---
title: "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?"
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url: "https://nerd-notes.com/ubq/119980/"
date_modified: "2026-08-21T08:31:26+00:00"
---

# 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?

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?

- **A.** \(\text{Zn(s)}\) will oxidize preferentially because \(\text{Zn}^{2+}\text{(aq)}\) has a more negative standard reduction potential than \(\text{Fe}^{2+}\text{(aq)}\), meaning \(\text{Zn(s)}\) is more easily oxidized than \(\text{Fe(s)}\).
- **B.** \(\text{Zn(s)}\) will oxidize preferentially because \(\text{Zn(s)}\) has a greater electronegativity than \(\text{Fe(s)}\), causing electrons to transfer spontaneously toward the \(\text{Zn(s)}\) electrode.
- **C.** \(\text{Fe(s)}\) will oxidize preferentially because \(\text{Fe}^{2+}\text{(aq)}\) has a less negative standard reduction potential than \(\text{Zn}^{2+}\text{(aq)}\), indicating that \(\text{Fe(s)}\) is more thermodynamically favorable to oxidize.
- **D.** \(\text{Fe(s)}\) will oxidize preferentially because \(\text{Fe}^{2+}\text{(aq)}\) is a weaker oxidizing agent than \(\text{Zn}^{2+}\text{(aq)}\), causing \(\text{Fe(s)}\) to lose electrons more readily.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119980/*