A student measures the potential of a cell made up with \(1.0 \mathrm{M}\) CuSO,
in one solution reservoir and 1.0 \(\mathrm{M} \mathrm{Ag}_{2} \mathrm{SO}_{4}\)
in the other. There is a metallic copper (Cu) electrode in the CuSO, and a
metallic silver (Ag) electrode in the \(A g_{2} S O_{4}\), 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 \(0.45 \mathrm{V}\), and that the copper
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.
