{2}(s)+3 O C l^{-}(a q)+4 H_{2} O(l) longrightarrow I O_{3}^{-}(a q)+ ) ( 4 C l^{-}(a q)+2 H^{+}(a q) ) ( mathbf{D} cdot I_{2}(s)+5 O C l^{-}(a q)+7 H_{2} O(l) longrightarrow I O_{3}^{-}(a q)+ ) ( 5 C l^{-}(a q)+2 H^{+}(a q) ) | 11 |
| 400 | 5. Which ordering of compounds is according to the decreasing order of the oxidation state of nitrogen? (a) HNO, NO, NHẠCl, N, (b) HNO2, NO, N, NH,CI (c) HNO, NHCl, NO, N, (d) NO, HNO, NHẠCl, N, | 11 |
| 401 | ( C N^{ominus} ) ion is oxidised by a powerful oxidising agent to ( N O_{3}^{ominus} ) and ( C O_{2} ) or ( C O_{3}^{2-} ) depending on the acidity of the reaction mixture. ( boldsymbol{C N}^{ominus} longrightarrow boldsymbol{C O}_{2}+boldsymbol{N O}_{3}^{ominus}+boldsymbol{H}^{oplus}+boldsymbol{n} e^{-} ) What is the number ( (n) ) of electrons involved in the process? | 11 |
| 402 | The oxidation reaction always takes place with a reduction reaction. Why is isolated oxidation reaction not possible? | 11 |
| 403 | Q. 20 Nitric acid is an oxidising agent and reacts with PbO but it does not react with Pb0,. Explain why? | 11 |
| 404 | The oxidation state of the underlined element in the given compound is: ( boldsymbol{N} boldsymbol{a}_{2}left[underline{boldsymbol{F}} e(boldsymbol{C} boldsymbol{N})_{5} boldsymbol{N} boldsymbol{O}right] ) ( A cdot-2 ) ( B .+2 ) ( c cdot+3 ) D. none of these | 11 |
| 405 | Assertion The oxidation state of ( S ) in ( H_{2} S_{2} O_{8} ) is 6 Reason Maximum oxidation state of ( S ) is 6 because the maximum oxidation state of an element is its number of valence electron. 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 |
| 406 | Chlorine is used to purify drinking water. Excess of chlorine is harmful. The excess of chlorine is removed by treating with sulphur dioxide. Present a balanced equation for the redox change taking place in water | 11 |
| 407 | The oxidation number of the nitrogen atom in the ammonium ion is : ( A cdot+3 ) ( B .+2 ) ( c cdot+1 ) ( D cdot-2 ) E. – – | 11 |
| 408 | Balance the following equation by ion electron method. ( M n O_{4}^{-}+H^{+}+H_{2} O_{2} rightarrow M n^{2+}+ ) ( boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{O}_{2} ) | 11 |
| 409 | Titration curves for ( 0.1 mathrm{M} ) solutions of three weak acids ( H A_{1}, H A_{2} ) ans ( H A_{3} ) with ionization constants ( boldsymbol{K}_{1}, boldsymbol{K}_{2} ) and ( K_{3} ) respectively are plotted in the figure.which of the following is/are true? ( mathbf{A} cdot K_{2}=left(K_{1}+K_{3}right) / 2 ) B . ( K_{1}K_{2} ) D. ( K_{2}>K_{3} ) | 11 |
| 410 | A number which is assigned to each atom or ion in a compound which explains its degree of oxidation is called: A. oxidation degree B. oxidation number c. oxidation state D. both ( B ) and ( C ) | 11 |
| 411 | 42 DIN Q13. Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions. (a) 2AgBr(s) + CH 0,(aq) —>2Ag(s) + 2HBr(aq) + CH,0, (aq) (b) HCHO) + 2[AgNH,), (aq) + 3OH (aq) » 2Ag(s) + HCOO (aq) + 4NH, (aq) + 2H2O(1) (c) HCHOI) + 2Cu2+ (aq) + 50H(aq) → Cu,O(s) + HCOO (aq) + 3H2O(1) (d) N,H.(I) + 2H20 (1) ► N.(g) + 4H2O(1) (e) Pb(s) + PbO (s) + 2H,SO, aq) 2PbSO4(s) + 2H20(1) | 11 |
| 412 | Bleaching powder ( left(C a O C l_{2}right) ) has two types of chlorine atoms with oxidation number of +1 and ( -1 . ) It can be represented as: A ( cdot C a^{2+}left(C l O_{2}^{-}right) C l^{-} ) в. ( C a^{2+}left(C l O_{3}^{-}right) C l^{-} ) c. ( C a^{2+}left(C l O^{+}right) C l^{-} ) D. ( C a^{2+}left(C l O^{-}right) C l^{-} ) | 11 |
| 413 | Given ( 4 N H_{3}(g)+5 O_{2}(g) rightarrow ) ( mathbf{4} boldsymbol{N} boldsymbol{O}(boldsymbol{g})+boldsymbol{6} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) The above reaction is an example of: (i) displacement reaction (ii) combination reaction (iii) redox reaction (iv) neutralisation reaction A ( . ) (i) and (iv) B. (ii) and (iii) c. (i) and (iii) D. (iii) and (iv) | 11 |
| 414 | Balance the following equation by ion electron method. ( Z n+B r O_{4}^{-}+O H^{-}+H_{2} O rightarrow ) ( left[boldsymbol{Z n}(boldsymbol{O H})_{4}right]^{2-}+boldsymbol{B r}^{-} ) | 11 |
| 415 | The oxidation state of ( mathrm{Mn} ) in ( boldsymbol{K}_{mathbf{2}} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{boldsymbol{4}} ) is: ( A cdot+5 ) ( B cdot+4 ) ( c cdot+7 ) ( D cdot+6 ) | 11 |
| 416 | Ag, SO, + 2H,0 + SOZ 4. On the reaction 2Ag + 2H, SO sulphuric acid acts as (a) an oxidizing agent (C) a catalyst The Qyidation in (b) a reducing agent (d) an acid as well as an oxidant 5 | 11 |
| 417 | Oxidation means (gain/loss) of ( O_{2} ) and reduction means gain of hydrogen. | 11 |
| 418 | 0.28 Match the items in Column I with relevant items in Column II. Column 1 Column II A. Tons having positive charge 1. +7 B. The sum of oxidation number of 2 -1 oth all atoms in a neutral molecule с. Oxidation number of hydrogen 3 +1 O ion (HT) D O xidation number of fluorine in NaF E lons having negative charge 5. Cation Anion | 11 |
| 419 | The ratio of oxygen atom having -2 and -1 oxidation numbers in ( S_{2} O_{8}^{2-} ) is three If true enter 1 , else enter 0 A. | 11 |
| 420 | Which reaction does not represent autoredox or disproportionation? A ( cdot C l_{2}+2 O H^{-} rightarrow C l^{-}+C l O^{-}+H_{2} O ) B. ( 2 H_{2} O_{2} rightarrow 2 H_{2} O+O_{2} ) ( mathbf{c} cdot 2 C u^{+} rightarrow C u^{+2}+C u ) D. ( left(N H_{4}right)_{2} C r_{2} O_{7} longrightarrow N_{2}+C r_{2} O_{3}+4 H_{2} O ) | 11 |
| 421 | Arrange the following in the order of increasing oxidation number of nitrogen: ( N H_{3}, N_{3} H, N_{2} O, N O, N_{2} O_{5} ) | 11 |
| 422 | Assertion ( F_{2} ) undergoes disproportionation reaction. Reason Fluorine shows both positive and negative oxidation states. 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 |
| 423 | Explain how ( Z n+2 A g N O_{3} rightarrow 2 A g+ ) ( Z nleft(N O_{3}right)_{2} ) is a redox reaction. | 11 |
| 424 | Match the compounds given in column I with oxidation states of carbon given in column II and mark the apropriate choice. ( (A) ) (B) The the ( begin{array}{llll}text { Column I } & & text { Column II } \ & & \ C_{6} H_{12} O_{6} & text { (i) } & +3 \ & C H C l_{3} & text { (ii) } & -3 \ & C H_{3} C H_{3} & text { (iii) } & +2 \ & (C O O H)_{2} & text { (iv) } & 0end{array} ) (c) (D) ( A ) ( (A) rightarrow(text { iv }),(B) rightarrow(text { iii }),(C) rightarrow(text { ii }),(D) rightarrow(i) ) B. ( (A) rightarrow(text { i }),(B) rightarrow(text { ii }),(C) rightarrow(text { iii }),(D) rightarrow(text { iv }) ) C. ( (A) rightarrow(text { ii }),(B) rightarrow(text { iii }),(C) rightarrow(text { iv }),(D) rightarrow(i) ) ( D cdot(A) rightarrow(text { iii }),(B) rightarrow(text { ii }),(C) rightarrow(i),(D) rightarrow(text { iv }) ) | 11 |
| 425 | Which of the one is not true about redox reactions? A. Share of electrons B. Transfer of electrons c. Gain of oxygen D. Loss of Hydrogen | 11 |
| 426 | Assertion Oxidation involves loss of electrons and reduction involves gain of electrons. Reason The overall reaction in which oxidation and reduction occurs simultaneously is called redox reaction. 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 |
| 427 | Arrange the following in increasing order of oxidation state of ( N i ) ( boldsymbol{K}_{2}left[boldsymbol{N} boldsymbol{i}(boldsymbol{C} boldsymbol{N})_{4}right], boldsymbol{K}_{2}left[boldsymbol{N} boldsymbol{i} boldsymbol{F}_{6}right], boldsymbol{N} boldsymbol{i}(boldsymbol{C} boldsymbol{O})_{4} ) A ( cdot N i(C O)_{4}, K_{2}left[N i(C N)_{4}right], K_{2}left[N i F_{6}right] ) B . ( K_{2}left[N i(C N)_{4}right], N i(C O)_{4}, K_{2}left[N i F_{6}right] ) c. ( N i(C O)_{4}, K_{2}left[N i F_{6}right], K_{2}left[N i(C N)_{4}right] ) D. ( K_{2}left[N i F_{6}right], K_{2}left[N i(C N)_{4}right], K_{2}left[N i(C N)_{4}right]^{prime} ) | 11 |
| 428 | What is the oxidising agent in the following reaction? ( mathbf{2} boldsymbol{F} boldsymbol{e}_{boldsymbol{a} boldsymbol{q}}^{mathbf{2}+}+boldsymbol{C l}_{mathbf{2}(boldsymbol{g})} rightarrow mathbf{2} boldsymbol{F} boldsymbol{e}_{(boldsymbol{a q})}^{mathbf{3}+}+mathbf{2} boldsymbol{C l}_{(boldsymbol{a} boldsymbol{q})}^{-} ) A ( cdot F e^{2} ) в. ( C l_{2} ) ( mathrm{c} cdot F e^{3} ) D. ( C l^{-} ) | 11 |
| 429 | 09. Consider the reactions: (a) 6CO2(8) 6H2O(l) CH4,06(s) + 60,(8) (b) 03(8) + H,0,1)→ H2O(l) +202(8) Why it is more appropriate to write these reactions as: (a) 6CO2(8) + 12H,O(1) CH20c(s) + 6H2O(l) + 60 (8) (6) 03(8) + H,0,1) → H2O(1) + 0,(g) + O. (8) Also suggest a technique to investigate the path of above (a) and (b) redox reactions. | 11 |
| 430 | Find the oxidation state of bromine in ( mathrm{HBrO}_{3} ) ( A cdot-3 ) B . – ( c cdot 1 ) ( D .3 ) E. 5 | 11 |
| 431 | Determine the change in oxidation number of sulphur in ( H_{2} S ) and ( S O_{2} ) respectively in the following reaction. ( 2 H_{2} S+S O_{2} rightarrow 2 H_{2} O+3 S ) A .0,+2 в. +2,-4 c. -2,+2 ( mathbf{D} cdot+4,0 ) | 11 |
| 432 | Justify that the following reactions are redox reactions. ( mathbf{A} cdot C u O(s)+H_{2}(g) rightarrow C u(s)+H_{2} O(g) ) B ( cdot F e_{2} O_{3}(s)+3 C O(g) rightarrow 2 F e(s)+3 C O_{2}(g) ) ( mathbf{c} cdot 4 B C l_{3}(g)+3 L i A l H_{4}(s) rightarrow 2 B_{2} H_{6}(s)+3 L i C l(s)+ ) ( 3 A l C l_{3}(s) ) D ( cdot 2 K(s)+F_{2}(g) rightarrow 2 K^{+} F^{-}(s) ) | 11 |
| 433 | In the reaction: ( S_{2} O_{8}^{2-}+2 I^{-} rightarrow ) ( 2 S O_{4}^{2-}+I_{2} ) A. oxidation of iodide into iodine takes place B. reduction of iodine into iodide takes place c. both oxidation and reduction of iodine takes place D. none of the above | 11 |
| 434 | A balanced chemical equation is in accordance with: A. Avogadro’s Law B. Law of constant proportion c. Law of conservation of mass D. Law of gaseous volumes | 11 |
| 435 | [ begin{array}{c} begin{array}{c} O \ C end{array}-H \ H-C_{1}^{prime} O-H \ H end{array} ] Write oxidation No. of each ( C ) atom. | 11 |
| 436 | The oxidation number of ( P t ) in ( left[boldsymbol{P t}left(boldsymbol{C}_{2} boldsymbol{H}_{4}right) boldsymbol{C l}_{3}right]^{-} ) is : | 11 |
| 437 | Write balanced chemical equation for the following. Action of ozone on hydrogen peroxide. | 11 |
| 438 | Balance the following equation: ( boldsymbol{K} boldsymbol{C l} boldsymbol{O}_{3}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow boldsymbol{K} boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4}+ ) ( boldsymbol{H} boldsymbol{C l O}_{4}+boldsymbol{C l O}_{2} ) A ( cdot 3 K C l O_{3}+3 H_{2} S O_{4} rightarrow 3 K H S O_{4}+H C l O_{4}+2 C l O_{2}+ ) ( H_{2} O ) в. ( K C l O_{3}+5 H_{2} S O_{4} rightarrow 3 K H S O_{4}+3 H C l O_{4}+2 C l O_{2}+ ) ( 3 H_{2} O ) c. ( 3 K C l O_{3}+4 H_{2} S O_{4} rightarrow 3 K H S O_{4}+2 H C l O_{4}+ ) ( 2 C l O_{2}+H_{2} O ) D. None of these | 11 |
| 439 | Find the oxidation number of elements in each case. ( S ) in ( N a_{2} S_{2} O_{3}, S_{4}, S_{8} ) and ( N a_{2} S_{2} O_{7} ) ( mathbf{A} cdot+2,0,0,+6 ) B. +1,1,0,+5 c. 0,0,1,+4 D. None of these | 11 |
| 440 | Determine the oxidation state of the underlined element in ( underline{I} C l ) A ( .+1 ) B. +4 ( c cdot+2 ) D. +3 | 11 |
| 441 | ( ln F e C r_{2} O_{4}, ) the oxidation number of ( f e ) and Cr are: ( A cdot+2 ) and +3 B. 0 and +2 ( c cdot+2 ) and +6 D. 2 and | 11 |
| 442 | For joining railway tracks, ferric oxide is reacted with aluminium to produce aluminium oxide and iron. The balanced chemical equation for the given reaction is ( boldsymbol{F e}_{2} boldsymbol{O}_{3(x)}+boldsymbol{2} boldsymbol{A} boldsymbol{l}_{(x)} rightarrow ) Ferricoxide ( begin{array}{cc}boldsymbol{A} boldsymbol{l}_{2} boldsymbol{O}_{boldsymbol{3}(boldsymbol{x})} & boldsymbol{+} boldsymbol{2} boldsymbol{F} boldsymbol{e}_{(boldsymbol{x})} \ text {Aluminium oxide} & text {Iron}end{array} ) Which of the following substances is oxidized in the given reaction? A ( cdot A l_{2} O_{3} ) в. ( F e_{2} O_{3} ) ( c . A l ) D. ( F e ) | 11 |
| 443 | Balance the following equation by ion electron method. ( boldsymbol{P}_{4}+boldsymbol{O H}^{-}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{2}^{-}+boldsymbol{P H}_{3} ) | 11 |
| 444 | Cen when no current 10ws uvugu ce Q16. Calculate the oxidation number of Cr in [Cr ( HO)Jion. | 11 |
| 445 | What sorts of informations can you draw from the following reaction? ( (boldsymbol{C N})_{2}(boldsymbol{g})+mathbf{2 O H}^{-}(boldsymbol{a q}) rightarrow ) ( boldsymbol{C N}^{-}(boldsymbol{a q})+boldsymbol{C N O ^ { – }}(boldsymbol{a q})+boldsymbol{H}_{2} boldsymbol{O}(l) ) | 11 |
| 446 | What are the oxidation number of the underlined elements in each of the following and how do you rationalise your results? ( boldsymbol{K} underline{boldsymbol{I}}_{mathbf{3}} ) | 11 |
| 447 | Which of the following statement(s) is/are true? This question has multiple correct options A. All reactions are oxidation and reduction reactions. B. Oxidising agent is itself reduced. c. oxidation and reduction always go side by side D. Oxidation number during reduction decreases. | 11 |
| 448 | In a galvanic cell, the electrons flow from: A. anode to cathode through the solution B. cathode to anode through the solution C. anode to cathode through the external circuit D. cathode to anode through the external circuit | 11 |
| 449 | 2. Oxalic acid H,C,0, reacts with permanganate on according to the balanced equation given below. How many milliliter of 0.0154 M KMnO solution is required to react 25.0 mL of 0.0208 MH,C,0, solution? 5H_C20_(aq) + 2MnO2 +6H*(aq) → 2Mn2+(aq) + 10CO2(g) + 8H2O(1) (a) 13.5 mL (b) 18.5 mL (c) 33.8 mL (d) 84.4 mL | 11 |
| 450 | Write balanced chemical equation for the reaction of calcium oxide with water? | 11 |
| 451 | The number of redox reactions from the following equations are: a. ( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{F} boldsymbol{e}^{3+} longrightarrow boldsymbol{F} boldsymbol{e}^{2+}+boldsymbol{S} downarrow+boldsymbol{H}^{oplus} ) b. ( boldsymbol{I}^{ominus}+boldsymbol{I} boldsymbol{O}_{3}^{ominus}+boldsymbol{H}^{oplus} longrightarrow boldsymbol{I}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) c. ( boldsymbol{B} boldsymbol{i}(boldsymbol{s})+boldsymbol{N} boldsymbol{O}_{3}^{ominus}+boldsymbol{H}^{oplus} longrightarrow boldsymbol{N} boldsymbol{O}_{2}+ ) ( B i^{3+}+H_{2} O ) ( mathbf{d .} boldsymbol{I}^{ominus}+boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O} longrightarrow boldsymbol{I}_{2}+stackrel{ominus}{boldsymbol{O}} boldsymbol{H} ) e. ( boldsymbol{C u}(boldsymbol{s})+boldsymbol{A} boldsymbol{u}^{oplus} longrightarrow boldsymbol{A} boldsymbol{u}(boldsymbol{s})+boldsymbol{C} boldsymbol{u}^{2+} ) | 11 |
| 452 | Calculate the equilibrium constant for the redox reaction at ( 25^{circ} mathrm{C}, S r_{(s)}+ ) ( M g_{(a q)}^{2+} rightarrow S r_{(a q)}^{2+}+M g_{(s)}, ) that occurs in a galvanic cell. ( boldsymbol{E}_{M g^{2+} / M g}^{o}=-2.37 mathrm{V} ) and ( boldsymbol{E}_{boldsymbol{S r}^{2}+/ boldsymbol{S} boldsymbol{r}}^{o}=-boldsymbol{2} . boldsymbol{8} boldsymbol{9} boldsymbol{V} ) A ( cdot 2.69 times 10^{15} ) В. ( 2.69 times 10^{17} ) D. ( 3.69 times 10^{15} ) | 11 |
| 453 | Aqueous solutions of magnesium chloride and silver nitrate are mixed to form solid silver chloride and aqueous magnesium nitrate.The balanced net ionic equation contains which of the following terms? ( mathbf{A} cdot A g_{(a q)}^{+} ) B. ( M g_{(a q)}^{2+} ) c. ( N O_{3(a q)}^{-} ) D. ( 2 N O_{3(a q)}^{-} ) E ( .3 A g C l_{s} ) | 11 |
| 454 | Why can ( M n O_{2} ) be reduced by ‘ ( A l^{prime} ) and not by carbon? | 11 |
| 455 | Which one is the oxidising agent in the reaction given below? ( mathbf{2} boldsymbol{C r} boldsymbol{O}_{mathbf{4}}^{2-}+mathbf{2} boldsymbol{H}^{+} rightarrow boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+boldsymbol{H}_{2} boldsymbol{O} ) A . ( H^{+} ) в. ( C r_{2} O_{7}^{-2} ) ( c cdot C r^{2} ) D. None | 11 |
| 456 | Write the following equation in ionic form. ( M n O_{2}+4 H C l rightarrow M n C l_{2}+2 H_{2} O+ ) ( C l_{2} ) | 11 |
| 457 | Write the stoichiometric coefficient for the following reaction: ( boldsymbol{x} boldsymbol{I}_{2}+boldsymbol{y} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{I} boldsymbol{O}_{3}^{-}+boldsymbol{z} boldsymbol{I}^{-}+boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O} ) B. ( x-(3), y-(2), z-(3) ) ( c cdot x-(3), y-(6), z-(5) ) ( D cdot x-(3), y-(3), z-(3) ) | 11 |
| 458 | Select the incorrect statement for developing of an exposed camera film involving the reaction. A. Hydroquinol acts as reductant. B. ( A g^{+} ) acts as oxidant. C. Hydroquinol and AgBr undergoes redox change D. It involves intramolecular change. | 11 |
| 459 | Four ( C l_{2} ) molecules undergo a loss and gain of 6 mole of electrons to form two oxidation states of ( C l ) in auto redox change. What are the ( +v e ) and ( -v e ) oxidation states of ( C l ) in the change: A ( cdot C l^{5+}, C l^{circ} ) в. ( C l^{7+}, C l^{-} ) ( mathbf{c} cdot C l^{3+}, C l^{circ} ) D. ( C l^{3+}, C l^{-} ) | 11 |
| 460 | The following reaction is balanced if ( boldsymbol{X}+boldsymbol{Y} ) is ( mathbf{5} boldsymbol{H}_{2} boldsymbol{O}_{2}+boldsymbol{X} boldsymbol{C l} boldsymbol{O}_{2}+mathbf{2} boldsymbol{O} boldsymbol{H}^{-} rightarrow ) ( boldsymbol{X} boldsymbol{C l}^{-}+boldsymbol{Y} boldsymbol{O}_{2}+boldsymbol{6} boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 461 | Identify the redox reaction taking place in a beaker. ( left.mathbf{A} cdot Z n_{(} sright)+C u_{(a q)}^{2+} rightarrow Z n_{(a q)}^{2++}+C u(s) ) B. ( left.C u(s)+2 A g_{(a q)}^{+} rightarrow C u_{(a q)}^{2+}+2 A g_{(} sright) ) C ( left.cdot C u_{(} sright)+Z n_{(a q)}^{2+} rightarrow Z n(s)+C u_{(a q)}^{2+} ) ( left.text { D. }left.2 A g_{(} sright)+C u_{(a q)}^{2+} rightarrow 2 A g_{(a q)}^{+}+C u_{(} sright) ) | 11 |
| 462 | Write balanced net ionic equation for the following reactions in acidic solution: ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{N} boldsymbol{O}_{3}^{-}+boldsymbol{N} boldsymbol{O}(boldsymbol{g}) ) A ( cdot H N O_{2}(a q) rightarrow H N O_{3}^{-}+2 N O(g)+H_{2} O ) B ( cdot 2 H N O_{2}(a q) rightarrow 2 H N O_{3}^{-}+2 N O(g)+2 H_{2} O ) ( mathrm{c} cdot 3 mathrm{HNO}_{2}(a q) rightarrow mathrm{NO}_{3}^{-}+2 mathrm{NO}(g)+mathrm{H}_{2} mathrm{O}+mathrm{H}^{+} ) D. None of the above | 11 |
| 463 | Given are two figures of Daniell cell(X) and (Y). Study the figures and mark the incorrect statement from the following. A . In fig( ( (x) ) ) electrons flow from ( Z n ) rod to ( C u ) rod hence current flows from ( C u ) to ( Z nleft(E_{text {ext}}1.1 mathrm{V}right) ) ( c . ln operatorname{fig}(x), Z n ) dissolves at anode and ( C u ) deposits at cathode D. In fig ( ( gamma ) ), ( Z n ) is deposited at ( C u ) and ( C u ) is deposited at ( z_{n} ) | 11 |
| 464 | Which of the following changes represents a disproportional reaction(s)? ( mathbf{A} cdot C l_{2}+2 O H^{-} rightarrow C l O^{-}+C l^{-}+H_{2} O ) B. ( C u_{2} O+2 H^{+} rightarrow C u+C u^{2+}+H_{2} O ) ( mathbf{C} cdot 2 H C u C l_{2} frac{text {dilution with}}{text {water}} C u+C u^{2+}+4 C l^{-}+2 H^{+} ) D. All of the above | 11 |
| 465 | Which of the following is a redox reaction: A ( cdot 2 operatorname{Na}left[A g(C N)_{2}right]+Z n rightarrow N a_{2}left[operatorname{Zn}(C N)_{4}right]+2 A g ) в. ( B a O_{2}+H_{2} S O_{4} rightarrow B a S O_{4}+H_{2} O_{2} ) c. ( N_{2} O_{5}+H_{2} O rightarrow 2 H N O_{3} ) D. ( A g N O_{3}+K I longrightarrow A g I+K N O_{3} ) | 11 |
| 466 | Assertion The only way to get ( F_{2} ) from ( F^{-} ) is to oxidise electrolytically Reason The recovery of halogens from their halides requires an oxidation 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 |
| 467 | ( boldsymbol{F} e^{2+} rightarrow boldsymbol{F} e^{3+}+boldsymbol{e}^{-} ; boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-}+boldsymbol{5} boldsymbol{e}^{-} rightarrow ) ( M n^{2+}, ) the ratio of stoichiometric coefficient of ( F e^{2+} ) and ( M n O_{4}^{-} ) in the balanced redox reaction is: A .1: 5 B. 5: 1 c. 2: 3 ( D cdot 6: 1 ) | 11 |
| 468 | Calculate the oxidation number: (i) ( M o ) in ( left(N H_{4}right)_{2} M o O_{4} ) (ii) ( N i ) in ( N i(C N)_{4}^{2-} ) | 11 |
| 469 | In the given reaction, ( mathbf{2} boldsymbol{K}_{mathbf{4}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right](boldsymbol{a} boldsymbol{q})+boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) longrightarrow ) ( mathbf{2} boldsymbol{K}_{mathbf{3}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right](boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{K} boldsymbol{O} boldsymbol{H}(boldsymbol{a} boldsymbol{q}) ) Which of the following processes takes place? A. Oxidation due to removal of potassiummm B. Oxidation due to removal of iron c. Reduction due to removal of potassium D. Oxidation due to removal of electronegative element | 11 |
| 470 | Assertion Oxidation number of chromium in ( boldsymbol{C r} boldsymbol{O}_{5} ) is ( +boldsymbol{6} ) Reason Oxidation number of each oxygen atom in ( C r O_{5} ) is -2 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 |
| 471 | 3. Which of the following is most powerful oxidizing agent in the following (a) o (b) KMnO (C) H,02 (d) K,Cr, | 11 |
| 472 | Given reaction ( boldsymbol{H} boldsymbol{C} boldsymbol{H} boldsymbol{O} rightarrow boldsymbol{C} boldsymbol{H}_{3} boldsymbol{O} boldsymbol{H}+ ) ( H C O O^{-} ) is an example of A. intermolecular redox change B. intramolecular redox change c. disproportionation or auto redox D. none of these | 11 |
| 473 | Assertion Following reaction is a disproportionation reaction: ( boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{2} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{B} boldsymbol{r} boldsymbol{O}^{-}+boldsymbol{B} boldsymbol{r}^{-}+ ) ( 2 H_{2} O ) Reason ( B r_{2} ) is oxidized to ( B r O^{-} ) as well as reduced to ( B r^{-} ) 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 |
| 474 | toppr Q туре your question reactions that are physically separated. So that the electrons must travel through a wire from the reducing agent to the oxidizing agent. The reducing agent loses electrons and is oxidized in a reaction that takes To maintain a net zero charge in each compartment, there is a limited flow of ions through a salt bridge. For example, in a car battery the reducing agent is oxidized by the following reaction, which involves a lead | 11 |
| 475 | Loss of an electron is called : A. reduction B. oxidation c. ( A ) or ( B ) D. none of the above | 11 |
| 476 | Which of the following is/are correct about blue per chromate? This question has multiple correct options A. It has two peroxide bonds. B. It has four oxygen atoms having oxidation number -1. C ( . ) It reacts with ( H_{2} S O_{4} ) to give oxygen D. It acts as oxidant as well as reductant. | 11 |
| 477 | ( boldsymbol{H}_{2}+boldsymbol{C l}_{2} rightarrow boldsymbol{H} boldsymbol{C l} ) The above reaction is an example of which of the following reaction? A. Combination reaction B. Decomposition reaction c. Displacement reaction D. Double displacement reaction | 11 |
| 478 | Q4. Fluorine reacts with ice and results in the change: HO(s) + F.(g) HF(g) + HOF(8) Justify that this reaction is a redox reaction. TATO N 1 bolo baye | 11 |
| 479 | Reaction occurring in lead storage battery is a kind of: A. disproportionation B. comproportionation c. oxidation D. reduction | 11 |
| 480 | ( boldsymbol{S} boldsymbol{O}_{2} ) reduces ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-} ) to ( boldsymbol{C r}^{2+} ). The change in oxidation number of ( boldsymbol{C r} ) is: | 11 |
| 481 | HOCl( (a q) ) is the molecule that kills bacteria wen chlorine is added to water The following reaction produces this molecule ( boldsymbol{C l}_{2}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(l) rightleftharpoons boldsymbol{H} boldsymbol{O} boldsymbol{C l}(boldsymbol{a} boldsymbol{q})+ ) ( boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q})+boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q}) ) Which statement about this reaction is correct? A. Chlorine is both oxidised and reduced B. Chlorine is oxidised but not reduced c. Hydrogen is both oxidised and reduced D. Hydrogen is oxidised but not reduced | 11 |
| 482 | Identify disproportionation reaction A. ( C H_{3}+2 O_{2} rightarrow C O_{2}+2 H_{2} O ) в. ( C H_{4}+4 C l_{2} rightarrow C C l_{4}+4 H C l ) c. ( 2 F_{2}+2 O H^{-} rightarrow 2 F^{-}+O F_{2}+H_{2} O ) D. ( 2 N O_{2}+2 O H^{-} rightarrow N O_{2}^{-}+N O_{3}^{-}+H_{2} O ) | 11 |
| 483 | Out of the following redox reactions ( boldsymbol{I} cdot boldsymbol{N} boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{3} stackrel{Delta}{rightarrow} boldsymbol{N}_{2} boldsymbol{O}+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O} ) III.N ( boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{2} stackrel{Delta}{rightarrow} boldsymbol{N}_{2}+mathbf{2} boldsymbol{H}_{2} boldsymbol{O} ) IIII.PCl( _{5} stackrel{Delta}{rightarrow} P C l_{3}+C l_{2} ) disproportionation is not shown in: A . I and II B. II and III c. I and III D. I, II and III | 11 |
| 484 | Statement I: The ( A l^{3+} ) ion needs to be reduced to form aluminum metal. Statement II: Reduction is a gain of electrons. A. Both Statement I and Statement II are correct and Statement II is the correct explanation of Statement B. Both Statement I and Statement II are correct, but Statement II is not the correct explanation of Statement I. c. Statement I is correct, but Statement II is incorrect D. Statement I is incorrect, but Statement II is correct | 11 |
| 485 | ( boldsymbol{A l}+boldsymbol{N} boldsymbol{O}_{mathbf{2}}^{-} rightarrow boldsymbol{A l}(boldsymbol{O} boldsymbol{H})_{4}^{-}+boldsymbol{N} boldsymbol{H}_{3} ) The oxidizing agent for this reaction is A . ( A l ) в. ( N ) ( c cdot O ) D. both ( A ) and ( B ) | 11 |
| 486 | Which of the following species are oxidised and reduced in the following (unbalanced) reaction? ( boldsymbol{C N}^{-}+boldsymbol{O C l}^{-} longrightarrow boldsymbol{N}_{2}+boldsymbol{H} boldsymbol{C O}_{3}^{-}+ ) ( C l^{-} ) A. oxidized- ( C, N ) in ( C N^{-} ) “, reduced ( -O C l^{-} ) B. Oxidized- ( N, C N^{-}, H C O_{3}^{-} ; N_{2} ) reduced ( -C O C l^{-} ) C. oxidized- ( C, N, H C O_{3}^{-} ; N_{2} ) reduced ( -O C l^{-}, C N^{-} ) D. None of these | 11 |
| 487 | Photographic paper is developed with alkaline hydroquinone. Select the correct answer. A. Hydroquinone is the oxidant B. ( A g^{+} ) is the oxidant C ( . B r^{-} ) is the oxidant D. ( A g^{+} ) is the reductant | 11 |
| 488 | Give equations for the decomposition of a metallic ¡] chloride ii] nitrate with conc. ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) | 11 |
| 489 | Q10. (a) Calculate the oxidation number of (i) C in CH,COOH (ii) S in 5,062 (b) Give one example of disproportionation reaction. | 11 |
| 490 | Consider the following reaction, taking place in a container fitted with a movable piston. ( 2 S O_{2}(g)+O_{2}(g) rightarrow 2 S O_{3}(g) ) Suppose we place two moles each of ( boldsymbol{S O}_{2} ) and ( boldsymbol{O}_{2} ) in the reaction vessel at ( 25^{circ} mathrm{C}, ) and adjust the volume to give a total pressure of 1.0 atm. The reaction is ignited by a spark, and goes to completion. The temperature is returned to ( 25^{circ} mathrm{C} ) Which of the following best describes this system after reaction is complete? ( A cdot S O_{2} ) is limiting. The volume of the system remains the same B. Neither reactant is limiting. The volume of the system decreases C. ( S O_{2} ) is limiting. The volume of the system decreases. D. ( O_{2} ) is limiting. The volume of the system remains the same | 11 |
| 491 | The oxidation number of Na in NaCl: A. 0 B. – – ( c cdot+1 ) D. 2 ( E cdot+2 ) | 11 |
| 492 | Which of the following is not a disproportionation reaction? ( N H_{4} N O_{3} stackrel{Delta}{longrightarrow} N_{2} O+H_{2} O ) II. ( boldsymbol{P}_{4} stackrel{Delta}{longrightarrow} boldsymbol{P} boldsymbol{H}_{3}+boldsymbol{H} boldsymbol{P} boldsymbol{O}_{2}^{ominus} ) III. ( boldsymbol{P C l}_{5} stackrel{boldsymbol{Delta}}{longrightarrow} boldsymbol{P C l}_{3}+boldsymbol{C l}_{2} ) IV. ( boldsymbol{I} boldsymbol{O}_{3}^{ominus}+boldsymbol{I}^{ominus} longrightarrow boldsymbol{I}_{2} ) A . ।, ॥ B. I, III, IV c. ॥, IV D. ।, II | 11 |
| 493 | The ( p H ) of a ( 10 m l ) aqueous solution of ( H C l ) is ( 4 . ) The amount of water to be added to this solution in order to change its ( p H ) from 4 to 5 is? A. ( 30 m ) в. ( 60 mathrm{ml} ) ( c .90 m l ) D. ( 120 m l ) | 11 |
| 494 | ( 2 C u I rightarrow C u+C u I_{2}, ) the reaction is : A. redox B. neutralisation c. displacement D. none of the above | 11 |
| 495 | Find the oxidation number of elements in each case: ( C r ) in ( boldsymbol{C r} boldsymbol{O}_{2} boldsymbol{C l}_{2}, boldsymbol{N} boldsymbol{a}_{2} boldsymbol{C r}_{3} boldsymbol{O}_{10}, boldsymbol{C r}_{2}left(boldsymbol{S O}_{4}right)_{3} ) and ( left[boldsymbol{C r} boldsymbol{O}_{8}right]^{3-} ) A. +6,+6,+3,+5 В. +5,+6,+3,+4 ( mathbf{c} cdot+4,+6,+2,+5 ) D. None of the above | 11 |
| 496 | The decomposition of ( K C I O_{3} ) to ( K C l ) and ( O_{2} ) on heating is an example of : A. intermolecular redox change B. intramolecular redox change c. disproportionation or auto redox change D. none of the above | 11 |
| 497 | Reduction reaction is: A. addition of electron B. decrease in oxidation state of element C . addition of hydrogen D. all of these | 11 |
| 498 | An oxidation number can be: A . positive B. negative c. zero D. all of these | 11 |
| 499 | Which of the following have been arrange in order of decreasing oxidation number of sulphur? This question has multiple correct options A ( cdot N a_{2} S_{4} O_{6}>H_{2} S_{2} O_{7}>N a_{2} S_{2} O_{3}>S_{8} ) в. ( S O_{2}^{+}>S O_{4}^{2-}>S O_{3}^{2-}>H S O_{4} ) c. ( H_{2} S O_{5}>H_{2} S O_{3}>S C l_{2}>H_{2} S ) D. ( H_{2} S O_{4}>S O_{2}>H_{2} S>H_{2} S_{2} O_{8} ) | 11 |
| 500 | Bromine reacts with the hot aqueous alkali to give bromide and bromate. What is the change that is brought about in the oxidation state of bromine to bromate? A ( .-1 ) to +5 B. 0 to +5 ( c cdot 0 ) to +7 D. None of these | 11 |
| 501 | ( boldsymbol{C H}_{4}+boldsymbol{O}_{2} rightarrow boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) is: A. combustion reaction B. redox Reaction c. both ( A ) and ( B ) D. none of the above | 11 |
| 502 | Fill in the blanks. Sulphur ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ) to produce nitrogen dioxide. | 11 |
| 503 | Which of the following is/are reduction reaction ? A. Hydrogenation of alkene and alkyne B. Ozonolysis with ( O_{3} / Z n ) c. Halogenation of alkene D. All of these | 11 |
| 504 | The oxidation state(s) of ( C l ) in ( C a O_{2} C l_{2} ) (bleaching powder) is/are: ( A cdot+1 ) only B. – – ‘ only ( c cdot+1 ) and -1 D. none of these | 11 |
| 505 | Formulate a call for each of the following reactions; ( S n^{2+}(a q)+2 A g C l(s) longrightarrow S n^{4+}(a q)+ ) ( 2 A g(s)+2 C l^{-}(a q) ) ( M g(s)+B r_{2}(l) longrightarrow M g^{2+}(a q)+ ) ( 2 B r^{-}(a q) ) | 11 |
| 506 | The balanced equation in acidic medium is : ( boldsymbol{S}_{2} boldsymbol{O}_{3}^{2-}+boldsymbol{S} boldsymbol{b}_{2} boldsymbol{O}_{5} stackrel{boldsymbol{H}^{+}}{rightarrow} boldsymbol{S b} boldsymbol{O}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{3} ) A ( cdot 3 S_{2} O_{3}^{2-}+2 S b_{2} O_{5}+6 H^{+} 3 H_{2} O rightarrow 4 S b O+6 H_{2} S O_{3} ) B . ( 2 S_{2} O_{3}^{2-}+2 S b_{2} O_{5}+6 H^{+} 3 H_{2} O rightarrow 4 S b O+4 H_{2} S O_{3} ) ( mathrm{c} cdot 3 S_{2} O_{3}^{2-}+2 S b_{2} O_{5}+4 H^{+} 2 H_{2} O rightarrow 4 S b O+2 H_{2} S O_{3} ) D. none of these | 11 |
| 507 | What is the oxidation number of ( M n ) in ( M n O_{2} ? ) ( A cdot+2 ) B. +4 ( c cdot-2 ) D. – | 11 |
| 508 | dic medium are required 12. Equal moles of K Cr,0, in acidic medium for oxidation of by 1 mole of (a) FeSO3 (b) FeS204 (c) Fe (SO2)3 (d) Al2(SO3)2 | 11 |
| 509 | In the reaction, ( boldsymbol{X}+boldsymbol{I}_{2}+mathbf{2} boldsymbol{H} boldsymbol{C l} rightarrow boldsymbol{S} boldsymbol{n} boldsymbol{C l}_{4}+mathbf{2 H I} ) The correct option regarding ( X ) is/are: A. It is an strong reducing agent B. It is an angular molecule C. It is used as a reagent in test of ( H g^{2+} ) radical D. All of the above | 11 |
| 510 | Consider the following reaction. [ left.right|_{mathbf{C H O}} ^{mathbf{C H O}}+left.mathbf{O H}^{-} longrightarrowright|_{mathbf{C H}_{2} mathbf{O H}} ^{mathbf{O O}^{-}} ] A. It is not a disproportionation reaction B. It is intramolecular redox reaction C. ( O H^{-} ) is reducing as well as oxidising agent D. ( (C H O)_{2} ) is a reducing as well as oxidising agent | 11 |
| 511 | How many gram of ( K M n O_{4} ) is contained in 4 litre of ( 0.05 N ) solution. The ( K M n O_{4} ) is to used as an oxidant in acid medium ( left(M_{W}=158right): ) A. ( 1.58 g ) B. ( 15.8 g ) c. ( 6.32 g ) D. ( 31.6 g ) | 11 |
| 512 | Of the following acids, the one that is strongest is : A. ( H B r O_{4} ) в. НОС l c. ( H N O_{2} ) D. ( H_{3} P O_{3} ) | 11 |
| 513 | Which statement is correct about the following reaction? ( mathrm{ZnO}+mathrm{CO} rightarrow mathrm{Zn}+mathrm{CO}_{2} ) A. zno is being oxidized B. co is being reduced ( mathrm{C} cdot mathrm{CO}_{2} ) is being oxidized D. zno is being reduced | 11 |
| 514 | The reduced product formed when chlorine reacts with ( boldsymbol{H}_{2} boldsymbol{S} ) : A . ( N a C l ) в. ( C u ) c. ( operatorname{Fe}left(O H_{3}right) ) D. ( H C l ) | 11 |
| 515 | ( H_{2} S_{2} O_{8} ) and ( H_{2} S O_{5} ) both have +6 oxidation state of sulphur. It is due to the: A. presence of peroxy group B. presence of superoxo group c. presence of neutral group D. presence of ozone | 11 |
| 516 | ( boldsymbol{C l O}_{3}^{-}+boldsymbol{C l}^{-} rightarrow boldsymbol{C l}_{2}+boldsymbol{C l O}_{2} ) Which of the following is correct for this reaction: A. Its a disproportion reaction B. ( C l ) is both oxidised and reduced c. ( C l ) is both reducing and oxydising agent D. All of these | 11 |
| 517 | Which of the statements about the reaction below are incorrect? ( 2 P b O(s)+C(s) rightarrow 2 P b(s)+C O_{2}(g) ) (a) Lead is getting reduced. (b) Carbon dioxide is getting oxidised. (c) Carbon is getting oxidised. (d) Lead oxide is getting reduced. A ( cdot(a) ) and ( (b) ) B. (a) and (c) ( c cdot(a),(b) ) and ( (c) ) D. All | 11 |
| 518 | In the following (unbalanced) reaction: ( boldsymbol{I}^{-}+boldsymbol{O}_{3} longrightarrow boldsymbol{O}_{2}+boldsymbol{I}_{2} ) What is oxidising agent? ( A cdot O_{3} ) B . ( I^{-} ) c. None D. Both | 11 |
| 519 | Give a clear idea about how ( M n O_{4}^{-}, C r O_{4}^{2-}, C r_{2} O_{7}^{2-} ) changes its oxidation state when it is in the acidic, basic and neutral medium. | 11 |
| 520 | Oxidation number of the nitrogen atom in ( H N O_{3} ) is : A . – B. +1 ( c cdot 0 ) ( D cdot+4 ) ( mathrm{E} cdot+5 ) | 11 |
| 521 | The balanced equation in basic medium is : ( boldsymbol{C l O}_{2}+boldsymbol{S b O}_{2}^{-} rightarrow boldsymbol{C l O}_{2}^{-}+boldsymbol{S b}(boldsymbol{O H})_{6}^{-} ) A ( cdot 2 C l O_{2}+S b O_{2}^{-}+2 O H^{-}+2 H_{2} O rightarrow 2 C l O_{2}^{-}+ ) ( S b(O H)_{6} ) B . ( 2 C l O_{2}+5 S b O_{2}^{-}+2 O H^{-}+3 H_{2} O rightarrow 2 C l O_{2}^{-}+ ) ( 2 S b(O H)_{6} ) ( mathrm{c} cdot 2 mathrm{ClO}_{2}+mathrm{SbO}_{2}^{-}+3 mathrm{OH}^{-}+4 mathrm{H}_{2} mathrm{O} rightarrow 2 mathrm{ClO}_{2}^{-}+ ) ( 3 S b(O H)_{6} ) D. None of these | 11 |
| 522 | Addition of silver nitrate to sodium chloride solution causes preciptation of silve chloride. This is an example reaction | 11 |
| 523 | An oxidation process involves: A. increase in oxidation number B. Decrease in oxidation number c. Addition of electrons D. Removal of electronegative element | 11 |
| 524 | Balance the following equation in basic medium by ion-electron method and oxidation number methods and identify the oxidising agent and the reducing agent ( boldsymbol{C l}_{2} boldsymbol{O}_{7}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{C l O}_{2}^{-}(boldsymbol{a q})+ ) ( boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{H}^{+} ) | 11 |
| 525 | The metals undergoing disproportionation are A. sn B. Na ( c cdot c u ) D. ( c a ) | 11 |
| 526 | In the reaction of ( Z n+F e S O_{4} rightarrow ) ( Z n S O_{4}+F e ) A. zn gets oxidized B. Fe gets oxidized c. zn is oxidizing agent D. zn and Fe both get oxidized | 11 |
| 527 | Match the Column-I with Column-II. | 11 |
| 528 | Which of the following is incorrect about ( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7} ? ) A ( . ) It can be prepared from ( K_{2} C r O_{4} ) B. It is used in redox titrations c. It is stable in both acid & base D. It is orange in colour | 11 |
| 529 | The complete balanced equation is: ( boldsymbol{C l}_{2}+boldsymbol{I O}_{3}^{-}+boldsymbol{O H}^{-} rightarrow boldsymbol{I} boldsymbol{O}_{4}^{-}+boldsymbol{C l}^{-}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ) A ( cdot C l_{2}+I O_{3}^{-}+2 O H^{-} rightarrow I O_{4}^{-}+2 C l^{-}+H_{2} O ) в. ( 4 C l_{2}+I O_{3}^{-}+4 O H^{-} rightarrow I O_{4}^{-}+C l^{-}+H_{2} O ) c. ( C l_{2}+I O_{3}^{-}+3 O H^{-} rightarrow I O_{4}^{-}+2 C l^{-}+H_{2} O ) D. none of these | 11 |
| 530 | Q.14 The exhibition of various oxidation states by an element is also related to the outer orbital electronic configuration of its atom. Atom (s) having which of the following outermost electronic configurations will exhibit more than one oxidation state in its compounds. (2) 35′ (b) 3d 452 (c) 3d24s? (d) 3s 3p | 11 |
| 531 | Balance the following equation by oxidation number method. ( boldsymbol{F} boldsymbol{e}_{2}left(boldsymbol{S} boldsymbol{O}_{4}right)_{3}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{3}+boldsymbol{H}_{2} boldsymbol{O} rightarrow ) ( boldsymbol{F} boldsymbol{e} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) | 11 |
| 532 | ( y=8 ) ( y=4 ) ( y ) | 11 |
| 533 | What is the atomic number of the following elements Potassium iodide, lodine is | 11 |
| 534 | Find the oxidation number of nitrogen in each case: ( N ) in ( N H_{3}, N H_{2} O H, N a N_{3} ) and ( N H_{4} N O_{2} ) ( mathbf{A} cdot_{-3,-1,-frac{1}{3},+3 &-3} ) B. ( _{-3,-2,-frac{1}{3},+1} ) D. None of the above | 11 |
| 535 | Identify ( X ) in the equation given below. ( boldsymbol{F} boldsymbol{e} boldsymbol{C l}_{3}+boldsymbol{S O}_{2}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{C l}_{2}+ ) ( boldsymbol{H} boldsymbol{C l}+boldsymbol{X} ) A ( . H_{2} S ) в. ( S O_{3} ) c. ( H_{2} S O_{4} ) D. ( H_{2} S O_{3} ) | 11 |
| 536 | In balancing the reaction ( boldsymbol{x} boldsymbol{Z} boldsymbol{n}+ ) ( N O_{3}^{-}+y H^{+} rightarrow x Z n^{2+}+N H_{4}^{+}+ ) ( z H_{2} O, x, y ) and ( z ) are respectively: A .4,10,3 в. 3,8,3 ( mathrm{c} cdot 3,10,3 ) D. 4,3,10 | 11 |
| 537 | Which of the following does not define reduction? A. Gain of electron and addition of hydrogen B. Removal of oxygen c. Decrease in oxidation state D. Removal of electron, removal of hydrogen, addition of oxygen and increase in oxidation state | 11 |
| 538 | Zinc granules are added in excess to ( mathbf{5 0 0} boldsymbol{m L} ) of ( mathbf{1 . 0} boldsymbol{M} ) nickel nitrate solution at ( 25^{circ} C ) until the equilibrium is reached. If the standard reduction potentials of ( Z n^{2+} / Z n ) and ( N i^{2+} / N i ) are -0.75 and -0.24 volt respectively find out the concentration of ( N i^{2+} ) ions in solution at equilibrium. | 11 |
| 539 | ( B r_{2}+H_{2} O_{2} rightarrow ) (in acidic medium) Complete the reaction. | 11 |
| 540 | In a reaction, 4 mol of electrons are transferred to one mol of ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ) when it acts as an oxidant. The possible reduction product is : A. 0.5 mol ( N_{2} ) B. 0.5 mol ( N_{2} ), c. 1 mol ( N O_{2} ) D. 1 mol ( N H_{3} ) | 11 |
| 541 | ( K M n O_{4} ) is acidified for redox titrations by: A. ( H C l ) в. ( H N O_{3} ) c. ( H_{2} S O_{4} ) D. any of these | 11 |
| 542 | ( 2 K_{2} C r_{2} O_{7}+8 H_{2} S O_{4} rightarrow 2 K_{2} S O_{4}+ ) ( 2 C r_{2}left(S O_{4}right)_{3}+8 H_{2} O+3 O_{2} ) Is the above reaction correct? A. True B. False | 11 |
| 543 | Q21. In the reaction M,O, + 4HCI which species is oxidised. M.CI+ CI+ | 11 |
| 544 | A mixed solution of potassium hydroxide and sodium carbonate required ( 15 mathrm{mL} ) of ( frac{N}{20} H C l ) solution when titrated with phenolphthalein as an indicator. But the same amount of the solution when titrated with methyl orange as an indicator required ( 25 mathrm{ml} ) of the same acid. The amount of ( K O H ) present in the solution is : A. ( 0.014 mathrm{g} ) B. ( 0.14 mathrm{g} ) c. ( 0.028 mathrm{g} ) D. ( 1.4 mathrm{g} ) | 11 |
| 545 | ( mathbf{3} N_{2} H_{4}+2 B r O_{3}-3 N_{2}+ ) ( 2 B r^{-}+6 H_{2} O ) The above reaction shows: A. intermolecular redox B. auto-redox C. intramolecular redox D. either of these | 11 |
| 546 | Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions ( boldsymbol{P b}_{(s)}+boldsymbol{P b O}_{2(s)}+mathbf{2 H}_{2} boldsymbol{S O}_{4(a q)} rightarrow ) ( 2 P b S O_{4(s)}+2 H_{2} O_{(l)} ) | 11 |
| 547 | When ( K M n O_{4} ) acts as an oxidising agent and forms ( M n^{+2}, ) the number of electrons transferred per molecule of ( K M n O_{4} ) is : | 11 |
| 548 | The oxidation number of Cr is +6 in This question has multiple correct options | 11 |
| 549 | Assign oxidation number to the underlined element in ( boldsymbol{H}_{4} underline{boldsymbol{P}}_{2} boldsymbol{O}_{7} ) | 11 |
| 550 | The complete balanced equation is: ( boldsymbol{C u}+boldsymbol{N} boldsymbol{O}_{3}^{-}+ldots . rightarrow boldsymbol{C u}^{2+}+boldsymbol{N} boldsymbol{O}_{2}+ ) A ( cdot C u+4 H^{+}+2 N O_{3}^{-} rightarrow C u^{2+}+2 N O_{2}+2 H_{2} O ) B . ( C u+6 H^{+}+N O_{3}^{-} rightarrow C u^{2+}+2 N O_{2}+2 H_{2} O ) c. ( C u+4 H^{+}+2 N O_{3}^{-} rightarrow 2 C u^{2+}+N O_{2}+2 H_{2} O ) D. none of these | 11 |
| 551 | Which of the following not represents redox reactions? ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{2} stackrel{theta}{boldsymbol{O}} boldsymbol{H} longrightarrow boldsymbol{2} boldsymbol{C r} boldsymbol{O}_{4}^{2-}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ) II. ( Z n+C u S O_{4} longrightarrow Z n S O_{4}+C u ) III. ( 2 M n O_{4}^{ominus}+3 M n^{2+}+4 stackrel{theta}{O} H longrightarrow ) ( mathbf{5} M n O_{2}+2 H_{2} O ) IV. ( 2 C u^{oplus} longrightarrow C u+C u^{2+} ) ( A ) в. ।, ॥ c. ॥ा, ।॥ D. ॥, ॥I, IV | 11 |
| 552 | Which of the following is not a redox reaction? A ( cdot 2 N O+O_{2} rightarrow 2 N O_{2} ) в. ( C l_{2}+H_{2} O rightarrow H C l+H C l O ) ( mathrm{c} cdot 2 mathrm{Cr} mathrm{O}_{4}^{2-}+2 mathrm{H}^{+} rightarrow mathrm{Cr}_{2} mathrm{O}_{7}^{2-}+mathrm{H}_{2} mathrm{O} ) D. ( M n O_{4}^{-}+8 H^{+} rightarrow M n^{2+}+4 H_{2} O ) | 11 |
| 553 | The oxidation number of phosphorus in ( boldsymbol{B} boldsymbol{a}left(boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{2}right)_{2} ) is: ( A cdot+3 ) B. +2 ( c cdot+1 ) D. – | 11 |
| 554 | Which of the following is/are redox reactions? This question has multiple correct options A. ( B a O_{2}+H_{2} S O_{4} rightarrow B a S O_{4}+H_{2} O_{2} ) в. ( 2 B a O+O_{2} rightarrow 2 B a O_{2} ) ( mathbf{c} cdot 2 K C I O_{3} rightarrow 2 K C l+3 O_{2} ) D. ( S O_{2}+2 H_{2} S rightarrow 2 H_{2} O+3 S ) | 11 |
| 555 | tion) 08. (a) Balance the following equation by oxidation number method or by.com method, MnO, Fe2+ → Mn2+ + Fe3+ acidic medium (b) Consider the cell, Zn | Zn2+ (aq) || Cu2+(aq)| Cu The standard electrode potentials are E° Zn2+/Zn = -0.76 V; E° Cu-T/Cu = +0.34 write down the cell reaction. | 11 |
| 556 | Balance the following equation by ion electron method. ( M n O_{4}^{2-}+H_{2} O rightarrow M n O_{4}^{-}+O H^{-}+ ) ( M n O_{2} ) | 11 |
| 557 | Which one of the following is not a redox reaction? A. ( C a C O_{3} rightarrow C a O+C O_{2} ) В. ( 2 H_{2}+O_{2} longrightarrow 2 H_{2} O ) ( ^{mathrm{c}} cdot_{N a+H_{2} O} rightarrow N a O H+frac{1}{2} H_{2} ) D. ( _{M n C l_{3}} rightarrow M n C l_{2}+frac{1}{2} C l_{2} ) | 11 |
| 558 | Oxidation number of ( N a ) in ( N a-H g ) amalgam is zero. If true enter 1 , else enter 0 . ( A cdot 1 ) | 11 |
| 559 | Consider the following redox reaction: ( 2 S_{2} O_{3}^{2-}+I_{2} longrightarrow S_{4} O_{6}^{2-}+2 I^{ominus} ) This question has multiple correct options A ( cdot S_{2} O_{3}^{2-} ) gets reduced to ( S_{4} O_{6}^{2} ) B. ( S_{2} O_{3}^{2-} ) gets oxidised to ( S_{4} O_{6}^{2} ) c. ( I_{2} ) gets reduced to ( I^{ominus} ) ( mathbf{D} cdot I_{2} ) gets oxidised to ( I^{ominus} ) | 11 |
| 560 | Dissolution of ( C a H_{2} ) in water is an auto-redox process. If true enter 1 , else enter 0 ( A ) | 11 |
| 561 | Consider the reactions: ( 2 S_{2} O_{3}^{2-}(a q)+I_{2}(s) longrightarrow S_{4} O_{6}^{2-}(a q)+ ) ( 2 I^{-}(a q) ) ( boldsymbol{S}_{2} boldsymbol{O}_{3}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{B} boldsymbol{r}_{2}(boldsymbol{l})+boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(l) longrightarrow ) ( mathbf{2} boldsymbol{S} boldsymbol{O}_{4}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{4} boldsymbol{B} boldsymbol{r}^{-}(boldsymbol{a} boldsymbol{q})+mathbf{1 0} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) ) Why does the same reductant thiosulphate react differently with iodine and bromine? | 11 |
| 562 | Dvide the following redox equations into oxidation half equation and reduction half equation. ( boldsymbol{a}) boldsymbol{P}_{(s)}+boldsymbol{P} boldsymbol{O}_{4(a q)}^{3} boldsymbol{H} boldsymbol{P} boldsymbol{O}_{3(a q)}^{2} ) ( boldsymbol{b}) boldsymbol{H} boldsymbol{N} boldsymbol{O}_{2(a q)} longrightarrow boldsymbol{N} boldsymbol{O}_{3(a q)}^{-}+boldsymbol{N} boldsymbol{O}_{(g)} ) ( boldsymbol{c}) boldsymbol{I} boldsymbol{O}_{boldsymbol{3}(boldsymbol{a q})}^{-}+boldsymbol{R e}_{(s)} longrightarrow boldsymbol{R e} boldsymbol{O}_{4(boldsymbol{a q})}+boldsymbol{I}_{(a q)} ) | 11 |
| 563 | The reaction of white phosphorus with aqueous ( N a O H ) gives phosphine along with another phosphorus containing compound. The reaction type, the oxidation states of phosphorus in phosphine and the other product are, respectively: A. redox reaction; -3 and -5 B. redox reaction; +3 and +5 c. disproportionation reaction; -3 and +1 D. disproportionation reaction; -3 and +3 | 11 |
| 564 | Which compound amongst the following has the highest oxidation number for ( M n ? ) ( boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}, boldsymbol{K}_{2} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}, boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2} ) and ( boldsymbol{M} boldsymbol{n}_{2} boldsymbol{O}_{3} ) | 11 |
| 565 | (a) Draw the labelled diagram of Daniell cell. (b) Write the half-reactions of oxidation and reduction taking place on electrodes. | 11 |
| 566 | Assertion The alkali metals are strong oxidizing agents. Reason The one electron in their valence shell is easily lost. 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 incorrect but Reason is correct D. Both Assertion and Reason are incorrect | 11 |
| 567 | Write the following equation in ionic form: a) ( M n O_{2}+4 H C l rightarrow M n C l_{2}+ ) ( mathbf{2} boldsymbol{H}_{mathbf{2}} boldsymbol{O}+boldsymbol{C} boldsymbol{l}_{mathbf{2}} ) b) ( 2 N a H C O_{3}+H_{2} S O_{4} rightarrow ) ( N a_{2} S O_{4}+H_{2} O+C O_{2} ) A ( cdot ) a) ( M n O_{2}+4 H^{+}+4 C l^{-} rightarrow M n^{2+}+2 C l^{-}+2 H_{2} O+ ) ( C l_{2} ) b) ( 2 N a^{+}+2 H C O_{3}^{-}+2 H^{+}+S O_{4}^{2-} rightarrow 2 N a^{+}+ ) ( S O_{4}^{2-}+2 H_{2} O+C O_{2} ) B. a) ( 2 M n O_{2}+8 H^{+}+4 C l^{-} rightarrow 2 M n^{2+}+2 C l^{-}+ ) ( 4 H_{2} O+C l_{2} ) b) ( 2 N a^{+}+2 H C O_{3}^{-}+2 H^{+}+S O_{4}^{2-} rightarrow 2 N a^{+}+ ) ( S O_{4}^{2-}+2 H_{2} O+C O_{2} ) c. a) ( M n O_{2}+4 H^{+}+3 C l^{-} rightarrow M n^{2+}+C l^{-}+2 H_{2} O+ ) ( C l_{2} ) b) ( 2 N a^{+}+2 H C O_{3}^{-}+2 H^{+}+S O_{4}^{2-} rightarrow 2 N a^{+}+ ) ( S O_{4}^{2-}+2 H_{2} O+C O_{2} ) D. None of these | 11 |
| 568 | Consider the following reaction: ( boldsymbol{H} boldsymbol{C H O}+mathbf{2}left[boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}right]^{+}+boldsymbol{3} boldsymbol{O} boldsymbol{H}^{-} rightarrow ) ( mathbf{2 A g}+boldsymbol{H C O O}^{-}+mathbf{4 N H}_{mathbf{3}}+mathbf{2 H}_{mathbf{2}} boldsymbol{O} ) Which of the following statements regarding oxidation and reduction is correct? ( mathbf{A} cdot H C H O ) is oxidised to ( H C O O^{-} ) and ( left[A gleft(N H_{3}right)_{2}right]^{+} ) is reduced to ( A g ) B. ( H C H O ) is reduced to ( H C O O^{-} ) and ( left[A gleft(N H_{3}right)_{2}right]^{+} ) is oxidised to ( A g ) ( mathbf{C} cdotleft[A gleft(N H_{3}right)_{2}right]^{+} ) is reduced to ( A g ) while ( O H^{-} ) is oxidised to ( H C O O^{-} ) ( mathbf{D} cdotleft[A gleft(N H_{3}right)_{2}right]^{+} ) is oxidised to ( N H_{3} ) while ( H C H O ) is reduced to ( H_{2} O ) | 11 |
| 569 | 0.30 Assertion (A) In the reaction between potassium permanganate and potassium iodide, permanganate ions act as oxidising agent. Reason (R) Oxidation state of manganese changes from +2 to +7 during the reaction. (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) Both A and R are false | 11 |
| 570 | Which of the following is a redox reaction? A . Reaction of ( H_{2} S O_{4} ) with ( N a O H ) B. In atmosphere, formation of ( O_{3} ) from ( O_{2} ) by lightening c. Formation of oxides of nitrogen from nitrogen and oxygen by lightening D. Evaporation of ( H_{2} O ) | 11 |
| 571 | 17. In the balance chemical reaction, 10, +al+bH – CH2O + dl, a, b, c and d respectively correspond to: (a) 5,6,3, 3 (b) 5,3,6,3 (c) 3,5, 3,6 (d) 5, 6, 5,5 | 11 |
| 572 | is a degradation phenomenon in which the electrons in a plastic are so strongly attracted to oxygen atoms. A. Oxidation B. Reduction c. Hydrolysis D. Polymerization | 11 |
| 573 | Identify the true statement regarding Daniel cell: A. zinc ions flows across salt bridge B. ( K^{+} ) ions move from salt bridge to ( C u / C u^{+2} ) half cell C. Oxidation takes place at copper electrode D. Flow of current takes place from copper electrode to zinc electrode | 11 |
| 574 | A redox reaction is one in which: A. both the substance are reduced. B. both the substance are oxidised. C. one substance is reduced and other is oxidised. D. all of the above. | 11 |
| 575 | Balance the following in basic medium: ( boldsymbol{F} boldsymbol{e}_{3} boldsymbol{O}_{4}+boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-} rightarrow boldsymbol{F} boldsymbol{e}_{2} boldsymbol{O}_{3}+boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2} ) A ( cdot 6 F e_{3} O_{4}+2 M n O_{4}^{-}+H_{2} O rightarrow 9 F e_{2} O_{3}+2 M n O_{2} ) ( 2 O H^{-} ) B. ( 6 F e_{3} O_{4}+4 M n O_{4}^{-}+H_{2} O rightarrow 9 F e_{2} O_{3}+5 M n O_{2}+ ) ( O H^{-} ) ( mathrm{c} cdot 6 mathrm{Fe}_{3} mathrm{O}_{4}+mathrm{MnO}_{4}^{-}+mathrm{H}_{2} mathrm{O} rightarrow 9 mathrm{Fe}_{2} mathrm{O}_{3}+3 mathrm{MnO}_{2}+ ) ( 2 O H^{-} ) D. None of these | 11 |
| 576 | Q8. What is meant by reducing agent? Name the best reducing agent. | 11 |
| 577 | The change in the oxidation number of the underlined nitrogen atom in the following chemical reactions are : a. Nitrous acid ( left(H underline{N} O_{2}right) ) reduces ( M n O_{4}^{ominus} ) in acid solution b. Nitrous acid ( left(H underline{N} O_{2}right) ) oxidises ( I^{ominus} ) to ( I_{2} ) in acid solution. ( A cdot(a)+3 ) to +5 ( (b)+3 t 0+2 ) B. (a) +3 to +6 ( (b)+3 t 0+2 ) ( c cdot(a)+3 t a+5 ) ( (b)+3 t 0+1 ) D. ( (a)+3 ) to +2 ( (b)+3 t 0+5 ) | 11 |
| 578 | In the given reaction, ( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7}+ ) ( boldsymbol{X} boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{Y} boldsymbol{S} boldsymbol{O}_{2} rightarrow boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+ ) ( boldsymbol{C r}_{2}left(boldsymbol{S O}_{4}right)_{3}+boldsymbol{Z H}_{2} boldsymbol{O} . ) Find ( mathbf{X}, mathbf{Y} ) and ( mathbf{Z} ) | 11 |
| 579 | In a chemical reaction, oxidation is always accompanied by reduction If true enter 1 , else enter 0 . ( A ) | 11 |
| 580 | Which of the following is a disproportionation reaction? A ( cdot C u_{2} O+2 H^{+} rightarrow C u+C u^{2+}+H_{2} O ) B ( cdot 2 C r O_{4}^{2-}+2 H^{+} rightarrow C r_{2} O_{7}^{2-}+H_{2} O ) ( mathrm{c} cdot mathrm{CaCO}_{3}+2 mathrm{H}^{+} rightarrow mathrm{Ca}^{2+}+mathrm{H}_{2} mathrm{O}+mathrm{CO}_{2} ) D. ( C r_{2} O_{7}^{2-}+2 O H^{-} rightarrow 2 C r O_{4}^{2-}+H_{2} O ) | 11 |
| 581 | Which of the following behaves as both oxidising and reducing agents? A. ( H_{2} S O_{4} ) в. ( S O_{4} ) c. ( H_{2} ) D. ( H N O_{3} ) | 11 |
| 582 | The value of ( n ) in the following reaction is : ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{n} e^{-}+mathbf{1 4 H}^{+} rightarrow boldsymbol{2 C r}^{3+}+ ) ( mathbf{7} boldsymbol{H}_{mathbf{2}} boldsymbol{O} ) | 11 |
| 583 | 10. In which of the following reactions, equivalent mass the underlined is equal to molar mass? (a) Cl2 + 20H- CH- + CIO +H2O (b) 2HCHO + OH-HCOO- + CH,OH (C) 2MnO – MnO2 + MnO, (d) 2KCIO3 -> 2KCI + 302 | 11 |
| 584 | The ion ( A^{n+} ) is oxidised to ( A O_{3}^{-} ) by ( M n O_{4}^{-} ) changing to ( M n^{2+} ) in acid medium. Given that ( 2.68 times 10^{-3} ) mole of ( A^{n+} ) required ( 1.61 times 10^{-3} ) mole ( M n O^{-} ) What is the value of n? | 11 |
| 585 | Q3. Consider a voltaic cell constructed with the following substances: Cr+ (aq) + 3e Cr(s) MnO4 (aq) + SH+ (aq) + 5e – Mr** (aq) + 4H,O(1) E° = -0.74 V E° = +1.51 V (a) Which substances are oxidised and reduced in this cell? (b) Which are the negative and positive electrode? . | 11 |
| 586 | Assertion When an electric current is passed through an aqueous solution of sodium chloride, sodium ions move towards cathode and chloride ions move towards anode. Reason Cathode is a negatively charged electrode and therefore attracts ( boldsymbol{N} boldsymbol{A}+ ) ions. Anode is a positively charged electrode and therefore attracts ( C l- ) ions A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion c. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 11 |
| 587 | In the following reaction: ( boldsymbol{A}^{+}+boldsymbol{B} rightarrow boldsymbol{A}+boldsymbol{B}^{+} ) oxidizing agent is: A ( . A^{+} ) в. ( B ) c. Both of them D. None of them | 11 |
| 588 | The redox reaction ( Z n(s)+ ) ( boldsymbol{P b C l}_{2}(boldsymbol{a q}) longrightarrow boldsymbol{P b}(boldsymbol{s})+boldsymbol{Z n C l}_{2}(boldsymbol{a q}) ) can be represented as following half equations ( : Z n(s) longrightarrow Z n^{2+}(a q)+ ) ( 2 e^{-}(text {oxidation }) ) and ( P b^{2+}(a q)+ ) ( 2 e^{-} longrightarrow P b(s)(text { reduction }) ) If true enter 1 , else enter 0 . ( A ) | 11 |
| 589 | A molecule is reduced means it: A. loses electron. B. gains proton c. loses proton and electrons D. gains electron. | 11 |
| 590 | In balancing the half reaction, ( S_{2} O_{3}^{2-} rightarrow S(s), ) the number of electrons that must be added on the left is : | 11 |
| 591 | Balance the following equation by ion electron method: ( boldsymbol{H} boldsymbol{g} boldsymbol{S}+boldsymbol{C l}^{-}+boldsymbol{H}^{+}+boldsymbol{N} boldsymbol{O}_{3}^{-} rightarrow ) ( boldsymbol{H} boldsymbol{g} boldsymbol{C l}_{4}^{2-}+boldsymbol{S}+boldsymbol{N} boldsymbol{O}+boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 592 | Complete the following ionic equation: ( mathbf{3} M n O_{4}^{2-}+4 H^{+} rightarrow ) | 11 |
| 593 | Which of the following arrangements represent increasing oxidation number of the central atom? A ( cdot C r O_{2}^{-}, C l O_{3}^{-}, C r O_{4}^{2-}, M n O_{4}^{-} ) B . ( C l O_{3}^{-}, C r O_{4}^{2-}, M n O_{4}^{-}, C r O_{2}^{-} ) c. ( C r O_{2}^{-}, C l O_{3}^{-}, M n O_{4}^{-}, C r O_{4}^{2-} ) D. ( C r O_{4}^{2-}, M n O_{4}^{-}, C r O_{2}^{-}, C l O_{3}^{-} ) | 11 |
| 594 | The oxidation states exhibited by hydrogen in its various molecular forms/compounds are : A . – – ‘ only B. zero only ( c cdot+1,-1 ) and 0 D. +1 only | 11 |
| 595 | What coefficient of ( A g N O_{3} ) is required to balance the following equation? ( C u+A g N O_{3} rightarrow C uleft(N O_{3}right)_{2}+A g ) ( mathbf{A} cdot mathbf{0} ) B. 1 c. 2 D. 3 | 11 |
| 596 | When zinc reacts with very dilute ( H N O_{3}, ) the oxidation state of nitrogen changes from: A. +5 to +1 B. +5 to -3 ( c cdot+5 t o+4 ) D. +5 to +3 | 11 |
| 597 | Metals exhibit ….. oxidation states in their compounds. A. Positive B. Negative c. Neutral D. none of these | 11 |
| 598 | 1. Among the following molecules, in which does bromine show the maximum oxidation number? (a) Hg, (Bro,), (b) Br-a (c) KBrO (d) Br₂ itinaxidotion number in their | 11 |
| 599 | When potassium chloride and lead ( (I I) ) nitrate react in an aqueous solution, which of the following terms will be present in the balanced molecular equation? A ( cdot P b C l_{s} ) B ( cdot P b_{2} C l_{(s)} ) ( mathbf{c} cdot K N O_{3(a q)} ) D. ( 2 K N O_{3(a q)} ) E ( cdot 2 K C l_{2(s)} ) | 11 |
| 600 | ( ln K H, ) the oxidation number of hydrogen is: A ( .+2 ) B. +1 c. 0 D. – E. -2 | 11 |
| 601 | 11. A substance which gets oxidised, during a redox reaction, is known as (a) oxidizing agent (b) reducing agent c) either oxidising or reducing agent (d) None of the above | 11 |
| 602 | The number of moles of ( K_{2} C r_{2} O_{7} ) that will be needed to react with one mole of ( H_{2} S ) in acidic medium is : A ( cdot frac{1}{6} ) B. ( frac{1}{3} ) ( c cdot frac{2}{5} ) D. ( frac{2}{3} ) | 11 |
| 603 | Which of the following equations is a balanced one? ( mathbf{A} cdot 5 B i O_{3}^{-}+22 H^{+}+M n^{2+} rightarrow 5 B i^{3+}+7 H_{2} O+M n O_{4}^{-} ) B. ( 5 B i O_{3}^{-}+14 H^{+}+2 M n^{2+} rightarrow 5 B i^{3+}+7 H_{2} O+2 M n O_{4}^{-} ) ( mathbf{c} cdot 2 B i O_{3}+4 H^{+}+M n^{2+} rightarrow 2 B i^{3+}+2 H_{2} O+M n O_{4}^{-} ) D. ( 6 B i O_{3}^{-}+12 H^{+}+3 M n^{2+} rightarrow 6 B i^{3+}+6 H_{2} O+3 M n O_{4}^{-} ) | 11 |
| 604 | A redox reaction simply involves the transfer of electrons from reductant to oxidant If true enter 1 , else enter 0 . ( A ) | 11 |
| 605 | A dilute ferrous sulphate solution was gradually added to the beaker containing acidified potassium permanganate solution. The light purple colour of the solution fades and finally disappears. Which of the following is the correct explanation for the observation? ( mathbf{A} cdot K M n O_{4} ) is an oxidising agent, it oxidises ( F e S O_{4} ) B. ( F e S O_{4} ) acts as an oxidising agent and oxidises ( K M n O_{4} ) C. The colour disappears due to dilution; no reaction is involved D. ( K M n O_{4} ) is an unstable compound and decomposes in presence of ( F e S O_{4} ) to a colourless compound | 11 |
| 606 | Give the oxidation state of underlined. ( N a_{2} S_{4} O_{6} ) | 11 |
| 607 | Q4. (a) Give two important functions of salt bridge. (b) Balance the following equation by oxidation number method: Fe2+ + Cr, 02- + H–> Fe3+ + Cr3+ + H2O | 11 |
| 608 | “Reaction of potassium iodide solution with lead nitrate solution” is the example of : This question has multiple correct options A. Chemical replacement reaction B. Neutralisation reaction c. Precipitation reaction D. Chemical double decomposition reaction | 11 |
| 609 | Oxidation number of ( S ) in ( left(C H_{3}right)_{2} S ) is ( mathbf{A} cdot mathbf{0} ) B. +1 ( c .-2 ) D. +3 | 11 |
| 610 | The number of electrons required to balance the given equation is ( N O_{3}^{-}+4 H^{+}+e^{-} longrightarrow 2 H_{2} O+N O ) ( mathbf{A} cdot mathbf{5} ) B. 2 ( c cdot 3 ) D. | 11 |
| 611 | Which of the following is/are disproportionation reaction(s)? This question has multiple correct options A ( cdot 2 C C l_{3} C H O+N a O H rightarrow C C l_{3} C O O N a+ ) ( C C l_{3} C H_{2} O H ) в. ( N H_{4} N O_{3} rightarrow N_{2} O+2 H_{2} O ) c. ( 2 K C l O_{3} rightarrow 2 K C l+3 O_{2} ) D. ( 5 C l_{2}+6 O H^{-} rightarrow C l O_{3}^{-}+5 C l^{-}+3 H_{2} O ) | 11 |
| 612 | The role of fluorspar (CaF,) which is added in small quantities in the electrolytic reduction of alumina dissolved in fused cryolite (Na AlF,) is: (a) as a catalyst (b) to make the fused mixture very conducting (c) to increase the temperature of the melt (d) to decrease the rate of oxidation of carbon at the anode | 11 |
| 613 | Q. 49 Why in the redox titration of KMnO4 vs oxalic acid, we heat oxalic acid solution before starting the titration? ne As we know with inerne | 11 |
| 614 | Oxalic acid dihydrate, ( boldsymbol{H}_{2} boldsymbol{C}_{2} boldsymbol{O}_{4} ) ( 2 H_{2} O(s) ) is often used as a primary reagent to standardise sodium hydroxide solution. Which of these facts are reasons to choose this substance as a primary standard? I. It is diprotic. II. It is a stable compound that can be weighed directly in air. III. It is available in pure form. A. III only B. I and II only c. ॥ and III only D. I. II and III | 11 |
| 615 | Oxidation of NO in air produces: в. ( N_{2} O_{3} ) ( c cdot N O_{2} ) D. ( N_{2} O_{5} ) | 11 |
| 616 | The oxidation state of ( A, B, ) and ( C ) in a compound are +2,+5 and -2 respectively. The compound is : ( mathbf{A} cdot A_{2}(B C)_{2} ) B ( cdot A_{2}(B C)_{3} ) ( mathbf{c} cdot A_{3}left(B C_{4}right)_{2} ) D. ( A_{2}left(B C_{4}right)_{3} ) | 11 |
| 617 | Assertion Lower parts of the ship or bridge is coated with tar. Reason It is to increase rusting. A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion C. Assertion is correct but Reason is incorrect D. Assertion is incorrect but Reason is correct | 11 |
| 618 | The oxidation state of oxygen of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) in the final products when it reacts with ( C l O_{3}^{ominus} ) is : ( mathbf{A} cdot mathbf{0} ) B. ( c cdot-1 ) D. – – | 11 |
| 619 | Select redox reaction from the following A ( . Z n+C u S O_{4} rightarrow Z n S O_{4}+C u ) в. ( C a O+2 H C l rightarrow C a C l_{2}+H_{2} O ) c. ( N a O H+2 H C l rightarrow N a C l_{2}+H_{2} O ) D. ( C a C O_{3} rightarrow C a O+C O_{2} ) | 11 |
| 620 | The substance oxidized and the oxidizing agent in the following reaction are respectively: ( Z n+H_{2} S O_{4} rightarrow Z n S O_{4}+H_{2} ) A. zinc atoms and hydrogen ions B. zinc ions and hydrogen atoms c. hydrogen ions and zinc atoms D. hydrogen atoms and zinc ions | 11 |
| 621 | The following intramolecular redox reaction shows a loss and gain of how much electrons? ( left(N H_{4}right)_{2} C r_{2} O_{7} rightarrow N_{2}+C r_{2} O_{3}+ ) ( 4 H_{2} O ) A. Six B. Seven c. Eight D. None of these | 11 |
| 622 | Find oxidation number of Magnese in ( boldsymbol{K}_{2} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} ) | 11 |
| 623 | Select the species having zero oxidation state at the underlined elements. This question has multiple correct options ( mathbf{A} cdotleft(C H_{3}right)_{2} S O ) B. ( underline{C}_{12} mathrm{H}_{22} mathrm{O}_{11} ) c. ( H_{2} S O_{3} ) D. ( underline{N}_{2} H_{4} ) | 11 |
| 624 | When zinc is added to ( C u S O_{4} ) solution, copper is precipitated because : A ( cdot C u^{+2} ) is reduced B. ( C u^{+2} ) is oxidised c. ( C u S O_{4} ) is ionized D. ( C u S O_{4} ) is hydrolysed | 11 |
| 625 | In which of the following processes is nitrogen oxidized? A ( cdot N H_{4}^{oplus} rightarrow N_{2} ) B ( . N O_{3}^{ominus} longrightarrow N O ) ( mathrm{c} cdot mathrm{NO}_{2} longrightarrow mathrm{NO}_{2}^{circ} ) D. ( N O_{3}^{ominus} longrightarrow N H_{4}^{oplus} ) | 11 |
| 626 | Is the following reaction is a redox reaction? ( boldsymbol{B} boldsymbol{a} boldsymbol{O}_{2}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow boldsymbol{B} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{O}_{2} ) | 11 |
| 627 | Q. 15 Identify the correct statements with reference to the given reaction PA +30H + 3H,0 PH2 + 3H,POZ (a) Phosphorus is undergoing reduction only (b) Phosphorus is undergoing oxidation only (c) Phosphorus is undergoing oxidation as well as reduction (d) Hydrogen is undergoing neither oxidation nor reduction | 11 |
| 628 | Consider the given reaction. This question has multiple correct options A. It is disproportionation reaction. B. It is intramolecular redox reaction C. ( O H^{-} ) is a reducing as well as oxidising agent D. ( C H O-C H O ) is a reducing as well as oxidising agentt | 11 |
| 629 | Balance the following equations by ion electron method: ( boldsymbol{C l}_{2}+boldsymbol{I O}_{3}^{-}+boldsymbol{O H}^{-} rightarrow boldsymbol{I} boldsymbol{O}_{4}^{-}+boldsymbol{C l}^{-}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 630 | The oxidation number of ( C ) in ( boldsymbol{C H}_{4}, boldsymbol{C H}_{3} boldsymbol{C l}, boldsymbol{C H}_{2} boldsymbol{C l}_{2}, boldsymbol{C H} boldsymbol{C l}_{3} ) and ( C C l_{4} ) are respectively : в. +2,+4,0,-4,-2 c. -4,-2,0,+2,+4 D. -2,-4,0,+4,+2 | 11 |
| 631 | The sum of the oxidation number of the carbon atoms in ( C H_{3} C H O ) is: A . -2 B. +2 ( c .-4 ) D. – | 11 |
| 632 | Which of the following reactions takes place at anode? A. Reduction B. Oxidation c. Decomposition D. Dissolution | 11 |
| 633 | The oxidation state of iron in the coordination sphere of prussian blue is: ( A cdot+2 ) B. 0 ( c cdot+1 ) D. +3 | 11 |
| 634 | For the galvanic cell, ( boldsymbol{C u}left|boldsymbol{C u}^{2+} | boldsymbol{A} boldsymbol{g}^{+}right| boldsymbol{A} boldsymbol{g} ) Which of the following observations is not correct? A. Cu acts as anode and Ag acts as cathode B. Ag electrode loses mass and Cu electrode gains mass C. Reaction at anode, ( C u rightarrow C u^{2+}+2 e^{-} ) D. copper is more reactive than silver | 11 |
| 635 | Write balanced net ionic equation for the following reactions in acidic solution. [ begin{array}{l} boldsymbol{S}_{4} boldsymbol{O}_{6}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{A l}(boldsymbol{s}) rightarrow boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{a} boldsymbol{q})+ \ boldsymbol{A l}^{3+}(boldsymbol{a} boldsymbol{q}) end{array} ] ( mathbf{A} cdot S_{4} O_{6}^{2-}(a q)+6 A l(s)+20 H^{+} rightarrow 4 H_{2} S(a q)+ ) [ 6 A l^{3+}(a q)+6 H_{2} O ] ( mathbf{B} cdot 2 S_{4} O_{6}^{2-}(a q)+6 A l(s)+20 H^{+} rightarrow 4 H_{2} S(a q)+ ) [ 2 A l^{3+}(a q)+6 H_{2} O ] ( mathbf{c} cdot S_{4} O_{6}^{2-}(a q)+5 A l(s)+20 H^{+} rightarrow 4 H_{2} S(a q)+ ) [ 3 A l^{3+}(a q)+6 H_{2} O ] D. None of the above | 11 |
| 636 | The sum of the coefficients in the balanced equation of ( boldsymbol{C o}+boldsymbol{N} boldsymbol{i}^{2+} rightarrow ) ( boldsymbol{C o}^{boldsymbol{3}+}+boldsymbol{N} boldsymbol{i}, ) is: A . 5 B. 2 ( c cdot 3 ) D. 10 E . 13 | 11 |
| 637 | In reduction of dichromate by ( boldsymbol{F} boldsymbol{e}(boldsymbol{I} boldsymbol{I}) ) the number of electrons involved per chromium atoms is: ( A cdot 2 ) B. 3 ( c cdot 4 ) D. | 11 |
| 638 | The complete balanced equation is: ( M n O_{2}+H_{2} O_{2} rightarrow M n O_{4}^{-}+H_{2} O ) (Basic medium) A ( cdot 3 mathrm{H}_{2} mathrm{O}_{2}+2 mathrm{MnO}_{2}+2 mathrm{OH}^{-} rightarrow 2 mathrm{MnO}_{4}^{-}+4 mathrm{H}_{2} mathrm{O} ) B. ( 3 H_{2} O_{2}+M n O_{2}+3 O H^{-} rightarrow 2 M n O_{4}^{-}+5 H_{2} O ) ( mathrm{c} cdot mathrm{H}_{2} mathrm{O}_{2}+2 mathrm{MnO}_{2}+mathrm{OH}^{-} rightarrow 2 mathrm{MnO}_{4}^{-}+4 mathrm{H}_{2} mathrm{O} ) D. none of these | 11 |
| 639 | A reaction in which there is a transfer of electrons from one reactant to another is called a (combustion/redox) reaction. | 11 |
| 640 | 0.01 mole of ( N a_{2} C_{2} O_{4} ) dissolve in alkaline solution. This solution is titrated with ( mathrm{V} mathrm{ml} ) 0.1 ( boldsymbol{M} boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} ) solution. Find out ( V ) A .200 в. ( frac{200}{3} ) c. 40 D. ( frac{100}{3} ) | 11 |
| 641 | Which one of the following statements is not correct? A. Oxidation number of ( sin left(N H_{4}right)_{2} S_{2} O_{8} ) is +6 B. Oxidation number of 0 s in ( O s O_{4} ) is +8 C. Oxidation number of ( sin H_{2} S O_{5} ) is +8 Dexidation number of 0 in ( K O_{2} ) is ( -frac{1}{2} ) | 11 |
| 642 | A solution contains ( boldsymbol{F e}^{+2}, boldsymbol{F e}^{+mathbf{3}} ) and ( boldsymbol{I}^{-} ) ions. This solution was treated with iodine at ( 35^{circ} mathrm{C} ). Then the favourable redox reaction is: (Given that ( boldsymbol{E}_{boldsymbol{F} e^{+3} / boldsymbol{F} e^{+2}}^{boldsymbol{o}}= ) ( left.+mathbf{0 . 7 7 V} ; quad boldsymbol{E}_{I_{2} / I^{-}}^{o}=mathbf{0 . 5 3 6} boldsymbol{V}right) ) A ( . I_{2} ) will be reduced to ( I^{-} ) B. there will be no redox reaction c. ( I^{-} ) will be oxidised to ( I_{2} ) D. ( F e^{+} ) will be oxidised to ( F e^{+3} ) | 11 |
| 643 | de ion according to 18. Bleaching powder reacts with iodide ion the following unbalanced equation: OCI + I + H 12 + CI+H,0 A 0.6000 g sample of bleaching powder re 35.24 mL of 0.1084 N Na S203 to titrate the libe iodine. The percentage of Cl in the sample is (a) 22.58% C1 (b) 5.15% CI (c) 11.29% C1 (d) 45.16% C1 | 11 |
| 644 | When an atom reacts chemically and gains one or more electrons, it is said to have been? A. Catalyzed B. Oxidized c. Reduced D. Decomposed | 11 |
| 645 | Oxidation number of ( mathrm{P} ) in ( boldsymbol{P}_{2} boldsymbol{O}_{7}^{4-} ) is : ( A cdot+3 ) ( B cdot+4 ) ( c cdot+5 ) ( D cdot+6 ) | 11 |
| 646 | Using the standard half-cell potential listed, calculate the equilibrium constant for the reaction: ( boldsymbol{C o}(s)+mathbf{2} boldsymbol{H}^{+}(boldsymbol{a q}) longrightarrow boldsymbol{C o}^{2+}(boldsymbol{a q})+ ) ( boldsymbol{H}_{2}(boldsymbol{g}) quad boldsymbol{a t} quad boldsymbol{2} boldsymbol{9} boldsymbol{8} boldsymbol{K} ) ( boldsymbol{C o}^{2+}(boldsymbol{a q})+boldsymbol{2 e}-longrightarrow boldsymbol{C o}(boldsymbol{s}) boldsymbol{E}^{0}= ) ( -0.277 V ) A ( cdot 2.3 times 10^{9} ) B . ( 4.8 times 10^{4} ) C ( .4 .8 times 10^{7} ) D. ( 4.8 times 10^{11} ) | 11 |
| 647 | Arrange the following in increasing order of oxidation states of ( M n ) ( boldsymbol{K}_{2} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}, boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2}, boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} ) | 11 |
| 648 | ( H_{2} S O_{4} ) cannot be used to dry up ( H_{2} S ) because it oxidises ( H_{2} S ) to ( S O_{2} ) and ( S ) If true enter 1 , else enter 0 . A. | 11 |
| 649 | Iron (III) oxide on heating with carbon monoxide gas form solid iron and liberates carbon dioxide gas. This is a: A. precipitation reaction B. double decomposition reaction c. synthesis reaction D. redox reaction | 11 |
| 650 | The ratio of coefficient of ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3}, boldsymbol{F} boldsymbol{e}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) and ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{3} ) in the following redox equation, ( boldsymbol{F e}+ ) ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} rightarrow boldsymbol{F} boldsymbol{e}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}+boldsymbol{N} boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{3}+ ) ( H_{2} O ) in the balanced form will be? A .10: 1: 4 B . 10: 4: 1 c. 4: 10: 1 D. 4: 1: 10 | 11 |
| 651 | The passage of electricity in the Daniell cell when ( Z n ) and ( C u ) electrodes are connected is from: A. ( C u ) to ( Z n ) in the cell B. ( C u ) to ( Z n ) outside the cell c. ( Z n ) to ( C u ) outside the cell D. ( Z n ) to ( C u ) in the cell | 11 |
| 652 | The decomposition of ( K C l O_{3} ) on heating is an example of: | 11 |
| 653 | In substance ( M gleft(H X O_{3}right), ) the oxidation number of ( X ) is : ( mathbf{A} cdot mathbf{0} ) B. +2 ( c cdot+3 ) D. +4 | 11 |
| 654 | What is the oxidation state of sulphur in the following. a) ( boldsymbol{S F}_{mathbf{6}} ) b) ( N a_{2} S_{2} O_{3} ) | 11 |
| 655 | 5. The reaction of white phosphorus with aqueous NaOH gives phosphine along with another phosphorus containing compound. The reaction type, the oxidation states of phosphorus in phosphine and the other product are respectively: (a) redox reaction; -3 and -5 (b) redox reaction; +3 and +5 (c) disproportionation reaction; -3 and +1 (d) disproportionation reaction; -3 and +3 | 11 |
| 656 | The reaction given below is interpreted as: ( boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) rightarrow boldsymbol{2} boldsymbol{H} boldsymbol{C l}(boldsymbol{g})+boldsymbol{S}(boldsymbol{s}) ) A. ( H_{2} S ) is getting oxidized and ( C l_{2} ) is getting reduced B. ( H_{2} S ) is getting reduced and ( C l_{2} ) is getting oxidized c. only ( H_{2} S ) is oxidized D. Both ( H_{2} S ) and ( C l_{2} ) are reduced | 11 |
| 657 | Equivalent weight of ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{2} ) when it disproportionates into ( P H_{3} ) and ( H 3 P O_{3}(text { mol. wt. }=M) ) is : ( mathbf{A} cdot M ) в. ( frac{M}{2} ) c. ( frac{M}{4} ) D. ( frac{3 M}{4} ) | 11 |
| 658 | The oxidation numbers of phosphorus in ( B aleft(H_{2} P O_{2}right)_{2} ) and xenon in ( N a_{4} X e O_{6} ) respectively are: ( A cdot+3 ) and +4 B. +2 and +6 ( c cdot+1 ) and +8 D. -1 and -6 | 11 |
| 659 | In the reaction given below, identify the specie undergoing oxidation and reduction ( boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g})+boldsymbol{C l}_{2} rightarrow boldsymbol{2} boldsymbol{H} boldsymbol{C l}(boldsymbol{g})+boldsymbol{S}(boldsymbol{s}) ) | 11 |
| 660 | The value of ( n ) in the equation, ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+mathbf{1 4} boldsymbol{H}^{+}+boldsymbol{n} boldsymbol{e}^{-} rightarrow boldsymbol{2} boldsymbol{C r}^{boldsymbol{3}+}+ ) ( mathbf{7} H_{2} O ) is: ( A cdot 2 ) B. 3 ( c cdot 4 ) D. 6 | 11 |
| 661 | 2. Assertion : A cation is formed after the removal of electrons. Reason: An element always looses one electron to form cation. | 11 |
| 662 | Oxidation numbers of ( M n ) in its compounds ( M n C l_{2}, M n(O H)_{3} ) ( M n O_{2} ) and ( K M n O_{4} ) respectively are: ( A cdot+2,+4,+7,+3 ) B. +2,+3,+4,+7 ( c cdot+7,+3,+2,+4 ) ( D cdot+7,+4,+3,+2 ) | 11 |
| 663 | Which is not a disproportionation reaction? ( A ) B. [ begin{array}{l} mathrm{CHO} \ mathrm{COOH} end{array}+mathrm{OH}^{-} longrightarrow begin{array}{l} mathrm{CH}_{2} mathrm{OH} quad mathrm{COO}^{-} \ mathrm{COO}^{-}+mid \ mathrm{COO}^{-} end{array} ] c. ( N a H+H_{2} O longrightarrow N a O H+H_{2} ) D. All of the above | 11 |
| 664 | A decomposition reaction taking place due to passage of electric current is called | 11 |
| 665 | When an alkali metal is reacted with hydrogen then metallic hydride is formed. In this reaction: A. hydrogen is oxidized B. hydrogen is reduced c. hydrogen is neither oxidised nor reduced D. hydrogen is oxidized as well as reduced | 11 |
| 666 | DL 2. Which of the following halogens do not exhibit a positive oxidation number in their compounds? (a) F (6) Br (c) 1 (d) ai 3. TAZbioboru | 11 |
| 667 | ( H_{2} O_{2} ) oxidises ( M n O_{2} ) to ( M n O_{4}^{-} ) in basic medium. ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) and ( boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2} ) react in the molar ratio of ( x: y . ) What is the value of ( boldsymbol{x}+boldsymbol{y} ? ) | 11 |
| 668 | Type of redox reaction that occur in volcanic eruptions is: A. disproportionation B. comproportionation c. reduction D. both ( A ) and ( B ) | 11 |
| 669 | What is the correct representation of reaction occurring when HCl is heated with ( M n O_{2} ? ) ( mathbf{A} cdot M n O_{4}^{-}+5 C l^{-}+8 H^{+} rightarrow M n^{2+}+5 C l^{-}+5 H_{2} O ) B. ( M n O_{2}+2 C l^{-}+4 H^{+} rightarrow M n^{2+}+C l_{2}+2 H_{2} O ) ( mathbf{c} cdot 2 M n O_{2}+4 C l^{-}+8 H^{+} rightarrow 2 M n^{2+}+2 C l_{2}+4 H_{2} O ) D. ( M n O_{2}+4 H C l rightarrow M n C l_{4}+C l_{2}+H_{2} O ) | 11 |
| 670 | Balance the following equations by ion electron method: ( boldsymbol{I}_{2}+boldsymbol{O H}^{-} rightarrow boldsymbol{I} boldsymbol{O}_{3}^{-}+boldsymbol{I}^{-}+boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 671 | Write balanced redox reactions of the following: ( boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) ) reduces ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}(boldsymbol{a} boldsymbol{q}) ) to green coloured ( C r^{3+}(a q) ) in acidic medium. A ( cdot C r_{2} O_{7}^{2-}+3 H_{2} O_{2}+8 H^{+} rightarrow 2 C r^{3+}+3 O_{2}+7 H_{2} O ) B . ( C r_{2} O_{9}^{2-}+3 H_{2} O_{2}+4 H^{+} rightarrow 2 C r^{3+}+3 O_{2}+7 H_{2} O ) c. ( C r_{2} O_{7}^{2-}+3 H_{2} O_{2}+8 H^{+} rightarrow 2 C r^{3+}+3 O_{2}+9 H_{2} O ) D. None of these | 11 |
| 672 | Justify that the following reactions are redox reactions: ( boldsymbol{C u O}(boldsymbol{s})+boldsymbol{H}_{2}(boldsymbol{g}) rightarrow boldsymbol{C u}(boldsymbol{s})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) ) | 11 |
| 673 | When P reacts with caustic soda, the products are ( boldsymbol{P H}_{3} ) and ( boldsymbol{N a H}_{2} boldsymbol{P O}_{2} . ) The reaction is an example of A. Oxidation B. Reduction c. Both oxidation and reduction D. Neutralisation | 11 |
| 674 | In the reaction ( : boldsymbol{C l}_{2}+boldsymbol{O H}^{-} rightarrow boldsymbol{C l}^{-}+ ) ( boldsymbol{C l O}_{boldsymbol{4}}^{-}+boldsymbol{H}_{2} boldsymbol{O} ? ) A. Chlorine is oxidised B. Chlorine is reduced C. Chlorine is oxidised as well as reduced D. Chlorine is neither oxidised nor reduced | 11 |
| 675 | In the following reaction: ( mathbf{3} boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{6} boldsymbol{C} boldsymbol{O}_{3}^{2-}+boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O} rightarrow mathbf{5} boldsymbol{B} boldsymbol{r}^{-}+ ) ( boldsymbol{B} boldsymbol{r} boldsymbol{O}_{3}^{-}+boldsymbol{6} boldsymbol{H} boldsymbol{C} boldsymbol{O}_{3}^{-} ) This question has multiple correct options A. bromine is oxidised and carbonate is reduced B. bromine is oxidised c. bromine is neither oxidised nor reduced D. bromine is reduced | 11 |
| 676 | What is an example of a single replacement reaction? A. ( A+X rightarrow A X ) в. ( A X rightarrow A+X ) c. ( A+B X rightarrow A X+B ) D. ( A X+B Y rightarrow A Y+B X ) E . ( A+X rightarrow B+Y ) | 11 |
| 677 | State whether the following conversions are oxidation or reduction? ( boldsymbol{P b O}_{2}+boldsymbol{S O}_{2} rightarrow boldsymbol{P b S O}_{4} ) | 11 |
| 678 | The volume of ( C O_{2} ) produced at STP by decomposition of ( 4.2 g ) of ( N a H C O_{3} ) according to the reaction: ( 2 N a H C O_{3} rightarrow N a_{2} C O_{3}+H_{2} O+C O_{2} ) ( mathbf{A} cdot 150 mathrm{m} ) B. ( 569 mathrm{ml} ) c. ( 1.68 L ) D. ( 5.6 L ) | 11 |
| 679 | Statement: Reducing agents are mostly non-metals while oxidizing agents are mostly metals. State whether the given statement is | 11 |
| 680 | Oxidation number of nitrogen in which among the oxides of nitrogen is the lowest? A. Nitric oxide B. Nitrous oxide c. Nitrogen dioxide D. Dinitrogen trioxide | 11 |
| 681 | In redox reaction: A. energy is absorbed. B. energy is released. C. transfer of electrons takes place between species. D. catalyst increases the rate of reaction. | 11 |
| 682 | 8. Which of the following are not redox reactions? (a) Mg + N2 – Mg3N2 (6) K[Fe (CN).] + H2SO, +H, O K ,SO, + CO + FeSO, + (NH2)2SO4 (c) 12 + 3Cl2 → ICI, (d) CuSO4 + NH3-> [Cu (NH3)4] SO, TABichana | 11 |
| 683 | The oxidation number of ( C r ) is +6 in : This question has multiple correct options A ( cdot operatorname{Fe} C r_{2} O_{4} ) в. ( K C r O_{3} C l ) ( mathrm{c} cdot mathrm{Cr} mathrm{O}_{5} ) ( mathrm{D} cdotleft[mathrm{Cr}(mathrm{OH})_{4}right]^{8} ) | 11 |
| 684 | ( 20 m L ) solution of ( 0.1 ~ M ) ferrous sulphate was completely oxidised using a suitable oxidising agent. What is the number of electrons exchanged? A. ( 1.204 times 10^{22} ) в. 193 c. 1930 D. ( 1.204 times 10^{2} ) | 11 |
| 685 | UL WJ ILUJUIL WUL JUPUL llais uererly WILL DI, du Q15. Justify giving reactions that among halogens, fluorine is the best oxidant and among hydrohalic compounds, Iydroiodic acid is the best reductant. | 11 |
| 686 | Write the balanced equations for the reaction occurring when gold is dissolved in aqua regia. A ( cdot 2 A u+3 H N O_{3}+11 H C l rightarrow 2 H A u C l_{4}+3 N O C l+ ) ( 6 H_{2} O ) B . ( 2 A u+3 H N O_{3}+13 H C l rightarrow 2 H A u C l_{4}+2 N O C l+ ) ( 8 H_{2} O ) c. ( 2 A u+5 H N O_{3}+11 H C l rightarrow 2 H A u C l_{4}+2 N O C l+ ) ( 8 H_{2} O ) D. None of these | 11 |
| 687 | Which of the following is not an intermolecular redox reaction? ( mathbf{A} cdot M g C O_{3} longrightarrow M g O+C O_{2} ) B. ( O_{2}+2 H_{2} longrightarrow 2 H_{2} O ) ( mathbf{c} cdot K+H_{2} O longrightarrow K O H+(1 / 2) H_{2} ) D. ( M n B r_{3} longrightarrow M n B r_{2}+(1 / 2) B r_{2} ) | 11 |
| 688 | 10ml of ( N H_{4} C l, 20 mathrm{ml} ) of ( N / 2 H_{2} S O_{4} ) and ( 30 mathrm{ml} ) of ( N / 3 H N O_{3} ) are mixed together and volume made to one litre. Normality of resulting solution is: A. ( 30 N / 100 ) в. ( N / 10 ) c. ( N / 20 ) D. ( N / 40 ) | 11 |
| 689 | In the reaction, ( mathbf{3} boldsymbol{C u} boldsymbol{O}+mathbf{2 N H}_{3} longrightarrow boldsymbol{N}_{2}+mathbf{3} boldsymbol{H}_{2} boldsymbol{O}+ ) ( mathbf{3} C u ) the change of ( N H_{3} ) to ( N_{2} ) involves: A . Loss of 6 electrons per mole of ( N_{2} ) B. Loss of 3 electrons per mole of ( N_{2} ) c. Gain of 6 electrons per mole of ( N_{2} ) D. Gain of 3 electrons per mole of ( N_{2} ) | 11 |
| 690 | In the following reaction ( P b ) undergoes: ( boldsymbol{P b}(s)+boldsymbol{P b O}_{2}(boldsymbol{s})+mathbf{2} boldsymbol{H}_{2} boldsymbol{S O}_{4}(boldsymbol{a q}) rightarrow ) ( 2 P b S O_{4}(s)+2 H_{2} O(l) ) A. disproportionation B. comproportionation c. reduction D. oxidation | 11 |
| 691 | Which of the following reactions does not involve oxidation-reduction? This question has multiple correct options A ( cdot 2 R b+2 H_{2} O rightarrow 2 R b O H+H_{2} ) в. ( 2 C u I_{2} rightarrow 2 C u I+I_{2} ) c. ( N H_{4} C l+N a O H rightarrow N a C l+N H_{3}+H_{2} O ) D. ( _{4 K C N}+F e(C N)_{2} rightarrow K_{4}left[F e(C N)_{6}right] ) | 11 |
| 692 | Assertion In the reaction, ( left.left.2 C u_{2} O_{(s)}+C u_{2} S_{(} sright) rightarrow 6 C u_{(} sright)+ ) ( boldsymbol{S} boldsymbol{O}_{2(boldsymbol{g})} ) copper acts as a reductant and sulphur acts as an oxidant Reason The given reaction is not a redox reaction 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 |
| 693 | Following reaction describes the rusting of iron. ( 4 F e+3 O_{2} rightarrow 4 F e^{3+}+6 O^{2-} ) Which one of the following statement is (are) correct? This question has multiple correct options A. This is an example of a oxidation reaction B. Metallic iron is oxidised to ( F e^{3} ) c. ( F e^{3+} ) is an oxidizing agent D. Metallic iron is a strong reducing agent | 11 |
| 694 | When phosphorus reacts with caustic soda, the products are ( P H_{3} ) and ( N a H_{2} P O_{2} . ) This reaction is an example of. A. Oxidation B. Reduction c. Disproportionation D. None of these | 11 |
| 695 | Assertion In the process of drying dishes with a towel, the wetting agent is the dish and the drying agent is the towel Reason The wetting agent gets wet during the 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 |
| 696 | Which is not a disproportionation reaction? ( A ) B. [ begin{array}{ll} text { CHO } & text { CH }_{2} text { OH } quad text { COO }^{-} \ text {COOH } & text { COO }^{-}+mid end{array} ] c. ( N a H+H_{2} O rightarrow N a O H+H_{2} ) D. All of the above | 11 |
| 697 | ( boldsymbol{A}: mathbf{2} boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{5}} boldsymbol{C H} boldsymbol{O}+boldsymbol{K} boldsymbol{O H} longrightarrow ) ( boldsymbol{C}_{6} boldsymbol{H}_{5} boldsymbol{C O O K}+boldsymbol{C}_{6} boldsymbol{H}_{5} boldsymbol{C H}_{2} boldsymbol{O H} ) ( boldsymbol{B}: mathbf{3} boldsymbol{C l}_{2}+boldsymbol{6} boldsymbol{K O H} longrightarrow mathbf{5} boldsymbol{K} boldsymbol{C l}+ ) ( boldsymbol{K} boldsymbol{C l O}_{3}+boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O} ) Select the correct statement. A. Both are redox reactions B. Both are disproportionation reaction c. ( A ) is a disproportionation reaction and ( B ) is a redox reaction D. ( A ) is a redox reaction and ( B ) is a disproportionation reaction. | 11 |
| 698 | 1. Find the value of x in NaxBO, | 11 |
| 699 | What are the conditions for a species to act as a donor and an acceptor during dative bond formation? | 11 |
| 700 | In the following reaction, the correct statements are: ( M g+2 H^{+} rightarrow M g^{2+}+H_{2} ) 1. ( M g ) is a reducing agent, ( H^{+} ) is an oxidising agent 2. ( M g ) is oxidising agent, ( H^{+} ) is a reducing agent. A. only 1 B. only 2 c. both D. none | 11 |
| 701 | Which of the following behaves as both oxidizing and reducing agents? A. ( H_{2} S O_{4} ) в. ( S O_{2} ) c. ( H_{2} ) D. ( H N O_{3} ) | 11 |
| 702 | ( boldsymbol{C u O}+boldsymbol{H}_{2} rightarrow boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C u} ) Above reaction is an example of : A. redox reaction B. synthesis reaction c. neutralisation D. analysis reaction | 11 |
| 703 | Which of the following is/are disproportionation reactions? This question has multiple correct options ( ^{mathbf{A}} cdot_{H_{2}} O_{2} rightarrow H_{2} O+frac{1}{2} O_{2} ) B . ( H N O_{3}+H C l rightarrow N O+C l_{2}+H_{2} O ) c. ( 3 C l O^{-} rightarrow C l O_{3}^{-}+2 C l^{-} ) D. ( C l_{2}+H_{2} O rightarrow H C l+H C l O ) | 11 |
| 704 | Assertion Conversion of potassium ferrocyanide to potassium is an oxidation process. Reason Oxidation is the additon of oxygen 1 electronegative element to a substance or removal of hydrogen / electropositive element from a 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 |
| 705 | What is the oxidation number of underlined element? [ boldsymbol{B} boldsymbol{a}left(boldsymbol{H}_{2} underline{boldsymbol{P}} boldsymbol{O}_{2}right)_{2} ] | 11 |
| 706 | Balance the following redox reaction in basic medium. ( boldsymbol{C l}_{2}+boldsymbol{I} boldsymbol{O}_{3}^{-}+boldsymbol{O H}^{-} longrightarrow boldsymbol{I} boldsymbol{O}_{4}^{-}+boldsymbol{C l}^{-} ) A ( cdot C l_{2}+I O_{3}^{-}+3 O H^{-} rightarrow I O_{4}^{-}+5 C l^{-}+H_{2} O ) B. ( C l_{2}+I O_{3}^{-}+2 O H^{-} rightarrow I O_{4}^{-}+2 C l^{-}+H_{2} O ) c. ( C l_{2}+2 I O_{3}^{-}+2 O H^{-} rightarrow I O_{4}^{-}+5 C l^{-}+H_{2} O ) D. None of the above | 11 |
| 707 | When Magnesium is burnt in air, a white ash remain as left over. What is this? ( mathbf{A} cdot M g O_{2} ) в. ( M g O ) c. ( M g ) D. ( M g_{3} O ) | 11 |
| 708 | For the redox reaction ( M n O_{4}^{ominus}+C_{2} O_{4}^{2-}+H^{oplus} longrightarrow M n^{2+}+ ) ( boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) the correct coefficients of the reactions for the balanced reaction are: ( begin{array}{lll}text { A. } M n O_{4}^{ominus} & C_{2} O_{4}^{2-} & H^{oplus}end{array} ) ( 2 quad 5 quad 16 ) B. ( M n O_{4}^{ominus} quad C_{2} O_{4}^{2-} quad H^{oplus} ) ( 16 quad 5 quad 2 ) ( begin{array}{lll}text { c. } M n O_{4}^{ominus} & C_{2} O_{4}^{2-} & H^{oplus}end{array} ) 16 D. ( M n O_{4}^{ominus} quad C_{2} O_{4}^{2-} quad H^{oplus} ) | 11 |
| 709 | Which of the following is a redox reaction? ( mathbf{A} cdot H_{2} S O_{4} ) with ( N a O H ) B. In atmosphere, ( O_{3} ) from ( O_{2} ) by lightning C. Nitrogen oxides form nitrogen and oxygen by lightning D. Evaporation of ( H_{2} O ) | 11 |
| 710 | Identify the type of reaction taking place in ( boldsymbol{F e}+boldsymbol{C u S O}_{4} rightarrow boldsymbol{C u}+boldsymbol{F e} boldsymbol{S O}_{4} ) A. Redox reaction B. Displacement reaction c. Neutralization reaction D. Precipitation reaction | 11 |
| 711 | The reaction, ( Z n^{2+}(a q)+2 e^{-} rightarrow Z n(s) ) is: A. oxidation B. reduction c. redox reduction D. none of the above | 11 |
| 712 | What is the sum of oxidation numbers of all the carbon atoms except that attached to ( -C H O ) group in ( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{5}} boldsymbol{C} boldsymbol{H} boldsymbol{O} ? ) A . -6 B. -5 c. -4 D. – – | 11 |
| 713 | Name the reducing agent in the following: ( mathbf{3} M n O_{2}+4 A l rightarrow 3 M n+2 A l_{2} O_{3} ) ( mathbf{A} cdot M n ) B. ( A l ) ( mathrm{c} cdot M n O_{2} ) D. ( A l_{2} O_{3} ) | 11 |
| 714 | The above reaction is a type of intramolecular disproportionation reaction. If true enter 1 , else enter 0 . [ underbrace{mathrm{CHO}}_{mathrm{CHO}} stackrel{mathrm{OH}^{-}}{longrightarrow} underbrace{mathrm{COO}^{-}}_{mathrm{CH}_{2} mathrm{OH}} ] ( A ) | 11 |
| 715 | In the reaction, ( C l_{2}+O H^{-} rightarrow C l^{-}+ ) ( C l O_{4}^{-}+H_{2} O, ) chlorine is? A. Oxidised B. Reduced c. Oxidised as well as reduced D. Neither oxidised nor reduced | 11 |
| 716 | Reaction of magnesium ribbon with dilute sulphuric acid to form magnesium sulphate and hydrogen is a combination reaction. A. True B. False | 11 |
| 717 | Match the reactions in column I with their respective characteristics given in column II. | 11 |
| 718 | Identify disproportionation reaction. ( mathbf{A} cdot C H_{4}+2 O_{2} rightarrow C O_{2}+2 H_{2} O ) ( mathbf{B} cdot C H_{4}+4 C l_{2} rightarrow C C l_{4}+4 H C l ) ( mathbf{c} cdot 2 F_{2}+2 O H^{-} rightarrow 2 F^{-}+O F_{2}+H_{2} O ) D. ( 2 N O_{2}+2 O H^{-} rightarrow N O_{2}^{-}+N O_{3}^{-}+H_{2} O ) | 11 |
| 719 | Complete and balance the following compound ( boldsymbol{C a}_{mathbf{5}}left(boldsymbol{P O}_{4}right)_{3} boldsymbol{F}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}+ ) ( boldsymbol{H}_{2} boldsymbol{O} stackrel{boldsymbol{H} e a t}{rightarrow}-ldots-ldots-+boldsymbol{C} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4} ) ( 2 H_{2} O+_{-}-_{-}– ) | 11 |
| 720 | The number of electrons required to balance the following equation is: ( N O_{3}^{-}+4 H^{+}+e^{-} rightarrow 2 H_{2} O+N O ) ( mathbf{A} cdot mathbf{5} ) B. 4 ( c .3 ) D. 2 | 11 |
| 721 | Assertion Oxidation is the gain of oxygen. Reason Reduction is the loss of oxygen. | 11 |
| 722 | Question 22. What is meant by ‘disproportionation’? Give two examples of disproportionation reaction in aqueous solution. | 11 |
| 723 | Consider a titration of potassium dichromate solution with acidified Mohr’s salt solution using diphenylamine as indicator. The number of moles of Mohr’s salt required per mole of dichromate is: A . 3 B. 4 c. 5 D. 6 | 11 |
| 724 | Number of moles of ( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7} ) reduced by one mole of ( S n^{2+} ) ions is : A ( cdot frac{1}{3} ) B. 3 ( c cdot frac{1}{6} ) D. 6 | 11 |
| 725 | How many grams of ( 70 % ) concentrated nitric acid solution should be used to prepare ( 250 mathrm{mL} ) of ( 2.0 mathrm{M} ? ) A ( cdot 45.0 mathrm{g} ) conc. ( mathrm{H} mathrm{NO}_{3} ) B. 90.0 g conc. H ( mathrm{NO}_{3} ) c. 70.0 conc. ( H N O_{3} ) D. 54.0 g conc. H NO | 11 |
| 726 | ( 2 K(s)+F_{2}(g) rightarrow 2 K^{+} F^{-}(s) ) is a type of reaction. A. disproportionation B. combustion c. corrosion D. redox | 11 |
| 727 | 32. Browning of paper in ola books is caused by (1) frequent use (2) lack of aeration (3) collection of dust (4) oxidation of cellulose | 11 |
| 728 | Choose the correct options – A. Reaction between lead nitrate and potassium iodide is double decomposition reaction. B. Reaction between copper oxide and hydrogen is redox reaction. C. Reactions in which heat is absorbed are called exothermic reactions D. Both (A) and (B). | 11 |
| 729 | Formation of calcium oxide and carbon dioxide by heating limestone is an example of double decomposition reaction. A. True B. False | 11 |
| 730 | Statement 1: Oxidation and reduction occur together Statement 2: In redox reactions, electrons must be gained and lost. A. Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1 B. Both 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 |
| 731 | Sulphur dioxide bleaches colouring matter by A. dehydration B. oxidation c. decomposition D. reduction | 11 |
| 732 | Assign oxidation numbers to each atom in ( boldsymbol{N} boldsymbol{H}_{mathbf{4}} boldsymbol{N} boldsymbol{O}_{2} ) A. ( N=4,-4 ; H=1 ; O=-2 ) B. ( N=-3 ; H=1 ; O=3 ) c. ( N=-1 ; H=1 ; O=-2 ) | 11 |
| 733 | In the reaction, ( 4 C r O_{5}+6 H_{2} S O_{4} rightarrow ) ( 2 C r_{2}left(S O_{4}right)_{3}+6 H_{2} O+7 O_{2}, ) which statement is wrong? A. It is a disproportionation reaction. B. It is an intramolecular redox reaction c. ( C r O_{5} ) acts as oxidant and reductant both. D. cracts as oxidant and 0 acts as reductant | 11 |
| 734 | Balance the following equations. (i) ( boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2}+boldsymbol{H} boldsymbol{C l} rightarrow boldsymbol{K} boldsymbol{C l}+ ) ( M n C l_{2}+H_{2} O+C l_{2} ) (ii) ( boldsymbol{N} boldsymbol{H}_{3}+boldsymbol{O}_{3} rightarrow boldsymbol{N} boldsymbol{O}+boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 735 | Before: ( C u O+ ) porcelain boat ( =62.869 g ) ( C a C l_{2}+U-t u b e=80.483 g ) After:Porcelain boat+contents = ( 54.869 g ) CaCl ( _{2}+ ) U-tube ( =89.483 mathrm{g} ) Reactions: ( Z n(s)+2 H C l(a q) rightarrow ) ( Z n C l_{2}(a q)+H_{2}(g) ) then ( H_{2}(g)+ ) ( boldsymbol{C u} boldsymbol{O}(boldsymbol{s}) rightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g})+boldsymbol{C u}(boldsymbol{s}) ) What type of reaction occurred in the porcelain boat? A . Electrolysis B. Double displacement c. Reduction and oxidation D. Decomposition or analysis E. Combination or synthesis | 11 |
| 736 | The oxidation number of ( S ) in ( N a_{2} S_{4} O_{6} ) is : A . +2.5 B. +2 and +3 (two ( S ) have +2 and other two have +3 ) ( mathrm{c} cdot+2 ) and +3 (three ( S ) have +2 and one ( S ) has +3 D. +5 and 0 (two S have +5 and the other two ( S ) have 0 ) | 11 |
| 737 | Identify tthe compounds which are reduced and oxidised in the following reaction. ( mathbf{3} N_{2} boldsymbol{H}_{4}+mathbf{2} boldsymbol{B} boldsymbol{r} boldsymbol{O}_{3}^{-} rightarrow mathbf{3} boldsymbol{N}_{2}+mathbf{2} boldsymbol{B} boldsymbol{r}^{-}+ ) ( mathbf{6} boldsymbol{H}_{2} boldsymbol{O} ) A ( cdot N_{2} H_{4} ) is oxidised and ( B r O_{3}^{-} ) is reduced B. ( B r O_{3}^{-} ) is oxidised and ( N_{2} H_{4} ) is reduced C. ( B r O_{3}^{-} ) is both reduced and oxidised D. This is not a redox reaction | 11 |
| 738 | Number of which two chemical species will be same in the given procedure? A. ( M n O_{2} ) в. ( I_{2} ) c. ( I^{-} ) D. ( S_{2} O_{3}^{2} ) | 11 |
| 739 | Consider the following ( boldsymbol{E}^{0} ) values: ( boldsymbol{E}_{boldsymbol{F} boldsymbol{e}^{3+} / boldsymbol{F} e^{2+}}^{boldsymbol{0}}=boldsymbol{0 . 7 7 V} ) ( E_{S n^{2+} / S n}^{0}=-0.14 V ) Under standard conditions the potential for the reaction, is: ( boldsymbol{S} boldsymbol{n}(boldsymbol{s})+boldsymbol{2} boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{2} boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{a} boldsymbol{q})+ ) ( boldsymbol{S} boldsymbol{n}^{2+}(boldsymbol{a} boldsymbol{q}) ) A . ( 0.91 mathrm{V} ) B. 1.40V c. ( 1.68 v ) D. 0.63v | 11 |
| 740 | Hydrogen sulphide gets reduced to sulphur. A . True B. False | 11 |
| 741 | When a piece of magnesium ribbon is placed in a beaker of copper sulfate solution, which one of the following is most likely to happen? A. A vigorous reaction immediately takes place, with the release of a lot of heat B. The blue colour of the copper sulfate solution gets darker c. The blue colour of the copper sulfate solution gets lighter. D. The magnesium catches fire | 11 |
| 742 | Oxidation number is ( mathrm{S} ) in ( left(C H_{3}right)_{2} S O ) is : A. zero B. +1 ( c cdot+2 ) ( D cdot+3 ) | 11 |
| 743 | The oxidation state of iodine in ( boldsymbol{H}_{4} boldsymbol{I} boldsymbol{O}_{mathbf{6}}^{-} ) is? ( A cdot+7 ) B. – ( c .+5 ) D. +1 | 11 |
| 744 | The permanganate ion is an excellent oxidizing agent in aqueous solutions. When the half reaction, ( M n O_{4}^{-}+ ) ( boldsymbol{H}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) is balanced, the correct coefficients for the species involved are: A. 1,4,4,1,2 B. 1,4,2,1,2 c. 1,4,3,1,2 D. 1,4,1,1,2 | 11 |
| 745 | 09. Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions, (a) 2AgBr(s) + C,H,O, (aq) — 2Ag(s) + 2HBr(aq) + C.H.O.(aq) (6) HCHOW) + 2[Ag(NH2).1 (aq) + 3OH (ag) Ag(s) + HCOO (aq) + 4NH (aq) + 2H,01) (c) NH4) + 2H,0,0) – Ng(g) + 4H,O) | 11 |
| 746 | Which of the following represent redox reactions? ( mathrm{Cr}_{2} mathrm{O}_{7}^{2-}+2^{ominus} boldsymbol{O} boldsymbol{H} longrightarrow 2 boldsymbol{C r} boldsymbol{O}_{4}^{2-}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ) II. ( Z n+C u S O_{4} longrightarrow Z n S O_{4}+C u ) III. ( 2 M n O_{4}^{ominus}+3 M n^{2+}+4 stackrel{theta}{O} H longrightarrow ) ( mathbf{5} M n O_{2}+2 H_{2} O ) IV. ( 2 C u^{oplus} longrightarrow C u+C u^{2+} ) A . ।, । । в. ।, ॥ c. ॥ा, ।ा D. ॥, ॥I, IV | 11 |
| 747 | Solid calcium oxide was taken in a container and water was added slowly to it- (i) State two observations made in the experiment. (ii) Write the name and the chemical formula. | 11 |
| 748 | 10. In the ethylene molecule the two carbon atoms have the oxidation numbers. (a) -1, -1 (6) -2,-2 (c) -1, -2 2 (d) +2,2 5 d) | 11 |
| 749 | ( 10=0 ) ( alpha ) ( alpha ) ( alpha ) | 11 |
| 750 | Assertion The two Fe atoms in ( F e_{3} O_{4} ) have different oxidation numbers. Reason ( F e^{2+} ) ions decolourise ( K M n O_{4} ) Solution. 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 |
| 751 | Consider the reactions: ( mathbf{2} S_{2} O_{3}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{I}_{2}(boldsymbol{s}) rightarrow boldsymbol{S}_{4} boldsymbol{O}_{6}^{2-}(boldsymbol{a} boldsymbol{q})+ ) ( 2 I^{-}(a q) ) ( boldsymbol{S}_{2} boldsymbol{O}_{3}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{B} boldsymbol{r}_{2}(boldsymbol{l})+boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) rightarrow ) ( mathbf{2} boldsymbol{S} boldsymbol{O}_{mathbf{4}}^{mathbf{2}-}(boldsymbol{a} boldsymbol{q})+boldsymbol{4} boldsymbol{B} boldsymbol{r}^{-}(boldsymbol{a} boldsymbol{q})+mathbf{1 0} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) ) Why does the same reductant, thiosulphate react differently with iodine and bromine? | 11 |
| 752 | Which of the reactants act as oxidant or reductant if any: ( boldsymbol{C a}+boldsymbol{C l}_{2} rightarrow boldsymbol{C a} boldsymbol{C l}_{2} ) A ( cdot C l_{2} ) в. ( C a ) c. Both of these D. None of these | 11 |
| 753 | ( boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{A} boldsymbol{X}+boldsymbol{B} boldsymbol{Y} longrightarrow boldsymbol{H} boldsymbol{A}+boldsymbol{O} boldsymbol{Y}+ ) ( boldsymbol{X}_{2} boldsymbol{B} ) In the above-unbalanced redox reaction, the oxidation number of ( boldsymbol{X} ) is -2 and neither ( X ) nor water is involved in the redox process. If the above reaction is balanced with the smallest whole-number coefficients, the sum of the stoichiometric coefficients of all the compounds is : ( A cdot 9 ) B. 8 ( c .7 ) D. 6 | 11 |
| 754 | Q7. Suggest a list of substances where carbon can exhibit oxidation states from nitrogen from -3 to +5. 4 to +4 and | 11 |
| 755 | What is the oxidation number of underlined element? [ underline{I} C l_{3} ] | 11 |
| 756 | Match the reactions in list I with the number of electrons that participate in list II. | 11 |
| 757 | Which one of the following substances is a good oxidising agent? A. coke B. water c. Hydrogen peroxide D. sulphur dioxide | 11 |
| 758 | Match the Column-I with Column-II. | 11 |
| 759 | During the oxidation of arsenite ion, ( A s O_{3}^{3-}, ) to arsenate ion, ( A s O_{4}^{3-}, ) in alkaline medium, the number of moles of hydroxide ions consumed per mole of arsenite ion is ( A cdot 2 ) B. 3 ( c cdot 2 / 3 ) D. 3/2 | 11 |
| 760 | Identyfy oxidation and reduction process for the reaction- ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s})+boldsymbol{F}_{2}(boldsymbol{g}) rightarrow boldsymbol{H} boldsymbol{F}(boldsymbol{g})+boldsymbol{H} boldsymbol{O} boldsymbol{F}(boldsymbol{g}) ) | 11 |
| 761 | ( boldsymbol{H} boldsymbol{C l}(boldsymbol{a} boldsymbol{q})+boldsymbol{Z} boldsymbol{n}(boldsymbol{s}) rightarrow boldsymbol{Z} boldsymbol{n} boldsymbol{C l}_{2}(boldsymbol{a q})+ ) ( boldsymbol{H}_{2}(boldsymbol{g}) ) In the reaction above, which term best describes the role of ( boldsymbol{H} boldsymbol{C l}(boldsymbol{a} boldsymbol{q}) ? ) A. Bronsted acid B. Oxidizing agent c. Reducing agent D. Precipitate E. Cathode | 11 |
| 762 | The non-metals undergoing disproportionation are This question has multiple correct options ( A cdot P_{4} ) в. ( C l_{2} ) ( c cdot I_{2} ) D. | 11 |
| 763 | Choose the correct option regarding change in oxidation number of the underlined atom in the following conversion. ( boldsymbol{H}_{2} underline{boldsymbol{S}} boldsymbol{O}_{5}+boldsymbol{2} boldsymbol{K} boldsymbol{I} rightarrow boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{I}_{2} ) ( A cdot 2 ) B. 3 ( c ) D. No Change | 11 |
| 764 | In which of the following reactions have the underlined substance been reduced? A. Carbonmonoxide + copperoxide ( rightarrow ) carbondioxide ( + ) Carbon copper в. ( frac{text { Copperoxide }}{text { water }}+ ) hydrochloricacid ( rightarrow ) copperchloride ( + ) c. Hydrogen( + )ironoxide( rightarrow )iron ( + )water D. ( underline{S t e a m}+ )iron ( rightarrow ) ironoxide ( + )hydrogen | 11 |
| 765 | The addition of oxygen to a substance is called A. oxidation B. reduction c. synthesis D. none of these | 11 |
| 766 | Dichloroacetic acid ( left(boldsymbol{C H} boldsymbol{C l}_{2} boldsymbol{C O}_{2} boldsymbol{H}right) ) is oxidized to ( C O_{2}, H_{2} O ) and ( C l_{2} ) by 1.2 equivalents of an oxidizing agent. Same amount of the acid can neutralize ‘X’ moles of ( N H_{2} ) to give ammonium dichloroacetate.’ ( X^{prime} ) is A. 0.4 B. 0.3 ( c cdot 0.2 ) D. 0.1 | 11 |
| 767 | Which of the following are primary standard? This question has multiple correct options A . Oxalic acid B. Potassium permanganate c. Potassium dichromate D. Sodium hydroxide | 11 |
| 768 | Q5. Write the O.N of all the atoms for the following well known oxidants? (i) KMnO, (ii) K,Cr,0, (iii) KCIO, | 11 |
| 769 | In acid medium, the standard reduction potential of ( N O ) converted to ( N_{2} O ) is ( mathbf{1 . 5 9} boldsymbol{V} ). Its standard potential in alkaline medium would be: A. ( -1.59 V ) В. ( -0.764 V ) c. ( 0.764 V ) D. ( 0.062 V ) | 11 |
| 770 | In a balanced equation, ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}+ ) ( boldsymbol{x} boldsymbol{H} boldsymbol{I} rightarrow boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{y} boldsymbol{I}_{2}+boldsymbol{z} boldsymbol{H}_{2} boldsymbol{O}, ) the values of ( x, y ) and ( z ) are respectively: A. ( x=3, y=5, z=2 ) в. ( x=4, y=8, z=5 ) c. ( x=8, y=4, z=4 ) D. ( x=5, y=3, z=1 ) | 11 |
| 771 | When hydrogen sulphide gas is passed through a blue solution of copper sulphate, a black precipitate of copper sulphide is formed. This is an example of? (a) combination reaction (b) displacement reaction (c) decomposition reaction (d) double decomposition reaction | 11 |
| 772 | In cyanide method, silver metal is obtained as given in the following reaction: ( mathbf{2} boldsymbol{K}left[boldsymbol{A} boldsymbol{g}(boldsymbol{C} boldsymbol{N})_{2}right]+boldsymbol{Z} boldsymbol{n} longrightarrow ) ( boldsymbol{K}_{2}left[boldsymbol{Z} boldsymbol{n}(boldsymbol{C} boldsymbol{N})_{4}right]+boldsymbol{2} boldsymbol{A} boldsymbol{g} ) In this : A. ( A g ) has been oxidised and ( Z n ) has been reduced B. ( A g^{+} ) has been reduced and ( Z n ) has been oxidised c. both the metals have been oxidised D. both the metals have been reduced | 11 |
| 773 | In redox reactions, oxidation state of oxidising agent and reducing agent respectively A. Increases and decreases B. Decreases and increases c. Increases and remains same D. Decreases and remains same | 11 |
| 774 | From the given reactions which is a redox reaction? This question has multiple correct options ( mathbf{A} cdot C u O(s)+H_{2}(g) rightarrow C u(s)+H_{2} O(l) ) B ( cdot 2 C u(s)+O_{2}(g) rightarrow 2 C u O(s) ) ( mathbf{c} cdot C(s)+2 H_{2}(g) rightarrow C H_{4}(g) ) D. ( 4 A l(s)+3 O_{2}(g) rightarrow 2 A l_{2} O_{3}(s) ) | 11 |
| 775 | Carbon and oxygen combine to form two oxides, carbon monoxide and carbon dioxide in which the ratio of the weights of carbon and oxygen is respectively 12: 16 and 12: 32 These figures illustrate the: A. Law of multiple proportions B. Law of reciprocal proportions c. Law of conservation of mass D. Law of constant proportions | 11 |
| 776 | Q.8 Which of the following arrangements represent increasing oxidation number of the central atom ? (a) Cro, CIOZ, Croa. MnO4 (b) CIO3, Croa. Mno. Croz (c) Croz, CIO3, MnO,, Cro (d) Croa. Mnoz, CrO2, CIO | 11 |
| 777 | When ( C u O ) reacts with hydrogen, ( dots )……. is reduced. A. ( C u O ) в. ( H_{2} ) c. ( C u ) D. ( H_{2} O ) | 11 |
| 778 | Why do fireflies glow at night? A. Fireflies contain an organic compound. B. Chemical reaction involves emission of visible light. C. Fireflies produce two chemicals which mix with each other and oxygen. D. All of the above. | 11 |
| 779 | One mole of ( N_{2} H_{4} ) loses 10 moles of electrons to form a new compound ( boldsymbol{A} ) Assuming that all the nitrogen appears in the new compound, what is the oxidation state of nitrogen in ( A ) ? [There is no change in the oxidation state of hydrogen ( ] ) A ( .+1 ) B. -3 ( c cdot+3 ) D. +5 | 11 |
| 780 | Give half cell equation of Daniel cell takes place at cathode. | 11 |
| 781 | Which of the following reaction is an example of a redox reaction? A. ( X e F_{2}+P F_{5} rightarrow[X e F]^{+}+P F_{6} ) в. ( X e F_{6}+H_{2} O rightarrow X e O F_{4}+2 H F ) c. ( X e F_{6}+2 H_{2} O rightarrow X e O_{2} F_{2}+4 H F ) D. ( X e F_{4}+O_{2} F_{2} rightarrow X e F_{6}+O_{2} ) | 11 |
| 782 | Balance the following equations by oxidation number method. ( boldsymbol{H}_{2} boldsymbol{O}_{2}+boldsymbol{C l} boldsymbol{O}_{2}+boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{C l}^{-}+boldsymbol{O}_{2}+ ) ( boldsymbol{H}_{2} boldsymbol{O} ) | 11 |
| 783 | One gas bleaches the colour of flowers by reduction while the other gas by oxidation. The two gases are, respectively: A ( cdot cos 2 l_{2} ) в. ( H_{2} S & B r_{2} ) ( mathrm{c} cdot operatorname{SO}_{2} & C l_{2} ) D. ( N H_{3} & S O_{3} ) | 11 |
| 784 | “Nitric oxide reacts with oxygen to form reddish brown nitrogen dioxide gas”” Choose the correct equation for the above reaction A ( cdot 2 N O+O_{2} rightarrow 2 N O_{2} ) в. ( N_{2} O+O_{2} rightarrow N O_{2}+N O ) C. ( N a N O_{3} stackrel{text {heat}}{longrightarrow} 2 mathrm{NaNO}_{2}+mathrm{O}_{2} ) D. ( 2 N O_{3}+O_{2} rightarrow 2 N O_{2}+2 O_{2} ) | 11 |
| 785 | Other things being equal, the EMF of a Daniell cell may be increased by A. Keeping low temperature B. Using large copper electrodes c. using large zinc electrodes D. Decreasing concentration of ( C u^{2+} ) ions | 11 |
| 786 | mpounds exchange their (a A The reactions in which two compounds radicals to form two new compounds are called (a) displacement reaction (b) decomposition reaction (c) double displacement reaction (d) isomerisation reaction ronction and tell thiob | 11 |
| 787 | In calcium hypophosphite, oxidation number of phosphorus is ( mathbf{A} cdot mathbf{0} ) B. +1 ( c cdot+3 ) D. + 5 | 11 |
| 788 | Which of the following half-reactions is correctly balanced? A ( cdot M n O_{4}^{-} rightarrow M n^{2+}+4 H_{2} O ) B. ( C u+2 A g^{+} rightarrow 2 A g+C u^{2+} ) ( mathbf{c} cdot H_{2}+O H^{-} rightarrow 2 H_{2} O ) ( mathbf{D} cdot P b^{2+}+2 e^{-} rightarrow P b ) E ( cdot 2 F^{-}+2 e^{-} rightarrow F_{2} ) | 11 |
| 789 | Assertion Moles of KMnO4 required for oxidation of Fe2 in acidic and basic medium will be different. Reason Final oxidation state to which M will be reduced will be different in case of acidic and basic medium. 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 |
| 790 | Oxidation state of carbon in ( boldsymbol{C} boldsymbol{H} boldsymbol{C l}_{3} ) is : ( A cdot+1 ) ( B .+2 ) ( c cdot+4 ) D. – – | 11 |
| 791 | 17. The number of moles of Mohr’s salt required per mole of dichromate ion is: (a) 3 (b) 4 2 (c) 5 (d) 6 | 11 |
| 792 | Which of the following has least tendency in +3 oxidation state to show disproportionation reaction. A . ( N ) в. ( P ) ( c . B i ) D. ( S b ) | 11 |
| 793 | Which of the following is a dispropprtonation reaction? A ( cdot C a C O_{3}+2 H^{+} rightarrow C a^{2+}+C O_{2} ) B ( cdot 2 C r O_{4}^{2-}+rightarrow C r_{2} O_{7}^{2+} H_{2} O ) c. ( C r_{2} O_{4}^{2-}+rightarrow 2 C r O_{4}^{2-}+H_{2} O ) D. ( C u_{2} O+2 H^{+} rightarrow C u^{2+}+H_{2} O ) | 11 |
| 794 | ( ldots B r O_{3}^{-}(a q)+ldots B r^{-}(a q)+ ) ( ldots boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow ldots boldsymbol{B} boldsymbol{r}_{2}(boldsymbol{l})+ldots boldsymbol{H}_{2} boldsymbol{O} ) After balancing the above equation. What is the ratio of coefficient ( B r O_{3}^{-} ) to ( B r^{-} ? ) A .1: 5 B. 1: 3 ( c cdot 1: 2 ) D. 1: E. 2: 3 | 11 |
| 795 | Which of the following is not a redox reaction? A. ( C a C O_{3} rightarrow C a O+C O_{2} ) в. ( O_{2}+2 H_{2} rightarrow 2 H_{2} O ) c. ( _{N a+H_{2} O rightarrow N a O H+frac{1}{2} H_{2}} ) D. ( M n C l_{3} rightarrow M n C l_{2}+frac{1}{2} C l_{2} ) | 11 |
| 796 | Q. 18 Mn0% undergoes disproportionation reaction in acidic medium but Mno does not. Give reason. | 11 |
| 797 | In the following redox reaction: ( boldsymbol{Z} boldsymbol{n}(boldsymbol{s})+boldsymbol{N} boldsymbol{O}_{boldsymbol{3}}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) longrightarrow ) ( Z n^{2+}(a q)+N H_{4}^{+}(a q) ) ( Z n(s) ) and ( N O_{3}^{-}(a q) ) respectively are respectively: A. oxidant and reductant B. reductant and oxidant c. both oxidant D. both reductant | 11 |
| 798 | Find the oxidation number of Ni in ( left[boldsymbol{N} boldsymbol{i}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right]^{4-} ) | 11 |
| 799 | ( boldsymbol{x} boldsymbol{N a O H}+boldsymbol{H}_{2} boldsymbol{S O}_{4} rightarrow boldsymbol{N a}_{2} boldsymbol{S O}_{4}+ ) ( boldsymbol{y} boldsymbol{H}_{2} boldsymbol{O} . ) Balance the given chemical equation and find the value of ( x ) and ( y ) A .2,1 в. 2,2 c. 2,3 D. 1,2 | 11 |
| 800 | In the following reaction: ( boldsymbol{x} boldsymbol{Z} boldsymbol{n}+boldsymbol{y} boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3}(boldsymbol{d} boldsymbol{i} l) longrightarrow ) ( boldsymbol{a} boldsymbol{Z} boldsymbol{n}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}+boldsymbol{b} boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{c} boldsymbol{N} boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{3} ) What is the sum of the coefficients ( (a+b+c) ? ) | 11 |
| 801 | Excess of KI reacts with ( C u S O_{4} ) solution and then ( N a_{2} S_{2} O_{3} ) solution is added to it. Which of the statement is incorrect for this reaction? A ( cdot C u_{2} I_{2} ) is formed B. ( C u I_{2} ) is formed c. ( N a_{2} S_{2} O_{3} ) is oxidised D. Evolved ( I_{2} ) is reduced | 11 |
| 802 | ( boldsymbol{H}_{2} boldsymbol{O}_{2}+boldsymbol{O}_{3} rightarrow boldsymbol{H}_{2} boldsymbol{O}+mathbf{2} boldsymbol{O}_{2}, ) in this reaction A. ( H_{2} O_{2} ) is bleached B. ( H_{2} O_{2} ) is oxidised C. ( H_{2} O_{2} ) is dehydrated D. ( H_{2} O_{2} ) is neither oxidised nor reduced | 11 |
| 803 | ( M n O_{4}^{2-}(1 text { mole }) ) in neutral aqueous medium disproportionate to A ( cdot 2 / 3 ) mole ( M n O_{4}^{-} ) and ( 1 / 3 ) mole ( M n O_{2} ) B . 1/3 mole ( M n O_{4}^{-} ) and ( 2 / 3 ) mole ( M n O_{2} ) ( mathrm{c} cdot 1 / 3 ) mole of ( M n_{2} O_{7} ) and ( 1 / 3 ) mole of ( M n O_{2} ) D. ( 2 / 3 ) mole of ( M n_{2} O_{7} ) and ( 1 / 3 ) mole of ( M n O_{2} ) | 11 |
| 804 | Iron is extracted from iron oxide using carbon monoxide as shown. iron oxide ( + ) carbon monoxide ( rightarrow ) iron ( + ) carbon dioxide Which statement is correct? A. Carbon monoxide is oxidised to carbon dioxide B. Carbon monoxide is reduced to carbon dioxide C. Iron is oxidised to iron oxide D. Iron oxide is oxidised to iron | 11 |
| 805 | Which of the following is not a redox reaction? A. Burning of candle B. Rusting of iron c. Dissolving a saltin water D. Dissolving Zn in dil. ( H_{2} S O_{4} ) | 11 |
| 806 | From the periodic table select three possible non-metals which can show disproportionation reaction. | 11 |
| 807 | Redox indicators are substances that undergo a colour change at specific A ( . p H ) B. electrode potential c. both ( A ) and ( B ) D. none of them | 11 |
| 808 | Which of the following is not a disproportionation reaction? A ( cdot 2 P h C H O quad A l(O E t)_{3}, P h C O O C H_{2} P h ) c. ( N a H+H_{2} O longrightarrow N a O H+H_{2} ) D. All | 11 |
| 809 | Which of the following statements is wrong? A. Acidified ( K M n O_{4} ) solution decolourises on the addition of sodium oxalate B. In the reaction between ( B r_{2} ) and ( C s I, B r_{2} ) is an oxidising agent and ( C s I ) is a reducing agent c. In the reaction ( 2 K_{2} S_{2} O_{3}+I_{2} rightarrow 2 K I+K_{2} S_{4} O_{6} ), the change in the oxidation number of ( S ) is 0.5 D. ( C ) has the same oxidation number in both ( C H_{4} ) and ( C O_{2} ) | 11 |
| 810 | When phosphorus reacts with caustic soda, the products are ( P H_{3} ) and ( N a H_{2} P O_{2} . ) This reaction is an example of A. Oxidation B. Reduction c. Oxidation and reduction (Redox) D. Neutralization | 11 |
| 811 | Q13. Calculate the oxidation number of sulphur in H.So, and Na SO4 A TO | 11 |
| 812 | The oxidation number of Phosphorus in ( M g_{2} P_{2} O_{7} ) is: ( A cdot+3 ) ( B .+2 ) ( c cdot+5 ) ( D cdot-3 ) | 11 |
| 813 | If true enter 1 , else enter 0 . Following reaction is disproportionation reaction: ( N H_{4}^{+}+N O_{3}^{-} longrightarrow N_{2} O+2 H_{2} O ) ( A ) | 11 |
| 814 | Balance the following equations in acidic medium by both oxidation number and ion electron methods and identify the oxidants and the reductants : ( M n O_{4}^{-}(a q)+C_{2} H_{2} O_{4}(a q) rightarrow ) ( M n^{2+}(a q)+C O_{2}(g)+H_{2} O(l) ) | 11 |
| 815 | What is the oxidation state of chlorine in hypochlorous acid? ( A cdot+1 ) B. +3 ( c .+5 ) ( D cdot+7 ) | 11 |
| 816 | Which of the following pairs of elements show similar set of oxidation state? A. ( O^{16}, O^{18} ) в. ( N a, K ) c. ( C, B e ) D. ( Z n, R b ) | 11 |
| 817 | If a substance gains oxygen during a reaction, it is being oxidized. If it loses oxygen, it is being reduced. Oxidation and Reduction always take place together, so that if one substance is oxidized, another is reduced. Using this idea, say which substance is oxidised and which substance is reduced in each reaction ¡) ( M g+O_{2} rightarrow 2 M g O ) ( (s) ) ( (s) ) ii) ( Z n O+C rightarrow Z n+C O ) iii) ( F e_{2} O_{3}+3 C O rightarrow 2 F e+3 C O_{2} ) iv) ( C r_{2} O_{3}+2 A l rightarrow 2 C r+A l_{2} O_{3} ) | 11 |
| 818 | In balancing the half reaction: ( S_{2} O_{3}^{2-} rightarrow S(s), ) the number of electrons that must be added is : A. 2 on the right B. 2 on the left c. 3 on the right D. 4 on the left | 11 |
| 819 | The oxidation number of sulphur in the sulphur molecule ( left(S_{8}right) ) is : | 11 |
| 820 | All combustion reactions are oxidation- reduction reactions. If true enter 1 , else enter 0 . ( A ) | 11 |
| 821 | Which of the statements about the reaction below are incorrect? ( 2 P b O(s)+C(s) rightarrow 2 P b(s)+C O_{2}(g) ) (a) Lead is getting reduced. (b) Carbon dioxide is getting oxidised (c) Carbon is getting oxidised. (d) Lead oxide is getting reduced A ( cdot(a) ) and ( (b) ) B. (a) and (c) ( c cdot(a),(b) ) and ( (c) ) D. All | 11 |
| 822 | is not 1. Multip Column I Column II A. C+02 → CO2 +heat (p) Exothermic B. CaCO, A + CaO +CO, (q) Combination CN2+O2 → 2NO (r) Endothermic D. HCI+NH,OH → (s) Decomposition NH,C1+H,O+12.3kJ. heat not on | 11 |
| 823 | Explain daniel cell with cell diagram, representation and process taking place in the cell. | 11 |
| 824 | 7. The oxidation number of carbon is zero in (a) HCHO (b) CH.CI, (c) (e) all of the above H₂O, (d) CH2 | 11 |
| 825 | The reaction used to join railway tracks involves reducing agent: ( A cdot A ) в. Мв ( c cdot c ) D. co | 11 |
| 826 | Formation of ( S O_{3} ) from ( S O_{2} ) and ( O_{2} ) is a reaction. | 11 |
| 827 | Q20. Write four informations about the reaction: (CN),(8) + 2OH(aq) CN (aq) + CNO (aq) + H2O(l) | 11 |
| 828 | How much electric charge is required to oxidise: (a) 1 mole of ( H_{2} O ) to ( O_{2} ) and (b) 1 mole of ( F e O ) to ( F e_{2} O_{3} ) | 11 |
| 829 | ( boldsymbol{C u O}(boldsymbol{s})+boldsymbol{H}_{2}(boldsymbol{g}) rightarrow boldsymbol{C u}(boldsymbol{s})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ) In this reaction, is reduced. A. copper oxide B. copper c. hydrogen D. water | 11 |
| 830 | The no. of cells which may be constructed with different ( E_{c e l l}^{o} ) values for the reaction ( boldsymbol{F} boldsymbol{e}+boldsymbol{2} boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+} rightarrow boldsymbol{3} boldsymbol{F} boldsymbol{e}^{2+} boldsymbol{i} boldsymbol{s} ) | 11 |
| 831 | UU 5. The oxidation number of the carboxylic carbon atom in CH,COOH is (a) +2 (6) + 4 (c) +1 (d) +3 | 11 |
| 832 | The ( C l^{-} ) ion is formed, when ( ^{prime} C l^{prime} ) atom loses an electron. A. True B. False | 11 |
| 833 | Which of the following reactions is not oxidation-reduction reaction? ( mathbf{A} cdot H oplus+O H^{ominus} rightarrow H_{2} O ) B ( cdot frac{1}{2} H_{2}+frac{1}{2} C l_{2} rightarrow H C l ) ( mathrm{c} cdot mathrm{CaCO}_{3} rightarrow mathrm{CaO}+mathrm{CO}_{2} ) D. ( A ) and ( C ) | 11 |
| 834 | What is redox reaction? Explain with one example. | 11 |
| 835 | Balance the following equations: ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{I}^{-}+boldsymbol{H}^{+} rightarrow boldsymbol{C r}^{3+}+boldsymbol{I}_{2}+ ) ( H_{2} O ) ( mathbf{A} cdot C r_{2} O_{7}^{2-}+6 I^{-}+14 H^{+} rightarrow 2 C r^{3+}+3 I_{2}+7 H_{2} O ) B. ( C r_{2} O_{7}^{2-}+I^{-}+14 H^{+} rightarrow 2 C r^{3+}+3 I_{2}+7 H_{2} O ) ( mathbf{c} cdot C r_{2} O_{7}^{2-}+6 I^{-}+7 H^{+} rightarrow 2 C r^{3+}+I_{2}+7 H_{2} O ) D. None of these | 11 |
| 836 | Select the strongest oxidant oxoanion and weakest oxidant oxanion among the following: ( boldsymbol{V} boldsymbol{O}_{4}^{3-}, boldsymbol{C r} boldsymbol{O}_{4}^{2-}, boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{2-}, boldsymbol{F} boldsymbol{e} boldsymbol{O}_{4}^{2-} ) A. Strongest: ( F e O_{4}^{2-} ; ) weakest ( : V O_{4}^{3} ) B. Strongest: ( V O_{4}^{3-} ); weakest: ( F e O_{4}^{2} ) c. Both are equally strong D. None of these | 11 |
| 837 | In the reaction ( rightarrow ) ( M N O_{2}+4 H C L rightarrow M n C l_{2}+ ) ( mathbf{2} boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C} boldsymbol{l}_{2} ) (a) name the compound (i) oxidised (ii) reduced (b) define oxidation of reduction on its basis. | 11 |
| 838 | Oxidation number and covalency of sulphur in ( S_{8} ) molecule respectively are ( mathbf{A} cdot 6 & 8 ) B. ( 0 & 8 ) c. ( 0 & 2 ) D. ( 6 & 2 ) | 11 |
| 839 | In a conjugate pair of reductant and oxidant, the reductant has: A. lower ox. no B. higher ox. no ( c . ) same ox. no D. either of these | 11 |
| 840 | Fill up the table from the given choice. Element Oxidation number -2 in most compounds (i) in Oxygen ( quad H_{2} O_{2} ) and (ii) in ( O F_{2} ) Halogen – 1 for (iii) in all its compounds (iv) in most of its compounds Hydrogen (v)in binary metallic hydrides Sulphur (vi) in all sulphides ( mathbf{A} cdot(i)+1(i i)+1(i i i) C l(i v)+1(v)-1(v i)+2 ) B. ( (i)-1(i i)+2(i i i) F(i v)+1(v)-1(v i)-2 ) ( mathbf{c} cdot(i)-1(i i)+1(i i i) F(i v)+1(v)+2(v i)+2 ) D. ( (i)+1(i i)+2(i i i) C l(i v)+1(v)+1(v i)+6 ) | 11 |
| 841 | The value of ( ^{prime} n^{prime} ) in the reaction is: ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+mathbf{1 4} boldsymbol{H}^{+}++boldsymbol{n} boldsymbol{F} boldsymbol{e}^{2+} rightarrow ) ( 2 C r^{3+}+n F e^{3+}+7 H_{2} O ) ( A cdot 2 ) B. 3 ( c cdot 6 ) D. | 11 |
| 842 | 1113 ICU (113)41 04 4 9. Which one among the following is not example of autoredox reaction (a) P, + OHH , PO, + PH, (b) H, O H ,O + O2 (c) S, 0,2- 0,2 +S (d) AgCI + NH, Āg (NH3)2] CI 10 | 11 |
| 843 | Which of the these are disproportionation reactions? I. ( 2 mathrm{C}_{6} mathrm{H}_{5} mathrm{CHO}-^{mathrm{A}left(mathrm{CC}_{2} mathrm{H}_{5}right)_{3}} mathrm{C}_{6} mathrm{H}_{5} mathrm{COOCH}_{2} mathrm{C}_{6} mathrm{H}_{5} ) III. ( mathrm{Cl}_{2}+2 mathrm{OH}^{-} longrightarrow mathrm{Cl}^{-}+mathrm{ClO}^{-}+mathrm{H}_{2} mathrm{O} ) IV. ( 2 mathrm{KClO}_{3} longrightarrow 2 mathrm{KCl}+3 mathrm{O}_{2} ) ( mathbf{A} cdot ) ।, ॥।, ॥ ॥ в. ॥, IV c. ॥, ॥ा, । v D. I, IV | 11 |
| 844 | Which of the following reaction equation is wrongly labeled? ( mathbf{A} cdot F e+C r^{3+} rightarrow F e^{3+}+C r(r e d o x) ) B ( cdot K B r+H_{2} O rightarrow H B r+K O H ) (hydrolysis) ( mathbf{c} cdot C H_{4}+2 O_{2} rightarrow C O_{2}+2 H_{2} O ) (combustion) D. ( C H_{4}+C l_{2} rightarrow C H_{3} C l+H C l ) (addition) E ( cdot C O_{2}+H_{2} O rightarrow H_{2} C O_{3} ) (synthesis) | 11 |
| 845 | Find the oxidation number of elements in each case. ( O ) in ( O_{2}, O_{3}, O F_{2} ) and ( B a O_{2} ) в. 0,0,+2,+1 c. 0,0,+1,0 D. None of the above | 11 |
| 846 | Enzyme catalysed reaction of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) is a disproportionation redox process. If true enter 1 , else enter 0 . ( A ) | 11 |
| 847 | Permanganate ion reacts with bromide ion in basic medium to give magnesium dioxide and bromate ion.Write the balanced ionic equation for the reaction. | 11 |
| 848 | Write balanced redox reactions of the following: 4 moles of ( S n^{2+}(a q) ) reduces ( I O_{4}^{-} ) to ( boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q}) ) A ( cdot 4 S n^{2+}+I O_{4}^{-}+8 H^{+} rightarrow 6 S n^{4+}+I^{-}+4 H_{2} O ) B . ( 4 S n^{2+}+I O_{8}^{-}+8 H^{+} rightarrow 4 S n^{4+}+I^{-}+4 H_{2} O ) c. ( 4 S n^{2+}+I O_{4}^{-}+8 H^{+} longrightarrow 4 S n^{4+}+I^{-}+4 H_{2} O ) D. none of these | 11 |
| 849 | heat Column I A. C+0, → CO, B. H2S+ Cl2 → 2HCI + S C. 12+H2S → 2HI + S D. H2 + Cl2 → 2HC1 Column II (p) Displacement (q) Oxidation (r) Combination (s) Reduction | 11 |
| 850 | Determine the. oxidation state of chromium in the finfll product formed by the reaction between KI and acidified potassium dichromate solution. ( A cdot+3 ) ( B .+2 ) ( c cdot+1 ) ( D ldots-3 ) | 11 |
| 851 | Which of the reactants act as oxidant or reductant if any: ( 2 C u S O_{4}+S O_{2}+2 K B r+2 H_{2} O rightarrow ) ( 2 C u B r+2 H_{2} S O_{4}+K_{2} S O_{4} ) A ( . C u S O_{4} ) в. ( S O_{2} ) c. Both of these D. None of these | 11 |
| 852 | Indicate in each reaction which one is oxidised or reduced if any: ( mathbf{2} N boldsymbol{a}_{2} boldsymbol{S}+mathbf{4} boldsymbol{H} boldsymbol{C l}+boldsymbol{S} boldsymbol{O}_{3} rightarrow mathbf{4} boldsymbol{N} boldsymbol{a} boldsymbol{C l}+ ) ( 3 S+2 H_{2} O ) In the above reaction, which one of the following is oxidised? A ( cdot N a_{2} S ) в. ( H C l ) c. ( N a C l ) D. None of these | 11 |
| 853 | ( boldsymbol{C N}^{-} longrightarrow boldsymbol{C N O}^{-} ) The number of electrons that must be added in balancing the half reaction is: ( mathbf{A} cdot mathbf{0} ) B. 1 on the right c. 1 on the left D. 2 on the right | 11 |
| 854 | Latha dropped some crystals of ( K M n O_{4} ) in a beaker of water and observing to know what happens.What is the phenomenon that occurs in the experiment? | 11 |
| 855 | Balance the following equation. ( boldsymbol{F} boldsymbol{e} boldsymbol{S}_{2}+boldsymbol{O}_{2} rightarrow boldsymbol{F} boldsymbol{e}_{2} boldsymbol{O}_{3}+boldsymbol{S} boldsymbol{O}_{2} ) | 11 |
| 856 | Determine the standard reduction potential for the half reaction. [ boldsymbol{C l}_{2}+mathbf{2} e^{-} rightarrow mathbf{2} boldsymbol{C l}^{-} ] Given: ( boldsymbol{P t}^{2+}+mathbf{2} boldsymbol{C l}^{-} rightarrow boldsymbol{P t}+ ) [ begin{array}{l} boldsymbol{C l}_{2}, boldsymbol{E}_{c e l l}=-mathbf{0 . 1 5} boldsymbol{V} \ boldsymbol{P t}^{2+}+boldsymbol{2} e^{-} rightarrow boldsymbol{P t}, boldsymbol{E}=1.20 boldsymbol{V} end{array} ] | 11 |
| 857 | Using electron-transfer concept, identify the oxidant and reductant in the following redox reactions. (a) ( Z n(s)+2 H^{+}(a q) longrightarrow ) ( Z n^{2+}(a q)+H_{2}(g) ) (b) ( 2left[F e(C N)_{6}right]^{3-}(a q)+2 O H^{-}(a q)+ ) ( boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{2}left[boldsymbol{F} e(boldsymbol{C} boldsymbol{N})_{6}right]^{4-}(boldsymbol{a} boldsymbol{q})+ ) ( mathbf{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ) (c) ( 2left[F e(C N)_{6}right]^{3-}(a q)+2 O H^{-}(a q)+ ) ( boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{2}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right]^{4-}(boldsymbol{a} boldsymbol{q})+ ) ( boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}(l) ) | 11 |
| 858 | An excess of ( A g N O_{3} ) is added to ( 100 m L ) of a ( 0.01 M ) solution of dichlorotetraaquachromium (III) chloride. The number of moles of ( A g C l ) precipitated would be: A. 0.001 B. 0.002 c. 0.003 D. 0.01 | 11 |
| 859 | Which of the reactants act as oxidant or reductant if any: ( 2 I^{-}+H_{2} O_{2} rightarrow 2 O H^{-}+I_{2} ) ( mathbf{A} cdot H_{2} O_{2} ) B . ( I^{-} ) c. Both of these D. None of these | 11 |
| 860 | The species that undergo(es) disproportionation in alkaline medium is/are: This question has multiple correct options A ( cdot C l_{2} ) B . ( M n O_{4}^{2} ) ( c cdot N O_{2} ) D. ( C l O_{4}^{-} ) | 11 |
| 861 | In which of the following, iron is present in its lowest oxidation state? A ( cdot ) FeSO( _{4} cdot 7 mathrm{H}_{2} ) O в. ( F e(C O)_{5} ) ( mathrm{c} . F e_{e, 94} mathrm{O} ) D. ( F e_{3} O_{4} ) | 11 |
| 862 | In the reaction: ( boldsymbol{I}_{2}+2 boldsymbol{S}_{2} boldsymbol{O}_{3}^{2-} rightarrow boldsymbol{2} boldsymbol{I}^{-}+ ) ( boldsymbol{S}_{4} boldsymbol{O}_{6}^{2-} ) A ( cdot I_{2} ) is a reducing agent B . ( I_{2} ) is an oxidising agent c. ( S_{2} O_{3}^{2-} ) is a reducing agent D. ( S_{2} O_{3}^{2-} ) is an oxidising agent | 11 |
| 863 | For the redox reaction: ( boldsymbol{x} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-}+boldsymbol{y} boldsymbol{H}_{2} boldsymbol{C}_{2} boldsymbol{O}_{4}+boldsymbol{z} boldsymbol{H}^{+} rightarrow ) ( boldsymbol{m} boldsymbol{M} boldsymbol{n}^{2+}+boldsymbol{n} boldsymbol{C} boldsymbol{O}_{2}+boldsymbol{p} boldsymbol{H}_{2} boldsymbol{O} ) The values of ( x, y, m ) and ( n ) are: A. 10,2,5,2 В. 2,5,2,10 c. 6,4,2,5 D. 3,5,2,10 | 11 |
| 864 | ( boldsymbol{C}_{4} boldsymbol{H}_{10}(boldsymbol{g})+boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+ ) ( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) ) Find the coefficient of ( C O_{2} ), when the above equation is balanced using the lowest whole-number terms? ( A cdot 4 ) B. 2 ( c cdot 13 ) D. 10 E. 8 | 11 |
| 865 | Many grain products, including cereals and others that identify themselves as a ‘source of iron’ list something called reduced iron’ among the ingredients. To which of the following would the term reduced iron’ most likely be referring? A. Compounds containing iron (III) ions B. Compounds containing iron (II) ions c. Iron metal D. oxides of iron | 11 |
| 866 | Calculate the oxidation number of the underlined elements. a. ( underline{P H}_{3} ) b. ( underline{S} O_{2} ) ( boldsymbol{H} underline{boldsymbol{N}} boldsymbol{O}_{3} ) d. ( boldsymbol{H}_{3} underline{boldsymbol{P}} boldsymbol{O}_{mathbf{4}} ) ( begin{array}{llll}text { A. } text { a. }-3 ; & text { b. }+4 ; & text { c. }+5 ;end{array} ) +5 В. а. ( -3 ; quad ) b. ( +2 ; quad ) с. ( +5 ; ) d. +5 c. a. ( -3 ; ) b. +4 c. +5 +4 D. None of these | 11 |
| 867 | Which statement below is incorrect regarding balanced equations? A. ( C+O_{2} rightarrow C O_{2} ) is balanced and is a synthesis reaction B. ( C a C O_{3} rightarrow C a O+C O_{2} ) is balanced and is a decomposition reaction C ( . N a+C l_{2} rightarrow N a C l ) is not balanced but demonstrates a synthesis reaction D. ( K I+P bleft(N O_{3}right)_{2} rightarrow P b I_{2}+K N O_{3} ) is balanced and is a single replacement reaction E ( cdot 2 H_{2} O rightarrow 2 H_{2}+O_{2} ) is balanced and demonstrates a redox reaction | 11 |
| 868 | Hydrochloric acid solution ( A ) and ( B ) have a concentration of ( 0.5 N ) and ( 0.1 N ) respectively. The volume of solutions ( boldsymbol{A} ) and ( B ) required to make 2 litres of ( mathbf{0 . 2} mathbf{N} mathbf{H} mathbf{C l} ) are: A. 0.5 Lof ( A+1.5 ) Lof ( B ) B. 1.5 Lof ( A+0.5 ) Lof ( B ) c. 1.0 Lof ( A+1.0 ) Lof ( B ) D. 0.75 Lof ( A+1.25 ) Lof ( B ) | 11 |
| 869 | Q5. What is the oxidation state of Ni in Ni (CO) ? | 11 |
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