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)}** → Cu**^{2+}_{(aq)}** + 2Ag **_{(s)}** is 4 × 10**^{16}**. Find E° **_{(cell)}** for the cell reaction.**

_{(g)}

^{+}

_{(aq)}

^{2+}

_{(aq)}

_{(s)}

^{16}

_{(cell)}

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 M**^{2+}** (aq) + 2e**^{+}** → M (s) at 45°C?**

^{2+}

^{+}

a) E°_{(M2+/M)} + 0.315log_{10} (1 / [M]^{+2})

b) E° _{(M2+/M)} + 0.0425log_{10} (1 / [M]^{+2})

c) E° _{(M2+/M)} + 0.0315log_{10} (1 / [M]^{+2})

d) E° _{(M2+/M)} + 0.0326log_{10} (1 / [M]^{+2})

**Answer: **E° _{(M2+/M)} + 0.0315log_{10} (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)}** → Ni**^{2+}_{(0.02M)}** + 2Ag**_{(s)}**. What is the concentration of Ag**^{+}** ions?**

_{(s)}

^{+}

_{(n)}

^{2+}

_{(0.02M)}

_{(s)}

^{+}

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 ZnSO**_{4}** 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)**

_{4}

_{(Zn+2/Zn)}

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 sta****ndard 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 t****he potential is given in volts?**

a) 8.314 J mol^{-1}K^{-1}

b) 0.0821 L atm mol^{-1}K^{-1}

c) 8.205 m^{3} atm mol^{-1}K^{-1}

d) 1.987 cal mol^{-1}K^{-1}

**Answer: **8.314 J mol^{-1}K^{-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}** × log**_{10}** (Anode /**** Cathode)?**

_{(cell)}

_{(cell)}

^{-3}

_{10}

a) 2

b) 6

c) 4

d) 1

**Answer: **6

**9****. Find the number of electrons transferred in the equation Cu**_{(g)}** + 2Ag**^{+}_{(aq)}** → Cu**^{2+}_{(aq)}** + 2Ag**_{(s)}**.**

_{(g)}

^{+}

_{(aq)}

^{2+}

_{(aq)}

_{(s)}

a) 4

b) 3

c) 2

d) 1

**Answer: **2

**1****0****. The standard oxidation potential of Ni/Ni**^{2+}** 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 [Ni**^{2+}**] = 1M)**

^{2+}

^{2+}

a) 5.08

b) 4

c) 4.5

d) 5.25

**Answer: **5.08

**11****. Calculate the equilibrium constant for the reaction Fe + CuSO**_{4}** ****⇌**** FeSO**_{4}** + Cu at 25°C.**

_{4}

_{4}

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

a) 3.46 × 10^{30}

b) 3.46 × 10^{26}

c) 3.22 × 10^{30}

d) 3.22 × 10^{26}

**Answer: **3.22 × 10^{30}

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

Pt, H_{2} | 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