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Cumene process

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First stage of Hock process: alkylation of benzene with propylene.
Second stage of Hock process: autoxidation of cumene.

The cumene process (cumene-phenol process, Hock process) is an industrial process for synthesizing phenol and acetone from benzene and propylene. The term stems from cumene (isopropyl benzene), the intermediate material during the process. It was invented by R. Ūdris and P. Sergeyev in 1942 (USSR),[1] and independently by Heinrich Hock in 1944.[2][3]

This process converts two relatively cheap starting materials, benzene and propylene, into two more valuable ones, phenol and acetone. Other reactants required are oxygen from air and small amounts of a radical initiator. Most of the worldwide production of phenol and acetone is now based on this method. In 2022, nearly 10.8 million tonnes of phenol was produced by the cumene process.[4] In order for this process to be economical, there must also be demand for the acetone by-product as well as the phenol.[5]


Steps of the process

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Cumene is formed in the gas-phase Friedel–Crafts alkylation of benzene by propene. Benzene and propene are compressed together to a pressure of 30 standard atmospheres at 250 °C in presence of a catalytic Lewis acid. Phosphoric acid is often favored over aluminium halides. Cumene is oxidized in air, which removes the tertiary benzylic hydrogen from cumene and hence forms a cumene radical:

The cumene radical then bonds with an oxygen molecule to give cumene peroxide radical, which in turn forms cumene hydroperoxide (C6H5C(CH3)2O2H) by abstracting a benzylic hydrogen from another cumene molecule. This latter cumene converts into cumene radical and feeds back into subsequent chain formations of cumene hydroperoxides. A pressure of 5 atm is used to ensure that the unstable peroxide is kept in liquid state.

Cumene hydroperoxide undergoes a rearrangement reaction in an acidic medium (the Hock rearrangement) to give phenol and acetone. In the first step, the terminal hydroperoxy oxygen atom is protonated. This is followed by a step in which the phenyl group migrates from the benzyl carbon to the adjacent oxygen and a water molecule is lost, producing a resonance stabilized tertiary carbocation. The concerted mechanism of this step is similar to the mechanisms of the Baeyer–Villiger oxidation[6] and Criegee rearrangement reactions, and also the oxidation step of the hydroboration–oxidation process.[7] In 2009, an acidified bentonite clay was proven to be a more economical catalyst than sulfuric acid as the acid medium.

The resulting carbocation is then attacked by water, forming a hemiacetal-like structure. After transfer of a proton from the hydroxy oxygen to the ether oxygen, the ion falls apart into phenol and acetone.

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Alternatives to acetone co-production

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Cyclohexylbenzene can replace isopropylbenzene. Via the Hock rearrangement, cyclohexylbenzene hydroperoxide cleaves to give phenol and cyclohexanone. Cyclohexanone is an important precursor to some nylons.[8]

Starting with the alkylation of benzene with mixture of 1 and 2-butenes, the cumene process produces phenol and butanones.[5]

Alternatives to phenol production

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  • Hydroquinone is prepared by dialkylation of benzene with propene to give 1,4-diisopropylbenzene. This compound reacts with air to afford the bis(hydroperoxide). Analogous to the behavior of cumene hydroperoxide, it rearranges in acid to give acetone and hydroquinone. Oxidation of hydroquinone gives 1,4-benzoquinone:[9]
  • Resorcinol is analogously prepared by converting 1,3-Diisopropylbenzene into the bis(hydroperoxide), which fragments to resorcinol and acetone.[10]
  • 2-Naphthol can also be produced by a method analogous to the cumene process.[11]
  • 3-Chlorophenol, which does not arise by chlorination of phenol, can be produced by cumene process beginning with the alkylation of chlorobenzene with propylene.[12]
  • Cresols are produced from isopropyltoluene.[13]

Acetone processing

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Crude acetone is hydrogenated in the liquid phase over Raney nickel or a mixture of copper and chromium oxide to give isopropyl alcohol. This process is useful, when it is coupled with excess acetone production.[14] Mitsui & Co. developed additional step(s) to hydrogenating acetone and dehydrating the isopropanol product to propene, which is recycled as a starting reactant.[5]

Byproducts

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Byproducts of the cumene process to produce phenol and acetone are acetophenone and alpha-methylstyrene.

See also

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References

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  1. ^ "Latvian". Archived from the original on 2016-03-03. Retrieved 2011-02-27.
  2. ^ Hock, H. and Lang, S. (1944), Autoxydation von Kohlenwasserstoffen, IX. Mitteil.: Über Peroxyde von Benzol-Derivaten. Berichte der deutschen chemischen Gesellschaft (A and B Series), 77: 257–264 doi:10.1002/cber.19440770321
  3. ^ Concise Encyclopedia Chemistry (1993) Mary Eagleso
  4. ^ "Phenol Market Size, Share, Analysis & Forecast, 2035 – ChemAnalyst". ChemAnalyst. Retrieved 2024-04-09.
  5. ^ a b c "Direct Routes to Phenol". Archived from the original on 2007-04-09. Retrieved 2006-12-26.
  6. ^ Streitwieser, A; Heathcock, C.H. (1992). "30". Introduction to Organic Chemistry. Kosower, E.M. (4th ed.). New York: MacMillan. pp. 1018. ISBN 0-02-418170-6.
  7. ^ K.P.C., Vollhardt; N.E. Schore (2003). "22". Organic Chemistry: Structure and Function (4th ed.). New York: Freeman. p. 988. ISBN 0-7167-4374-4.
  8. ^ Plotkin, Jeffrey S. (2016-03-21). "What's New in Phenol Production?". American Chemical Society. Archived from the original on 2019-10-27. Retrieved 2018-01-02.
  9. ^ Gerhard Franz, Roger A. Sheldon "Oxidation" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2000 doi:10.1002/14356007.a18_261
  10. ^ K. W. Schmiedel; D. Decker (2012). "Resorcinol". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a23_111.pub2. ISBN 978-3527306732.
  11. ^ Gerald Booth "Naphthalene Derivatives" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a17_009.
  12. ^ François Muller; Liliane Caillard (2011). "Chlorophenols". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a07_001.pub2. ISBN 978-3527306732.
  13. ^ Roger A. Sheldon (1983). "Synthesis and uses of alkyl hydroperoxides and dialkyl peroxides". In Patai, Saul (ed.). Syntheses and Uses of Hydroperoxides and Dialkylperoxides. PATAI'S Chemistry of Functional Groups. John Wiley & Sons. pp. 161–200. doi:10.1002/9780470771730.ch6. ISBN 978-0-471-10218-2.
  14. ^ Papa, A. J. "Propanols". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a22_173. ISBN 978-3527306732.
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