What does the term "chemical equilibrium" refer to in chemical reactions?

The term "chemical equilibrium" refers to a specific condition in a chemical reaction where the rates of the forward and reverse reactions are equal. At this point, the concentrations of reactants and products remain constant over time, even though the reactions continue to occur in both directions. This dynamic balance allows the system to maintain a stable state while still undergoing continuous chemical processes.

This is important because it emphasizes that, contrary to a common misunderstanding, equilibrium does not mean that the reactions have stopped; rather, the rates of the two opposing reactions have reached a balance. Therefore, while reactants and products may still be present in the reaction mixture, their concentrations do not change, allowing for a state of chemical equilibrium to be established. This principle is foundational in the study of chemical reactions and is critical for understanding concepts related to reaction dynamics and the effects of changing conditions on a system at equilibrium.