Use the table of standard reduction potentials in your textbook to complete the following table. An example is provided:
Electrodes | Half-reactions | E red (V)
-------------|------------------|----------
Zn(s) | Zn2+(aq) | -0.76
Cu(s) | Cu2+(aq) | +0.34
Cu(s) | Cu+(aq) | +0.34
Cu(s) | Ni2+(aq) | +0.57
Pb(s) | Pb2+(aq) | -0.13
Pb(s) | Ag+(aq) | -0.13