---
title: "A student investigates the thermodynamic properties of a reaction between two gases at \\(298\\text{ K}\\), represented by the balanced equation below.  \\[ \\text{X(g)} + \\text{Y(g)} \\rightleftharpoons \\text{XY(g)} \\]  The reaction has a standard enthalpy change, \\(\\Delta H^\\circ\\), of \\(-10.0\\text{ kJ/mol}_{\\text{rxn}}\\) and a standard entropy change, \\(\\Delta S^\\circ\\), of \\(-110.0\\text{ J}/(\\text{mol}_{\\text{rxn}}\\cdot\\text{K})\\). Given that \\(2.303 RT \\approx 5.70\\text{ kJ/mol}\\) at \\(298\\text{ K}\\) and \\(\\Delta G^\\circ = -2.303 RT \\log_{10} K\\), what is the value of the equilibrium constant, \\(K\\), for the reaction at \\(298\\text{ K}\\)?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/121529/"
date_modified: "2026-08-23T05:05:05+00:00"
---

# A student investigates the thermodynamic properties of a reaction between two gases at \(298\text{ K}\), represented by the balanced equation below.

\[
\text{X(g)} + \text{Y(g)} \rightleftharpoons \text{XY(g)}
\]

The reaction has a standard enthalpy change, \(\Delta H^\circ\), of \(-10.0\text{ kJ/mol}_{\text{rxn}}\) and a standard entropy change, \(\Delta S^\circ\), of \(-110.0\text{ J}/(\text{mol}_{\text{rxn}}\cdot\text{K})\). Given that \(2.303 RT \approx 5.70\text{ kJ/mol}\) at \(298\text{ K}\) and \(\Delta G^\circ = -2.303 RT \log_{10} K\), what is the value of the equilibrium constant, \(K\), for the reaction at \(298\text{ K}\)?

A student investigates the thermodynamic properties of a reaction between two gases at \(298\text{ K}\), represented by the balanced equation below.

\[
\text{X(g)} + \text{Y(g)} \rightleftharpoons \text{XY(g)}
\]

The reaction has a standard enthalpy change, \(\Delta H^\circ\), of \(-10.0\text{ kJ/mol}_{\text{rxn}}\) and a standard entropy change, \(\Delta S^\circ\), of \(-110.0\text{ J}/(\text{mol}_{\text{rxn}}\cdot\text{K})\). Given that \(2.303 RT \approx 5.70\text{ kJ/mol}\) at \(298\text{ K}\) and \(\Delta G^\circ = -2.303 RT \log_{10} K\), what is the value of the equilibrium constant, \(K\), for the reaction at \(298\text{ K}\)?

- **A.** \(1.0 \times 10^{-4}\)
- **B.** \(1.8 \times 10^{-2}\)
- **C.** \(1.0 \times 10^{2}\)
- **D.** \(1.0 \times 10^{4}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121529/*