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Class 12 Chemistry Practice Test: Electrochemistry - Nernst Equation
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Class 12 Chemistry Practice Test: Electrochemistry - Nernst Equation
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12 Questions

1. 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)
2. What is the pH of HCl solution when the hydrogen gas electrode shows a potential of -0.22 V at standard temperature and pressure?
3. What is the correct Nernst equation for M2+ (aq) + 2e+ → M (s) at 45°C?
4. 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)
5. What is the correct Nernst equation for M2+ (aq) + 2e+ → M (s) at 45°C?
6. 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)?
7. 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)
8. 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.
9. What is the value of universal gas constant in Nernst equation when the potential is given in volts?
10. Find the number of electrons transferred in the equation Cu(g) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s).
11. Find the number of electrons transferred in the equation Cu(g) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s).
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.

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