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Chemistry AQA GCSE:
Haber Process + Fertilisers

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Q1-11: Ammonia is produced industrially in the Haber Process. The reaction is exothermic.

N2(g)   +   3H2(g)2NH3(g)

ammonia molecule
1. What is the main source of the hydrogen used in the Haber Process?
  • A.   natural gas
  • B.   water
  • C.   air
  • D.   hydrochloric acid
2. What is the main source of the nitrogen used in the Haber Process?
  • A.   fertilizers
  • B.   natural gas
  • C.   air
  • D.   coal
3. What happens to the unreacted nitrogen and hydrogen gases in the Haber Process?
  • A.  they are collected and sold
  • B.   they are recycled back into the reactor
  • C.   they are collected and used at a later date
  • D.    they are thrown away as waste products
4. Approximately what temperature in degrees celcius is used in the Haber Process?
5. Why is a higher temperature NOT used in the Haber Process?
  • A.   The equilibrium would move to the left reducing the amount of ammonia
  • B.   The equilibrium would move to the right increasing the amount of ammonia
  • C.   The rate of reaction would be slower at a higher temperature.
  • D.   The rate of reaction would be faster at a higher temperature.
6. Why is a lower temperature NOT used in the Haber Process?
  • A.   The equilibrium would move to the left reducing the amount of ammonia
  • B.   The equilibrium would move to the right increasing the amount of ammonia
  • C.   The rate of reaction would be too slow at a lower temperature.
  • D.   The rate of reaction would be too fast at a lower temperature.
7. Approximately what pressure is used in the Haber Process?

8. What would happen to the rate at which equilibrium is reached, and the position of equilibrium, if a lower pressure was used?

  Rate Position of equilibrium
A increases Moves to the right
B increases Moves to the left
C decreases Moves to the right
D decreases Moves to the left
9. Why is a higher pressure NOT used in the Haber Process?
  • A.   The equilibrium would move to the right increasing the amount of ammonia
  • B.   The equilibrium would move to the left decreasing the amount of ammonia
  • C.   High pressures are expensive to maintain
  • D.   The rate of reaction would increase
10. A catalyst is used in the Haber Process. What material is used for the catalyst?
  • A.   iron
  • B.   nickel
  • C.   copper
  • D.   manganese oxide

11. What effect does the catalyst have on the rate of reaction and the position of equilibrium?

  Rate Position of equilibrium
A increases Moves to the right
B increases No effect
C decreases Moves to the right
D decreases No effect