Question

Which statement correctly describes a chemical reaction at equilibrium?

(1) The concentrations of the products and reactants are equal.
(2) The concentrations of the products and reactants are constant.
(3) The rate of the forward reaction is less than the rate of the reverse reaction.
(4) The rate of the forward reaction is greater than the rate of the reverse reaction.

Answer 1

A chemical reaction at equilibrium is correctly described by the constant concentrations of products and reactants, implying that the forward and reverse reactions occur at equal rates.

Step-by-step explanation:

The statement that correctly describes a chemical reaction at equilibrium is: The concentrations of the products and reactants are constant. A system at equilibrium is characterized by the forward and reverse reactions occurring at equal rates, meaning that there is no net change in the concentration of reactants and products over time.

However, the concentrations of products and reactants at equilibrium do not necessarily have to be equal; they simply remain unchanged. This state is described as dynamic equilibrium, emphasizing that the reaction has not stopped but is continuously occurring in both the forward and reverse directions at the same rate. Therefore, option (2) is correct.

Answer 2

(2) or (B)

Step-by-step explanation:

the concentrations of the products and the reactants are constant. That is a result of a dynamic equilibrium. The dynamic equilibrium is reached when the rates of forward reaction and the reverse reaction are equals, which yields to a zero net change in the concentrations of products and reactants.