Effect of Catalyst on Equilibrium
The use of appropriate catalyst will increase the rate of reaction thereby decreasing the time required to reach the equilibrium position. A catalyst can’t change the equilibrium constant Hence, the relative ratio of concentration of reactants and products remain unaffected.
For reversible reaction, catalyst helps in reaching the equilibrium position by increasing the rate of forward and backward reaction.
Eg: Haber’s Process
N2(g) + 3H2(g) ⇄ 2NH3(g)
In Haber’s process the yield of ammonia is low at high temperature and reaction is slow at low temperature. So, in order to increase the speed of reaction at low temperature mixture of iron and molybdenum is added as a catalyst.
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