Question

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

\[\ce{Ag{^{+}_{(aq)}}}\] and Cu_(aq)

Answer 1

The reaction is: 

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

The corresponding cell is:

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

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

= 0.80 − (+ 0.34)

= + 0.46 V

Since \[\ce{E{^{\circ}_{cell}}}\] is positive, the reaction is feasible.