The haber process
This presentation is the property of its rightful owner.
Sponsored Links
1 / 15

The Haber Process PowerPoint PPT Presentation


  • 195 Views
  • Uploaded on
  • Presentation posted in: General

The Haber Process. Oops!!!. N 2(g) + 3 H 2(g) D 2 NH 3(g). A brief summary of the Haber Process. The Haber Process combines nitrogen from the air with hydrogen derived mainly from natural gas (methane) into ammonia. The reaction is reversible and the production of ammonia is exothermic.

Download Presentation

The Haber Process

An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Presentation Transcript


The haber process

The Haber Process


The haber process

Oops!!!


The haber process

N2(g) + 3 H2(g)D 2 NH3(g)


A brief summary of the haber process

A brief summary of the Haber Process

  • The Haber Process combines nitrogen from the air with hydrogen derived mainly from natural gas (methane) into ammonia. The reaction is reversible and the production of ammonia is exothermic.

  • N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ


Some notes on the conditions

Some notes on the conditions

N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ

  • Pressure

  • According to Le Chatelier’s Principle, should a high or low pressure favour the production of ammonia?


Some notes on the conditions1

Some notes on the conditions

N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ

  • Pressure

  • A high pressure should favour the production of ammonia.


Some notes on the conditions2

Some notes on the conditions

N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ

  • Pressure

  • Economic Considerations

  • The cost of maintaining a high pressure reaction system increases with the amount of pressure. The usual pressure is about 200 atmospheres.


Some notes on the conditions3

Some notes on the conditions

N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ

  • Temperature

  • According to LeChatelier’s Principle, should a high or low temperature favour the production of ammonia?


Some notes on the conditions4

Some notes on the conditions

N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ

  • Temperature

  • A low temperature favours the production of ammonia.


Some notes on the conditions5

Some notes on the conditions

N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ

  • Temperature

  • Economic Considerations

  • An extremely low temperature slows the reactions so much that it takes too long for the system to produce much ammonia when starting with hydrogen and nitrogen. That is, it takes a long time to reach equilibrium.


Some notes on the conditions6

Some notes on the conditions

N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ

  • Temperature

  • Economic Considerations

  • The temperature normally used is about 450oC


Some notes on the conditions7

Some notes on the conditions

N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ

  • The Catalyst

  • Finely-divided iron is used. It has small amounts of magnesium and aluminum oxides added to increase its efficiency as a catalyst.


Some notes on the conditions8

Some notes on the conditions

N2(g) + 3 H2(g)D 2 NH3(g) DH = -92 kJ

  • Recycling

  • At each pass of the gases through the reactor, only about 15% of the nitrogen and hydrogen converts to ammonia. (This figure also varies from plant to plant.) By continual recycling of the unreacted nitrogen and hydrogen, the overall conversion is about 98%.


The haber process

http://www.chemguide.co.uk/physical/equilibria/haber.htmlHaber process


  • Login