Which of the following is TRUE for a system that is in dynamic equilibrium?


A)
The forward reaction goes to 100% completion.

B)
The concentration of products is equal to the concentration of the reactants.

C)
The reaction rate of the forward reaction approaches zero.

D)
Both the forward and reverse reactions come to a halt

E)
none of the answers

B is not right.

To determine the answer to this question, we need to understand what dynamic equilibrium means in the context of a chemical system.

In a chemical reaction, equilibrium is reached when the forward and reverse reactions occur at the same rate and there is no net change in the concentrations of the reactants and products over time.

Now, let's go through each option and see which one is true for a system in dynamic equilibrium:

A) The forward reaction goes to 100% completion.
This statement is not true. In dynamic equilibrium, both the forward and reverse reactions are still occurring, although they are happening at equal rates. The reaction does not go to 100% completion.

B) The concentration of products is equal to the concentration of the reactants.
This statement is also not necessarily true. While it is true that the concentrations of reactants and products are constant in dynamic equilibrium, they do not have to be equal. The concentrations will simply reach a point where they remain constant and do not change over time.

C) The reaction rate of the forward reaction approaches zero.
This statement is true. In dynamic equilibrium, the reaction rate of the forward reaction becomes equal to the reaction rate of the reverse reaction. As a result, the net reaction rate approaches zero, indicating that the forward reaction is happening at the same rate as the reverse reaction.

D) Both the forward and reverse reactions come to a halt.
This statement is not true. In dynamic equilibrium, both the forward and reverse reactions are still occurring. However, their rates are equal, resulting in a state where there is no net change in the concentrations of the reactants and products.

E) None of the answers.
Based on our analysis, option C is the correct answer. The reaction rate of the forward reaction approaches zero in dynamic equilibrium.

The correct answer is B) The concentration of products is equal to the concentration of the reactants.

In a system that is in dynamic equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction. This means that while the reactions are still occurring, the concentrations of the reactants and products no longer change over time. The system reaches a point where the concentrations of the reactants and products remain constant, establishing a balance between the forward and reverse reactions. Therefore, the concentration of products is equal to the concentration of the reactants in a system at dynamic equilibrium.