In an exergonic reaction, how does the internal energy of products compare to that of the reactants?

In an exergonic reaction, the internal energy of the products is lower than that of the reactants. This is a fundamental aspect of exergonic reactions, which are characterized by a release of energy as the reaction progresses.

The term "exergonic" comes from the combination of Greek roots meaning "energy out." In these reactions, the system releases energy to the surroundings, often resulting in work being done or heat being emitted. As a result, the products are at a lower energy state compared to the reactants because the energy that was stored in the bonds of the reactants has been released during the conversion to products.

This energy difference can have significant implications for the spontaneity of the reaction; exergonic reactions tend to occur without needing an external input of energy, as they move towards a state of lower energy and greater stability. Understanding the relationship between the energy levels of reactants and products in exergonic reactions is crucial for grasping key biological processes, including cellular respiration and metabolic pathways.