Final answer:
As a reaction approaches equilibrium, the rate of the forward reaction decreases while the rate of the reverse reaction increases, until both rates equalize and the system reaches equilibrium with constant reactant and product concentrations.
Step-by-step explanation:
As a chemical reaction approaches equilibrium, the rates of the forward and reverse reactions change. Initially, the rate of the forward reaction is higher because the concentrations of the reactants are higher. As the reactions proceed, the concentration of reactants decreases while the concentration of products increases, making the reverse reaction more prevalent. Eventually, the rates of the forward and reverse reactions become equal, and equilibrium is reached. This does not mean that the reactions stop, but rather that the rates are balanced, and the concentrations of reactants and products remain constant over time.
Correct terminology is crucial in understanding and communicating about reversible reactions. The direction in which we choose to write the reaction can be relevant for clarity but does not alter the inherent nature of the reaction as the system will reach the same equilibrium state from either direction.