Equilibrium is a state in which the forward and reverse reactions of a chemical reaction occur at equal rates, resulting in no net change in the amount of reactants or products.
Equilibrium is achieved when the concentration of reactants and products reach a steady state. This can be achieved by adjusting the temperature, pressure, or concentration of reactants and products.
The factors that affect equilibrium include temperature, pressure, and concentration of reactants and products. Changes in these factors can shift the equilibrium position and alter the amount of products and reactants present.
Equilibrium constant (K) is calculated by taking the ratio of the concentration of products to the concentration of reactants, each raised to the power of their respective coefficients in the balanced chemical equation.
Le Chatelier's principle states that when a system at equilibrium is disturbed, it will shift in a direction that minimizes the effect of the disturbance. For example, if the concentration of reactants is increased, the equilibrium will shift to the right to form more products and reduce the excess reactants.