Andrussow process: Difference between revisions
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The process is based on a reaction that was discovered by [[Leonid Andrussow]] in 1927. In the following years he developed the process that is named after him. HCN is also produced in the [[BMA process]]. |
The process is based on a reaction that was discovered by [[Leonid Andrussow]] in 1927. In the following years he developed the process that is named after him. HCN is also produced in the [[BMA process]]. |
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==Process details== |
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This reaction is very [[exothermic reaction|exothermic]]. The change of [[Standard enthalpy of formation|enthalpy]] of this reaction is equal to ''-481.06 kJ''.<ref>{{Citation | first=Gyula | last=Deák | title=Menné reakcie v organickej chémii|year = 1980|publisher=Vydavateľstvo technickej a ekonomickej literatúry| location = Bratislava| page = 14}}</ref> The [[heat]] provided by the main reaction serves as a catalyst for other side reactions. |
This reaction is very [[exothermic reaction|exothermic]]. The change of [[Standard enthalpy of formation|enthalpy]] of this reaction is equal to ''-481.06 kJ''.<ref>{{Citation | first=Gyula | last=Deák | title=Menné reakcie v organickej chémii|year = 1980|publisher=Vydavateľstvo technickej a ekonomickej literatúry| location = Bratislava| page = 14}}</ref> The [[heat]] provided by the main reaction serves as a catalyst for other side reactions. |
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:CH<sub>4</sub> + H<sub>2</sub>O → CO + 3 H<sub>2</sub> |
:CH<sub>4</sub> + H<sub>2</sub>O → CO + 3 H<sub>2</sub> |
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Revision as of 00:06, 8 November 2023
The Andrussow process is the dominant industrial process for the production of hydrogen cyanide.[1] It involves the reaction of methane, ammonia, and oxygen. A catalyst, typically platinum, is required.[2][3]
- 2 CH4 + 2 NH3 + 3 O2 → 2 HCN + 6 H2O
The process is based on a reaction that was discovered by Leonid Andrussow in 1927. In the following years he developed the process that is named after him. HCN is also produced in the BMA process.
Process details
This reaction is very exothermic. The change of enthalpy of this reaction is equal to -481.06 kJ.[4] The heat provided by the main reaction serves as a catalyst for other side reactions.
- CH4 + H2O → CO + 3 H2
- 2 CH4 + 3 O2 → 2 CO + 4 H2O
- 4 NH3 + 3 O2 → 2 N2 + 6 H2O
These side reactions can be reduced by only short exposures to the catalyst of the order of 0.0003s.[5]
References
- ^ Gail, E.; Gos, S.; Kulzer, R.; Lorösch, J.; Rubo, A.; Sauer, M. "Cyano Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a08_159.pub2. ISBN 978-3527306732.
- ^ Leonid Andrussow (1927). "Über die schnell verlaufenden katalytischen Prozesse in strömenden Gasen und die Ammoniak-Oxydation (V)". Berichte der Deutschen Chemischen Gesellschaft. 60 (8): 2005–2018. doi:10.1002/cber.19270600857.
- ^ L. Andrussow (1935). "Über die katalytische Oxydation von Ammoniak-Methan-Gemischen zu Blausäure (The catalytic oxidation of ammonia-methane-mixtures to hydrogen cyanide)". Angewandte Chemie. 48 (37): 593–595. doi:10.1002/ange.19350483702.
- ^ Deák, Gyula (1980), Menné reakcie v organickej chémii, Bratislava: Vydavateľstvo technickej a ekonomickej literatúry, p. 14
- ^ Pirie, J M (1958). "The Manufacture of Hydrocyanic Acid by the Andrussow Process" (PDF). Platinum Metals Rev. 2 (1): 7–11. Archived from the original (PDF) on 31 January 2013. Retrieved 28 March 2014.