1. Le Chatelier's Principle and Equilibrium
By: Shelby Toler

2. 2 SO3(g) ↔ 2 SO2 (g) + O2 (g) ΔH° = 197.78 kJ
Increasing the temperature of the reaction.
Right

3. 2 SO3(g) ↔ 2 SO2 (g) + O2 (g) ΔH° = 197.78 kJ
Increasing the pressure on the reaction.
Left

4. 2 SO3(g) ↔ 2 SO2 (g) + O2 (g) ΔH° = 197.78 kJ
Adding more O2 when the reaction is at equilibrium
Left

5. 2 SO3(g) ↔ 2 SO2 (g) + O2 (g) ΔH° = 197.78 kJ
Removing O2 from the system when the reaction is at equilibrium
Right

6. Adding more NO2 when the reaction is at equilibrium.
N2O4(g) ↔ 2NO ΔH° = 58.0 kJ
Adding more NO2 when the reaction is at equilibrium.
Left

7. Increasing the pressure
N2O4(g) ↔ 2NO ΔH° = 58.0 kJ
Increasing the pressure
Left

8. N2O4(g) ↔ 2NO ΔH° = 58.0 kJ
Increase the volume
Right

9. Increasing the temperature.
N2O4(g) ↔ 2NO ΔH° = 58.0 kJ
Increasing the temperature.
Right

10. 3H2(g) + N2(g) ↔ 2NH3(g) ΔH° = -92.38 kJ
Increasing the temperature of the reaction.
Left

11. 3H2(g) + N2(g) ↔ 2NH3(g) ΔH° = -92.38 kJ
Adding more N2 when the reaction is at equilibrium
Right

12. 3H2(g) + N2(g) ↔ 2NH3(g) ΔH° = -92.38 kJ
Removing H2 when the reaction is at equilibrium.
Left

13. 3H2(g) + N2(g) ↔ 2NH3(g) ΔH° = -92.38 kJ
Increasing the pressure
Right

14. 3H2(g) + N2(g) ↔ 2NH3(g) ΔH° = -92.38 kJ
Increasing the volume.
Left

15. Increasing the pressure on the reaction.
2CO (g) + O2 (g) ↔ 2CO2 (g)‏
Increasing the pressure on the reaction.
Right

16. Adding more O2 when the reaction is at equilibrium
2CO (g) + O2 (g) ↔ 2CO2 (g)‏
Adding more O2 when the reaction is at equilibrium
Right

17. Adding another reactant to the reaction
2CO (g) + O2 (g) ↔ 2CO2 (g)‏
Adding another reactant to the reaction
Right

18. 2CO (g) + O2 (g) ↔ 2CO2 (g)‏
Increasing the volume.
Left

19. Increasing the pressure on the reaction
N2 (g) + O2 (g) ↔ 2NO (g)‏
Increasing the pressure on the reaction
No Shift

20. Adding more O2 when the reaction is at equilibrium
N2 (g) + O2 (g) ↔ 2NO (g)‏
Adding more O2 when the reaction is at equilibrium
Right

21. Adding another reactant to the reaction
N2 (g) + O2 (g) ↔ 2NO (g)‏
Adding another reactant to the reaction
Right

22. N2 (g) + O2 (g) ↔ 2NO (g)‏
Increasing the Volume
No Shift

23. PCl3(g) + Cl2(g) <----> PCl5(g)‏
What could you do to increase Pcl5?
Increase the pressure
Decrease the volume

24. PCl3(g) + Cl2(g) <----> PCl5(g)‏
What could you do to increase Cl2?
Decrease the pressure
Increase the volume

25. N2 (g) + 3H2 (g) <---> 2NH3 (g)‏
What could you do to increase NH3?
Increase the pressure
Decrease the volume

26. N2 (g) + 3H2 (g) <---> 2NH3 (g)‏
What could you do to decrease N2?
Increase the pressure
Decrease the volume