Le Chatelier Principle

Equilibrium for 2CrO₄^2- + 2H⁺ → Cr₂O₇^2- + H₂O. What happen when H⁺ ion are added to the system?

• Position of equilibrium will shift to left

• Color of system will turn from orange to yellow

• K_c will be higher

• Equilibrium will shift to right to decrease the added H⁺ ion

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

For CoCI₄^2- +6H₂O →Co(H₂O)₆²⁺ + 4CI^-. What happen when CI^- ions are added?

• Position of equilibrium will shift to right

• Color of system will turn from blue to pink

• Concentration of reactants and products remain unchanged

• Equilibrium shift to left to reduce the added CI^- ions

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 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

Tags

NGSS.HS-PS1-4

NGSS.HS-PS1-5

What does Le Chatelier's Principle state about a system at equilibrium when it is subjected to a change in concentration, temperature, or pressure?

• The system will shift in the direction that increases the change.

• The system will remain unchanged.

• The system will shift in the direction that opposes the change.

• The system will shift in random directions until a new equilibrium is established.

Tags

NGSS.HS-PS1-5

According to Le Chatelier's Principle, if the concentration of a reactant is increased, the equilibrium of the reaction will:

• Shift to the left, favoring the formation of reactants

• Shift to the right, favoring the formation of products

• Remain unchanged

• Increase the overall reaction rate without shifting the equilibrium

Tags

NGSS.HS-PS1-5

2SO₂(g)+O₂(g)⇌2SO₃(g)
Adding SO₂(g) will

• shift equilibrium right

• shift equilibrium left

• increase rate of reaction

• have no change

Tags

NGSS.HS-PS1-5

2SO₂(g)+O₂(g)⇌2SO₃(g)

Removing O₂(g) will

• shift equilibrium right

• shift equilibrium left

• increase pressure

• have no change

Which of the following statements is TRUE regarding the effect of pressure on the equilibrium of a gaseous reaction?

• Increasing pressure always shifts the equilibrium to the side with more gas molecules

• Decreasing pressure always shifts the equilibrium to the side with fewer gas molecules

• Increasing pressure shifts the equilibrium to the side with fewer gas molecules

• Pressure has no effect on the equilibrium of a gaseous reaction

In the context of Le Chatelier's Principle, how does the addition of a catalyst affect a chemical equilibrium?

• It shifts the equilibrium to the right

• It shifts the equilibrium to the left

• It does not shift the equilibrium but increases the rate at which equilibrium is achieved

• It increases the equilibrium constant

Tags

NGSS.HS-PS1-6