Using the standard electrode potentials given in the Table $8.1$,predict if the reaction between the following is feasible:
$(a)$ $Fe^{3+}_{(aq)}$ and $I^{-}_{(aq)}$
$(b)$ $Ag^{+}_{(aq)}$ and $Cu_{(s)}$
$(c)$ $Fe^{3+}_{(aq)}$ and $Cu_{(s)}$
$(d)$ $Ag_{(s)}$ and $Fe^{3+}_{(aq)}$
$(e)$ $Br_{2(aq)}$ and $Fe^{2+}_{(aq)}$

(N/A) The possible reaction between $Fe^{3+}_{(aq)} + I^{-}_{(aq)}$ is $2Fe^{3+}_{(aq)} + 2I^{-}_{(aq)} \to 2Fe^{2+}_{(aq)} + I_{2(s)}$.
Oxidation: $2I^{-}_{(aq)} \to I_{2(s)} + 2e^{-}; E^{\circ} = -0.54 \ V$
Reduction: $[Fe^{3+}_{(aq)} + e^{-} \to Fe^{2+}_{(aq)}] \times 2; E^{\circ} = +0.77 \ V$
Overall: $E^{\circ}_{cell} = +0.77 - 0.54 = +0.23 \ V$. Since $E^{\circ}_{cell} > 0$,the reaction is feasible.
$(b)$ The possible reaction between $Ag^{+}_{(aq)} + Cu_{(s)}$ is $2Ag^{+}_{(aq)} + Cu_{(s)} \to 2Ag_{(s)} + Cu^{2+}_{(aq)}$.
Oxidation: $Cu_{(s)} \to Cu^{2+}_{(aq)} + 2e^{-}; E^{\circ} = -0.34 \ V$
Reduction: $[Ag^{+}_{(aq)} + e^{-} \to Ag_{(s)}] \times 2; E^{\circ} = +0.80 \ V$
Overall: $E^{\circ}_{cell} = +0.80 - 0.34 = +0.46 \ V$. Since $E^{\circ}_{cell} > 0$,the reaction is feasible.
$(c)$ The possible reaction between $Fe^{3+}_{(aq)} + Cu_{(s)}$ is $2Fe^{3+}_{(aq)} + Cu_{(s)} \to 2Fe^{2+}_{(aq)} + Cu^{2+}_{(aq)}$.
Oxidation: $Cu_{(s)} \to Cu^{2+}_{(aq)} + 2e^{-}; E^{\circ} = -0.34 \ V$
Reduction: $[Fe^{3+}_{(aq)} + e^{-} \to Fe^{2+}_{(aq)}] \times 2; E^{\circ} = +0.77 \ V$
Overall: $E^{\circ}_{cell} = +0.77 - 0.34 = +0.43 \ V$. Since $E^{\circ}_{cell} > 0$,the reaction is feasible.
$(d)$ The possible reaction between $Ag_{(s)} + Fe^{3+}_{(aq)}$ is $Ag_{(s)} + Fe^{3+}_{(aq)} \to Ag^{+}_{(aq)} + Fe^{2+}_{(aq)}$.
Oxidation: $Ag_{(s)} \to Ag^{+}_{(aq)} + e^{-}; E^{\circ} = -0.80 \ V$
Reduction: $Fe^{3+}_{(aq)} + e^{-} \to Fe^{2+}_{(aq)}; E^{\circ} = +0.77 \ V$
Overall: $E^{\circ}_{cell} = +0.77 - 0.80 = -0.03 \ V$. Since $E^{\circ}_{cell} < 0$,the reaction is not feasible.
$(e)$ The possible reaction between $Br_{2(aq)} + Fe^{2+}_{(aq)}$ is $Br_{2(aq)} + 2Fe^{2+}_{(aq)} \to 2Br^{-}_{(aq)} + 2Fe^{3+}_{(aq)}$.
Oxidation: $[Fe^{2+}_{(aq)} \to Fe^{3+}_{(aq)} + e^{-}] \times 2; E^{\circ} = -0.77 \ V$
Reduction: $Br_{2(aq)} + 2e^{-} \to 2Br^{-}_{(aq)}; E^{\circ} = +1.09 \ V$
Overall: $E^{\circ}_{cell} = +1.09 - 0.77 = +0.32 \ V$. Since $E^{\circ}_{cell} > 0$,the reaction is feasible.