- Equation: N₂ + 3H₂ ⇌ 2NH₃
- Forward reaction is exothermic
- Nitrogen source: air (78% N₂)
- Hydrogen source: natural gas (methane + steam)
- Temperature: ~450°C (compromise)
- Pressure: ~200 atm (compromise)
- Catalyst: iron
- Unreacted gases are recycled
- Main use: manufacture of fertilisers (NPK fertilisers)
- Equilibrium yield at 450°C/200 atm is only ~15–25% — recycling makes it viable
This key facts covers Key Facts within The Haber Process & Fertilisers for GCSE Chemistry. Revise The Haber Process & Fertilisers in Rates of Reaction for GCSE Chemistry with 6 exam-style questions and 6 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 8 of 13 in this topic. Use this key facts to connect the idea to the wider topic before moving on to questions and flashcards.
Practice questions for The Haber Process & Fertilisers
In the Haber process, where is the nitrogen obtained from?
State the equation for the Haber process and give the conditions used. Include the catalyst.
Quick recall flashcards
State the three conditions used in the Haber process.
1. Temperature: ~450°C
2. Pressure: ~200 atmospheres
3. Catalyst: iron
Unreacted N₂ and H₂ are recycled.
Write the equation for the Haber process.
N₂ + 3H₂ ⇌ 2NH₃
The ⇌ shows the reaction is reversible.
The forward reaction is exothermic.