During a chemical reaction, what is the relationship between reactants and products in terms of energy in an exothermic reaction?

In an exothermic reaction, the overall energy change results in the release of energy to the surroundings, often in the form of heat. This means that the energy contained in the products is lower than the energy present in the reactants. The reactants start with a certain amount of energy, and as the reaction occurs, some of this energy is transformed into another form, typically released as heat or light, leading to stability in the products formed.

Since the products have less energy than the reactants, this energy difference is what drives the reaction forward and is a fundamental characteristic of exothermic processes. Thus, concluding that products have less energy than reactants correctly reflects the energy dynamics of exothermic reactions.