Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R:

Assertion A: In equation ${∆}_{\mathrm{r}}\mathrm{G}=-{\mathrm{nFE}}_{\mathrm{cell}}$ value of ${∆}_{\mathrm{r}}\mathrm{G}$ depends on $\mathrm{n}$.
Reason R: ${\mathrm{E}}_{\mathrm{cell}}$ is an intensive property and ${∆}_{\mathrm{r}}\mathrm{G}$ is an extensive property.

In the light of the above statements, choose the correct answer from the options given below:

The emf of the following cell is $1.229 \mathrm{V}$ at $298 \mathrm{K}$.

$\mathrm{Pt},{\mathrm{H}}_2\left(1\mathrm{atm}\right)\left|{\mathrm{H}}^{+}\left(1\mathrm{M}\right)\right|{\mathrm{O}}_2\left(1\mathrm{atm}\right),\mathrm{Pt}$ 

${\mathrm{H}}_2+\frac{1}{2}{\mathrm{O}}_2\rightleftharpoons {\mathrm{H}}_2\mathrm{O}$

The standard free energy change for the cell reaction is________ $\left[\mathrm{F}=9.649\times {10}^4 \mathrm{C} {\mathrm{mol}}^{-1}\right]$

The standard electrode potential ${\mathrm{E}}^o$ and its temperature coefficient $\left(\frac{\mathrm{dE}}{\mathrm{dT}}\right)$ for a cell are $2\hspace{0.17em}\mathrm{V}$ and $-5{\times 10}^{-4}\mathrm{\hspace{0.17em}} \mathrm{V} {\mathrm{K}}^{-1}$ at $\mathrm{300\hspace{0.17em}}\mathrm{K}$, respectively. The reaction is $\mathrm{Zn} \left(\mathrm{s}\right)+{\mathrm{Cu}}^{2+} \left(\mathrm{aq}\right)\to {\mathrm{Zn}}^{2+} \left(\mathrm{aq}\right)+\mathrm{Cu} \left(\mathrm{s}\right)$. The standard reaction enthalpy $\left({\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{H}}^{-}\right)$ at $300\hspace{0.17em}\mathrm{K}$ in $\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ is 

$[$Use $\mathrm{R}=8 \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}$ and $\mathrm{F}=96,500 \mathrm{C}\hspace{0.17em}{\mathrm{mol}}^{-1}]$

For the cell reaction

$2\mathrm{F}{\mathrm{e}}^{3+}\left(\mathrm{a}\mathrm{q}\right)+2{\mathrm{I}}^{-}\left(\mathrm{a}\mathrm{q}\right)\to 2\mathrm{F}{\mathrm{e}}^{2+}\left(\mathrm{a}\mathrm{q}\right)+{\mathrm{I}}_2\left(\mathrm{a}\mathrm{q}\right)$

${\mathrm{E}}_{\mathrm{c}\mathrm{e}\mathrm{l}\mathrm{l}}^0=0.24\mathrm{V}$ at $298\mathrm{ }\mathrm{K}.$ The standard Gibbs energy $\left({\mathrm{\Delta }}_{\mathrm{r}}{\mathrm{G}}^{\mathrm{o}}\right)$ of the cell reaction is:

[Given that Faraday constant $\mathrm{F}=96500\mathrm{ }\mathrm{C}\mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$ ]

The standard emf of the cell $\left({\mathrm{E}}_{\text{cell }}°\right.$ and equilibrium constant $\left({\mathrm{K}}_{\mathrm{eq}}\right)$ of the following reaction of $298 \mathrm{K}$

${\mathrm{Cd}}^{2+}+4{\mathrm{NH}}_3\rightleftharpoons \mathrm{Cd}{\left({\mathrm{NH}}_3\right)}_4^{2+}$

The value of ${\mathrm{E}}_1^{\mathrm{o}}$ is

The standard e.m.f. of the cell, $\mathrm{Cd}\left(\mathrm{s}\right)\left|{\mathrm{CdCl}}_2\left(\mathrm{aq}\right)\left(0.1\mathrm{M}\right)\right|\left|\mathrm{AgCl}\left(\mathrm{s}\right)\right|\mathrm{Ag}\left(\mathrm{s}\right)$ in which the cell reaction is $\mathrm{Cd}\left(\mathrm{s}\right)+2\mathrm{AgCl}\left(\mathrm{s}\right)⟶2\mathrm{Ag}\left(\mathrm{s}\right)+{\mathrm{Cd}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{Cl}}^{-}\left(\mathrm{aq}\right)$ is $0.6915 \mathrm{V}$ at $0°\mathrm{C}$ and $0.6753 \mathrm{V}$ at $25°\mathrm{C}$. The enthalpy change of the reaction at $25°\mathrm{C}$ is

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

${\mathrm{E}}_{\mathrm{cell}}^{°}$ at $25°\mathrm{C}$ for the cell is $0.22 \mathrm{V}.$ The equilibrium constant at $25°\mathrm{C}$ is

According to the expression $\mathrm{\Delta G}°=-\mathrm{nFE}°$, the cell reaction is spontaneous when

(Notations and symbols carry their usual meanings)