---
title: "At \\(300 \\text{ K}\\), a chemical reaction has a standard Gibbs free energy change of \\(\\Delta G^\\circ = -10.0 \\text{ kJ/mol}\\). At this temperature, the product \\(RT\\) is equal to \\(2.5 \\text{ kJ/mol}\\). Which of the following expressions is equal to the standard equilibrium constant, \\(K\\), for the reaction at \\(300 \\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/119326/"
date_modified: "2026-08-19T12:39:49+00:00"
---

# At \(300 \text{ K}\), a chemical reaction has a standard Gibbs free energy change of \(\Delta G^\circ = -10.0 \text{ kJ/mol}\). At this temperature, the product \(RT\) is equal to \(2.5 \text{ kJ/mol}\). Which of the following expressions is equal to the standard equilibrium constant, \(K\), for the reaction at \(300 \text{ K}\)?

At \(300 \text{ K}\), a chemical reaction has a standard Gibbs free energy change of \(\Delta G^\circ = -10.0 \text{ kJ/mol}\). At this temperature, the product \(RT\) is equal to \(2.5 \text{ kJ/mol}\). Which of the following expressions is equal to the standard equilibrium constant, \(K\), for the reaction at \(300 \text{ K}\)?

- **A.** \(e^{-4}\)
- **B.** \(e^{0.25}\)
- **C.** \(e^{4}\)
- **D.** \(e^{10}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119326/*