First slide

Nernst Equation

Question

For a cell reaction involving a two-electron change, the standard e.m.f. of the cell is found to be 0.295 V at 25⁰C. The equilibrium constant of the reaction at 25⁰C will be

Moderate

A

1 × 10^–10
B

29.5 × 10^–2
C

10
D

1 × 10¹⁰

Solution

From Thermodynamics ${ΔG}^{o} = - 2.303 {RTlogK}_{c}$
${ΔG}^{O} = - {nFE}^{o}$
Equating both and simplifying
${logK}_{c} = \frac{{nFE}^{o}}{2.303 RT} = \frac{{nE}^{o}}{0.0591} = \frac{2 \times 0.295}{0.0591} = 10$
$K_{c} = 10^{10}$

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