Which of the following statements correctly describes any chemical reaction that has reached equilibrium?

(A) The concentration 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 areequal.

Equilibrium is the balance condition that is attained by a chemical reaction. Every chemical reaction tries to achieve the equilibrium condition.

The products are the substance that is produced at the end of the chemical reaction. The reactants are the initial substance that participates in the reaction.

In a chemical reaction, reactants undergo a chemical reaction to produce products.

Thus, the product concentration and reactant concentration do notindicate that the reaction is in equilibrium.

Therefore, the given statement is false.

The reaction is reversible and irreversible. The reaction can occur both in the forward and the reverse direction. When the reaction is irreversible, the reverse reaction cannot take place.

Without reversible reaction, it is difficult to predict the equilibrium only with the forward reaction.

Thus, when the reaction is irreversible, the equilibrium of the reaction is not attained.

Therefore, the given statement is false.

The reaction is ina halted condition.This means that the reaction does not proceed any further.

Thus, the halted condition differs from the conditionof equilibrium.

Therefore, the given statement is false.

Equilibrium is the condition determined by the rate of the reaction.The rate is the speed of the reaction that is taking place.

The reaction that occurs due to the conversion of reactants into products is referred to as a forward reaction. The reaction which results in the formation of products from reactants is known as the reverse reaction.

Thus, the reaction rates of both of these reactions become equal,which indicates that the reaction is in equilibrium.

Therefore, the given statement is true.