Equilibrium is reached when the rates of the forward and reverse reactions are equal from "summary" of Chemistry by Russell Kuhtz
Equilibrium in a chemical reaction is a delicate balance between the rates of the forward and reverse reactions. When the rates of the forward and reverse reactions are equal, the system is said to be at equilibrium. This means that the concentrations of reactants and products remain constant over time, even though the reactions are still occurring. At equilibrium, the rates of the forward and reverse reactions are not zero; rather, they are equal. This dynamic state of equilibrium is a result of the constant interconversion of reactants and products. It is important to note that equilibrium does not mean that the reactions have stopped, but rather that the rates of the forward and reverse reactions are balanced. In a chemical reaction at equilibrium, the concentrations of reactants and products no longer change because the rates of the forward and reverse reactions are equal. This balance is a result of the establishment of a dynamic equilibrium, where reactants are continuously being converted into products and products are continuously being converted back into reactants. The concept of equilibrium is crucial in understanding how chemical reactions proceed. It allows us to predict the behavior of a system under different conditions and determine the composition of the system at equilibrium. By studying the rates of the forward and reverse reactions, scientists can gain valuable insights into the nature of chemical reactions and the factors that influence their outcomes.- Equilibrium is a dynamic state in which the rates of the forward and reverse reactions are equal. This balance allows for the continuous interconversion of reactants and products, leading to a stable system where concentrations remain constant over time. Understanding the concept of equilibrium is essential in predicting the behavior of chemical reactions and studying their underlying mechanisms.
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