Final answer:
At equilibrium in a chemical reaction, the rates of forward and reverse reactions are equal, the reactants and products are formed and consumed at equal rates, and the concentrations of reactants and products remain constant, characterizing a dynamic equilibrium.
Step-by-step explanation:
When a reaction has reached equilibrium, three key conditions are true:
- The rate of the forward reaction is equal to the rate of the reverse reaction.
- The reactants and products are consumed and formed at equal rates.
- The concentrations of reactants and products remain constant.
This state is known as dynamic equilibrium, where the reaction continues to occur in both directions at the same rate, but the macroscopic properties, such as concentration, remain unchanged. It's crucial to note that reaching equilibrium doesn't mean that the concentrations of reactants and products are equal; rather, it means they are not changing over time.