A cell reaction with n = 1 has E deg_cell = 0.1182 V at 298 K. Taking (2.303RT)/(F) = 0.0591 V, the equilibrium constant of the reaction is

NEET levelSingle correct optionDifficulty 1 of 3ec063

A cell reaction with $n = 1$ has $E_{cell}^{\circ} = 0.1182 V$ at 298 K. Taking $\frac{2.303 RT}{F} = 0.0591 V$ , the equilibrium constant of the reaction is

At equilibrium

E = 0

, so the Nernst equation gives

E^{\circ} = \frac{0.0591}{n} lo g K

, i.e.

lo g K = \frac{n E ^{\circ}}{0.0591} = \frac{1 \times 0.1182}{0.0591} = 2

. Hence

K = 1 0^{2} = 100

. Option C gives

lo g K

instead of

K

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