The EMF of the cell Ni/$N{i}^{2+}$  (0.01M) //$C{l}^{-}\left(0.01M\right)/C{l}_2$ , Pt is ___V if the SRP of nickel and chlorine electrodes are  -0.25V and +1.36V respectively.                      

${\mathrm{Ni}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Ni};{\mathrm{E}}^{°}=-0.25\mathrm{V}$

${\mathrm{Cl}}_2+2{\mathrm{e}}^{-}\to 2{\mathrm{Cl}}^{-};{\mathrm{E}}^{°}=+1.36\mathrm{V}$

on reversing the Ni electrode

$$\begin{gathered} \mathrm{Ni}\to {\mathrm{Ni}}^{2+}+2{\mathrm{e}}^{-};{\mathrm{E}}^{°}=+0.25\mathrm{V} \\ \mathrm{Cl}+2{\mathrm{e}}^{-}\to 2{\mathrm{Cl}}^{-};{\mathrm{E}}^{°}=+1.36\mathrm{V} \\ \mathrm{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_} \\ \mathrm{Overall} \mathrm{reaction}: \mathrm{Ni}+{\mathrm{Cl}}_2\to {\mathrm{Ni}}^{2+}+2{\mathrm{Cl}}^{-};{\mathrm{E}}_{\mathrm{cell}}^{°}=1.61\mathrm{V} \end{gathered}$$

The Nernst equation is written as

${\mathrm{E}}_{\mathrm{cell}}={\mathrm{E}}_{\mathrm{cell}}^{°}-\frac{0.0591}{\mathrm{n}}\log \left[{\mathrm{Ni}}^{2+}\right]{\left[{\mathrm{Cl}}^{-}\right]}^2$

$=1.61-\frac{0.0591}{2}\log \left[0.01\right]{\left[0.01\right]}^2$

On solving, ${\mathrm{E}}_{\mathrm{cell}}=+1.79\mathrm{V}$