What does equilibrium in a chemical reaction mean?

Equilibrium in a chemical reaction signifies a dynamic balance between the forward and reverse reactions, where the rates of both processes are equal. At this state, the concentration of reactants and products remains constant over time, even though both reactions continue to occur. This does not imply that the reactants have been completely converted to products, nor does it suggest that the reaction has ceased.

In a state of equilibrium, the concentrations of both reactants and products are stable, which results in no net change in the system. This balance allows for the possibility of changes in concentration due to external factors such as temperature or pressure, but as long as these conditions remain constant, the system will maintain equilibrium.

Understanding this concept is crucial for predicting how changes in reaction conditions will affect the concentrations of reactants and products in chemical systems, which plays a significant role in industrial processes, chemical manufacturing, and various applications in chemistry.