Effect of Addition of an Inert gas on Equilibrium
All the gases which do not participate in reaction are considered as inert gas. The effect of addition of inert gas on equilibrium at different conditions in discussed below:
Addition of an Inert Gas at Constant Volume
When an inert gas is added to the equilibrium at a constant volume, then the total pressure of the system will increase. But the concentrations of reactants and products will remain unaffected. Therefore, there will be no effect on the equilibrium.
Addition of an Inert Gas at Constant Pressure
When an inert gas is added to the equilibrium at a constant pressure, the volume increases. The number of moles per unit volume of various reactants and products decreases. Thus to overcome this the equilibrium will shift to direction with increased number of moles. Addition of inert gas at constant pressure will shift the equilibrium to backward direction.
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