Final answer:
Delta G increases with increasing Delta H (bond energy) and decreases with increasing entropy.
Step-by-step explanation:
The statement is true. Delta G, or Gibbs free energy, is a measure of the spontaneity of a reaction. It is affected by both the change in enthalpy (Delta H) and the change in entropy.
When Delta H (bond energy) increases, it means that more energy is required to break the bonds in the reactants, resulting in a higher energy barrier for the reaction. This leads to a higher Delta G, indicating that the reaction is less spontaneous.
On the other hand, when entropy increases, meaning that there is a greater dispersal of energy and more disorder, the overall Delta G decreases. This is because spontaneous reactions tend to involve an increase in entropy.