Effect of Concentration Change on Equilibrium
In chemical equilibrium, increasing the concentrations of the reactants results in shifting the reaction in favor of products so as to oppose the effect of increase of concentration of reactants. Hence, the rate of forward reaction increases. Similarly, increasing the concentrations of the products results in shifting the reaction in favor of reactants so as to oppose the effect of increase of concentration of reactants. Hence, the rate of backward reaction increases.
Effect of Change in Concentration of Reactant
- If the concentration of reactant increases, the equilibrium will shift in the direction so as to favor the formation of product.
2SO2(g) + O2(g) ⇄ 2SO3(g)
- If the concentration of reactant decreases, the equilibrium will shift in the direction to favor the increase in concentration of reactant. Hence, the reaction will be in backward direction.
For example, If the concentration of SO2 or O2 is increased then the reaction will shift in the direction so as to oppose the increase in concentration of reactants. Hence, the reaction will shift in forward direction and vice versa will be in the case of decrease in concentration of reactant.
Effect of Change in Concentration of Product
- If the concentration of product increases, the equilibrium will shift in the direction so as to favor the formation of reactant. Hence, the direction of reaction will shift to backward direction
PCl3(g) + Cl2(g) ⇄ PCl5(g)
- If the concentration of product decreases, the equilibrium will shift to favour increase in product. Hence, the direction of reaction will be in forward direction
For example, If the concentration of PCl5 is decreased, then the rate of reaction is also increased which leads to decrease in concentration of chlorine and increase in concentration of phosphorus pentachloride. Hence, equilibrium will shift to right so rate of forward reaction increases and vice-versa will be in the case of increase of concentration of product.
Le Chateliers Principle
Le Chatelier’s Principle is a fundamental concept in chemistry that describes how a chemical system at equilibrium responds to changes in temperature, pressure, or concentration of reactants or products. This principle is named after the French chemist Henry Louis Le Chatelier, who formulated it in the late 19th century. Equilibrium refers to the state of balance which tells that there is equal weight on both sides of the scale. Chemical equilibrium is attained when the rate of forward reaction is equal to the rate of backward reaction.
In this article, we will have a thorough knowledge of equilibrium, Le Chatelier’s principle, and the effect of various factors on chemical equilibrium.
Table of Content
- What is Le Chatelier’s Principle of Equilibrium?
- Effect of Concentration Change on Equilibrium
- Effect of Change in Pressure on Equilibrium
- Effect of Volume Change on Product Formation
- Effect of Change in Temperature on Equilibrium
- Effect of Catalyst on Equilibrium
- Effect of Addition of an Inert gas on Equilibrium
- Application of Le Chatelier’s Principle