In an exergonic reaction, what relationship can be indicated between reactants and products?

In an exergonic reaction, the defining characteristic is that energy is released during the reaction process. This release of energy is indicative of the relationship between the reactants and the products. In these reactions, the reactants possess more free energy compared to the products.

This means that as the reaction progresses, the energy stored in the chemical bonds of the reactants is transformed into products that have lower energy states. This energy difference is what allows the reaction to occur spontaneously. The concept of free energy is crucial here, with the Gibbs free energy being a primary concern in determining whether a reaction is exergonic or endergonic. In the case of exergonic reactions, the change in free energy (ΔG) is negative, reaffirming that the products are at a lower energy level than the starting materials.

This principle helps in understanding various biological processes, such as cellular respiration, where the breakdown of glucose releases energy that can be harnessed for cellular activities.