Electrochemistry · Nernst equation

An electrochemical cell consists of the following two redox couples,

$\mathrm{M}^{x+}$(aq)/M(s) [$E^\ominus_\mathrm{red} = +0.15$ V] and

$\ce{Fe^3+}$(aq)/Fe(s) [$E^\ominus_\mathrm{red} = -0.036$ V]

The cell EMF ($E_\mathrm{cell}$) is recorded to be 0.2057 V.

If the reaction quotient of the electrochemical reaction is found to be $10^{-2}$, then the value of x is (Nearest integer)

[Given : M is a p-block metal and $\dfrac{2.303RT}{F} = 0.059$ V]