At 298K, the standard electrode potentials of Cu^2+/ Cu, Zn^2+/ Zn, Fe^2+/ Fe and Ag^+/ Ag are 0.34V, -0.76V, -0.44V and 0.80V, respectively. On the…

The given standard reduction potentials of $\mathrm{Zn},\mathrm{Cu},\mathrm{Ag}$Zn,Cu,Ag and $\mathrm{Fe}$Fe are;

$$E{^{\circ}}_{\frac{{\mathrm{Zn}}^{2+}}{\mathrm{Zn}}}=-0.76V,E{^{\circ}}_{\frac{{\mathrm{Cu}}^{2+}}{\mathrm{cu}}}=0.34V E{^{\circ}}_{\frac{{\mathrm{Ag}}^{+}}{\mathrm{Ag}}}=0.80V,\mathrm{and}E{^{\circ}}_{\frac{{\mathrm{Fe}}^{2+}}{\mathrm{Fe}}}=-0.44V$$E∘ZnZn2+​​=−0.76V,E∘cuCu2+​​=0.34VE∘AgAg+​​=0.80V,andE∘FeFe2+​​=−0.44V

The condition for reaction to occur, $E{^{\circ}}_{\mathrm{Cell}}={(E{^{\circ}}_{\mathrm{SRP}})}_{\mathrm{reduction}\mathrm{reaction}}-{(E{^{\circ}}_{\mathrm{SRP}})}_{\mathrm{oxidation}\mathrm{reaction}}$E∘Cell​=(E∘SRP​)reductionreaction​−(E∘SRP​)oxidationreaction​ must have the positive value.

$$(A){\mathrm{Cu}}^{2+}(\mathrm{aq})+\mathrm{Fe}\rightarrow \mathrm{Cu}+{\mathrm{Fe}}^{2+}(\mathrm{aq})$$(A)Cu2+(aq)+Fe→Cu+Fe2+(aq)

$$E{^{\circ}}_{\mathrm{Cell}}=0.34+0.44 E{^{\circ}}_{\mathrm{Cell}}=0.78V$$E∘Cell​=0.34+0.44E∘Cell​=0.78V

$$(B)\mathrm{Zn}+{\mathrm{Fe}}^{2+}(\mathrm{aq})\rightarrow {\mathrm{Zn}}^{2+}(\mathrm{aq})+\mathrm{Fe}$$(B)Zn+Fe2+(aq)→Zn2+(aq)+Fe

$$E{^{\circ}}_{\mathrm{Cell}}=-0.44+0.76 E{^{\circ}}_{\mathrm{Cell}}=+0.32V$$E∘Cell​=−0.44+0.76E∘Cell​=+0.32V

$$(C){\mathrm{Cu}}^{2+}(\mathrm{aq})+2\mathrm{Ag}\rightarrow 2{\mathrm{Ag}}^{+}(\mathrm{aq})+\mathrm{Cu}$$(C)Cu2+(aq)+2Ag→2Ag+(aq)+Cu

$$E{^{\circ}}_{\mathrm{Cell}}=0.34-0.80 E{^{\circ}}_{\mathrm{Cell}}=-0.46V$$E∘Cell​=0.34−0.80E∘Cell​=−0.46V

$$(D)\mathrm{Zn}+{\mathrm{Cu}}^{2+}(\mathrm{aq})\rightarrow {\mathrm{Zn}}^{2+}(\mathrm{aq})+\mathrm{Cu}$$(D)Zn+Cu2+(aq)→Zn2+(aq)+Cu

$$E{^{\circ}}_{\mathrm{Cell}}=0.34+0.76 E{^{\circ}}_{\mathrm{Cell}}=+1.10V$$E∘Cell​=0.34+0.76E∘Cell​=+1.10V

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