$\Delta G$ is negative, if $E _{\text {cell }}$ is positive

Anode : $\quad Cu ( s ) \longrightarrow Cu ^{-2}\left( C _{1}\right)+2 e ^{-}: E ^{\circ}$

$\frac{\text { Cathode }: Cu ^{+2}\left( C _{2}\right)+2 e ^{-} \longrightarrow Cu ( S ):- E ^{\circ}}{\text { Cell reaction }: Cu ^{+2}\left( C _{2}\right) \longrightarrow Cu ^{+2}\left( C _{1}\right) E _{\text {cell }}^{\circ}=0}$

$E _{\text {cell }}= E _{\text {cell }}^{\circ}-\frac{2.303 RT }{ nF } \log Q$

$E _{\text {cell }}=0-\frac{2.303 RT }{ nF } \log \left(\frac{ C _{1}}{ C _{2}}\right)$

$E _{\text {cell }}>0:$ if $\frac{ C _{1}}{ C _{2}}<1 \Rightarrow C _{1}< C _{2}$