Electrochemistry MCQ For NEET Pdf Download (Nernst Equation)

Electrochemistry MCQ For NEET Pdf Download (Nernst Equation) for AIIMS, NEET, JEE provides a comprehensive coverage of the fundamental concepts in the fields of Electrochemistry. It contains a variety of questions from previous years’ AIIMS, NEET and JEE papers.

Electrochemistry MCQ For NEET Pdf Download (Nernst Equation)

1. The equilibrium constant for a cell reaction, Cu(g) + 2Ag+(aq) ? Cu2+(aq) + 2Ag (s) is 4 × 1016. Find E° (cell) for the cell reaction.

a) 0.63 V

b) 0.49 V

c) 1.23 V

d) 3.24 V

Answer: 0.49 V

2. What is the correct Nernst equation for M2+ (aq) + 2e+ ? M (s) at 45°C?

a) E°(M2+/M) + 0.315log10 (1 / [M]+2)

b) E° (M2+/M) + 0.0425log10 (1 / [M]+2)

c) E° (M2+/M) + 0.0315log10 (1 / [M]+2)

d) E° (M2+/M) + 0.0326log10 (1 / [M]+2)

Answer: E° (M2+/M) + 0.0315log10 (1 / [M]+2)

3. The e.m.f and the standard e.m.f of a cell in the following reaction is 5 V and 5.06 V at room temperature, Ni(s) + 2Ag+(n) ? Ni2+(0.02M) + 2Ag(s). What is the concentration of Ag+ ions?

a) 0.0125 M

b) 0.0314 M

c) 0.0625 M

d) 0.0174 M

Answer: 0.0174 M

4. Calculate the electrode potential of the given electrode.

Pt, Cl2(2 bar)| 2Cl–(0.02 M); E°(Cl2 | 2Cl–) = 3.4 V

a) 3.51 V

b) 3.55 V

c) 1.26 V

d) 2.95 V

Answer: 3.51 V

5. A zinc rod dipped in n molar solution of ZnSO4 has an electrode potential of -0.56 V. The salt is 98 percent dissociated at room temperature. What is the molarity of the solution? (E°(Zn+2/Zn) = -0.5 V)

a) 8.44 × 10-3 M

b) 9.44 × 10-4 M

c) 8.44 × 10-4 M

d) 9.44 × 10-3 M

Answer: 9.44 × 10-3 M

6. What is the pH of HCl solution when the hydrogen gas electrode shows a potential of -0.22 V at standard temperature and pressure?

a) 2.17

b) 2.98

c) 3.73

d) 3.14

Answer: 3.73

7. What is the value of universal gas constant in Nernst equation when the potential is given in volts?

a) 8.314 J mol-1K-1

b) 0.0821 L atm mol-1K-1

c) 8.205 m3 atm mol-1K-1

d) 1.987 cal mol-1K-1

Answer: 8.314 J mol-1K-1

8. What is the number of electrons transferred in an equation if the Nernst equation is E(cell) = E°(cell) – 9.83 × 10-3 × log10 (Anode / Cathode)?

a) 2

b) 6

c) 4

d) 1

Answer: 6

9. Find the number of electrons transferred in the equation Cu(g) + 2Ag+(aq) ? Cu2+(aq) + 2Ag(s).

a) 4

b) 3

c) 2

d) 1

Answer: 2

10. The standard oxidation potential of Ni/Ni2+ electrode is 0.3 V. If this is combined with a hydrogen electrode in acid solution, at what pH of the solution with the measured e.m.f. be zero at 25°C? (Assume [Ni2+] = 1M)

a) 5.08

b) 4

c) 4.5

d) 5.25

Answer: 5.08

11. Calculate the equilibrium constant for the reaction Fe + CuSO4 ? FeSO4 + Cu at 25°C.

(Given E°(OP/Fe) = 0.5 V°, E°(OP/Cu) = -0.4 V)

a) 3.46 × 1030

b) 3.46 × 1026

c) 3.22 × 1030

d) 3.22 × 1026

Answer: 3.22 × 1030

12. Calculate the e.m.f. of the half-cell given below.

Pt, H2 | HCl at 1-atmosphere pressure and 0.1 M. Given, E°(OP) = 2 V.

a) 4 V

b) 5.6 V

c) 3.4 V

d) 5.4 V

Answer: 5.4 V

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