In a cell, the following reactions take place

$\begin{array}{l}{\mathrm{Fe}}^{2+}\to {\mathrm{Fe}}^{3+}{\mathrm{e}}^{-}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}{\mathrm{E}}_{{\mathrm{Fe}}^{3+}/{\mathrm{Fe}}^{2+}}^{\circ }=0.77\mathrm{V}\\ 2{\mathrm{I}}^{-}\to {\mathrm{I}}_2+2{\mathrm{e}}^{-}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em}\hspace{0.25em} {\mathrm{E}}_{{\mathrm{I}}_2/{\mathrm{I}}^{-}}^{\circ }=0.54\mathrm{V}\end{array}$

The standard electrode potential for the spontaneous reaction in the cell is x × 10^–2 V 298
K. The value of x is __________ (Nearest Integer)