Le Chatelier

The following factors affect the position of equilibrium EXCEPT

• Concentration
• Pressure
• Temperature
• States of matter

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

2SO₂(g)+O₂(g) ⇌ 2SO₃(g) exothermic

Increasing the temperature will...

• shift equilibrium right

• shift equilibrium left

• reduce pressure

• have no change

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

2SO_2(g) + O_2(g) ⇌ 2SO_3(g) + exothermic

Removing O_2(g) will

• shift equilibrium right

• shift equilibrium left

• increase pressure

• have no change

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

2SO₂(g)+O₂(g) ⇌ 2SO₃(g) + Exothermic

Adding SO₃(g) will

• shift equilibrium right

• shift equilibrium left

• increase K

• have no change

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

2SO₂(g)+1O₂(g) ⇌ 2SO₃(g) exothermic

Increasing the volume of the container will...

• shift equilibrium right

• shift equilibrium left

• slow rate of reaction

• have no change

Tags

NGSS.HS-PS1-6

2SO₂(g) + O₂(g) ⇌ 2SO₃(g) exothemic

Using a catalyst

• shift equilibrium right

• shift equilibrium left

• increase the rate of reaction

• have no change

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

Which statement is not correct about the industrial preparation of ethanol by the hydration of ethene at 300 °C?

C₂H₄(g) + H₂O(g) ⇌ C₂H₅OH(g) ∆H = –46 kJ mol^–1

• The reaction is catalysed by an acid.

• The higher the pressure, the higher the equilibrium yield of ethanol.

• The higher the temperature, the higher the equilibrium yield of ethanol.

• A low equilibrium yield of ethanol is acceptable because unreacted ethene is recycled.

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

For this reaction at equilibrium, which combination of temperature and pressure would give the greatest equilibrium yield of products?

W(g) + X(g) ⇌ 2Y(g) + Z(g) ∆H = +47 kJ mol^–1

• High pressure and high temperature

• High pressure and low temperature

• Low pressure and high temperature

• Low pressure and low temperature

Tags

NGSS.HS-PS1-6

The forward reaction in this equilibrium is endothermic

COCl₂ (g) ⇌ CO(g) + Cl₂ (g)

Which statement is correct?

• If the total pressure is increased at constant temperature, the proportion of COCl₂ in the equilibrium mixture will decrease

• Use of a catalyst will increase the proportion of COCl₂ in the equilibrium mixture at constant temperature and pressure

• Reducing the equilibrium concentration of CO will increase the value of the equilibrium constant

• Raising the temperature from 373 K to 473 K will increase the value of the equilibrium constant

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

The following equilibrium was established in a container with volume V cm³ at 393 K and 200 kPa.

M₂(g) + R(g) ⇌ RM₂(g) ΔH = +150 kJ mol⁻¹

Which change would increase the yield of RM₂?

• change the pressure to 150 kPa

• change the temperature to 293 K

• remove RM₂ as it is formed

• change the volume of the vessel to 2V cm³

Tags

NGSS.HS-PS1-6