---
title: "At \\(300\\text{ K}\\), the reaction represented below has a standard Gibbs free energy change of \\(\\Delta G^\\circ = -11.5\\text{ kJ/mol}\\). \\[ 2\\,\\text{NO}_2(g) \\rightleftharpoons \\text{N}_2\\text{O}_4(g) \\] Given that \\(R = 8.3\\text{ J}/(\\text{mol}\\cdot\\text{K})\\) and \\(\\ln(10) \\approx 2.30\\), which of the following is closest to the value of the equilibrium constant, \\(K\\), at \\(300\\text{ K}\\)?"
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url: "https://nerd-notes.com/ubq/119805/"
date_modified: "2026-08-21T08:12:24+00:00"
---

# At \(300\text{ K}\), the reaction represented below has a standard Gibbs free energy change of \(\Delta G^\circ = -11.5\text{ kJ/mol}\). \[ 2\,\text{NO}_2(g) \rightleftharpoons \text{N}_2\text{O}_4(g) \] Given that \(R = 8.3\text{ J}/(\text{mol}\cdot\text{K})\) and \(\ln(10) \approx 2.30\), which of the following is closest to the value of the equilibrium constant, \(K\), at \(300\text{ K}\)?

At \(300\text{ K}\), the reaction represented below has a standard Gibbs free energy change of \(\Delta G^\circ = -11.5\text{ kJ/mol}\). \[ 2\,\text{NO}_2(g) \rightleftharpoons \text{N}_2\text{O}_4(g) \] Given that \(R = 8.3\text{ J}/(\text{mol}\cdot\text{K})\) and \(\ln(10) \approx 2.30\), which of the following is closest to the value of the equilibrium constant, \(K\), at \(300\text{ K}\)?

- **A.** \(1.0 \times 10^{-2}\)
- **B.** \(2.0\)
- **C.** \(4.6\)
- **D.** \(1.0 \times 10^2\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119805/*