All the energy released from the reaction $\mathrm{X}\to \mathrm{Y},{\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{G}}^{\mathrm{o}}=-\text{193 kJ mo}{\text{l}}^{-1}$ is used for oxidizing ${\mathrm{M}}^{+}$ as ${\mathrm{M}}^{+}\to {\mathrm{M}}^{3+}+2{\mathrm{e}}^{-},{\mathrm{E}}^{\mathrm{o}}=-0.25\mathrm{V}.$
Under standard conditions, the number of moles of ${\mathrm{M}}^{+}$ oxidized when one mole of X is converted to Y is [F = 96500 C $\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ ]