Le Chatelier's Principle Flashcards
What is Le Chatelier’s principle
When a change is made to an equilibrium system, the system will proceed in a way that will partially oppose the effect of the change
Factors that can disturb equilibrium:
- addition/removal of products/reactants
- changes in temperature
- changes in volume/pressure
Effect of adding products/reactants
If the volume of system has not changed, + a reactant/product increases the concentration of the reactant/product
- the system partially opposes this change by favouring the reaction that will decrease the concentration of the reactant/product
- will then re-establish equilibrium
- the concentration of the added species will be more than initial equilibrum
Application of Collision Theory
Increase in reactants –> more reactant particles with more collisions –> increased RoR
- same for products –> increase RoR of the re-formation of reactants
Effect of removing products/reactants
Will cause the system to favour the reaction that will increase the concentration of the reactant/product
- removing products –> favours forward reaction
- removing reactants –> favours backward reaction
Effect of a catalyst
- speed up a reaction without being consumed
- does not affect PoE
Effect of concentration on equilibrium
- +/- substances which increases/decreases conc. of substance being added
- increasing/decreasing volume which increases/decreases the conc. of all species in the system
- dilution which for solutions, decreases concentration of all species
Increasing/decreasing volume
Decrease volume
- instantaneous increase in the concentration of all species
- will favour the reaction that produces the least nnumber of particles –> to decrease conc.
Increase volume
- instantaneous decrease in the concentration of all species
- favour the reaction that produces more particles due –> to increase conc.
Effect of pressure on equilibrium
Occurs with a change of volume in the system
- decrease in volume = increase in pressure –> will favour the reaction that produces the least no. of particles
- increase in volume = decrease in pressure –> will favour the reaction that produces the most no. of particles
Effect of temperature on equilibrium - Endothermic
Increase in temp. –> increases kinetic energy –>more particles that can satisfy AE –> increase in no. of collisions –> increases RoR of both reactions
- favours the forward reaction
Decrease in temp.
- favours the backward reaction
Effect of temperature on equilibrium - Exothermic
Increase in temp. –> increases kinetic energy –>more particles that can satisfy AE –> increase in no. of collisions –> increase RoR of both reactions
- favours the backward reaction
Decrease in temp.
- favours the forward reaction