Industrial Processes Exam-style Questions | GCSE Chemistry Edexcel Higher Triple

Question 1

This question is about the production of ammonia from nitrogen and hydrogen.

State the name of the industrial process used to manufacture ammonia.

(0/1 marks)

Complete the balanced symbol equation to show the reaction between nitrogen and hydrogen to form ammonia.

(0/2 marks)

State the meaning of the ⇋ symbol.

(0/1 marks)

Iron is used as a catalyst in this process.

Explain the purpose of the iron catalyst.

(0/1 marks)

This process is completed at a temperature of 450°C.

Explain why a temperature of 450°C is used.

(0/3 marks)

Question 2

This question is about the Haber process and the production of ammonia.

Which of the following would increase the percentage yield of ammonia produced in the Haber process?

increase the pressure of the reaction

decrease the pressure of the reaction

include an iron catalyst

increase the temperature of the reaction

(0/1 marks)

Which of the following statements is correct when the reaction reaches equilibrium?

the reverse reaction starts to take place

the amounts of nitrogen, hydrogen and ammonia are equal

the amounts of nitrogen, hydrogen and ammonia become constant

the reaction stops

(0/1 marks)

The Haber process is carried out at 200 atmospheres.

Explain what effect a pressure lower than 200 atmospheres would have on:

the rate of attainment of equilibrium
the yield of ammonia.

(0/3 marks)

Explain the purpose of the iron catalyst in the Haber process.

(0/2 marks)

Question 3

This question is about the industrial process of making ammonia.

Ammonia is produced by reacting hydrogen with nitrogen.

The equation for the reaction is below.

N₂ + 3H₂ ⇋ 2NH₃

The production of ammonia is an exothermic reaction.

Explain the effect of increasing the temperature on the percentage yield of ammonia.

(0/2 marks)

State the name of the catalyst used in the Haber process.

(0/1 marks)

The reaction reaches a dynamic equilibrium.

What happens to the rate of the forward and backward reactions at dynamic equilibrium?

(0/1 marks)

State what happens to the position of the dynamic equilibrium and the yield of ammonia when the pressure is increased.

Explain why this shift occurs.

(0/4 marks)

Question 4

This question is about the Haber process.

Name the product produced by the Haber process.

(0/1 marks)

Explain why the product named in part a) can be extracted when the gases pass through a condenser.

(0/1 marks)

The chemical formula for the product of the Haber process is NH₃.

Draw a dot and cross diagram to represent a molecule of NH₃.

(0/3 marks)

State the type of bond found between the nitrogen and hydrogen atoms.

(0/1 marks)

Question 5

This question is about NPK fertilisers.

Some rocks contain calcium phosphate. When treated with acid they produce soluble salts, which can be used as fertilisers.

Write a word equation for the reaction between calcium phosphate and nitric acid.

(0/1 marks)

Fertilisers can be compared using their NPK value.

One fertiliser has an NPK value of 12:11:13.

Explain why this information is useful to farmers.

(0/2 marks)

Ammonia is used to make fertilisers.

Ammonia is formed during the Haber process. The equation for the Haber process is below.

N₂ + 3H₂ ⇋ 2NH₃

The Haber process takes place at a specific temperature and pressure.

State the temperature and pressure used in the Haber process.

(0/2 marks)

Describe how increasing the temperature would affect the percentage yield of ammonia.

(0/2 marks)