Consider the figure that shows ΔG° for a chemical process plotted against absolute temperature. From this plot, it is reasonable to conclude that

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From the plot, we can see that the ΔG° values increase as temperature increases. This means that the reaction becomes less favorable (less negative ΔG°) at higher temperatures. For spontaneous reactions, ΔG° must be negative, so the ΔH° term (enthalpy change) must be negative to counterbalance the positive ΔS° term (entropy change) at high temperatures. Since the slope of the graph is positive, we know that ΔS° is positive. Therefore, the only choice that fits these criteria is B, where ΔH° is positive and ΔS° is negative, since a positive ΔH° will make the reaction less favorable at high temperatures.

Consider the Figure That Shows ΔG° for a Chemical Process