Le Chatelier's Principle

[Irene Kang 3F]

Can someone list out what affects what in Le Chatelier?

[Jasmine Reblando 3A]

1. Change in concentration
- if we add more reactant for example, the forward reaction will speed up in order to restore more product and create the balance of equilibrium once again
- With this, the equilibrium has been shifted right since we added more reactants. Vice versa if we added more products.

2. Change in temperature
-If we add heat to the reactant side (meaning delta H is positive and an endothermic reaction) the equilibrium will be shifted right as we will need more heat on the product side in order to reestablish equilibrium. Vice versa if we added heat to the products.

3. Change in volume/pressure
-If we decrease volume, pressure goes up. This means the equilibrium will shift towards the side with the lesser amount of stoichiometric mols. For example Cl2---2Cl. An increase in pressure/decrease in volume would mean that this equilibrium will shift left because it is 1 mol vs. 2 mols. We want to balance it out, hence the favor towards the Cl2.

Best way to think of it is a seesaw. If something is added to one side, the other side will be favored in order to find that balance.