Le Chatelier's Principle and Equilibrium By: Shelby Toler

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

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

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

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

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

Increasing the pressure N2O4(g) ↔ 2NO2 ΔH° = 58.0 kJ Increasing the pressure Left

N2O4(g) ↔ 2NO2 ΔH° = 58.0 kJ Increase the volume Right

Increasing the temperature. N2O4(g) ↔ 2NO2 ΔH° = 58.0 kJ Increasing the temperature. Right

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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