Question

Using the standard electrode potential, predict if the reaction between the following is feasible:

Ag(s) and Fe³⁺ (aq)

Answer 1

The possible reaction between Ag_(s) and \[\ce{Fe^{3+}_{(aq)}}\] is given by,

\[\ce{Ag_{(s)} + 2Fe^{3+}_{ (aq)} -> Ag+_{ (aq)} + Fe^{2+}_{ (aq)}}\]

Oxidation half equation:	\[\ce{Ag_{(s)} -> Ag+_{(aq)} + e-}\]; E° = - 0.80 V
Reduction half equation:	\[\ce{Fe^{3+}_{ (aq)} + De^{3+}_{ (aq)} -> Ag+_{ (aq)} + Fe^{2+}_{ (aq)}}\]; E° = + 0.77 V
	\[\ce{Ag_{(s)} + Fe^{3+}_{ (aq)} -> Ag+_{ (aq)} + Fe^{2+}_{ (aq)}}\]; E° = - 0.03 V

Since E° for the overall reaction is negative, the reaction between Ag_(s) and Fe³⁺_(aq) is not feasible.