Assume a cell with the following reaction
$\mathrm{Cu}_{(\mathrm{s})}+2 \mathrm{Ag}^{+}\left(1 \times 10^{-3} \mathrm{M}\right) \rightarrow \mathrm{Cu}^{2+}(0.250 \mathrm{M})+2 \mathrm{Ag}_{(\mathrm{s})}$
$\mathrm{E}_{\mathrm{cell}}^{\ominus}=2.97 \mathrm{~V}$
$E_{\text {cell }}$ for the above reaction is $\_\_\_\_$ V.
(Nearest integer)
[Given : log 2.5 = 0.3979, T = 298 K]