What does "reaction equilibrium" mean in a chemical context?

In a chemical context, "reaction equilibrium" refers to a dynamic state in which the rates of the forward and reverse reactions are equal. This does not mean that the reactions have stopped; rather, it indicates that the concentration of reactants and products remains constant over time because the formation of products and the conversion of products back into reactants occur at the same rate.

At equilibrium, both the forward reaction (where reactants are transformed into products) and the reverse reaction (where products are converted back into reactants) are happening simultaneously and continuously. As a result, the system is in a state of balance, and the concentrations of all species involved in the reaction do not change, even though the reactions themselves continue to occur. This concept is essential for understanding how chemical reactions behave under different conditions and how they can shift in response to changes in concentration, pressure, or temperature, adhering to Le Chatelier's Principle.