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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 \( \mathrm{x} \times 10^{-2} \mathrm{~V} \) at \( 298 \mathrm{~K} \). The value of \( \mathrm{x} \) is (nearest integer)
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