The standard electrode potentials of the reactions are given below. MnO_4^-+8 H^++5 e^- ⇌ Mn^2++4 H_2 O, E^°=1.51 V; 2 CO_2+2 H^++2 e^- ⇌ H_2 C_2…

The standard electrode potentials of the reactions are given below. $$\begin{array}{ll} \mathrm{MnO}_4^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightleftharpoons \mathrm{Mn}^{2+}+4 \mathrm{H}_2 \mathrm{O} & \mathrm{E}^{\circ}=1.51 \mathrm{~V} \\ 2 \mathrm{CO}_2+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightleftharpoons \mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4 & \mathrm{E}^{\circ}=-0.49 \mathrm{~V} \end{array} $$ The equilibrium constant for the reaction $$2 \mathrm{MnO}_4^{-}+6 \mathrm{H}^{+}+5 \mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4 \rightleftharpoons 2 \mathrm{Mn}^{2+}+8 \mathrm{H}_2 \mathrm{O}+10 \mathrm{CO}_2 \text { is } 10^x \text {. } $$ The value of $\displaystyle x$ is \_\_\_\_. (Nearest integer) [Given : $\displaystyle \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \mathrm{~V}$ ]