Assume a cell with the following reaction Cu_( s ) +2 Ag^+(1 × 10^-3 M ) → Cu^2+(0.250 M )+2 Ag_( s ); E_cell^ =2.97 V E_cell for the above reaction…

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