Formation of Ammonia (Haber Process)
N2 + 3H2 → 2NH3
Overview
The Haber-Bosch process combines nitrogen from the atmosphere with hydrogen gas to produce ammonia. This reversible reaction requires high temperatures (400-500 C) and pressures (150-300 atm) along with an iron catalyst. It is arguably the most important industrial chemical reaction ever developed.
Participants
Everyday Example
Fertilizers that feed roughly half the world's population are produced from ammonia made by this process.
Industrial Importance
The Haber-Bosch process produces over 150 million tonnes of ammonia annually, essential for fertilizers, explosives, and numerous chemical syntheses. It consumes about 1-2% of global energy production.
Properties
- Type
- Synthesis
- Reversible
- Yes
- Energy
- Exothermic
- ΔH
- -92.4 kJ/mol
- Ea
- 230.0 kJ/mol
- Catalyst
- Iron with potassium and aluminum oxide promoters
Energy Profile Diagram
Exothermic reaction — energy is released
Related Reactions
Fischer-Tropsch Synthesis (General)
Formation of Aluminum Oxide
Formation of Barium Oxide
Formation of Barium Sulfate
Formation of Beryllium Oxide
Formation of Cadmium Oxide
Formation of Calcium Carbonate from Oxides
Formation of Calcium Hydroxide
Formation of Calcium Oxide (Quicklime)
Formation of Carbon Dioxide from Elements
Frequently Asked Questions
What is the equation for Formation of Ammonia (Haber Process)?
The balanced equation is: N₂ + 3H₂ → 2NH₃.
What type of reaction is Formation of Ammonia (Haber Process)?
Formation of Ammonia (Haber Process) is a synthesis reaction. It is reversible under certain conditions.
Is Formation of Ammonia (Haber Process) exothermic or endothermic?
Formation of Ammonia (Haber Process) is exothermic (releases energy). The enthalpy change (ΔH) is -92.4 kJ/mol.
What conditions are needed for Formation of Ammonia (Haber Process)?
This reaction requires a catalyst (Iron with potassium and aluminum oxide promoters) and activation energy of 230.0 kJ/mol.