Consider the figure below which shows ΔG° for a chemical process plotted against absolute temperature. Which one of the following is an incorrect conclusion, based on the information in the diagram?

Question

Quizplus · Accepted Answer

The graph shows that as temperature increases, ΔG° becomes more negative, indicating that the reaction becomes more spontaneous. This means that ΔH° must be positive (A is incorrect) and ΔS° must be positive (B is incorrect), since both factors contribute to a more positive ΔG° at low temperatures. Therefore, based on the graph, we can conclude that the reaction becomes more spontaneous at high temperatures (C is correct). Additionally, we can see that ΔS° increases with temperature while ΔH° remains constant (D is correct), since the slope of the ΔG° vs temperature plot reflects the change in entropy with temperature, while the intercept reflects the enthalpy change. Lastly, we cannot conclude that there exists a certain temperature at which ΔH° = TΔS°, since this equation would require both ΔH° and ΔS° to be constant with temperature, which is not necessarily the case based on the graph (E is incorrect).

Consider the Figure Below Which Shows ΔG° for a Chemical