Question

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

Ag_(s) and \[\ce{Fe^{3+}_{ (aq)}}\]

Using the standard electrode potentials, predict the reaction, if any, that occurs between the following:

Ag_(s) and \[\ce{Fe^{3+}_{ (aq)}}\]

Answer 1

The reaction is:

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

The corresponding cell is:

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

∴ \[\ce{E^{\circ}_{cell} = E^{\circ}_{Fe^{3+}/Fe^{2+}} - E^{\circ}_{Ag^+/Ag}}\]

= 0.77 − (+0.80)

= −0.03 V

Since \[\ce{E{^{\circ}_{cell}}}\] is negative, the reaction is not feasible.