The electrochemical cell shown below is a concentration cell.
$\mathrm{M}/{\mathrm{M}}^{2+}$(saturated solution of a sparingly soluble salt $\left.{\mathrm{MX}}_2\right)\parallel {\mathrm{M}}^{2+}\left(0.00001\mathrm{mol}{\mathrm{dm}}^{-3}/\mathrm{M}\right)$
The emf of the cell depends on the difference in concentration of M²⁺ ions at the two electrodes. The emf of the cell at 298 is 0.059 V.
The value of $\mathrm{\Delta G}\left(\mathrm{kJ} {\mathrm{mol}}^{-1}\right)$ for the given cell is (take $1\mathrm{F}=96500 \mathrm{C}{ \mathrm{mol}}^{-1}$)

• A

  -5.7

• B

  5.7

• C

  11.4

• D

  -11.4