A reaction in equilibrium is a state in which the forward and reverse reactions are occurring at equal rates, resulting in no net change in the concentration of reactants and products.
Equilibrium is reached when the rates of the forward and reverse reactions are equal. This can occur when the concentrations of reactants and products reach a constant value, or when the system reaches a state of dynamic equilibrium in which the concentrations of reactants and products are constantly changing but the overall ratio remains constant.
The position of equilibrium can be affected by changes in temperature, pressure, and concentration. Changes in these factors can shift the equilibrium towards the reactants or products, resulting in changes in the concentrations of reactants and products at equilibrium.
Catalysts do not affect the position of equilibrium in a chemical reaction, but they can increase the rate at which equilibrium is reached by lowering the activation energy required for the reaction. This results in a faster attainment of equilibrium with the same concentrations of reactants and products.
Yes, equilibrium can be altered or broken through changes in the conditions of the reaction. For example, if the concentration of reactants or products is changed, the equilibrium will shift to reach a new state of equilibrium. Similarly, changes in temperature or pressure can also alter the position of equilibrium in a chemical reaction.