Unit 4.1 Mastery Check
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Question 1 of 11
1. Question
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
1.1 Define reversible reaction.
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This response will be reviewed and graded after submission.
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Question 2 of 11
2. Question
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
1.2 Is forward reaction endothermic or exothermic
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Question 3 of 11
3. Question
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
1.3 Explain the effect of the increase in temperature on the equilibrium position using Le Chatelier’s principle
Hint
Follow steps given in section
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Question 4 of 11
4. Question
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
1.4 If the temperature of the system is decreased
1.4.1 Explain the effect of the decrease in temperature on the equilibrium position using Le Chatelier’s principle.
Hint
Follow steps given in section
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Question 5 of 11
5. Question
Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:
H2(g) + S(s) ⇌ H2S(g) ∆H < 0
Define the term chemical equilibrium.
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Question 6 of 11
6. Question
Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:
H2(g) + S(s) ⇌ H2S(g) ∆H < 0
Use Le Chatelier’s principle to explain how an increase in temperature will affect the number of moles of H2S at equilibrium
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Question 7 of 11
7. Question
Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:
H2(g) + S(s) ⇌ H2S(g) ∆H < 0
State Le Chatelier’s principle
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Question 8 of 11
8. Question
Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:
H2(g) + S(s) ⇌ H2S(g) ∆H < 0
Is the reaction reversible? Explain your answer
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Question 9 of 11
9. Question
Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:
H2(g) + S(s) ⇌ H2S(g) ∆H < 0
Which reaction has more number gaseous moles?
Hint
Follow steps given in sub-heading D when dealing with change in pressure
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Question 10 of 11
10. Question
Hydrogen gas, H2(g), reacts with sulphur powder, S(s), according to the following balanced equation:
H2(g) + S(s) ⇌ H2S(g) ∆H < 0
How will the increase in pressure affect the amount of H2S(g)? Explain your answer using Le Chatelier’s principle.
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Question 11 of 11
11. Question
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.