Given the equilibrium constant: ${\mathrm{K}}_{\mathrm{c}}$ of the reaction:

$\mathrm{Cu}\left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)\to {\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)$ is $10\times {10}^{15}$ , calculate the ${\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}$ of this reaction at $298 \mathrm{K}$

$\left[2.303\frac{\mathrm{RT}}{\mathrm{F}}\mathrm{\hspace{0.17em}}\mathrm{at}\mathrm{\hspace{0.17em}}298\mathrm{\hspace{0.17em}}\mathrm{K}=0.059\mathrm{\hspace{0.17em}}\mathrm{V}\right]$

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 $\mathrm{F}=96,500 \mathrm{C}\hspace{0.17em}{\mathrm{mol}}^{-1}]$

The standard reduction potentials, ${\mathrm{E}}^0$, for the half-reactions are as

$\begin{array}{l}\mathrm{Zn}\to {\mathrm{Zn}}^{2+}+2{\mathrm{e}}^{-}; {\mathrm{E}}^0=+0.76 \mathrm{V}\\ \mathrm{Fe}\to {\mathrm{Fe}}^{2+}+2{\mathrm{e}}^{-}; {\mathrm{E}}^0=+0.41 \mathrm{V}\end{array}$

the $\mathrm{emf}$ for the cell reaction,

${\mathrm{Fe}}^{2+}+\mathrm{Zn}\to {\mathrm{Zn}}^{2+}+\mathrm{Fe}$ is

Which is/are correct among the following?

Given, the half cell emf's ${\mathrm{E}}_{{{\mathrm{Cu}}^{+}}^2\mid \mathrm{Cu}}^0=0.337, {\mathrm{E}}_{{\mathrm{Cu}}^{+1}\mid \mathrm{Cu}}^0=0.521$

The standard reduction potential for ${\mathrm{Zn}}^{+2}/\mathrm{Zn}; {\mathrm{Ni}}^{+2}/\mathrm{Ni}$; and ${\mathrm{Fe}}^{+2}/\mathrm{Fe}$ are $-0.76\mathrm{V},-0.23\mathrm{V},-0.44\mathrm{V}$ 
respected. The reaction $\mathrm{X}+{\mathrm{Y}}^{+2}⟶{\mathrm{X}}^{+2}+\mathrm{Y}$ will be non-spontaneous when:

The electrode potentials for ${\mathrm{Cu}}^{2+}\left(\mathrm{aqueous}\right)+{\mathrm{e}}^{-}⟶{\mathrm{Cu}}^{+}\left(\mathrm{aqueous}\right)$ and ${\mathrm{Cu}}^{+} \left(\mathrm{aqueous}\right)+{\mathrm{e}}^{-}⟶\mathrm{Cu} \left(\mathrm{s}\right)$ are $+0.15 \mathrm{V}$ and $+0.50 \mathrm{V},$ respectively. The value of $\mathrm{E}{°}_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}$ will be: