Chemistry - Electrochemistry Question with Solution | TestHub

The electrochemical cell shown below is a concentration cell. $\mathrm{M}\mid {\mathrm{M}}^{2+}$ (saturated solution of a sparingly soluble salt, ${\mathrm{MX}}_2)\Vert {\mathrm{M}}^{2\perp }\left(0.001\mathrm{mol}{\mathrm{dm}}^{-3}\right)\mid \mathrm{M}$. The emf of the cell depends on the difference in concentrations of ${\mathrm{M}}^{2+}$ ions at the two electrodes. The emf of the cell at $298\mathrm{K}$ is $0.059\mathrm{V}$. Question:The value of $\Delta \mathrm{G}\left(\mathrm{kJ}{\mathrm{mol}}^{-1}\right)$ for the given cell is (take 1 $\mathrm{F}=96500{\mathrm{Cmol}}^{-1}$ )