Understanding Galvanic Cells
* Galvanic Cells: These are electrochemical cells that generate electricity through spontaneous redox reactions.
* Anode: The electrode where oxidation occurs (loss of electrons).
* Cathode: The electrode where reduction occurs (gain of electrons).
Determining the Anode
1. Identify the More Reactive Metal: Zinc is more reactive than aluminum. This means zinc has a greater tendency to lose electrons and oxidize.
2. Apply the Reactivity Series: The reactivity series of metals helps predict which metal will oxidize (act as the anode). Metals higher in the series are more reactive.
3. Conclusion: Since zinc is more reactive than aluminum, it will be the anode in the galvanic cell.
Reaction Summary
In this galvanic cell:
* Anode (Zinc): Zn(s) → Zn²⁺(aq) + 2e⁻ (Oxidation)
* Cathode (Aluminum): Al³⁺(aq) + 3e⁻ → Al(s) (Reduction)
Key Point: The overall reaction in the cell is the combination of these two half-reactions, with electrons flowing from the zinc anode to the aluminum cathode through an external circuit.
