Why does gibbs free energy decrease with temperature?

For a given reaction, an increase in temperature can result in a change in either the free energy (G) or the entropy (S) change.

Since I am unable to type the Greek letter, I will substitute "d" for it. The equation for the change in free energy is dG = dH - TdS, where H is the enthalpy, S is the entropy, and T is the Kelvin temperature. Since the change in G depends on minus T times the change in S, if the entropy decreases (i.e., dS is negative), then -TdS is positive. As a result, as the temperature rises, the free energy value increases.

In contrast, when entropy increases, dS will be positive and -TdS will become more negative as temperature rises, resulting in a decrease in the free energy's numerical value.

A reaction with a delta G of -2000 kJ yields more free energy than one with a delta G of -1000 kJ, but -1000 is a bigger number than -2000, so you have to be careful with the terminology!

The Gibbs free energy decreases with temperature because the entropy term (TΔS) becomes more dominant, outweighing the enthalpy term (ΔH).