The Haber Process
- Created by: joshbryan2000
- Created on: 13-03-18 19:02
View mindmap
- The Haber Process
- Produces ammonia which is used to make fertilisers
- Nitrogen+ Hydrogen --> Ammonia (+Heat)
- Reactants arent too expensive or difficult to obtain
- Nitrogen obtained from the air
- Hydrogen mainly comes from reacting methane from steam to form hydrogen and carbon dioxide
- Reactants are passed over an iron catalyst
- High temperatures and pressures are needed
- The reaction is reversible so some of the ammonia produced converts back to hydrogen and nitrogen and it eventually reaches a dynamic equillibrium
- High temperatures and pressures are needed
- Reactants arent too expensive or difficult to obtain
- Ammonia is formed as a gas but is cooled in a condenser
- Ammonia produced is then used to make ammonium nitrate - a nitrogen rich fertiliser
- The forward reaction is exothermic which means increasing the temperature will move equilibrium in the wrong way so the yield would be better at lower temperatures
- And from this, slower reactions means slower rate of reaction
- Higher pressures move the position of equilibrium to the products which maximises the percentage yield
Comments
No comments have yet been made