JEE Chemistry Practice Question

For the electrochemical cell, \[ \operatorname{Mg}(\mathrm{s})\left|\mathrm{Mg}^{2+}(\mathrm{aq}, 1 \mathrm{M}) \| \mathrm{Cu}^{2+}(\mathrm{aq}, 1 \mathrm{M})\right| \mathrm{Cu}(\mathrm{s}) \] the standard emf of the cell is $2.70 \mathrm{~V}$ at $300 \mathrm{~K}$. When the concentration of $\mathrm{Mg}^{2+}$ is changed to $\boldsymbol{x} \mathrm{M}$, the cell potential changes to $2.67 \mathrm{~V}$ at $300 \mathrm{~K}$. What is the value of $\boldsymbol{x}$? (given, $\frac{F}{R}=11500 \mathrm{~K} \mathrm{~V}^{-1}$, where $F$ is the Faraday constant and $R$ is the gas constant, $\ln (10)=2.30)$