How is chemical equilibrium achieved in a reversible reaction?

Chemical equilibrium in a reversible reaction is achieved when the rates of the forward and reverse reactions are equal.

In a reversible reaction, reactants are converted into products and products are converted back into reactants. This process continues until a state of balance, or equilibrium, is reached. At this point, the concentrations of the reactants and products remain constant over time, even though the reactions are still occurring. This is because the rate at which the reactants are forming products is equal to the rate at which the products are forming reactants.

The concept of chemical equilibrium is based on the principle of dynamic equilibrium. This principle states that in a closed system, the rates of the forward and reverse reactions will eventually become equal. This does not mean that the amounts of reactants and products are equal, but rather that their concentrations do not change over time.

The position of the equilibrium can be influenced by several factors, including temperature, pressure, and the concentration of the reactants and products. For example, increasing the temperature will usually favour the endothermic reaction (the reaction that absorbs heat), shifting the equilibrium position towards the products. Conversely, decreasing the temperature will favour the exothermic reaction (the reaction that releases heat), shifting the equilibrium position towards the reactants.

In summary, chemical equilibrium in a reversible reaction is a dynamic state where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of the reactants and products. This state is influenced by various factors, including temperature, pressure, and concentration. Understanding this concept is crucial for predicting the outcomes of chemical reactions and for manipulating these reactions to achieve desired results.