A simple galvanic cell uses zinc and copper electrodes with a zinc sulfate solution. If the cell is connected to a circuit and the zinc electrode dissolves while the copper electrode grows metal, what does this indicate about the direction of electron flow and the nature of the reactions at each electrode?

The electrons flow from the zinc electrode to the copper electrode through the external circuit. At the zinc electrode the oxidation reaction Zn → Zn²⁺ + 2e⁻ occurs, consuming zinc metal. At the copper electrode the reduction reaction Cu²⁺ + 2e⁻ → Cu occurs, depositing copper metal. This shows that the zinc electrode is the anode (oxidation) and the copper electrode is the cathode (reduction).

The answer shows application of knowledge about electrode roles, electron flow, and the reversible nature of reactions in rechargeable cells, testing the ability to explain the process in a specific example.