Consider the following redox reaction: $$ \mathrm{MnO}_4^{-}+\mathrm{H}^{+}+\mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4 \rightleftharpoons \mathrm{Mn}^{2+}+\mathrm{H}_2 \mathrm{O}+\mathrm{CO}_2 $$ The standard reduction potentials are given as below $\left(\mathrm{E}_{\text {red }}^{\circ}\right)$ $$...

For a certain reaction at $300 \mathrm{~K}, \mathrm{~K}=10$, then $\Delta \mathrm{G}^{\circ}$ for the same reaction is $\times 10^{-1} \mathrm{~kJ} \mathrm{~mol}^{-1}$. (Given $\left.\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)$ ]

The amount of electricity in Coulomb required for the oxidation of 1 mol of $\mathrm{H}_2 \mathrm{O}$ to $\mathrm{O}_2$ is $\times 10^5 \mathrm{C}$.

The values of conductivity of some materials at $298.15 \mathrm{~K}^{-1}$ in $\mathrm{Sm}^{-1}$ are $...