Consider this reaction at equilibrium.
Predict the effect (shift right, shift left, or no effect) of these changes.
(a) adding Cl2 to the reaction mixture
(b) adding COCl2 to the reaction mixture
(c) adding CO to the reaction mixture
Solution 63P :
Given reaction at equilibrium.
CO2(g) + Cl2(g) ⇋COCl2(g)
Le Chatelier's principle is also called as ‘The equilibrium law’. It states that ‘ The changes to an equilibrium system will result in a predictable shift that will counteract the change’. It is used to predict the changes in system that is caused due to temperature, pressure, volume or concentration.
According to Le Chatelier's principle :
- When a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance
- Adding additional reactant to a system will shift the equilibrium to the right which is towards the side of the products
- Removing the reactants from the system will cause the equilibrium to shift to the left which is towards reactant.
- Similarly, adding additional product to a system will shift the equilibrium to the left, in order to produce more reactants.
- Reducing the concentration of product will shift the equilibrium to the right, towards the products.