What defines dynamic equilibrium in a chemical reaction?

Dynamic equilibrium in a chemical reaction is characterized by the condition in which the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products over time, provided the system is closed. In this state, both the formation of products from reactants and the conversion of products back into reactants occur at the same rate, allowing the system to maintain a consistent composition despite the ongoing reactions.

This equality in reaction rates means that while individual molecules continue to react, the overall concentrations remain constant, leading to the concept of dynamic equilibrium. It is important to note that dynamic equilibrium does not imply that the reactants and products are present in equal amounts; rather, it means that their concentrations are stable and do not change as long as the conditions remain constant.

Other options present misconceptions about dynamic equilibrium. The greater rates of forward reactions imply a change in concentrations, not equilibriums. Equal concentrations of reactants and products do not necessarily signify equilibrium because the reaction could still be shifting, and stating that the reaction has reached completion contradicts the essence of dynamic equilibrium, where both reactants and products are present.