Explain that galvanic cells can be represented as cell diagrams, including anode and cathode half-equations.

A galvanic cell is constructed using a zinc electrode in \(1.0 \, \text{mol L}^{-1}\) zinc sulfate solution and a copper electrode in \(1.0 \, \text{mol L}^{-1}\) copper(II) sulfate solution. The cell is represented by the following cell diagram: \(\text{Zn(s)} \mid \text{Zn}^{2+}(\text{aq}) \parallel \text{Cu}^{2+}(\text{aq}) \mid \text{Cu(s)}\) Explain how the cell diagram represents the oxidation and reduction processes occurring at each electrode.