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Le Chatelier's Principle and Equilibrium

By: Shelby Toler. Le Chatelier's Principle and Equilibrium. 2 SO 3 (g) ↔ 2 SO 2 (g) + O 2 (g) ΔH° = 197.78 kJ. Increasing the temperature of the reaction. Right. 2 SO 3 (g) ↔ 2 SO 2 (g) + O 2 (g) ΔH° = 197.78 kJ. Increasing the pressure on the reaction. Left.

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Le Chatelier's Principle and Equilibrium

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

  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. N2O4(g) ↔ 2NO2ΔH° = 58.0 kJ Adding more NO2 when the reaction is at equilibrium. Left

  7. N2O4(g) ↔ 2NO2ΔH° = 58.0 kJ Increasing the pressure Left

  8. N2O4(g) ↔ 2NO2ΔH° = 58.0 kJ Increase the volume Right

  9. N2O4(g) ↔ 2NO2ΔH° = 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. 2CO (g) + O2 (g) ↔ 2CO2 (g)‏ Increasing the pressure on the reaction. Right

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

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

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

  21. 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

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