What characterizes dynamic equilibrium in chemical reactions?

Dynamic equilibrium in chemical reactions is characterized by equal rates of forward and reverse reactions, which results in no net change in the concentrations of reactants and products over time. This concept is fundamental in understanding how reversible reactions operate. At dynamic equilibrium, the system remains balanced, meaning that while the reactions continue to occur in both directions, the overall concentration of no individual species changes, giving an appearance of stasis.

The other options do not accurately capture the essence of dynamic equilibrium. Maintaining a constant concentration of reactants only, as mentioned in one of the choices, would not account for the concentrations of products, which would also remain constant at equilibrium. The idea of complete conversion of reactants to products contradicts the principle of equilibrium, which allows for both reactants and products to coexist at specific concentrations. Lastly, stating that only forward reactions are occurring ignores the essential feature of dynamic equilibrium, which is the coexistence and continuous action of both forward and reverse reactions.