In a cell, the following reactions take place

$\begin{aligned} &Fe^{2+} \to Fe^{3+} + e^- & E^\circ_{Fe^{3+}/Fe^{2+}} = 0.77 \text{ V} \\ &2I^- \to I_2 + 2e^- & E^\circ_{I_2/I^-} = 0.54 \text{ V} \end{aligned}$

The standard electrode potential for the spontaneous reaction in the cell is x $\times$ 10^$-$2 V 298 K. The value of x is ____________. (Nearest Integer)