If the change in entropy for a process is much less than the change in enthalpy, why might the entropy change be the dominant factor in determining the overall free energy of the process?

Question

Quizplus · Accepted Answer

The change in free energy ($\Delta G$) for a process is given by the equation $\Delta G = \Delta H - T\Delta S$, where $\Delta H$ is the change in enthalpy, $T$ is the temperature in Kelvin, and $\Delta S$ is the change in entropy. At around 300 K (approximately room temperature or human body temperature), even a small change in entropy ($\Delta S$) can significantly impact the $\Delta G$ value due to the multiplication by the temperature term. This makes the entropy change a dominant factor in determining the overall free energy of the process, especially in biochemical reactions that typically occur around this temperature.

If the Change in Entropy for a Process Is Much