A student investigates methods to protect underground iron structures from corrosion. In an experiment at \(298\text{ K}\), the student connects a strip of \(\text{Fe(s)}\) to a strip of \(\text{Zn(s)}\) with a conductive wire and exposes both metals to an aqueous electrolyte. Standard reduction potentials for relevant half-reactions are shown in the table below.

Half-reaction	\(E^\circ\text{ (V)}\)
\(\text{Zn}^{2+}\text{(aq)} + 2e^- \rightarrow \text{Zn(s)}\)	\(-0.76\)
\(\text{Fe}^{2+}\text{(aq)} + 2e^- \rightarrow \text{Fe(s)}\)	\(-0.44\)
\(\text{Ni}^{2+}\text{(aq)} + 2e^- \rightarrow \text{Ni(s)}\)	\(-0.26\)
\(\text{Cu}^{2+}\text{(aq)} + 2e^- \rightarrow \text{Cu(s)}\)	\(+0.34\)

Which of the following best predicts what will occur when the two connected metals are exposed to the electrolyte, and provides the correct justification?