The standard e.m.f of a cell, involving one electron change is found to be $0.591 \mathrm{~V}$ at…

The standard e.m.f of a cell, involving one electron change is found to be $0.591 \mathrm{~V}$ at $25^{\circ} \mathrm{C}$. The equilibrium constant of the reaction is $\left(\mathrm{F}=96,500 \mathrm{C} \mathrm{mol}^{-1}: \mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$
  1. $1.0 \times 10^1$
  2. $1.0 \times 10^{30}$
  3. $1.0 \times 10^{10}$
  4. $1.0 \times 10^5$

Solution

$\therefore \log \mathrm{K}_{\mathrm{eq}}=\frac{\mathrm{nE}^{\circ}}{0.0591} =\frac{1 \times 0.591}{0.0591}$ $\Rightarrow \mathrm{K}_{\mathrm{eq}}=10^{10}$

Asked in: MHT CET Full Test 10

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