Chemistry Question from JEE Main 2023 · 29 January, Shift 2

The equilibrium constant for the reaction: $Zn(s) + Sn^{2+}(aq) \rightleftharpoons Zn^{2+}(aq) + Sn(s)$

is $1 \times 10^{20}$ at $298 \, \text{K}$. The magnitude of standard electrode potential of $Sn^{2+}/Sn$ if $E^\circ_{Zn^{2+}/Zn} = -0.76 \, V$ is $\ldots \times 10^{-2} \, V$ (Nearest integer).