Formation of Ammonia (Haber Process)
N2 + 3H2 → 2NH3
Visão geral
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.
Participantes
Exemplo do cotidiano
Fertilizers that feed roughly half the world's population are produced from ammonia made by this process.
Importância industrial
O processo Haber-Bosch produz mais de 150 milhões de toneladas de amoníaco anualmente, essencial para fertilizantes que alimentam metade da população mundial. É responsável por cerca de 1-2% do consumo energético mundial.
Propriedades
- Tipo
- Synthesis
- Reversível
- Sim
- Energia
- Exotérmico
- ΔH
- -92,4 kJ/mol
- Ea
- 230,0 kJ/mol
- Catalisador
- Iron with potassium and aluminum oxide promoters
Diagrama de perfil de energia
Reação exotérmica — energia é liberada
Reações relacionadas
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.