Emf of the cell $\mathrm{Al}\left(\mathrm{s}\right)\left|{\mathrm{Al}}^{3+}\left({10}^{-3}\mathrm{M}\right)\right|\left|{\mathrm{Ag}}^{+}\left({10}^{-1}\mathrm{M}\right)\right|\mathrm{Ag}$  at 298 K is $\left({\mathrm{E}}_{\text{cell }}^0=2.46\mathrm{V}\right)$

$\mathrm{Al}⟶{\mathrm{Al}}^{3+}+3{\mathrm{e}}^{-}$

$\left[{\mathrm{Ag}}^{+}+{\mathrm{e}}^{-}⟶\mathrm{Ag}\right]\times 3$

over all reaction is :

Al + 3Ag⁺ $\to$Al⁺³ + 3Ag

$E_{\text{cell }}=2.46-\frac{0.0591}{3}\log \frac{{10}^{-3}}{{\left({10}^{-1}\right)}^3}$

$E_{\text{cell }}=2.46\mathrm{V}$