Answer:

Approximately under standard conditions.

Explanation:

Equation for the overall reaction:

.

Write down the ionic equation for this reaction:

.

The net ionic equation for this reaction would be:

.

In this reaction:

• Zinc loses electrons and was oxidized (at the anode): .
• Copper gains electrons and was reduced (at the cathode): .

Look up the standard potentials for each half-reaction on a table of standard reduction potentials.

Notice that is oxidation and is likely not on the table of standard reduction potentials. However, the reverse reaction, , is reduction and is likely on the table.

• for , and
• for .

The reduction potential of would be , the opposite of the reverse reaction .

The standard potential of the overall reaction would be the sum of the standard potentials of the two half-reactions:

.