Le Chatelier's Principle and the Haber Process (HT) Quiz
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5 questions, one answer each
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1. According to Le Chatelier's Principle, how does a system at equilibrium respond to an imposed change?
- A. It shifts to reinforce the change
- B. It shifts to counteract the change
- C. It stops reacting entirely
- D. It has no response
2. In the Haber process (N₂ + 3H₂ ⇌ 2NH₃), why does increasing pressure increase the yield of ammonia?
- A. There are more gas molecules on the product side
- B. There are fewer gas molecules on the product side
- C. Pressure has no effect on this reaction
- D. Ammonia is a liquid at the reaction conditions
3. The forward reaction of the Haber process is exothermic. What effect would a lower temperature have on the position of equilibrium?
- A. It would favour the reverse (endothermic) reaction
- B. It would favour the forward (exothermic) reaction, increasing ammonia yield
- C. It would have no effect on equilibrium position
- D. It would only affect the rate, not the yield
4. Why does the Haber process use 450 °C rather than a much lower temperature that would give a higher equilibrium yield?
- A. Lower temperatures are too expensive to achieve
- B. A lower temperature would make the reaction rate too slow for industrial use
- C. Iron catalysts do not work below 450 °C
- D. Ammonia decomposes below 450 °C
5. What effect does increasing the concentration of ammonia have on the Haber process equilibrium?
- A. It shifts equilibrium to produce more ammonia
- B. It shifts equilibrium towards nitrogen and hydrogen
- C. It has no effect on the equilibrium position
- D. It stops the reaction completely