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Introduction
Le Chatelier's Principle: When a system at equilibrium gets disrupted by a change in concentration, temperature, or pressure, it will naturally adjust itself back into equilibrium.
STRESS Introduced to System → SHIFT to Restore Equilibrium
How the System Responds
When the reaction shifts to one side, the concentration of that side increases as rates adjust.
Forward/Right - Favoring formation of products.
Reverse/Left - Favoring formation of reactants.
Change in Concentration:
An increase in reactant concentration temporarily shifts the reaction towards the products to use up the added reactants to restore equilibrium.
An increase in product concentration temporarily shifts the reaction towards the reactants to use up the added products to restore equilibrium.
Change in Pressure (Gaseous Reactions):
An increase in pressure temporarily shifts the reaction toward the side with fewer moles of gas to reduce pressure, therefore restoring equilibrium.
A decrease in pressure temporarily shifts the reaction toward the side with more moles of gas to increase pressure, therefore restoring equilibrium.
Change in Temperature (Changes K):
An increase in temperature shifts the equilibrium toward the endothermic reaction, which causes the system to absorb more heat.
A decrease in temperature shifts the equilibrium toward the exothermic reaction, which causes the system to release more heat.
In Summary...
More reactants: Equilibrium shifts right.
More products: Equilibrium shifts left.
Increase pressure: Shift to reaction with fewer gas moles.
Decrease pressure: Shift to reaction with more gas moles.
Increase temperature: Favor endothermic (absorbs heat).
Decrease temperature: Favor exothermic (releases heat).
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