The Haber Process
- Created by: Jasmin
- Created on: 08-04-13 18:32
View mindmap
- The Haber Process
- Produces ammonia (NH3) to make fertilisers
- N2(g) + 3H2(g) = 2NH3(g) (+heat)
- Nitrogen from air (78%)
- Hydrogen from natural gas
- Purified first
- Nitrogen from air (78%)
- Purified first
- Reversible reaction
- Industrial conditions
- Pressure: 200 atmospheres
- This pressure because low yield but cheaper
- Temperature: 450C
- High for speed not for a better equilibrium
- Conditions chosen to give reasonable yield as quickly as possible
- Pressure: 200 atmospheres
- Gas Stream contains hydrogen and nitrogen
- Nitrogen/hydrogen are compressed to 200atm, heated at 450C (faster, higher rate of reaction)
- Reaction vessel contains iron catalyst
- Mixture of gases emerging from reactor cooled. Ammonia liquefies and is separated
- Unreacted nitrogen and hydrogen are returned to the reaction vessel - recycled nothing wasted
- Mixture of gases emerging from reactor cooled. Ammonia liquefies and is separated
- Reaction vessel contains iron catalyst
- Nitrogen/hydrogen are compressed to 200atm, heated at 450C (faster, higher rate of reaction)
- PRESSURE
- 4 molecules on one side and 2 on the other
- Volume of reactants greater than volume of products
- Increase pressure, shift equilibrium to right - more ammonia produced
- To get maximum yield need increase pressure - lots of energy needed - expensive
- 4 molecules on one side and 2 on the other
- TEMPERATURE
- Forward reaction exothermic
- Low temperature, will increase amount of ammonia in reaction
- Mixture at equilibrium
- Low temperature, will increase amount of ammonia in reaction
- Forward reaction exothermic
Comments
No comments have yet been made