New
New
Year 11
•
OCR
•
Higher
Industrial equilibria: Haber Process
I can describe the Haber Process for the production of ammonia, explain the significance of equilibrium in this industrial process, and describe the conditions used.
New
New
Year 11
•
OCR
•
Higher
Industrial equilibria: Haber Process
I can describe the Haber Process for the production of ammonia, explain the significance of equilibrium in this industrial process, and describe the conditions used.
These resources will be removed by end of Summer Term 2025.
Switch to our new teaching resources now - designed by teachers and leading subject experts, and tested in classrooms.
Lesson details
Key learning points
- In a reversible reaction the desired product needs to be continuously removed from the reaction.
- Natural gas is a feedstock for industrial production of ammonia.
- Hydrogen, one of the raw materials in ammonia production, is produced from natural gas and steam.
- In industry, the Haber process is typically performed at 150-300 atmospheres, 400-450°C, with an iron catalyst.
- Ammonia production is energy-intensive and releases large amounts of carbon dioxide, contributing to global emissions.
Keywords
Natural gas - A mixture of gases which are rich in hydrocarbons, consisting largely of methane.
Feedstock - Refers to the raw materials used in chemical processes to produce other substances.
Raw material - The starting materials used to make products are known as the raw materials.
Haber process - An industrial method for producing ammonia from nitrogen and hydrogen.
Common misconception
Students find it difficult to understand why continuous removal of ammonia is required to increase yield.
Highlight that the Haber Process is a dynamic equilibrium. If ammonia is not continuously removed, the equilibrium will shift back towards the reactants, reducing the yield.
Incorporate interactive activities, such as role-playing the process with students acting as reactants and products to visually demonstrate the concept of continuous removal of ammonia.
Teacher tip
Equipment
None required.
Licence
This content is © Oak National Academy Limited (2024), licensed on Open Government Licence version 3.0 except where otherwise stated. See Oak's terms & conditions (Collection 2).
Lesson video
Loading...
Starter quiz
Download starter quiz
6 Questions
Q1.
Which of these statements are required for a dynamic equilibrium to be established?
all particles to be in the gas state
Correct answer: closed system
closed system
equal amounts of reactants and products
Correct answer: equal reaction rates for forward and backward reaction
equal reaction rates for forward and backward reaction
Correct answer: reversible reaction
reversible reaction
Q2.
The direction of reversible reactions can be influenced by changing conditions, e.g. an exothermic reaction is favoured by lowering the temperature, but at the same time the reaction rate .
Correct Answer: decreases, slows down, becomes slower
decreases, slows down, becomes slower
Q3.
True or false? At dynamic equilibrium all bonds between all atoms need to be broken and new bonds need to be formed.
True
Correct answer: False
False
Q4.
Consider this reaction:
CaCO$$_3(s)$$ ⇌ CaO$$_(s)$$ + CO$$_2(g)$$
What would happen if this was done in an open system?
Correct answer: the carbon dioxide gas leaves and the backward reaction can no longer occur
the carbon dioxide gas leaves and the backward reaction can no longer occur
the forward reaction stops and you are left with only calcium carbonate
there will be an equilibrium with only calcium carbonate and calcium oxide
Q5.
Industrial chemistry is different from chemistry in a school lab or a research lab. The of the work is larger; therefore the risks and safety measures are larger too.
Correct Answer: scale, size
scale, size
Q6.
What is wrong with the graph below?
Correct answer: at equilibrium the rates of the forward and backward reaction must be equal
at equilibrium the rates of the forward and backward reaction must be equal
the graphs for the forward and backward reaction have been swapped
the reactants and products should be mentioned in a rate of reaction graph
Exit quiz
Download exit quiz
6 Questions
Q1.
Traditional ammonia produced through the Haber process is called grey ammonia. Match the following terms with the correct definitions.
Correct Answer:blue ammonia,traditional ammonia, but involving carbon capture of the emissions
blue ammonia -
traditional ammonia, but involving carbon capture of the emissions
Correct Answer:green ammonia,ammonia produced through 100% renewable and carbon-free processes
green ammonia -
ammonia produced through 100% renewable and carbon-free processes
Q2.
Grey ammonia, through the Haber process, is the most common. Industrial production requires high pressure, large but safe apparatus, and a lot of energy. Which of the following statements are correct?
Correct answer: ammonia production is a reversible reaction
ammonia production is a reversible reaction
Correct answer: at equilibrium, there is ammonia but also nitrogen and hydrogen
at equilibrium, there is ammonia but also nitrogen and hydrogen
Correct answer: high pressures require strong equipment and a lot of energy
high pressures require strong equipment and a lot of energy
Correct answer: high temperature is needed to increase the rate of reaction
high temperature is needed to increase the rate of reaction
nitrogen and hydrogen are wasted when ammonia is condensed and removed
Q3.
The conditions for the Haber process are:
a compressor
a cooling tank
Correct answer: an iron catalyst
an iron catalyst
Correct answer: a pressure of 200 atm
a pressure of 200 atm
Correct answer: a temperature of 450$$^o$$C
a temperature of 450$$^o$$C
Q4.
In industry, ammonia is made with nitrogen from air, and hydrogen from natural gas, using the Haber process. Put the steps in order:
1 - nitrogen (from air) and hydrogen (from natural gas) are brought together
1
- nitrogen (from air) and hydrogen (from natural gas) are brought together
2 - a compressor increases the pressure to 200 atm
2
- a compressor increases the pressure to 200 atm
3 - the gas mixture is heated to 450$$^o$$C in a tank containing iron catalyst
3
- the gas mixture is heated to 450$$^o$$C in a tank containing iron catalyst
4 - the mixture enters a cooling tank so that ammonia is condensed
4
- the mixture enters a cooling tank so that ammonia is condensed
5 - liquid ammonia is collected
5
- liquid ammonia is collected
6 - unreacted nitrogen and hydrogen are recycled to make more ammonia
6
- unreacted nitrogen and hydrogen are recycled to make more ammonia
Q5.
Clara, Haber’s wife, was a chemist and pacifist, believing war and violence are unjustifiable. She felt her husband’s research was a “perversion of the ideals of science”. What made her feel that way?
Correct answer: she felt passionately that science must not be used for chemical warfare
she felt passionately that science must not be used for chemical warfare
she thought making ammonia was a bad influence on people’s health
she was forced to stop being a chemist because he was already a chemist
Q6.
As the global population continues to grow, production of ammonia will continue. What is ammonia not used for?
burning in engines
chemical store for renewable energy
Correct answer: cooling household refrigerators
cooling household refrigerators
making cleaning products
making fertilisers for agriculture