In a cell, the following reactions take place Fe^2+ → Fe^3++ e^- E_Fe^3+ / Fe^2+^°=0.77 V; 2 I^- → I_2+2 e^- E_I_2 / I^-^°=0.54 V The standard…

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