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