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Haber–bosch process

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Overview of the Haber Process for ammonia

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Haber–bosch process

  1. 1. Haber–Bosch process Ishmael Hutson 2A
  2. 2. How the process got its name • It was not until the early 20th century that Fritz Haber developed the first practical process to convert atmospheric nitrogen to ammonia, which is nutritionally available.
  3. 3. Importance • Prior to the discovery of the Haber process, ammonia had been difficult to produce on an industrial scale. Nitrogen fixation was already being done on an industrial scale using the Birkeland–Eyde process, but this is very energy-inefficient.
  4. 4. Uses of the product (Ammonia)
  5. 5. Amount Created Annually
  6. 6. Amount Created Annually by Region
  7. 7. Chemical reactions occurring N2 + 3 H2 → 2 NH3 (ΔH = −92.4 kJ·mol−1) High temperature favors the backward reactant (the low temperatures are too slow) [See ‘Typical Conditions’ Slide] The entire process is reversible
  8. 8. Typical conditions • Concentration of reactants: N2 + 3 H2 → 2 NH3 • Pressure: 4mol  2mol (favors products) • Volume: [amounts are proportioned to other constraints] • Temperature: 450-500 °C • Catalyst usage: Iron (Fe)
  9. 9. Bibliography • http://www.chemguide.co.uk/physical/equilibria/haber.html • http://www.greener-industry.org.uk/pages/ammonia/1ammoniaapq.htm • http://en.wikipedia.org/wiki/Ammonia_production • http://www.princeton.edu/~achaney/tmve/wiki100k/docs/Haber_process .html • http://en.wikipedia.org/wiki/History_of_the_Haber_process • http://en.wikipedia.org/wiki/Haber_process • http://www.princeton.edu/~hos/mike/texts/readmach/zmaczynski.htm • https://uk.answers.yahoo.com/question/index?qid=20090414151052AAcl mfp • http://en.citizendium.org/wiki/Haber_process • http://prezi.com/cwmh6eoaosl7/705-the-haber-process-or-haber-bosch-process/

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