R2.3 How Far? Le Chatelier's Principle

Front

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

Back

The equilibrium will shift to the right.

Front

Which changes shift the position of equilibrium to the right for the reaction N₂O₄ (g) ⇌ 2NO₂ (g) with ΔH = +58 kJ mol⁻¹? Options: I. Increasing the temperature, II. Decreasing the pressure, III. Adding a catalyst.

Back

I and II only

Front

What happens when the temperature of the following equilibrium system is increased?
CO(g) + 2H₂(g) ⇌ CH₃OH(g) ΔΗ = -91kJ

Back

A

Front

What is the effect of increasing temperature on the equilibrium?

Back

A.

Front

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

Back

Remains Constant

Front

Which change will favour the reverse reaction in the equilibrium?

Back

Increasing the temperature of the solution

Front

Impact of decreasing the volume of the equilibrium mixture at constant temperature for the reaction: CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g)

Back

The value of K remains constant.

Front

What would have happened at time = t₁ for the reaction: 2HI ⇌ H₂ + I₂?

Back

Addition of HI

Front

Which stresses shift the equilibrium right? Options: decrease in temperature and volume, increase in temperature and decrease in volume, decrease in temperature and increase in volume, increase in temperature and increase in volume.

Back

increase in temperature and increase in volume

Front

Some CO₂ is added to the equilibrium system at constant volume and a new equilibrium is established. Compared to the original equilibrium, what happens to the rates of the forward and reverse reactions?

Back

Both forward & reverse rates increase