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Le Chatelier's Principle and Equilibrium By: Shelby Toler

Le Chatelier's Principle and Equilibrium

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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. - PowerPoint PPT Presentation

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Page 1: Le Chatelier's Principle and Equilibrium

Le Chatelier's Principle and Equilibrium

By: Shelby Toler

Page 2: Le Chatelier's Principle and Equilibrium

2 SO3(g) ↔ 2 SO

2 (g) + O

2 (g)

ΔH° = 197.78 kJ

Increasing the temperature of the reaction.

Right

Page 3: Le Chatelier's Principle and Equilibrium

2 SO3(g) ↔ 2 SO

2 (g) + O

2 (g)

ΔH° = 197.78 kJ

Increasing the pressure on the reaction.

Left

Page 4: Le Chatelier's Principle and Equilibrium

2 SO3(g) ↔ 2 SO

2 (g) + O

2 (g)

ΔH° = 197.78 kJAdding more O2 when the reaction is at

equilibrium

Left

Page 5: Le Chatelier's Principle and Equilibrium

2 SO3(g) ↔ 2 SO

2 (g) + O

2 (g)

ΔH° = 197.78 kJRemoving O2 from the system when

the reaction is at equilibrium

Right

Page 6: Le Chatelier's Principle and Equilibrium

N2O

4(g) ↔ 2NO

2

ΔH° = 58.0 kJ

Adding more NO2 when the reaction is at equilibrium.

Left

Page 7: Le Chatelier's Principle and Equilibrium

N2O

4(g) ↔ 2NO

2

ΔH° = 58.0 kJ

Increasing the pressure

Left

Page 8: Le Chatelier's Principle and Equilibrium

N2O

4(g) ↔ 2NO

2

ΔH° = 58.0 kJ

Increase the volume

Right

Page 9: Le Chatelier's Principle and Equilibrium

N2O

4(g) ↔ 2NO

2

ΔH° = 58.0 kJ

Increasing the temperature.

Right

Page 10: Le Chatelier's Principle and Equilibrium

3H2(g) + N

2(g) ↔ 2NH

3(g)

ΔH° = -92.38 kJIncreasing the temperature of the reaction.

Left

Page 11: Le Chatelier's Principle and Equilibrium

3H2(g) + N

2(g) ↔ 2NH

3(g)

ΔH° = -92.38 kJAdding more N2 when the reaction is at

equilibrium

Right

Page 12: Le Chatelier's Principle and Equilibrium

3H2(g) + N

2(g) ↔ 2NH

3(g)

ΔH° = -92.38 kJRemoving H2 when the reaction is at

equilibrium.

Left

Page 13: Le Chatelier's Principle and Equilibrium

3H2(g) + N

2(g) ↔ 2NH

3(g)

ΔH° = -92.38 kJIncreasing the pressure

Right

Page 14: Le Chatelier's Principle and Equilibrium

3H2(g) + N

2(g) ↔ 2NH

3(g)

ΔH° = -92.38 kJ Increasing the volume.

Left

Page 15: Le Chatelier's Principle and Equilibrium

2CO (g) + O2 (g) ↔ 2CO

2 (g)

Increasing the pressure on the reaction.

Right

Page 16: Le Chatelier's Principle and Equilibrium

2CO (g) + O2 (g) ↔ 2CO

2 (g)

Adding more O2 when the reaction is at equilibrium

Right

Page 17: Le Chatelier's Principle and Equilibrium

2CO (g) + O2 (g) ↔ 2CO

2 (g)

Adding another reactant to the reaction

Right

Page 18: Le Chatelier's Principle and Equilibrium

2CO (g) + O2 (g) ↔ 2CO

2 (g)

Increasing the volume.

Left

Page 19: Le Chatelier's Principle and Equilibrium

N2 (g) + O

2 (g) ↔ 2NO (g)

Increasing the pressure on the reaction

No Shift

Page 20: Le Chatelier's Principle and Equilibrium

N2 (g) + O

2 (g) ↔ 2NO (g)

Adding more O2 when the reaction is at equilibrium

Right

Page 21: Le Chatelier's Principle and Equilibrium

N2 (g) + O

2 (g) ↔ 2NO (g)

Adding another reactant to the reaction

Right

Page 22: Le Chatelier's Principle and Equilibrium

N2 (g) + O

2 (g) ↔ 2NO (g)

Increasing the Volume

No Shift

Page 23: Le Chatelier's Principle and Equilibrium

PCl3(g) + Cl

2(g) <----> PCl

5(g)

What could you do to increase Pcl5?

Increase the pressureDecrease the volume

Page 24: Le Chatelier's Principle and Equilibrium

PCl3(g) + Cl

2(g) <----> PCl

5(g)

What could you do to increase Cl2?

Decrease the pressureIncrease the volume

Page 25: Le Chatelier's Principle and Equilibrium

N2 (g) + 3H

2 (g) <---> 2NH

3 (g)

What could you do to increase NH3?

Increase the pressureDecrease the volume

Page 26: Le Chatelier's Principle and Equilibrium

N2 (g) + 3H

2 (g) <---> 2NH

3 (g)

What could you do to decrease N2?

Increase the pressureDecrease the volume