Dynamic equilibrium:
Dynamic equilibrium is a state in a reversible chemical reaction where the rate of the forward reaction is equal to the rate of the reverse reaction. In other words, the concentrations of the reactants and products remain constant over time, but the reactions are still occurring.

Explanation:
In a dynamic equilibrium, the concentrations of the reactants and products are not equal. Here's why:

Concentration of reactants:
- At the beginning of the reaction, the concentration of the reactants is high, and the concentration of the products is low.
- As the reaction proceeds, the concentration of the reactants decreases because they are being consumed.
- However, the reaction is reversible, so some of the products will also revert back to reactants.
- As a result, even though the concentration of the reactants decreases, it will not become zero. There will always be some reactants present in the system.

Concentration of products:
- At the beginning of the reaction, the concentration of the products is low, and the concentration of the reactants is high.
- As the reaction proceeds, the concentration of the products increases because they are being formed.
- However, some of the products will also revert back to reactants.
- As a result, even though the concentration of the products increases, it will not become the same as the concentration of the reactants. There will always be some reactants present in the system.

Dynamic equilibrium:
- Eventually, the rates of the forward and reverse reactions become equal, and a dynamic equilibrium is established.
- At this point, the concentrations of both the reactants and products remain constant, but they are not equal.
- The reactants and products are continuously interconverting, but there is no net change in their concentrations.

Conclusion:
At dynamic equilibrium, the concentration of both the reactants and products are not equal. The reactants and products are continuously interconverting, but the concentrations remain constant.