---
title: "A student plots the standard Gibbs free energy change, \\(\\Delta G^\\circ\\), as a function of temperature, \\(T\\), for a chemical reaction, as shown in the graph below. Based on the graph, which of the following claims about the reaction is correct?"
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url: "https://nerd-notes.com/ubq/119330/"
date_modified: "2026-08-19T12:39:50+00:00"
---

# A student plots the standard Gibbs free energy change, \(\Delta G^\circ\), as a function of temperature, \(T\), for a chemical reaction, as shown in the graph below. Based on the graph, which of the following claims about the reaction is correct?

A student plots the standard Gibbs free energy change, \(\Delta G^\circ\), as a function of temperature, \(T\), for a chemical reaction, as shown in the graph below. Based on the graph, which of the following claims about the reaction is correct?

![A line graph plotting standard Gibbs free energy change, \(\Delta G^\circ\text{ (kJ/mol)}\), on the vertical y-axis versus absolute temperature, \(T\text{ (K)}\), on the horizontal x-axis. The y-axis ranges from \(-60\) to \(+60\) with major gridlines and tick marks at \(-60\), \(-30\), \(0\), \(30\), and \(60\). The x-axis ranges from \(0\) to \(600\) with major gridlines and tick marks at \(0\), \(100\), \(200\), \(300\), \(400\), \(500\), and \(600\). A single straight solid black trendline begins at \((0, 60)\), passes through \((300, 0)\), and ends at \((600, -60)\). No other text or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-graph-1-1787143190-uVi7KQ.jpg)

- **A.** The reaction is endothermic (\(\Delta H^\circ > 0\)) and becomes thermodynamically favorable at temperatures above \(300 \text{ K}\) because \(\Delta S^\circ < 0\).
- **B.** The reaction is exothermic (\(\Delta H^\circ < 0\)) and is thermodynamically favorable at all temperatures below \(300 \text{ K}\) because \(\Delta S^\circ > 0\).
- **C.** The reaction is endothermic (\(\Delta H^\circ > 0\)) and becomes thermodynamically favorable at temperatures above \(300 \text{ K}\) because \(T\Delta S^\circ\) exceeds \(\Delta H^\circ\).
- **D.** The reaction is exothermic (\(\Delta H^\circ < 0\)) and becomes thermodynamically unfavorable at temperatures above \(300 \text{ K}\) because \(T\Delta S^\circ\) exceeds \(\Delta H^\circ\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119330/*