Statement Type Electrochemistry Questions for NEET
In each of the following questions, a Statement I is given followed by a corresponding Statement II just below it
of the statements. Mark the correct answer from the following statements.
1. If both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I
2. If both Statement I and Statement II are correct and Statement II is not a correct explanation of Statement I
3. Statement I is correct but statement is false
4. Statement I is false but Statement II is correct
1. Statement I: On electrolysis of aqueous NaOH we will get H2 at cathode and O2 at anode
Statement II: Discharge potential of H+ is less than that of Na+
2. Statement I: In case of Hg cathode Na undergoes deposition
Statement II: Nature of electrode determines the deposition order
3. Statement I: In case of solids, conduction is electronic conduction
Statement II: Electronic conduction is due to flow of electrons
4. Statement I: Number of Faraday's required for the conversion of nitrobenzene to aniline is 8
Statement II: Change in oxidation number is 6
5. Statement I: Chemical equivalent of Mg is half of its atomic weight
Statement II: Charge present on Mg is +2
6. Statement I: H2 from acids cannot be released by Ag
Statement II: Ag is more reactive than H 7. Statement I: Zn2+ possesses greater oxidizing power than Sn2+
Statement II: The metal ion of the metal with lower –ve potential (or) higher +ve potential is a better oxidizing agent than metal ion of the metal with higher –ve potential or less +ve potential
8. Statement I: In Zn – Cu electrolytic cell Zn half- cell should be written on left-hand side
Statement II: Anode should be represented on left-hand side
9. Statement I: on dilution of the solution the electrode potential increases
Statement II: Effect of dilution on electrode potential depends on electrode whether it is metal or non-metal
10. Statement I: At the end of electrolysis using platinum electrodes an aqueous solution of copper sulphate turns colourless
Statement II: Copper in CuSO4 is converted to Cu(OH)2 during electrolysis
11. Statement I: In electrolysis, the quantity of electricity needed for depositing 1 mole of silver is different from that required for 1 mole of copper.
Statement II: The molecular weight of silver and copper are different.
12. Statement I: One coulomb of electric charge deposits weight equal to the electrochemical equivalent of the substance.
Statement II: One Faraday deposits one mole of the substance.
13. Statement I: Copper is dissolved at anode and deposited at cathode.
Statement II: Oxidation takes place at anode and reduction at cathode.
14. Statement I: 96,500 C charge is required for the reduction of one mole of silver ions.
Statement II: The amount of electricity (or) charge required for oxidation or reduction depends on the stoichiometry of the electrode reaction.
15. Statement I: If standard reduction potential for the reaction Ag+ + e → Ag is 0.80V. Then for the reaction 2Ag+ + 2e → 2Ag, it will be 1.60V
Statement II: If concentration of Ag+ ions is doubled, the electrode potential will not be doubled
16. Statement I: Auric chloride (AuCl3) solution cannot be stored in a vessel made of copper, iron, nickel, chromium, zinc or tin
Statement II: Gold is very precious metal.
17. Statement I: The potential difference between the two electrodes of galvanic cell is called the cell potential.
Statement II: Cell potential is equal to the emf of a cell.
18. Statement I: A negative value of standard reduc- tion potential means that reduction takes place on this electrode with reference to standard hydrogen electrode.
Statement II: The standard electrode potential of a half-cell has fixed value.
19. Statement I: Zinc displaces copper from copper sulphate solution.
Statement II: The E° value of zinc is –0.76 V and that of copper is +0.34
20. Statement I: Identification of cathode and anode is done by the use of thermometer.
Statement II: Higher is the value of reduction potential lesser would be its reduction power,
21. Statement I: When iron rod is immersed in NaCl solution such that half of its length is corroded and other half part when exposed to air is not corroded.
Statement II: Metal portion with less access to O2 corrodes.
22. Statement I: Pure zinc does not corrode in salt solutions.
Statement II: Metal with higher negative potential than that of H2 electrode under the conditions corrodes.
23. Statement I: Conc. HNO3 can be transported in aluminium can.
Statement II: Al becomes passive after initial reaction.
24. Statement I: Cu is less reactive than hydrogen.
Statement II: E°Cu+2/Cu is negative.
25. Statement I: Ecell should have a positive value for the cell to function.
Statement II: Ecathode < Eanode
26. Statement I: Conductivity of all electrolytes cathode anode decreases on dilution.
Statement II: On dilution number of ions per unit volume decreases.
27. Statement I: Λm for weak electrolytes shows sharp increase when the electrolytic solution is diluted.
Statement II: For weak electrolytes degree of dis- sociation increases with dilution of solution.
28. Statement I: Electrolysis of NaCl solution gives chlorine at anode instead of oxygen.
Statement II: Formation of oxygen at anode requires over voltage.
29. Statement I: For measuring resistance of an ionic solution an AC source is used.
Statement II: Concentration of ionic solution will change if DC source is used.
30. Statement I: Current stops flowing when Ecell = 0.
Statement II: Equilibrium of the cell reaction is attained.
Answer
Class-11
Class-12
1. If both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I
2. If both Statement I and Statement II are correct and Statement II is not a correct explanation of Statement I
3. Statement I is correct but statement is false
4. Statement I is false but Statement II is correct
1. Statement I: On electrolysis of aqueous NaOH we will get H2 at cathode and O2 at anode
Statement II: Discharge potential of H+ is less than that of Na+
2. Statement I: In case of Hg cathode Na undergoes deposition
Statement II: Nature of electrode determines the deposition order
3. Statement I: In case of solids, conduction is electronic conduction
Statement II: Electronic conduction is due to flow of electrons
4. Statement I: Number of Faraday's required for the conversion of nitrobenzene to aniline is 8
Statement II: Change in oxidation number is 6
5. Statement I: Chemical equivalent of Mg is half of its atomic weight
Statement II: Charge present on Mg is +2
6. Statement I: H2 from acids cannot be released by Ag
Statement II: Ag is more reactive than H 7. Statement I: Zn2+ possesses greater oxidizing power than Sn2+
Statement II: The metal ion of the metal with lower –ve potential (or) higher +ve potential is a better oxidizing agent than metal ion of the metal with higher –ve potential or less +ve potential
8. Statement I: In Zn – Cu electrolytic cell Zn half- cell should be written on left-hand side
Statement II: Anode should be represented on left-hand side
9. Statement I: on dilution of the solution the electrode potential increases
Statement II: Effect of dilution on electrode potential depends on electrode whether it is metal or non-metal
10. Statement I: At the end of electrolysis using platinum electrodes an aqueous solution of copper sulphate turns colourless
Statement II: Copper in CuSO4 is converted to Cu(OH)2 during electrolysis
11. Statement I: In electrolysis, the quantity of electricity needed for depositing 1 mole of silver is different from that required for 1 mole of copper.
Statement II: The molecular weight of silver and copper are different.
12. Statement I: One coulomb of electric charge deposits weight equal to the electrochemical equivalent of the substance.
Statement II: One Faraday deposits one mole of the substance.
13. Statement I: Copper is dissolved at anode and deposited at cathode.
Statement II: Oxidation takes place at anode and reduction at cathode.
14. Statement I: 96,500 C charge is required for the reduction of one mole of silver ions.
Statement II: The amount of electricity (or) charge required for oxidation or reduction depends on the stoichiometry of the electrode reaction.
15. Statement I: If standard reduction potential for the reaction Ag+ + e → Ag is 0.80V. Then for the reaction 2Ag+ + 2e → 2Ag, it will be 1.60V
Statement II: If concentration of Ag+ ions is doubled, the electrode potential will not be doubled
16. Statement I: Auric chloride (AuCl3) solution cannot be stored in a vessel made of copper, iron, nickel, chromium, zinc or tin
Statement II: Gold is very precious metal.
17. Statement I: The potential difference between the two electrodes of galvanic cell is called the cell potential.
Statement II: Cell potential is equal to the emf of a cell.
18. Statement I: A negative value of standard reduc- tion potential means that reduction takes place on this electrode with reference to standard hydrogen electrode.
Statement II: The standard electrode potential of a half-cell has fixed value.
19. Statement I: Zinc displaces copper from copper sulphate solution.
Statement II: The E° value of zinc is –0.76 V and that of copper is +0.34
20. Statement I: Identification of cathode and anode is done by the use of thermometer.
Statement II: Higher is the value of reduction potential lesser would be its reduction power,
21. Statement I: When iron rod is immersed in NaCl solution such that half of its length is corroded and other half part when exposed to air is not corroded.
Statement II: Metal portion with less access to O2 corrodes.
22. Statement I: Pure zinc does not corrode in salt solutions.
Statement II: Metal with higher negative potential than that of H2 electrode under the conditions corrodes.
23. Statement I: Conc. HNO3 can be transported in aluminium can.
Statement II: Al becomes passive after initial reaction.
24. Statement I: Cu is less reactive than hydrogen.
Statement II: E°Cu+2/Cu is negative.
25. Statement I: Ecell should have a positive value for the cell to function.
Statement II: Ecathode < Eanode
26. Statement I: Conductivity of all electrolytes cathode anode decreases on dilution.
Statement II: On dilution number of ions per unit volume decreases.
27. Statement I: Λm for weak electrolytes shows sharp increase when the electrolytic solution is diluted.
Statement II: For weak electrolytes degree of dis- sociation increases with dilution of solution.
28. Statement I: Electrolysis of NaCl solution gives chlorine at anode instead of oxygen.
Statement II: Formation of oxygen at anode requires over voltage.
29. Statement I: For measuring resistance of an ionic solution an AC source is used.
Statement II: Concentration of ionic solution will change if DC source is used.
30. Statement I: Current stops flowing when Ecell = 0.
Statement II: Equilibrium of the cell reaction is attained.
Answer
| 1 - 1 | 2 - 1 | 3 - 1 | 4 - 4 | 5 - 1 | 6 - 3 |
| 7 - 1 | 8 - 1 | 9 - 4 | 10 - 3 | 11 - 2 | 12 - 3 |
| 13 - 1 | 14 - 2 | 15 - 4 | 16 - 2 | 17 - 3 | 18 - 4 |
| 19 - 1 | 20 - 4 | 21 - 1 | 22 - 2 | 23 - 1 | 24 - 3 |
| 25 - 3 | 26 - 1 | 27 - 1 | 28 - 1 | 29 - 1 | 30 - 1 |
Class-11
Class-12
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