1 / 23

Le Chatelier’s Principle

Le Chatelier’s Principle. Disrupting Equilibrium. Equilibrium can be disrupted by: changing concentrations of reactants and/or products changing the temperature changing the pressure (gaseous reactions)

chin
Télécharger la présentation

Le Chatelier’s Principle

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related