In a cell, the following reactions take place
$\begin{array}{ll}\mathrm{Fe}^{2+} \rightarrow \mathrm{Fe}^{3+}+\mathrm{le}^{-} & \mathrm{E}_{\mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}}^0=0.77 \mathrm{~V} \\ 2 \mathrm{I}^{-} \rightarrow \mathrm{I}_2+2 \mathrm{e}^{-} & \mathrm{E}_{\mathrm{I}_2 \|^{-}}^0=0.54 \mathrm{~V}\end{array}$
The standard electrode potential for the spontaneous reaction in the cell is $x \times 10^{-2} \mathrm{~V} 298 \mathrm{~K}$. The value of $x$ is$\_\_\_\_$ (Nearest Integer)