What does it mean for a reaction to be at dynamic equilibrium?

When a reaction reaches dynamic equilibrium, it signifies that both the forward and reverse reactions are occurring simultaneously and at equal rates. This means that while reactants are being converted into products, products are also being converted back into reactants at the same rate. As a result, the concentrations of reactants and products remain constant over time, but not necessarily equal.

At this stage, the system is dynamic because the reaction components are continuously interacting, but there is no net change in their concentrations. This state contrasts with completion, where all reactants would completely convert to products, or a situation where only one direction of the reaction is happening, which would not be indicative of equilibrium.