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Chemistry Quiz - Production of Ammonia 1 (Questions)

Ammonia is made on a huge scale for fertilisers. This GCSE Chemistry quiz explores the Haber process, equilibrium, and how conditions change yield and rate in industry.

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Fascinating Fact:

Higher pressure increases the yield of ammonia because there are fewer gas molecules on the product side. Industrial processes use high pressure as a compromise between yield and cost.

In GCSE Chemistry, the Haber process shows how nitrogen and hydrogen react to form ammonia in a reversible reaction. Because the reaction reaches equilibrium, the amounts of reactants and products depend on the conditions used. You learn why industry uses a catalyst and carefully chosen temperature and pressure to make ammonia quickly enough, at a reasonable cost, while still getting a good yield for making fertilisers and other useful chemicals.

Key Terms

  • Haber process: An industrial method of making ammonia from nitrogen and hydrogen in a reversible reaction.
  • Equilibrium: The point where forward and reverse reactions happen at the same rate, so overall amounts stay constant.
  • Catalyst: A substance that speeds up a reaction without being used up, by lowering the activation energy.

Frequently Asked Questions

What is the Haber process in GCSE Chemistry?

The Haber process is the industrial production of ammonia by reacting nitrogen with hydrogen in a reversible reaction. The reaction is carried out using an iron catalyst under controlled temperature and pressure.

Why is the Haber process reversible and what does that mean?

The Haber process is reversible because ammonia can break down back into nitrogen and hydrogen as well as being formed. This means the reaction reaches equilibrium, so the yield depends on the conditions used.

What conditions are used in the Haber process and why?

Industry uses a moderate temperature and high pressure with an iron catalyst. These conditions are chosen as a compromise so the reaction is fast enough and the yield is high enough without costing too much energy.

Try These Related Quizzes

1. Plants need nitrogen to grow. How do we ensure that plants get the nitrogen that they need?
[ ] Increase the amount of nitrogen in the air around the plants
[ ] Increase the amount of nitrogen in the soil around the plants' roots
[ ] Increase the amount of nitrates in the soil around the plants' roots
[ ] Increase the amount of nitrates in the air around the plants
2. Why can't plants use the nitrogen in the air?
[ ] It's unreactive
[ ] It can't get into their leaves
[ ] It doesn't dissolve in water
[ ] It can't get into their roots
3. What is the name of the industrial process which turns nitrogen and hydrogen into ammonia?
[ ] Nitrogen process
[ ] Contact process
[ ] Haber process
[ ] Ammonia process
4. The raw materials for the Haber process are...
[ ] nitrogen from the air
hydrogen from water
[ ] nitrogen from the sea
hydrogen from natural gas
[ ] nitrogen from ammonia
hydrogen from the air
[ ] nitrogen from the air
hydrogen from natural gas
5. Name the catalyst used in the Haber process.
[ ] Platinum
[ ] Iron
[ ] Vanadium (V) oxide
[ ] Nickel catalyst
6. Pick the temperature at which the Haber process takes place most efficiently.
[ ] 20oC
[ ] 200oC
[ ] 450oC
[ ] 900oC
7. Pick the pressure at which the Haber process is carried out.
[ ] 200 atmospheres
[ ] 100 atmospheres
[ ] 50 atmospheres
[ ] 1 atmosphere
8. The reaction that produces ammonia is reversible. What does this mean?
[ ] The ammonia breaks down again into hydrogen and nitrogen
[ ] The ammonia doesn't break down into hydrogen and nitrogen
[ ] Ammonia is produced but then it reproduces itself
[ ] The hydrogen and nitrogen never stop reacting
9. To reduce the breaking down of ammonia into nitrogen and hydrogen, what is done?
[ ] Water is added to the ammonia
[ ] The nitrogen and hydrogen are forced to stop reacting
[ ] The ammonia is added to the hydrogen and nitrogen
[ ] The ammonia is cooled and removed
10. Pick the correct equation for the Haber process.
[ ] N2 + 3H2 → 2NH3
[ ] N2 + 3H2 → NH3
[ ] N2 + 3H2 ⇌ 2NH3
[ ] N2 + H2 ⇌ NH3

You can find more about this topic by visiting BBC Bitesize - Reversible reactions, ammonia and the Haber process [Chemistry only]

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Chemistry Quiz - Production of Ammonia 1 (Answers)
1. Plants need nitrogen to grow. How do we ensure that plants get the nitrogen that they need?
[ ] Increase the amount of nitrogen in the air around the plants
[ ] Increase the amount of nitrogen in the soil around the plants' roots
[x] Increase the amount of nitrates in the soil around the plants' roots
[ ] Increase the amount of nitrates in the air around the plants
Plants absorb nitrates from the soil through their roots
2. Why can't plants use the nitrogen in the air?
[x] It's unreactive
[ ] It can't get into their leaves
[ ] It doesn't dissolve in water
[ ] It can't get into their roots
Leguminous plants like peas and beans have bacteria that grow in nodules on their roots. These bacteria convert atmospheric nitrogen into nitrates that the plant can use
3. What is the name of the industrial process which turns nitrogen and hydrogen into ammonia?
[ ] Nitrogen process
[ ] Contact process
[x] Haber process
[ ] Ammonia process
The process was invented by a German chemist called Fritz Haber
4. The raw materials for the Haber process are...
[ ] nitrogen from the air
hydrogen from water
[ ] nitrogen from the sea
hydrogen from natural gas
[ ] nitrogen from ammonia
hydrogen from the air
[x] nitrogen from the air
hydrogen from natural gas
The hydrogen can also be obtained from some cracking reactions in the oil industry
5. Name the catalyst used in the Haber process.
[ ] Platinum
[x] Iron
[ ] Vanadium (V) oxide
[ ] Nickel catalyst
Catalysts are not used up during the reaction
6. Pick the temperature at which the Haber process takes place most efficiently.
[ ] 20oC
[ ] 200oC
[x] 450oC
[ ] 900oC
Lower temperatures give higher yields of ammonia but too slowly for it to be economically viable. Higher temperatures produce the ammonia faster but in too small a quantity to be economically viable
7. Pick the pressure at which the Haber process is carried out.
[x] 200 atmospheres
[ ] 100 atmospheres
[ ] 50 atmospheres
[ ] 1 atmosphere
This is 200 times the size of atmospheric pressure
8. The reaction that produces ammonia is reversible. What does this mean?
[x] The ammonia breaks down again into hydrogen and nitrogen
[ ] The ammonia doesn't break down into hydrogen and nitrogen
[ ] Ammonia is produced but then it reproduces itself
[ ] The hydrogen and nitrogen never stop reacting
A reversible reaction goes in both ways, from reactants to products and back again
9. To reduce the breaking down of ammonia into nitrogen and hydrogen, what is done?
[ ] Water is added to the ammonia
[ ] The nitrogen and hydrogen are forced to stop reacting
[ ] The ammonia is added to the hydrogen and nitrogen
[x] The ammonia is cooled and removed
This forces the reaction to go in the forwards direction
10. Pick the correct equation for the Haber process.
[ ] N2 + 3H2 → 2NH3
[ ] N2 + 3H2 → NH3
[x] N2 + 3H2 ⇌ 2NH3
[ ] N2 + H2 ⇌ NH3
A balanced equation has the same types of atom in the same numbers on both sides. In this case, there are two nitrogen atoms and six hydrogen atoms on the two sides of the equation. If you count up the numbers you quickly spot that there are two possibilities. Only one shows a reversible reaction.
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