It is also known as the Haber\n– Bosch process or Synthetic Ammonia process. Haber\u2019s process is considered as\none the most beneficial and efficient industrial processes to be used for the\nproduction of ammonia which is a colorless gas having a distinct odor. In the 20th<\/sup>\ncentury Fritz Haber, a German chemist developed a high-pressure devices and\nappropriate catalysts to carry out the process on a laboratory scale. He\nreceived the Nobel prize for his great achievement of manufacturing ammonia\neconomically feasible.<\/p>\n\n\n\n Before this in 1910\nanother chemist Carl Bosch created a design and a machine for the production on\na large industrial level. It was, however, an important development in this\nfield. He was hired by a German company BASF which assigned him the task of\nmanufacturing the ammonia on an industrial level. <\/p>\n\n\n\n Before the development of\nthe Haber process, it was very difficult to produce ammonia on an industrial\nscale with early methods i.e. Birkeland-Eyde process and Frank-Caro process\nboth being highly inefficient.<\/p>\n\n\n\n Ammonia (NH3<\/sub>)\nis considered as one of the very essential hydride that is present in an\natmosphere in trace amount. An atmospheric ammonia is formed by the bacterial\ndecomposition of nitrogenous matter of the plants and animals.<\/p>\n\n\n\n In 1774 ammonia was\nisolated by the reaction of ammonium chloride and lime. It was known as\nalkaline air. In 1788, Berthelot indicated that ammonia is a compound of\nhydrogen and nitrogen. Later in 1800, Davy established its formula NH3<\/sub>.<\/p>\n\n\n\n Ammonia (NH3) is manufactured during Haber\u2019s process. During this process, a pure Nitrogen and Hydrogen gases are reacted in the ratio of 1:3 by volume at high temperatures (400 C \u2013 500 o<\/sup>C) and pressure of 150-200 atm in the presence of a catalyst, iron, or Molybdenum as a promoter. This is a reversible reaction, and ammonia production is exothermic, with Fe\/Mo as catalyst and atmospheric pressure of 200-900 atm.<\/p>\n\n\n\n Raw\nmaterials:<\/strong><\/p>\n\n\n\n CH4<\/sub>(g)\n+ H2<\/sub>O \u2192 H2<\/sub>(g) + CO(g)<\/strong><\/p>\n\n\n\n Carbon\nmonoxide must be removed before feeding into Haber process. Hydrogen is also\nproduced from biomass and water using electrolysis process.<\/strong><\/strong><\/p>\n\n\n\n According to this diagram, nitrogen gas is taken from the air. Then it is combined with hydrogen atom that is extracted from natural gas in the ratio of 1:3 by volume i.e. in this process the mixture of nitrogen and hydrogen is added in the reactor by the ratio of 1:3 means 1volume of nitrogen is going to be added with 3volumes of hydrogen. According to Avogadro\u2019s Law during same temperature and pressure, an equal number of gases contains an equal number of molecules.<\/p>\n\n\n\n These gases are then\nallowed to pass through the beds of catalyst where cooling takes place. This is\nrequired to maintain equilibrium constant. In each pass different forms of\nconversion takes place and unreacted gases are recycled. Usually, iron is used\nas a catalyst while a temperature of 400 -450 o<\/sup>C and a pressure of 150-200 atm is maintained.\nApproximately 15% of the nitrogen and hydrogen is converted into ammonia (this\nmay vary from plant to plant) through continual recycling of unreacted gases\nlike nitrogen and hydrogen, and we attain the results about 98%. Finally, the\nammonia formed is cooled down to get a liquid solution which is then collected\nand is stored in containers.<\/p>\n\n\n\n The Haber\u2019s process\ninvolves an equilibrium reaction. Here we need to know about Le Chatelier\u2019s\nprinciple because it tells us how reaction conditions will impact on the\nproduction of ammonia.<\/p>\n\n\n\n So according to Le Chatelier\u2019s\nprinciple, the most favorable conditions to produce ammonia on an industrial\nscale is high pressure and low pressure. <\/p>\n\n\n\n Uses\nof Ammonia:<\/strong><\/p>\n\n\n\n Synthetic ammonia that is\nproduced today by a reaction between hydrogen and nitrogen is the root from\nwhich all the nitrogen-containing products are derived. The worldwide ammonia\nproduction is greater than one thirty million tons and, this is the sixth-largest\nproduced chemical. Ammonia is considered as the major raw material for\nagriculture and industry.<\/p>\n\n\n\n Production of ammonia\nthrough the Haber-Bosch process came in the early 1900s just before and during\nWorld War 1 and became a big wheel in the global sustainability very quickly.\nAs Germany entered the war and its requirement became high to make nitrates for\nexplosives and gunpowder. Other than the war, the animals waste was considered\nas the basic source of fertilizer which was not enough as the world\u2019s\nagricultural requirement was increasing day by day. On the other side, global\nnitrate supplies came from limited composting of plants waste and from deposits\nof Chile that were mined by the British companies. As the war was going between\nBritain and Germany, the ammonia supply was greatly reduced. In short without\ndevelopment in science i.e. Haber process Germany may not be able to fight the\nwar as long as it did. Some of its major uses are enlisted below:<\/p>\n\n\n\n Safety\ninformation:<\/strong><\/p>\n\n\n\n Generally, no significant health effects can be found\nin humans that are exposed to natural environmental concentrations of ammonia\nbut if the concentrations exceed than some of the instructions are as follows:<\/p>\n\n\n\n https:\/\/byjus.com\/chemistry\/haber-process\/<\/a><\/p>\n\n\n\n https:\/\/schools.aglasem.com\/<\/a><\/p>\n\n\n\n https:\/\/study.com\/academy\/lesson\/the-haber-process-commercial-uses-chemistry.html<\/a><\/p>\n\n\n\n https:\/\/medium.com\/@worldofchemical\/manufacturing-of-ammonia-by-habers-process-d3a79f8ab52f<\/a><\/p>\n\n\n\n https:\/\/www.chemguide.co.uk\/physical\/equilibria\/haber.html<\/a><\/p>\n","protected":false},"excerpt":{"rendered":" Introduction It is also known as the Haber – Bosch process or Synthetic Ammonia process. Haber\u2019s process is considered as one the most beneficial and efficient industrial processes to be used for the production of ammonia which is a colorless gas having a distinct odor. In the 20th century Fritz Haber, a German chemist developed … Read more<\/a><\/p>\n","protected":false},"author":6,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"rating_form_position":"","rating_results_position":"","mr_structured_data_type":""},"categories":[3],"tags":[],"multi-rating":{"mr_rating_results":[{"adjusted_star_result":4.5,"star_result":4.5,"total_max_option_value":5,"adjusted_score_result":4.5,"score_result":4.5,"percentage_result":90,"adjusted_percentage_result":90,"count":4,"post_id":837}]},"_links":{"self":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/837"}],"collection":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/users\/6"}],"replies":[{"embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/comments?post=837"}],"version-history":[{"count":3,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/837\/revisions"}],"predecessor-version":[{"id":868,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/posts\/837\/revisions\/868"}],"wp:attachment":[{"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/media?parent=837"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/categories?post=837"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/chemdictionary.org\/wp-json\/wp\/v2\/tags?post=837"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Definition:<\/strong><\/h2>\n\n\n\n
![\"\"](\"https:\/\/chemdictionary.org\/wp-content\/uploads\/2019\/09\/2019-09-27-18.png\" "\\"\\"")
<\/figure>\n\n\n\nProcess\nDetails<\/strong><\/h3>\n\n\n\n
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<\/figure>\n\n\n\nEquilibrium\nConsideration on Haber\u2019s process:<\/strong><\/h3>\n\n\n\n
Economic and Environmental aspect<\/strong><\/h3>\n\n\n\n
References:<\/strong><\/h4>\n\n\n\n