$\text{ The EMF of the cell Ni/ }{\mathrm{Ni}}^{2+}(0.01\mathrm{M})//$ ${\mathrm{Cl}}^{-}(0.01\mathrm{M})/{\mathrm{Cl}}_2$Pt is _____V. if the SRP of nickel and chlorine electrodes are – 0.25V and +1.36V
respectively

$$\begin{gathered} \mathrm{Given} \\ \mathrm{Ni}\left|{\mathrm{Ni}}_{(0.01\mathrm{M})}^{2+}\right|\left|\mathrm{C}{{\mathrm{l}}^{-}}_{(0.01\mathrm{M})}\right|\mathrm{Cl},\mathrm{Pt} \end{gathered}$$

The reactions are written as 

$$\begin{gathered} {\mathrm{Ni}}^{2+\hspace{0.17em}}+\hspace{0.17em}2{\mathrm{e}}^{-}\to \mathrm{Ni}; {\mathrm{E}}^{\mathrm{o}}=-0.25\mathrm{V} \\ {\mathrm{Cl}}_2+\hspace{0.17em}2{\mathrm{e}}^{-}\to 2{\mathrm{Cl}}^{-}; {\mathrm{E}}^{\mathrm{o}}= +1.36\mathrm{V} \end{gathered}$$

on reversing the Ni electrode 

$$\begin{gathered} \mathrm{Ni}\to {\mathrm{Ni}}^{2+ }+\hspace{0.17em}2{\mathrm{e}}^{-}; {\mathrm{E}}^{\mathrm{o}}=+0.25\mathrm{V} \\ \mathrm{Cl}+\hspace{0.17em}2{\mathrm{e}}^{-}\to 2{\mathrm{Cl}}^{-}; {\mathrm{E}}^{\mathrm{o}}=+1.36\mathrm{V} \\ \mathrm{\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_} \\ \mathrm{Overall} \mathrm{reaction} \mathrm{Ni}\hspace{0.17em}+\hspace{0.17em}{\mathrm{Cl}}_2\to {\mathrm{Ni}}^{2+ }+\hspace{0.17em}2{\mathrm{Cl}}^{-} {\mathrm{E}}_{\mathrm{cell} }^{\mathrm{o}}= 1.61\mathrm{V} \end{gathered}$$

The Nernst equation is written as 

$$\begin{gathered} {\mathrm{E}}_{\mathrm{cell}}^{ }={\mathrm{E}}_{\mathrm{cell}}^{\mathrm{o}}-\frac{0.0591}{\mathrm{n}}\log \left[{\mathrm{Ni}}^{2+}\right] {\left[{\mathrm{Cl}}^{-}\right]}^2 \\ =1.61- \frac{0.0591}{2} \log [0.01] {[0.01]}^2 \\ \mathrm{on} \mathrm{solving} \\ {\mathrm{E}}_{\mathrm{cell}}=+ 1.79\mathrm{V} \end{gathered}$$