Final answer:
Once equilibrium is reached for a catalyzed reaction, the rates of reaction for both the forward and reverse directions will be equal, signifying a dynamic equilibrium where the concentrations of reactants and products remain constant.
Step-by-step explanation:
Once equilibrium is reached for a catalyzed reaction, the rates of reaction for both directions will be equal. Equilibrium is achieved when the rate of the forward reaction and the rate of the reverse reaction become identical in magnitude, and as a result, the concentrations of the reactants and products remain constant over time; this is known as a dynamic equilibrium. It is important to understand that even though the concentrations remain constant, the reactions haven’t stopped. They continue to occur in both directions at the same rate.
The equilibrium constant, often represented with the symbol K, is derived from the rate constants of the forward and reverse reactions (k(ƒ) and k(r), respectively). K is equal to k(ƒ) divided by k(r). The constant nature of K indicates that the ratio of the concentration of products to the concentration of reactants remains the same at equilibrium.
A dynamic equilibrium can be visualized by an equation with a double arrow, indicating that the reaction progresses in both the forward and reverse directions at the same rate. Understanding the concept of equilibrium is vital in the study of chemical reactions, especially when predicting the concentration of reactants and products, and analyzing how systems respond to changes in conditions according to Le Châtelier's principle.