Formation of Ammonia (Haber Process)
N2 + 3H2 → 2NH3
Übersicht
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.
Teilnehmer
Alltägliches Beispiel
Fertilizers that feed roughly half the world's population are produced from ammonia made by this process.
Industrielle Bedeutung
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.
Eigenschaften
- Typ
- Synthesis
- Reversibel
- Ja
- Energie
- Exotherm
- ΔH
- -92,4 kJ/mol
- Ea
- 230,0 kJ/mol
- Katalysator
- Iron with potassium and aluminum oxide promoters
Energieprofil-Diagramm
Exotherme Reaktion — Energie wird freigesetzt
Verwandte Reaktionen
Formation of Nitrogen Dioxide
Formation of Potassium Chloride
Formation of Sodium Bicarbonate
Formation of Sodium Peroxide
Formation of Silicon Dioxide
Formation of Tungsten Carbide
Formation of Copper(II) Sulfide
Formation of Sulfur Dioxide
Formation of Hydrogen Sulfide
Formation of Carbon Monoxide
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.