Which of the following statements regarding energy is FALSE? Energy is defined as the capacity to do work, or to put matter into motion
The products of exergonic reactions contain more potential energy than the reactants that form them
Increasing the temperature of atoms and molecules increases their kinetic energy
Exchange reactions allow chemical energy from one molecule to be transferred to another

The correct answer is The products of exergonic reactions contain more potential energy than the reactants that form them.

Explanation:

It is considered false since the products in exothermic reactions have less energy than their reactants, since being exothermic they release energy in the form of heat to the environment that surrounds them.

An exothermic reaction gives energy to the environment that surrounds it at the end of the reaction, that is why the energy of the reactants will ALWAYS be greater than the final energy of the products, since as the reaction occurs, it loses energy and do not win.

The disorder and entropy in these reactions increases, complete combustion would be a clear example of exothermic reactions and their release of energy in the form of heat.

Exothermic reactions can be reversible or irreversible like all reactions.