A student measures the potential of a cell made up with 1 M CuSO, in one
solution reservoir and 1 M \(\mathrm{ZnSO}_{4}\) in the other. There is a
metallic copper \(\left(\mathrm{Cu}^{0}\right)\) electrode in the
\(\mathrm{CuSO}_{4}\) and a metallic zinc (Zn \(^{0}\) ) electrode in the ZnSO_,
and the cell is set up as shown in Figure \(32.1 .\) She finds that the
potential, or voltage, of the cell, \(E_{\text {call }}^{0}\) is \(1.076
\mathrm{V}\), and that the Zn electrode is negative.
a. At which electrode is oxidation occurring? _____
b. Write the equation for the oxidation half-reaction in this cell.
c. Write the equation for the reduction half-reaction in this cell.
d. Write the net ionic equation for the spontaneous oxidation-reduction
reaction that occurs in this cell.
