At 298K , the standard electrode potentials of Cu ^ 2 + / Cu, Zn ^...

The given standard reduction potentials of $Zn, Cu, Ag and Fe$ are;

$E° \dfrac{{Zn}^{2 +}}{Zn} = - 0 . 76V, E° \dfrac{{Cu}^{2 +}}{cu} = 0 . 34VE° \dfrac{{Ag}^{+}}{Ag} = 0 . 80V, andE° \dfrac{{Fe}^{2 +}}{Fe} = - 0 . 44V$

The condition for reaction to occur, $E{°}_{Cell} = {\left(E{°}_{SRP}\right)}_{reductionreaction} - {\left(E{°}_{SRP}\right)}_{oxidationreaction}$ must have the positive value.

\left(A\right){Cu}^{2 +}\left(aq\right) + Fe \to Cu + {Fe}^{2 +}\left(aq\right)$</p><p>$E{°}_{Cell} = 0 . 34 + 0 . 44E{°}_{Cell} = 0 . 78V$</p><p>\left(B\right)Zn + {Fe}^{2 +}\left(aq\right) \to {Zn}^{2 +}\left(aq\right) + Fe$

$E{°}_{Cell} = - 0 . 44 + 0 . 76E{°}_{Cell} = + 0 . 32V$

\left(C\right){Cu}^{2 +}\left(aq\right) + 2Ag \to 2{Ag}^{+}\left(aq\right) + Cu$</p><p>$E{°}_{Cell} = 0 . 34 - 0 . 80E{°}_{Cell} = - 0 . 46V$</p><p>\left(D\right)Zn + {Cu}^{2 +}\left(aq\right) \to {Zn}^{2 +}\left(aq\right) + Cu$

$E{°}_{Cell} = 0 . 34 + 0 . 76E{°}_{Cell} = + 1 . 10V$

Hence, the reaction given in $C$ option is not possible.