Statement Type Electrochemistry Questions for NEET

Statement Type Electrochemistry Questions for NEET

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.
1 - 12 - 13 - 14 - 45 - 16 - 3
7 - 18 - 19 - 410 - 311 - 212 - 3
13 - 114 - 215 - 416 - 217 - 318 - 4
19 - 120 - 421 - 122 - 223 - 124 - 3
25 - 326 - 127 - 128 - 129 - 130 - 1