---
title: "A galvanic cell operates according to the following balanced equation at \\(298\\text{ K}\\):  \\[\\text{X(s)} + 2\\text{Y}^+\\text{(aq)} \\rightarrow \\text{X}^{2+}\\text{(aq)} + 2\\text{Y(s)}\\]  The standard reduction potentials for the two half-reactions are given in the table below.  | Half-reaction | \\(E^\\circ\\text{ (V)}\\) | |—|—| | \\(\\text{Y}^+\\text{(aq)} + e^- \\rightarrow \\text{Y(s)}\\) | \\(+0.80\\) | | \\(\\text{X}^{2+}\\text{(aq)} + 2e^- \\rightarrow \\text{X(s)}\\) | \\(+0.30\\) |  Based on the information above and Faraday’s constant (\\(F = 96{,}500\\text{ J}/(\\text{V}\\cdot\\text{mol } e^-)\\)), what is the value of the standard Gibbs free energy change, \\(\\Delta G^\\circ\\), for the overall cell reaction at \\(298\\text{ K}\\)?"
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url: "https://nerd-notes.com/ubq/120360/"
date_modified: "2026-08-23T04:23:24+00:00"
---

# A galvanic cell operates according to the following balanced equation at \(298\text{ K}\):

\[\text{X(s)} + 2\text{Y}^+\text{(aq)} \rightarrow \text{X}^{2+}\text{(aq)} + 2\text{Y(s)}\]

The standard reduction potentials for the two half-reactions are given in the table below.

| Half-reaction | \(E^\circ\text{ (V)}\) |
|—|—|
| \(\text{Y}^+\text{(aq)} + e^- \rightarrow \text{Y(s)}\) | \(+0.80\) |
| \(\text{X}^{2+}\text{(aq)} + 2e^- \rightarrow \text{X(s)}\) | \(+0.30\) |

Based on the information above and Faraday’s constant (\(F = 96{,}500\text{ J}/(\text{V}\cdot\text{mol } e^-)\)), what is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the overall cell reaction at \(298\text{ K}\)?

A galvanic cell operates according to the following balanced equation at \(298\text{ K}\):

\[\text{X(s)} + 2\text{Y}^+\text{(aq)} \rightarrow \text{X}^{2+}\text{(aq)} + 2\text{Y(s)}\]

The standard reduction potentials for the two half-reactions are given in the table below.

| Half-reaction | \(E^\circ\text{ (V)}\) |
|---|---|
| \(\text{Y}^+\text{(aq)} + e^- \rightarrow \text{Y(s)}\) | \(+0.80\) |
| \(\text{X}^{2+}\text{(aq)} + 2e^- \rightarrow \text{X(s)}\) | \(+0.30\) |

Based on the information above and Faraday's constant (\(F = 96{,}500\text{ J}/(\text{V}\cdot\text{mol } e^-)\)), what is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the overall cell reaction at \(298\text{ K}\)?

- **A.** \(-96.5\text{ kJ/mol}_{\text{rxn}}\
- **B.** \(-48.3\text{ kJ/mol}_{\text{rxn}}\
- **C.** \(+48.3\text{ kJ/mol}_{\text{rxn}}\
- **D.** \(+96.5\text{ kJ/mol}_{\text{rxn}}\

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120360/*