Assertion: Reactions of electrolytic cell are reversed or stopped if current supply in electrolytic cell is stopped.

Reason: $\mathrm{\Delta G}$ is positive for the reaction taking place in electrolytic cell.

Assertion: $1$ $\mathrm{coulomb}$ electricity deposits $1$ $\mathrm{g}$-equivalent of a substance.

Reason: $1$$\mathrm{faraday}$ is charge on $1$ $\mathrm{mole}$ of electricity.

Assertion: If $\mathrm{SRP}$of substance is $-0.5\mathrm{V}$ then reduction of substance is possible only in basic medium.

Reason: $\mathrm{SRP}$ of water is $-0.8274\mathrm{V}$ and at reduction potential is zero at $\mathrm{pH}=7$

The chemical reaction,

$2\mathrm{AgCl}\left(\mathrm{s}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)⟶2\mathrm{HCl}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)$

taking place in a galvanic cell is represented by the notation:

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

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