Effect of Volume Change on Product Formation
According to Le Chatelier’s Principle
- When there is a decrease in volume, the equilibrium will shift in the direction with fewer number of gaseous moles.
- When there is a increase in volume, the equilibrium will shift in the direction with more number of gaseous moles.
Some examples of volume change are:
- Equilibrium will shift in forward direction as products have lesser number of moles.
2H2(g) + CO(g) ⇄ CH3OH(g)
- Equilibrium will shift in backward direction as reactants have lesser number of moles.
4NH3(g) + 5O2(g) ⇄ 4NO(g) + 6H2O(g)
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