Cathode = Cu2(s) + 2e- �¨ Cu(s)

Anode = 2H2O(l) �¨ O2(g) + 4H(g) + 4e-
Net = Cu2(s) + 2H2O(l) �¨ Cu(s) + O2(g) + 4H(g)
the minimum voltage that must be supplied to electrolyze aqueous copper(II) sulfate

To calculate the minimum voltage required to electrolyze aqueous copper(II) sulfate, we need to consider the standard reduction potentials of the half-reactions at the cathode and anode.

The given half-reactions are:
Cathode: Cu2+(s) + 2e- → Cu(s)
Anode: 2H2O(l) → O2(g) + 4H+(aq) + 4e-

The standard reduction potential for the cathode half-reaction can be found using a table of standard reduction potentials. The standard reduction potential for the reduction of Cu2+ to Cu is +0.34V.

However, since the half-reaction for the anode is not given, we will assume the reaction occurs at the standard hydrogen electrode (SHE) with a standard reduction potential of 0V. This is because the half-reaction for the anode involves the reduction of water, which can vary depending on the conditions.

To determine the overall cell potential (Ecell), we need to subtract the standard reduction potential of the anode half-reaction from the cathode half-reaction.

Ecell = Ecathode - Eanode
Ecell = +0.34V - 0V
Ecell = +0.34V

The minimum voltage required to electrolyze aqueous copper(II) sulfate is +0.34V.