The products formed when an aqueous solution of NaBr is electrolysed in a cell having inert electrodes are:

 

Assertion: According to Kohlrausch law the molar conductivity of a strong electrolyte at infinite dilution is the sum of molar conductivities of its ions.

Reason: The current carried by cation and anion is always equal.

The reduction potential at $\mathrm{pH}=14$ for the ${\mathrm{Cu}}^{2+}/\mathrm{Cu}$  couples is

$\text{ (Given }\left.{\mathrm{E}}_{{\dot{\mathrm{c}}}^{2+}/\mathrm{Cu}}^0=0.34\mathrm{V};{\mathrm{K}}_{\mathrm{sp}}\left[\mathrm{Cu}(\mathrm{OH}{)}_2\right]=1\times {10}^{-19}\right)$:

The minimum voltage required to electroyse alumina in the Hall-Heroult process is:

$\text{ (Given, }\left.{\mathrm{\Delta G}}_{\mathrm{f}}^0\left({\mathrm{Al}}_2{\mathrm{O}}_3\right)=-1520 \mathrm{kJ} {\mathrm{mol}}^{-1};{\mathrm{\Delta G}}_{\mathrm{f}}^0\left({\mathrm{CO}}_2\right)=-394 \mathrm{kJ} {\mathrm{mol}}^{-1}\right)$

The standard reduction potentials at $298 \mathrm{K}$ for the following half-cell reactions are given :

$\begin{array}{l}{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\rightleftharpoons \mathrm{Zn}\left(\mathrm{s}\right)-0.762\end{array}$

$\begin{array}{l}{\mathrm{Cr}}^{3+}\left(\mathrm{aq}\right)+3{\mathrm{e}}^{-}\rightleftharpoons \mathrm{Cr}\left(\mathrm{s}\right)-0.74\end{array}$

$2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}\rightleftharpoons {\mathrm{H}}_2\left(\mathrm{g}\right)+0.00$

${\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}\rightleftharpoons {\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)+0.77$

Which one of the following is the strongest reducing agent?