Equilibrium is a state in which opposing forces or processes are balanced, resulting in a stable system. In chemistry, it refers to a point at which the concentration of reactants and products in a reversible reaction remain constant over time.
The equilibrium constant, denoted as Keq, is determined by taking the ratio of the concentrations of products and reactants at equilibrium. It is calculated using the equilibrium expression, which is different for each chemical reaction.
According to Le Chatelier's principle, an increase in temperature will shift the equilibrium in the direction of the endothermic reaction (the reaction that absorbs heat). Conversely, a decrease in temperature will shift the equilibrium towards the exothermic reaction (the reaction that releases heat).
Yes, equilibrium can be reached in a closed system. In a closed system, the reactants and products are contained and cannot escape. As the reaction proceeds, the concentrations of reactants and products will change until they reach a state of equilibrium.
Catalysts do not affect the position of equilibrium, but they can speed up the rate at which equilibrium is reached. This is because they lower the activation energy required for the reaction to occur, allowing the reaction to reach equilibrium faster.
