- Haber process
- The industrial process for manufacturing ammonia from nitrogen and hydrogen using an iron catalyst at ~450°C and ~200 atm.
- Reversible reaction
- A reaction in which the products can react to re-form the original reactants; shown by ⇌.
- Equilibrium
- The state in a reversible reaction where the forward and reverse reaction rates are equal and concentrations remain constant.
- Le Chatelier's principle
- If a change is made to a system at equilibrium, the position of equilibrium shifts to oppose that change.
- Compromise conditions
- Conditions chosen in an industrial process to balance yield, rate, and economic cost rather than optimising any single factor.
This definitions covers Key Terms 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 7 of 13 in this topic. Make sure you can use the exact wording confidently, because definition marks are often lost through vague language.
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
Write the equation for the Haber process.
N₂ + 3H₂ ⇌ 2NH₃
The ⇌ shows the reaction is reversible.
The forward reaction is exothermic.
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.