Question

The following electrochemical cell is set up at 298 K:

\[\ce{Zn | Zn^{2+}_{ (aq)} (1 M) || Cu^{2+}_{ (aq)} (1 M) | Cu}\]

Given: \[\ce{E^{\circ}_{Zn^{2+}/Zn}}\] = −0.761 V, \[\ce{E^{\circ}_{Cu^{2+}/Cu}}\] = +0.339 V

Write the cell reaction.

Answer 1

\[\ce{Zn | Zn^{2+}_{ (aq)} (1 M) || Cu^{2+}_{ (aq)} (1 M) | Cu}\]

\[\ce{E^{\circ}_{Zn^{2+}/Zn}}\] = −0.761 V,

\[\ce{E^{\circ}_{Cu^{2+}/Cu}}\] = +0.339 V

Anode: Since zinc has a more negative standard reduction potential, it undergoes oxidation. 

Cathode: Copper has a more positive standard reduction potential it undergoes reduction.

Cell reaction: \[\ce{Zn_{(s)} + Cu^{2+}_{ (aq)} −> Zn^{2+}_{ (aq)} + Cu_{(s)}}\]