$$ \text { Match the following } $$

$$ \begin{array}{cccc} \hline & \begin{array}{c} \text { List-I } \\ \text { (Transition metal, M) } \end{array} & & \begin{array}{c} \text { List-II } \\ \left(E_{M^{2+} / M}^{\ominus}\right) \end{array} \\ \hline \text { (A) } & \mathrm{Ni} & \text { (I) } & -1.18 \\ \hline \text { (B) } & \mathrm{Mn} & \text { (II) } & -0.91 \\ \hline \text { (C) } & \mathrm{Fe} & \text { (III) } & -0.25 \\ \hline \text { (D) } & \mathrm{Cr} & \text { (IV) } & -0.44 \\ \hline \end{array} $$

The correct answer is

At 298 K , the following reaction takes place for a cell at the hydrogen electrode

$$ \mathrm{H}^{+}(a q)+e^{-} \longrightarrow \frac{1}{2} \mathrm{H}_2 \text { (1 bar) } $$

The solution pH is 10.0 . What is the hydrogen electrode potential in volts?

$$ \left(\frac{2303 R T}{F}=0.06 \mathrm{~V}\right) $$

The resistance of a conductivity cell filled with 0.1 M KCl solution is $100 \Omega$. If the resistance of the same cell when filled with 0.2 M KCl solution is $520 \Omega$, the molar conductivity of 0.02 M solution (in $\mathrm{S} \mathrm{cm}^2 \mathrm{~mol}^{-1}$ ) is (Given: conductivity of 0.1 M KCl solution $=1.29 \mathrm{Sm}^{-1}$ )

For which of the following the $E^{\ominus}\left(M^{3+} / M^{2+}\right)$ is negative?