Question:
an oxidation-reduction reaction in which 3 electrons are transferred has a $\Delta \mathrm{G}^{\circ}$ of $17.37 \mathrm{~kJ}$ $\mathrm{mol}^{-1}$ at $25^{\circ} \mathrm{C}$. The value of $\mathrm{E}_{\text {cell }}^{\circ}$ (in $\mathrm{V}$ ) is $\times 10^{-2}$
$\left(1 \mathrm{~F}=96,500 \mathrm{C} \mathrm{mol}^{-1}\right)$
Solution:
$\Delta \mathrm{G}^{\circ}=-\mathrm{AFE}^{\circ}=-3 \times 96500 \times \mathrm{E}^{\circ}$
$\Rightarrow \mathrm{E}^{\circ}=-6 \times 10^{-2} \mathrm{~V}$
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