Chapter 17, Problem 34QRT

In principle, a battery could be made from aluminum metal and chlorine gas.

1. (a) Write a balanced equation for the reaction that would occur in a battery using Al³⁺(aq) | Al(s) and Cl₂(g) | Cl⁻(aq) half-cells.
2. (b) Identify the half-reaction at the anode and at the cathode. Do electrons flow from the Al electrode when the cell does work? Explain.
3. (c) Calculate the standard potential, $E_{\text{cell}}^{°}$, for the battery.