R2.3 How Far? Le Chatelier's Principle

What will happen if the pressure is increased in the following reaction mixture at equilibrium? CO₂ (g) + H₂O ⇒ H⁺ (aq) + HCO₃^- (aq)

• The equilibrium will shift to the right.

• The equilibrium will shift to the left.

• There will be no shift.

N₂O₄ (g) ⇌ 2NO₂ (g) ΔH = +58 kJ mol^-1

Which changes shift the position of equilibrium to the right?

I. Increasing the temperature

II. Decreasing the pressure

III. Adding a catalyst

• I and II only

• I and III only

• II and III only

• I, II and III

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

What is the equilibrium constant expression, Kc, for the following reaction?

2NH₃ + 2O₂ ⇌ N₂O(g) + 3H₂O

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Tags

NGSS.HS-PS1-2

What happens when the temperature of the following equilibrium system is increased?

CO(g) + 2H₂(g) ⇌ CH₃OH(g) ΔΗ = -91kJ

• A

• B

• C

• D

Tags

NGSS.HS-PS1-5

What is the effect of increasing temperature on the equilibrium?

• A.

• B.

• C.

• D.

Tags

NGSS.HS-PS1-5

State the effect of an increase in the total pressure on the equilibrium constant, K.

• Increases

• Decreases

• Remains Constant

Tags

NGSS.HS-PS1-6

Which change will favour the reverse reaction in the equilibrium?

• Adding a catalyst.

• Adding H⁺

• Increasing the concentration of Cr₂O₇^2-

• Increasing the temperature of the solution

Tags

NGSS.HS-PS1-5

What is the impact of decreasing the volume of the equilibrium mixture at a constant temperature?

CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)

• The amount of H₂(g) remains the same but its concentration decreases.

• The forward reaction is favoured.

• The reverse reaction is favoured.

• The value of K remains constant.

What is the equilibrium constant expression, Kc, for the formation of hydrogen iodide from its elements? H₂(g) + I₂(g) → 2HI(g)

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Tags

NGSS.HS-PS1-6

What would have happened at time = t₁ for the reaction:

2HI ⇌ H₂ + I₂

• Addition of H₂

• Addition of HI

• C. addition of a catalyst

• D. a decrease in volume

Tags

NGSS.HS-PS1-5