Assume a cell with the following reaction ${\mathrm{Cu}}_{\left(\mathrm{s}\right)}+2{\mathrm{Ag}}^{+}\left(1\times {10}^{-3}\mathrm{M}\right)\to {\mathrm{Cu}}^{2+}(0.250\mathrm{M})+2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$
${\mathrm{E}}_{\mathrm{cell} }^{\circ }=2.97 \mathrm{V}$

${\mathrm{E}}_{\mathrm{cell} }$ for the above reaction is $\underline{ }$  $\mathrm{V}.$

(Nearest integer)

$[$ Given : $\log 2.5=0.3979, \mathrm{T}=298 \mathrm{K}]$