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 between nitrogen and hydrogen to make ammonia, NH₃.
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Answer
The balanced equation for the Haber process is:
N2(g)+3H2(g)⇌2NH3(g).
This equation indicates the reactants (nitrogen and hydrogen) on the left and the product (ammonia) on the right.
Step 2
Which row shows the typical conditions of temperature and pressure used in the Haber process?
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Answer
The correct row is D, which shows a temperature of 450 °C and a pressure of 200 atmospheres. These conditions are typical for maximizing ammonia production in the Haber process.
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. It increases the rate of the reaction between nitrogen and hydrogen, allowing ammonia to be produced more efficiently without being consumed in the reaction.
Step 4
Explain how the position of equilibrium changes if the temperature is decreased.
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Answer
According to Le Chatelier's principle, if the temperature of an exothermic reaction is decreased, the equilibrium position will shift to favor the formation of products in order to produce heat. Therefore, in the case of the Haber process, decreasing the temperature will shift the equilibrium to the right, resulting in an increased yield of ammonia, NH₃.
