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Understanding Le Chatelier's Principle: Disrupting Equilibrium and Its Effects

Le Chatelier's Principle helps predict the shifts in equilibrium when changes occur in concentration, temperature, and pressure during chemical reactions. A system at equilibrium will respond to disturbances by adjusting to counteract the change, ultimately restoring equilibrium. This principle is illustrated through examples like the reaction between N2O4 and NO2 at different temperatures. Understanding how factors such as catalysts, inert gases, and variations in reaction volume influence equilibrium is essential in chemistry.

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Understanding Le Chatelier's Principle: Disrupting Equilibrium and Its Effects

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  1. Le Chatelier’s Principle

  2. Disrupting Equilibrium Equilibrium can be disrupted by: • changing concentrations of reactants and/or products • changing the temperature • changing the pressure (gaseous reactions) When equilibrium is disrupted, the rate of the forward rxn no longer equals the rate of the reverse rxn

  3. Le Chatelier’s Principle • a way of predicting what happens to the relative rates of the forward and reverse reactions when equilibrium is disrupted The Law: • when a system at equilibrium is upset, the system responds by changing in a way which counteracts ( undoes) the disturbance • eventually equilibrium is restored

  4. Changing Concentration

  5. Changing Temperature

  6. Changing Volume NOTE: only impacts reactions involving gases

  7. Adding a Catalyst

  8. Adding an Inert Gas

  9. Examples 1) N2O4 (g)  2 NO2 (g) ΔH = + 24kJ/mol colourless brown

  10. Examples 1) N2O4 (g)  2 NO2 (g) ΔH = + 24kJ/mol colourless brown

  11. Example 1) N2O4 (g)  2 NO2 (g) ΔH = + 24kJ/mol colourless brown

  12. Examples 1) N2O4 (g)  2 NO2 (g) ΔH = + 24kJ/mol colourless brown

  13. Examples 1) N2O4 (g)  2 NO2 (g) ΔH = + 24kJ/mol colourless brown

  14. Examples 1) N2O4 (g)  2 NO2 (g) ΔH = + 24kJ/mol colourless brown

  15. Showing LCP Graphically T  new equilibrium Initial equilibrium rate of forward greater than rate of reverse

  16. Impact of Temperature on K Ex. From the previous graph, calculate K for the initial equilibrium and for the new equilibrium. On board

  17. Impact of Temperature on K

  18. Example [Co(H2O)6 ]2+ (aq) + 4Cl- (aq)  CoCl42- (aq) + 6 H2O (l) Pink Blue

  19. Example [Co(H2O)62+ (aq) + 4Cl- (aq)  CoCl42- (aq) + 6 H2O (l) Pink Blue

  20. Example [Co(H2O)62+ (aq) + 4Cl- (aq)  CoCl42- (aq) + 6 H2O (l) Pink Blue

  21. Example [Co(H2O)62+ (aq) + 4Cl- (aq)  CoCl42- (aq) + 6 H2O (l) Pink Blue

  22. Example [Co(H2O)62+ (aq) + 4Cl- (aq)  CoCl42- (aq) + 6 H2O (l) Pink Blue Based on the observations, is the forward rxnendo or exothermic?

  23. Example [Co(H2O)62+ (aq) + 4Cl- (aq)  CoCl42- (aq) + 6 H2O (l) Pink Blue Based on the observations, is the forward rxnendo or exothermic? ENDO

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