An electrochemical cell, consist of the following two redox couples, M^x+ ( aq ) / M ( s )[ E_red^Θ=+0.15 V ] and Fe^3+( aq ) / Fe ( s )[…

An electrochemical cell, consist of the following two redox couples, $\displaystyle \mathrm{M}^{x+}$ $\displaystyle (\mathrm{aq}) / \mathrm{M}(\mathrm{s})\left[\mathrm{E}_{\text {red }}^{\Theta}=+0.15 \mathrm{~V}\right]$ and $\displaystyle \mathrm{Fe}^{3+}(\mathrm{aq}) / \mathrm{Fe}(\mathrm{s})\left[\mathrm{E}_{\text {red }}^{\Theta}=-0.036 \mathrm{~V}\right]$. The cell EMF $\displaystyle \left(\mathrm{E}_{\text {cell }}\right)$ is recorded to be $\displaystyle 0.2057$ V. If the reaction quotient of the electrochemical reaction is found to be $\displaystyle 10^{-2}$, then the value of $\displaystyle x$ is $\displaystyle \_\_\_\_$ .(Nearest integer) [Given : M is a p-block metal and $\displaystyle \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \mathrm{~V}$ ]