Which statement is true about a reaction at equilibrium?

A. The reaction is not reversible.
B. The reaction concentrations of the reactants and products are always equal.
C. The reaction rates of the forward and reverse reaction are always equal.
D. The change in concentration for reactant and product is always equal to 1.

answer is C rate of forward reaction is always equal to rate of reverse reaction.

yes

The correct statement about a reaction at equilibrium is:

C. The reaction rates of the forward and reverse reactions are always equal.

To understand why this statement is true, we first need to understand what equilibrium means in a chemical reaction.

Equilibrium is a state in a chemical reaction where the concentrations of reactants and products remain constant over time. In other words, the reaction appears to be at a standstill, with the forward reaction occurring at the same rate as the reverse reaction.

Now, let's discuss why statement C is true. In a reversible reaction, both the forward and reverse reactions are occurring simultaneously. Initially, as the reaction begins, the forward reaction predominates, which means reactants are being converted into products at a faster rate. However, as the products build up, the reverse reaction becomes more favorable, resulting in the formation of reactants. This continues until the rate of the forward and reverse reactions become equal.

At equilibrium, the concentrations of reactants and products stabilize, meaning they remain constant over time. It's important to note that the concentrations of reactants and products at equilibrium are not necessarily equal. Instead, the ratio of their concentrations, known as the equilibrium constant, remains constant.

To determine the equilibrium constant, you would need to perform experiments and measure the concentrations of reactants and products at equilibrium. The equilibrium constant can be written using the law of mass action and the stoichiometry of the balanced chemical equation.

In summary, at equilibrium, the reaction rates of the forward and reverse reactions are always equal. It is the dynamic balance between these two rates that allows the concentrations of reactants and products to remain constant over time.