Which of the following statements correctly describes any chemical reaction that has reached equilibrium? (A)The concentrations of products and reactants are equal. (B)The reaction is now irreversible. (C)Both forward and reverse reactions have halted. (D)The rates of the forward and reverse reactions are equal.

Verified step by step guidance

1. Identify the definition of chemical equilibrium in a reaction.
2. Understand that at equilibrium, the rate of the forward reaction equals the rate of the reverse reaction.
3. Recognize that equilibrium does not imply equal concentrations of reactants and products.
4. Note that at equilibrium, reactions are still occurring, but there is no net change in concentrations.
5. Conclude that the correct statement is the one describing equal rates of forward and reverse reactions.

Key Concepts

Chemical Equilibrium

Chemical equilibrium is a state in a reversible reaction where the concentrations of reactants and products remain constant over time. This does not mean that the reactants and products are equal in concentration, but rather that their rates of formation are balanced.

Dynamic Nature of Equilibrium

Equilibrium is dynamic, meaning that both the forward and reverse reactions continue to occur, but at equal rates. This ongoing process allows the system to maintain constant concentrations of reactants and products, despite the reactions still taking place.

Reaction Rates

The rates of a chemical reaction refer to the speed at which reactants are converted into products. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction, leading to no net change in the concentrations of the substances involved.