Chemical equilibrium is a state in a chemical reaction where the concentrations of reactants and products remain constant over time. This means that the forward and reverse reactions are occurring at the same rate, resulting in no net change in the overall concentration of substances involved.
Chemical equilibrium is achieved when the rate of the forward reaction is equal to the rate of the reverse reaction. This can be achieved by changing the temperature, pressure, or concentrations of reactants and products in the reaction.
The factors that affect chemical equilibrium include temperature, pressure, and concentrations of reactants and products. Changes in these factors can shift the equilibrium position, resulting in changes in the concentrations of substances involved in the reaction.
The equilibrium constant, also known as Keq, can be calculated by taking the ratio of the concentrations of products to reactants at equilibrium. It is a measure of the extent of the reaction and is dependent on the temperature at which the reaction is taking place.
The direction of a reaction at equilibrium can be predicted by using Le Chatelier's principle. This principle states that if a stress is applied to a system at equilibrium, the system will shift in a direction that reduces the stress. This means that if the concentration of a reactant or product is increased, the reaction will shift in the opposite direction to reduce the concentration. The same applies for changes in temperature or pressure.