For the cell Cu ( s ) | Cu ^ 2 + ( aq ) ( 0 . 1M ) ‖ Ag ^ + ( aq )...

Cell reaction is :

$Cu ( s ) + 2{Ag}^{+} ( aq ) \to {Cu}^{2 +} ( aq ) + 2Ag ( s )$

Now, ${E}_{cell} = {E}_{Cell}^{o} - \dfrac{0 . 059}{2}log\dfrac{\left[{Cu}^{2 +}\right]}{{\left[{\text{ Ag }}^{+}\right]}^{2}}$$</p><p>${E}_{1} = 0 . 3095 = {E}_{Cell}^{o} - \dfrac{0 . 059}{2} \cdot log\dfrac{0 . 1}{( 0 . 01{)}^{2}}$.......\left(1\right)$

${E}_{2} = {E}_{Cell}^{o} - \dfrac{0 . 059}{2} \cdot log\dfrac{0 . 01}{( 0 . 001{)}^{2}} . . . . . . . . . . ( 2 )$

From ( 1 )$and ( 2 ) , {E}_{2} = 0 . 28V = 28 \times {10}^{- 2}V$