Haber process
- Created by: gcsestudentof2019
- Created on: 14-03-19 18:05
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- Haber Process
- Nitrogen and hydrogen are needed to make Ammonia
- Nitrogen is obtained easily from the air
- Hydrogen can be obtained from hydrocarbons from sources such and natural gas or crude oil
- The reaction in reversible so nitrogen breaks down again into nitrogen and hydrogen.
- The reaction reaches an equalibrium
- conditions
- In industry ammonia is made at a pressure of 200 atm and temperature of 450? in the presence of an iron catalyst.
- Higher pressures favor the forward reaction
- Yield will be best when the pressure is high although it can be too expensive
- The forward reaction is exothermic which means increasing the temperature will actually move the equilibrium position the wrong way
- Yield will be greater at lower temperature
- The lower temperature means a lower rate of reaction so industry compromise
- Iron catalyst speed up the reaction and reduces costs
- makes the reaction go faster which gets it to the equilibrium proportion more quickly
- Catalyst doesn't affect the position of the equilibrium
- without the catalyst the temperature would have to be raised even further to get a quick enough reaction, and that would reduce the % yield even further.
- makes the reaction go faster which gets it to the equilibrium proportion more quickly
- Nitrogen and hydrogen are needed to make Ammonia
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