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The electrochemical cell shown below is a concentration cell.
$$M \mid M^{2+}$$ (saturated solution of a sparingly soluble salt, $$MX_2$$) $$\parallel M^{2+}$$ (0.001 mol $$dm^{-3}$$) $$\mid M$$
The emf of the cell depends on the difference in concetration of $$M^{2+}$$ ions at the two electrodes. The emf of the cell at 298 is 0.059 V
The value of $$\triangle G (kJ mol^{-1})$$ for the given cell is (take 1F = 96500 C $$mol^{-1}$$)
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