A student constructed two standard electrochemical cells using Pb2+(aq) and
Ni2+(aq). In both cells a Pb(s) electrode was placed in the Pb2+(aq) solution.
In the first cell a Ni(s) electrode was placed in the Ni2+(aq) solution. In the
second cell an inert C(s) electrode was placed in the Ni2+(aq) solution instead
of the Ni(s) electrode.
Which of the following statements describes what occurs in each cell?
In the first cell, the Pb(s) electrode will act as the anode and undergo oxidation, releasing electrons. The Ni2+(aq) solution will act as the cathode and undergo reduction, accepting electrons. This results in the generation of an electrical current.
In the second cell, since an inert C(s) electrode is placed in the Ni2+(aq) solution instead of the Ni(s) electrode, there will be no redox reaction occurring at this electrode. As a result, there will be no generation of an electrical current. The Pb(s) electrode in the Pb2+(aq) solution will still undergo oxidation, but without a corresponding reduction reaction at the carbon electrode, no electrical current will be produced.