---
title: "A student constructs a galvanic cell at \\(298\\text{ K}\\) based on the reaction represented below.  \\[ \\text{Mg}(s) + \\text{Fe}^{2+}(aq) \\rightarrow \\text{Mg}^{2+}(aq) + \\text{Fe}(s) \\quad E^\\circ_{\\text{cell}} = +1.93\\text{ V} \\]  The initial concentration of \\(\\text{Fe}^{2+}(aq)\\) in the cathode compartment is \\(1.0\\text{ M}\\), and the initial concentration of \\(\\text{Mg}^{2+}(aq)\\) in the anode compartment is \\(0.010\\text{ M}\\). Which of the following correctly compares the initial cell potential, \\(E_{\\text{cell}}\\), to the standard cell potential, \\(E^\\circ_{\\text{cell}}\\), and provides the valid justification?"
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url: "https://nerd-notes.com/ubq/120341/"
date_modified: "2026-08-23T04:23:14+00:00"
---

# A student constructs a galvanic cell at \(298\text{ K}\) based on the reaction represented below.

\[ \text{Mg}(s) + \text{Fe}^{2+}(aq) \rightarrow \text{Mg}^{2+}(aq) + \text{Fe}(s) \quad E^\circ_{\text{cell}} = +1.93\text{ V} \]

The initial concentration of \(\text{Fe}^{2+}(aq)\) in the cathode compartment is \(1.0\text{ M}\), and the initial concentration of \(\text{Mg}^{2+}(aq)\) in the anode compartment is \(0.010\text{ M}\). Which of the following correctly compares the initial cell potential, \(E_{\text{cell}}\), to the standard cell potential, \(E^\circ_{\text{cell}}\), and provides the valid justification?

A student constructs a galvanic cell at \(298\text{ K}\) based on the reaction represented below.

\[ \text{Mg}(s) + \text{Fe}^{2+}(aq) \rightarrow \text{Mg}^{2+}(aq) + \text{Fe}(s) \quad E^\circ_{\text{cell}} = +1.93\text{ V} \]

The initial concentration of \(\text{Fe}^{2+}(aq)\) in the cathode compartment is \(1.0\text{ M}\), and the initial concentration of \(\text{Mg}^{2+}(aq)\) in the anode compartment is \(0.010\text{ M}\). Which of the following correctly compares the initial cell potential, \(E_{\text{cell}}\), to the standard cell potential, \(E^\circ_{\text{cell}}\), and provides the valid justification?

- **A.** \(E_{\text{cell}} < E^\circ_{\text{cell}}\), because \(Q > 1\), which makes the forward reaction less thermodynamically favored than under standard conditions.
- **B.** \(E_{\text{cell}} < E^\circ_{\text{cell}}\), because the total concentration of dissolved metal ions is less than \(2.0\text{ M}\), which reduces the cell potential.
- **C.** \(E_{\text{cell}} > E^\circ_{\text{cell}}\), because \(Q < 1\), which makes the forward reaction more thermodynamically favored than under standard conditions.
- **D.** \(E_{\text{cell}} > E^\circ_{\text{cell}}\), because the standard reduction potential of \(\text{Mg}^{2+}(aq)\) becomes more negative at lower concentrations.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120341/*