This statement is False.
While it is true that an increase in entropy (disorder) is a common characteristic of exergonic reactions, it does not necessarily mean that every reaction in which entropy increases is exergonic. Exergonic reactions are defined as those that proceed with a net release of free energy, typically leading to a spontaneous process. The Gibbs free energy change (ΔG) is the key factor here, where a negative ΔG indicates that a reaction is exergonic.
Entropy is only one part of the equation. The full relationship is captured by the Gibbs free energy equation:
ΔG = ΔH – TΔS
In this equation, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. Even if ΔS is positive (entropy increases), if the enthalpy change (ΔH) is also positive and large enough, it can lead to a positive ΔG, meaning the reaction would not be spontaneous or exergonic.
In conclusion, while increasing entropy can favor the spontaneity of a reaction, it does not guarantee that the reaction is exergonic without considering the enthalpy changes involved.