Le Chatelier's Principle & Types of Equations

The following factors affect the position of equilibrium EXCEPT

• Concentration
• Pressure
• Temperature
• States of matter

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

2SO_2(g) + O_2(g) ⇌ 2SO_3(g) + Heat

Removing O_2(g) 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

2SO₂(g) + O₂(g) ⇌ 2SO₃(g) + Heat

Using a catalyst

• shift equilibrium right

• shift equilibrium left

• increase the rate of reaction

• have no change

CoCI₄^2- +6H₂O →Co(H₂O)₆²⁺ + 4CI^-.

What would happen when H₂O is added?

• Position of equilibrium will shift to left (and become more blue)

• Position of equilibrium will shift to right (and become more pink)

• K_eq will increase as H₂O is added

• Position of equilibrium will shift to left to reduce the added H₂O

1N₂ + 3H₂ →2NH₃

When the pressure on the system is increased, the equilibrium position shifts to the right. Why?

• To increase the amount of products

• To reduce the pressure, as the right side has fewer molecules of gas

• K_eq will increase when it is shifted to the right

• To increase the pressure, as the right side has more molecules of gas

Tags

CCSS.RI.9-10.8