---
title: "The dissolution of potassium chloride, \\(\\text{KCl}(s)\\), in water is represented by the equation below.  \\[\\text{KCl}(s) \\rightarrow \\text{K}^+(aq) + \\text{Cl}^-(aq)\\]  For this process at \\(300\\text{ K}\\), the standard enthalpy change, \\(\\Delta H^\\circ\\), is \\(+17.0\\text{ kJ/mol}_{\\text{rxn}}\\) and the standard entropy change, \\(\\Delta S^\\circ\\), is \\(+70.0\\text{ J/(mol}_{\\text{rxn}}\\cdot\\text{K)}\\). Based on these data, what is the standard Gibbs free energy change, \\(\\Delta G^\\circ\\), for the dissolution of \\(\\text{KCl}(s)\\) at \\(300\\text{ K}\\)?"
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url: "https://nerd-notes.com/ubq/119966/"
date_modified: "2026-08-21T08:31:15+00:00"
---

# The dissolution of potassium chloride, \(\text{KCl}(s)\), in water is represented by the equation below.

\[\text{KCl}(s) \rightarrow \text{K}^+(aq) + \text{Cl}^-(aq)\]

For this process at \(300\text{ K}\), the standard enthalpy change, \(\Delta H^\circ\), is \(+17.0\text{ kJ/mol}_{\text{rxn}}\) and the standard entropy change, \(\Delta S^\circ\), is \(+70.0\text{ J/(mol}_{\text{rxn}}\cdot\text{K)}\). Based on these data, what is the standard Gibbs free energy change, \(\Delta G^\circ\), for the dissolution of \(\text{KCl}(s)\) at \(300\text{ K}\)?

The dissolution of potassium chloride, \(\text{KCl}(s)\), in water is represented by the equation below.

\[\text{KCl}(s) \rightarrow \text{K}^+(aq) + \text{Cl}^-(aq)\]

For this process at \(300\text{ K}\), the standard enthalpy change, \(\Delta H^\circ\), is \(+17.0\text{ kJ/mol}_{\text{rxn}}\) and the standard entropy change, \(\Delta S^\circ\), is \(+70.0\text{ J/(mol}_{\text{rxn}}\cdot\text{K)}\). Based on these data, what is the standard Gibbs free energy change, \(\Delta G^\circ\), for the dissolution of \(\text{KCl}(s)\) at \(300\text{ K}\)?

- **A.** \(-38.0\text{ kJ/mol}_{\text{rxn}}\)
- **B.** \(-4.0\text{ kJ/mol}_{\text{rxn}}\)
- **C.** \(+4.0\text{ kJ/mol}_{\text{rxn}}\)
- **D.** \(+38.0\text{ kJ/mol}_{\text{rxn}}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119966/*