What is dynamic equilibrium in a chemical reaction?

Dynamic equilibrium in a chemical reaction is when the rate of the forward reaction equals the rate of the reverse reaction.

In a chemical reaction, reactants are converted into products. However, in some reactions, the products can also revert back to the original reactants. This is known as a reversible reaction, represented by a double arrow in chemical equations. When the rate of the forward reaction (reactants turning into products) equals the rate of the reverse reaction (products turning back into reactants), the system is said to be in a state of dynamic equilibrium.

Dynamic equilibrium does not mean that the reaction has stopped. Instead, it signifies a state of balance where the concentrations of the reactants and products remain constant over time. This is because the forward and reverse reactions are still occurring, but at the same rate, so there is no net change in the amounts of reactants and products.

It's important to note that dynamic equilibrium can only occur in a closed system, where no reactants or products can enter or leave. This is because any change in the amounts of reactants or products would disrupt the balance and shift the equilibrium.

The concept of dynamic equilibrium is central to understanding many chemical processes and is a key part of the study of chemical kinetics and thermodynamics. It helps us understand how reactions occur and how we can manipulate conditions to favour either the forward or reverse reaction, which is particularly important in industrial processes.