What factors influence a negative Delta G?

A negative Delta G indicates that a reaction or process is spontaneous at constant temperature and pressure. The factors that influence Delta G are related to the changes in enthalpy (ΔH), entropy (ΔS), and temperature (T) as expressed in the Gibbs free energy equation:

ΔG = ΔH - TΔS.

When considering the equation, both the enthalpy and entropy changes are essential in determining the sign of Delta G. A negative Delta G can occur if:

1. There is a decrease in enthalpy (negative ΔH), indicating that the reaction releases energy (exothermic).

2. There is an increase in entropy (positive ΔS), suggesting greater randomness or disorder in the system.

Temperature plays a crucial role because it acts as a scaling factor for the entropy term. If the temperature is high enough, the TΔS term can outweigh the ΔH term, leading to a negative Delta G even in cases where enthalpy is positive. Thus, the combination of enthalpy and entropy changes, along with temperature, is what primarily influences the sign of Delta G.

This understanding highlights that the interplay of temperature, enthalpy, and entropy changes can lead to spontaneity in reactions, making