Le Chateleier's Principle

The following factors affect the position of equilibrium EXCEPT

• Concentration
• Pressure
• Temperature
• States of matter

For N₂O₄ (colorless)→ 2NO₂ (brown). By reducing pressure, equilibrium is shift to right. WHY?

• Shift to the right will increase the rate of reaction
• Color of system will turn from colorless to brown.
• More particles on the right, so K_c will increase
• More particles on the right, so pressure can increase again

For N₂ + 3H₂ →2NH₃ . When pressure is increased the equilibrium shift to right. Why?

• To increase the amount of products
• To reduce the pressure, as right has less number of molecule
• K_c will increase when it is shifted to the right
• So it will increase the rate of reaction

For N₂O₄ → NO₂ (ΔH = +ve). What will happen when temperature is increased?

• Position of equilibrium will shift to left
• Position of equilibrium will shift to right
• No change in position of equilibrium
• Equlibrium will not be affected

N₂O₄ → NO₂ (ΔH = +ve). Why when temperature is increased position of equilibrium is shifted to RIGHT?

• Forward reaction is endothermic, thus reducing the temp
• Forward reaction is exothermic, thus reducing the temp
• Forward reaction is endothermic, thus increasing the temp
• Forward reaction is exothermic, thus increasing the temp

2SO_2(g)+O_2(g) ⇌ 2SO_3(g) + Heat

Adding SO_2(g) will

• shift equilibrium right

• shift equilibrium left

• increase rate of reaction

• have no change

2SO₂(g)+O₂(g) ⇌ 2SO₃(g) + Heat

Increasing the temperature will...

• shift equilibrium right

• shift equilibrium left

• increase pressure

• have no change

2SO₂(g)+O₂(g) ⇌ 2SO₃(g) + Heat

Adding SO₃(g) will

• shift equilibrium right

• shift equilibrium left

• increase K

• have no change

2SO₂(g)+1O₂(g) ⇌ 2SO₃(g) + Heat

Increasing the volume of the container will...

• shift equilibrium right

• shift equilibrium left

• slow rate of reaction

• have no change

2SO₂(g)+1O₂(g) ⇌ 2SO₃(g) + Heat

Increasing the pressure on the system will...

• shift equilibrium right

• shift equilibrium left

• slow rate of reaction

• have no change