What is the Difference Between Dynamic Equilibrium and Equilibrium?

Dynamic equilibrium and equilibrium are related concepts in chemistry, but they have distinct meanings. Here are the key differences between the two:

• Dynamic Equilibrium:
• Exists when a reversible reaction occurs, meaning substances transition between reactants and products at equal rates, resulting in no net change.
• The concentration of neither reactants nor products changes.
• It is a particular example of a system in a steady state.
• Represents a balance between a forward reaction and a reverse reaction.
• Once dynamic equilibrium is established, the concentrations or partial pressures of all species involved in the process remain constant.
• Equilibrium:
• Refers to a state in which the forward and reverse reactions of a system proceed at equal rates, but the concentrations or partial pressures of the reactants and products are not necessarily equal.
• At equilibrium, the composition of the system no longer changes with time.
• The composition of an equilibrium mixture is independent of the direction from which equilibrium is approached.

In summary, dynamic equilibrium is a specific type of equilibrium where the concentrations of reactants and products remain constant due to equal rates of forward and reverse reactions. In contrast, equilibrium refers to a state in which the rates of forward and reverse reactions are equal, but the concentrations may not necessarily be constant.

Comparative Table: Dynamic Equilibrium vs Equilibrium

Here is a table comparing dynamic equilibrium and equilibrium:

Dynamic equilibrium is a state where the forward and reverse reactions occur at equal rates, and there is no net change in the reactant and product ratio. In contrast, equilibrium implies that both the forward and reverse reaction rates are equal, and there is no further chemical change in the system. Both static and dynamic equilibria can occur in either open or closed systems.