All the energy released from the reaction $\mathrm{X} \rightarrow \mathrm{Y}, \Delta_{\mathrm{r}} \mathrm{G}^{\circ}=-193 \mathrm{~kJ} \mathrm{~mol}^{-1}$ is used for oxidizing $\mathrm{M}^{+}$as $\mathrm{M}^{+} \rightarrow \mathrm{M}^{3+} +2 \mathrm{e}^{-}, \mathrm{E}^{\circ}=-0.25 \mathrm{~V}$. Under standard conditions, the number of moles of $\mathrm{M}^{+}$oxidized when one mole of X is converted to Y is $\left[F=96500 \mathrm{C} \mathrm{mol}^{-1}\right]$