Unit 4.1: Mastery Check

Hydrogen and iodine are sealed in a 2 dm3 container. The reaction is allowed to reach equilibrium at 700 K according to the following balanced equation:

H2(g) + I2(g) ⇌ 2HI(g) ΔH > 0

1. Define reversible reaction.

Hydrogen and iodine are sealed in a 2 dm3 container. The reaction is allowed to reach equilibrium at 700 K according to the following balanced equation:

H2(g) + I2(g) ⇌ 2HI(g) ΔH > 0

2. Is forward reaction endothermic or exothermic

Hydrogen and iodine are sealed in a 2 dm3 container. The reaction is allowed to reach equilibrium at 700 K according to the following balanced equation:

H2(g) + I2(g) ⇌ 2HI(g) ΔH > 0

3. Explain the effect of the increase in temperature on the equilibrium position using Le Chatelier’s principle.

Hydrogen and iodine are sealed in a 2 dm3 container. The reaction is allowed to reach equilibrium at 700 K according to the following balanced equation:

H2(g) + I2(g) ⇌ 2HI(g) ΔH > 0

If the temperature of the system is decreased.

4. Explain the effect of the decrease in temperature on the equilibrium position using Le Chatelier’s principle.

Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:

H2(g) + S(s) ⇌ H2S(g) ∆H < 0

5. Define the term chemical equilibrium.

Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:

H2(g) + S(s) ⇌ H2S(g) ∆H < 0

6. Use Le Chatelier’s principle to explain how an increase in temperature will affect the number of moles of H2S at equilibrium.

Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:

H2(g) + S(s) ⇌ H2S(g) ∆H < 0

7. State Le Chatelier’s principle

Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:

H2(g) + S(s) ⇌ H2S(g) ∆H < 0

8. Is the reaction reversible? Explain your answer.

Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:

H2(g) + S(s) ⇌ H2S(g) ∆H < 0

9. Which reaction has more number gaseous moles?

Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:

H2(g) + S(s) ⇌ H2S(g) ∆H < 0

10. How will the increase in pressure affect the amount of H2S(g)? Explain your answer using Le Chatelier’s principle.

The following reaction reaches chemical equilibrium in a sealed container at 70 ºC.

N₂O₄ (g) ⇌ 2 NO₂ (g)

What is the effect of adding more N₂O₄ on the number of moles of NO₂ at equilibrium? Explain using Le Chatelier’s principle