JEE Advanced 2015 · Paper 1, Chemistry question 27

All the energy released from the reaction $\mathbf X\to\mathbf Y$, $\Delta_rG^\circ=-193\ \mathrm{kJ\,mol^{-1}}$ is used for oxidizing $\ce{M+}$ as $\ce{M+ -> M^{3+} + 2e-}$, $E^\circ=-0.25$ V.

Under standard conditions, the number of moles of $\ce{M+}$ oxidized when one mole of X is converted to Y is

$[F=96500\ \mathrm{C\,mol^{-1}}]$