Chemical Equilibrium
In chemistry, equilibrium is state in dynamics of a chemical reaction when rate of forward reaction equals to the rate of backward reaction. At this state, concentrations of reactants and products remain unchanged over time. It is influenced by a variety of factors such as temperature, pressure (for gases), and concentration. It is quantitatively represented by various constants such as Kf, Kb, Kc and Kp discussed later in this article.
Le Chatelier’s Principle
Le Chatelier’s Principle states that,
When a chemical reaction is disturbed from its equilibrium state by changing conditions such as temperature, pressure, etc., the reaction proceeds in such a direction (forward or backward) so as to counteract the change occurred.
Law of Mass Action
Law of Mass Action relates to the rate of a chemical reaction. It states that the rate of a reaction is directly proportional to the concentrations of its reactants. More precisely, the rate of a chemical reaction is directly proportional to the product of its reactant concentrations raised to their respective stoichiometric coefficients at constant temperature and pressure. This implies that an increase in reactant concentration would lead the reaction to move forward at a faster rate. The law of mass action forms the basis for equilibrium constant expression, which helps in quantifying the dynamics of the reaction.
In this article, we will discuss what is meant by the Law of Mass Action, Equilibrium Constant, Chemical Equilibrium, applications of the law and related frequently asked questions.