Which of the following correctly describe an exergonic reaction? Select True or False for each statement. T/F The products have lower Gibbs free energy than the reactants. T/F Activation energy is required for the reaction to proceed. T/F The products always have lower entropy than the reactants. T/F The reaction always occurs quickly.

An exergonic reaction is a chemical process that releases energy, typically in the form of Gibbs free energy. In these reactions, the products have lower Gibbs free energy than the reactants, indicating that the reaction can occur spontaneously. This concept is crucial for understanding thermodynamics in biochemical processes.

Gibbs free energy (G) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. A negative change in Gibbs free energy (ΔG < 0) indicates that a reaction is exergonic and can occur spontaneously, while a positive change (ΔG > 0) suggests that the reaction is non-spontaneous.

Activation energy is the minimum energy required for a chemical reaction to occur. Even in exergonic reactions, activation energy is necessary to initiate the reaction, as it helps to overcome the energy barrier for the reactants to transform into products. This concept highlights that not all spontaneous reactions occur rapidly; they may still require a significant energy input to start.