How do you define dynamic equilibrium?

Dynamic equilibrium is a state where the rate of forward reaction equals the rate of the reverse reaction.

In more detail, dynamic equilibrium is a concept in chemistry that describes a state of balance in a reversible reaction. This doesn't mean that the reaction has stopped. Instead, it means that the reaction is still happening, but the concentrations of the reactants and products remain constant over time because the rates of the forward and reverse reactions have become equal.

Imagine a simple reversible reaction where A and B react to form C and D. At the start, A and B react to form C and D at a certain rate. As the reaction proceeds, the concentrations of A and B decrease, which slows down the forward reaction. Meanwhile, the concentrations of C and D increase, which speeds up the reverse reaction. Eventually, the forward and reverse reactions occur at the same rate, and the system reaches a state of dynamic equilibrium.

It's important to note that dynamic equilibrium can only occur in a closed system, where no reactants or products can enter or leave. If the system is disturbed, for example by changing the temperature or pressure, the equilibrium will shift to counteract the change. This is known as Le Chatelier's Principle.

In summary, dynamic equilibrium is a state of balance in a reversible reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. It's a fundamental concept in chemistry that helps us understand how reactions occur and how they can be controlled.