5 (a) Ammonia is manufactured in the Haber process by the reversible reaction between nitrogen and hydrogen - Edexcel - GCSE Chemistry - Question 5 - 2023 - Paper 1
Question 5
5 (a) Ammonia is manufactured in the Haber process by the reversible reaction between nitrogen and hydrogen.
(i) Write the balanced equation for the reversible reac... show full transcript
Worked Solution & Example Answer:5 (a) Ammonia is manufactured in the Haber process by the reversible reaction between nitrogen and hydrogen - Edexcel - GCSE Chemistry - Question 5 - 2023 - Paper 1
Step 1
Write the balanced equation for the reversible reaction.
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Answer
The balanced equation for the synthesis of ammonia in the Haber process is given by:
N2(g)+3H2(g)⇌2NH3(g)
This equation indicates that one molecule of nitrogen reacts with three molecules of hydrogen to produce two molecules of ammonia.
Step 2
Which row shows the typical conditions of temperature and pressure used in the Haber process?
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Answer
The typical conditions of temperature and pressure used in the Haber process are shown in Row D:
Temperature: 450 °C
Pressure: 200 atmospheres.
These conditions optimize the yield of ammonia.
Step 3
State the purpose of the iron.
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Answer
The purpose of the iron in the Haber process is to act as a catalyst. This means it helps to speed up the reaction without being consumed in the process, allowing the nitrogen and hydrogen to combine more quickly to form ammonia.
Step 4
Explain how the position of equilibrium changes if the temperature is decreased.
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Answer
If the temperature is decreased, the position of equilibrium will shift to the right, favoring the production of ammonia. This is because the formation of ammonia is an exothermic reaction, and according to Le Châtelier's principle, lowering the temperature will shift the equilibrium in the direction that produces heat, thus favoring the production of the product (NH₃).
