The chief commercial method of producing ammonia is by the Haber-Bosch process, which involves the direct reaction of elemental hydrogen and elemental nitrogen. Het Haber-Boschproces is de wijze waarop de meeste ammoniak wordt geproduceerd, door stikstofgas en waterstofgas zonder zuurstof in contact met een katalysator onder hoge druk te verhitten. Conversion: about 15% ammonia is produced per pass, but by re-circulating the gases yields of up to 98% are achieved. Asked by Wiki User. However, it would be extremely costly to build production plants that would be strong enough to withstand such a … To discover more about reaction rates, see rates of reaction . Who doesn't love being #1? Nitrogen (from air), and hydrogen (from natural gas (methane - C H 4) or the cracking of hydrocarbons), are reacted to make ammonia. OxNotes > GCSE/IGCSE Revision > IGCSE Chemistry > Industrial manufacture of Ammonia / Haber Process. Iron is used as catalyst now days, but the catalyst used in production is actually slightly more complicated than pure iron. Manufacture of ammonia by Haber’s process: When a mixture of nitrogen and hydrogen gas in the ratio 1:3 by volume is heated at a temperature of 450-500 0 C and 200-900 atmospheric pressure in the presence of iron as catalyst and molybdenum as promoter, ammonia gas is produced. The Haber process found other uses as well, particularly in military efforts in Germany during World War I. Using an effective iron catalyst can the reduce the cost of manufacturing ammonia by increasing the rate of reaction (more efficient) and lowering the energy requirements if the process can be done at lower temperatures (activation energy reduced). Haber first proposed the use of a high-pressure reaction technique. During Haber process: (a) A mixture of one volume of dry nitrogen gas and three volume of pure hydrogen gas are mixed and passed to the compressor and compressed to a pressure of about 200 atm. The Haber Process is always operated at very high pressures of about 200 atm in order to get high yields of ammonia. The Haber Process makes use of iron to speed up the reaction - but this doesn't improve the yield. It was the first industrial chemical process to use high pressure for a chemical reaction. The haber process is an example of a chemical industrial process that is used as part of the GCSE chemistry syllabus as a case study of how different conditions such as temperature and pressure can impact on the rate of reaction and also percentage yield. The commercial synthesis of ammonia began, not with the peaceful use of fertilizer, but with the necessities of war. Manufacture of nitrogen fertilizers uses about 5% of the world's natural gas production, equivalent to 1-2% of the world's annual energy consumption. Fertilizer generated from ammonia produced by the Haber process is estimated to be responsible for sustaining one-third of … Register to get answer. Haber Process is an Energy Glutton. It has potassium hydroxide added to it as a promoter so as to increase its efficiency. Ammonium nitrate is a very important fertiliser.. 1. Haber received much criticism for his involvement in the development of chemical weapons in pre-World War II Germany, both from contemporaries and from modern-day scientists. The catalyst is ground finely such that it has a large surface area of about 50 m 2 g-1, and the magnetite is reduced to iron. This process is called the Haber Process, or sometimes the Haber-Bosch Process after the two scientists. Haber developed the process at the beginning of the twentieth century, leading up to the First World War. 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