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Title: Propene  
Author: World Heritage Encyclopedia
Language: English
Subject: Isopropyl alcohol, Alkene, Ethylene, Benzene, Boronic acid
Collection: Alkenes, Commodity Chemicals, Gabaa Receptor Positive Allosteric Modulators, Gases, Monomers, Petrochemicals
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Skeletal formula of propene
IUPAC name
ChemSpider  Y
Jmol-3D images Image
RTECS number UC6740000
UN number 1077
In Liquefied petroleum gas: 1075
Molar mass 42.08 g·mol−1
Appearance Colorless gas
Density 1.81 kg/m3, gas (1.013 bar, 15 °C)
613.9 kg/m3, liquid
Melting point −185.2 °C (−301.4 °F; 88.0 K)
Boiling point −47.6 °C (−53.7 °F; 225.6 K)
0.61 g/m3
Viscosity 8.34 µPa·s at 16.7 °C
0.366 D (gas)
Safety data sheet External MSDS
Extremely Flammable F+
R-phrases 12
S-phrases 9-16-33
NFPA 704
Flash point −108 °C (−162 °F; 165 K)
Related compounds
Related alkenes;
related groups
Ethylene, Isomers of Butylene;
Allyl, Propenyl
Related compounds
Propane, Propyne
Propadiene, 1-Propanol
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
 Y  (: Y/N?)

Propene, also known as propylene or methylethylene, is an chemical formula C3H6. It has one double bond, and is the second simplest member of the alkene class of hydrocarbons.


  • Properties 1
  • Occurrence in nature 2
  • Production 3
  • Uses 4
  • Reactions 5
  • Environmental safety 6
  • Storage and handling 7
  • Pharmacology 8
  • See also 9
  • References 10


At room temperature and atmospheric pressure, propene is a gas, and as with many other alkenes, it is also colorless with a weak but unpleasant smell.[1]

Propene has a higher density and boiling point than ethylene due to its greater mass. It has a slightly lower boiling point than propane and is thus more volatile. It lacks strongly polar bonds, yet the molecule has a small dipole moment due to its reduced symmetry (its point group is Cs).

Propene has the same empirical formula as cyclopropane but their atoms are connected in different ways, making these molecules structural isomers.

Occurrence in nature

Propene is found in nature and is a byproduct of vegetation and fermentation processes. On September 30, 2013 NASA announced that the Cassini orbiter space craft, part of the Cassini-Huygens mission, had discovered small amounts of naturally occurring propene in the atmosphere of Titan (moon) using spectroscopy.[2][3]


Propene is produced from fossil fuelspetroleum, natural gas, and, to a much lesser extent, coal. Propene is a byproduct of oil refining and natural gas processing. During oil refining, ethylene, propene, and other compounds are produced as a result of cracking larger hydrocarbon molecules to produce hydrocarbons more in demand. A major source of propene is naphtha cracking intended to produce ethylene, but it also results from refinery cracking producing other products.[4] Propene can be separated by fractional distillation from hydrocarbon mixtures obtained from cracking and other refining processes; refinery-grade propene is about 50 to 70%.[4]

A shift to lighter steam cracker feedstocks with relatively lower propene yields and reduced motor gasoline demand in certain areas has reduced propene supply.

On-purpose production methods are becoming increasingly significant.[5] On-purpose production technologies include:

Olefin metathesis, also known as disproportionation, is a reversible reaction between ethylene and butenes in which double bonds are broken and then reformed to form propene.[5] Propene yields of about 90 wt% are achieved. This option may also be used when there is no butene feedstock. In this case, part of the ethylene feeds an ethylene-dimerization unit that converts ethylene into butene.

Propane dehydrogenation converts propane into propene and by-product hydrogen. The propene from propane yield is about 85 m%. Reaction by-products (mainly hydrogen) are usually used as fuel for the propane dehydrogenation reaction. As a result, propene tends to be the only product, unless local demand exists for hydrogen. This route is popular in regions, such as the Middle East, where there is an abundance of propane from oil/gas operations.[6] In this region, the propane output is expected to be capable of supplying not only domestic needs, but also the demand from China, where many PDH projects are scheduled to go on stream. However, as natural gas offerings in the USA are significantly increasing due to the rising exploitation of shale gas, propane prices are decreasing. Chemical companies are already planning to establish PDH plants in the USA to take advantage of the low price raw material, obtained from shale gas. Numerous plants dedicated to propane dehydrogenation are currently under construction around the world. There are already five licensed technologies.[7] The propane dehydrogenation process may be accomplished through different commercial technologies. The main differences between each of them concerns the catalyst employed, design of the reactor and strategies to achieve higher conversion rates.[8]

Methanol-to-Olefins/Methanol-to-Propene converts synthesis gas (syngas) to methanol, and then converts the methanol to ethylene and/or propene. The process also produces water as by-product. Synthesis gas is produced from the reformation of natural gas or by the steam-induced reformation of petroleum products such as naphtha, or by gasification of coal. A large amount of methanol is required to make a world-scale ethylene and/or propene plant.[9]

High severity fluid catalytic cracking (FCC) uses traditional FCC technology under severe conditions (higher catalyst-to-oil ratios, higher steam injection rates, higher temperatures, etc.) in order to maximize the amount of propene and other light products. A high severity FCC unit is usually fed with gas oils (paraffins) and residues, and produces about 20–25 m% propene on feedstock together with greater volumes of motor gasoline and distillate byproducts.

Olefins Cracking includes a broad range of technologies that catalytically convert large olefins molecules (C4-C8) into mostly propene and small amounts of ethylene.

Propene production has remained static at around 35 million tonnes (Europe and North America only) from 2000 to 2008, but it has been increasing in East Asia, most notably Singapore and China.[10] Total world production of propene is currently about half that of ethylene.


Propene is the second most important starting product in the petrochemical industry after ethylene. It is the raw material for a wide variety of products. Manufacturers of the plastic polypropylene account for nearly two thirds of all demand. Polypropylene is, for example, needed for the production of films, packaging, caps and closures as well as for other applications. Propene is also used for the production of important chemicals such as propylene oxide, acrylonitrile, cumene, butyraldehyde, and acrylic acid. In the year 2013 about 85 million tonnes of propene were processed worldwide.[11]

Propene and benzene are converted to acetone and phenol via the cumene process. Propene is also used to produce isopropanol (propan-2-ol), acrylonitrile, propylene oxide (epoxypropane) and epichlorohydrin.[12]

In industry and workshops, propene is used as an alternative fuel to acetylene in Oxy-fuel welding and cutting, brazing and heating of metal for the purpose of bending. It has become a standard in BernzOmatic products and others in MAPP substitutes,[13] now that true MAPP gas is no longer available.


Propene resembles other alkenes in that it undergoes addition reactions relatively easily at room temperature. The relative weakness of its double bond explains its tendency to react with substances that can achieve this transformation. Alkene reactions include: 1) polymerization, 2) oxidation, 3) halogenation and hydrohalogenation, 4) alkylation, 5) hydration, 6) oligomerization, and 7) hydroformylation.

Environmental safety

Propene is produced naturally by vegetation, particularly certain tree species. It is also a product of combustion, from forest fires and cigarette smoke to motor vehicle and aircraft exhaust. It is an impurity in some heating gases. Observed concentrations have been in the range of 0.1-4.8 parts per billion (ppb) in rural air, 4-10.5 ppb in urban air, and 7-260 ppb in industrial air samples.[4]

In the United States and some European countries a hazardous air pollutant under the Clean Air Act. With a relatively short half-life, it is not expected to bioaccumulate.[4]

Propene has low acute toxicity from inhalation. Inhalation of the gas can cause anesthetic effects and at very high concentrations, unconsciousness. However, the asphyxiation limit for humans is about 10 times higher (23%) than the lower flammability level.[4]

Storage and handling

Since propene is volatile and flammable, precautions must be taken to avoid fire hazards in the handling of the gas. If propene is loaded to any equipment capable of causing ignition, such equipment should be shut down while loading, unloading, connecting or disconnecting. Propene is usually stored as liquid under pressure, although it is also possible to store it safely as gas at ambient temperature in approved containers.[14]


Propene acts as a central nervous system depressant via allosteric agonism of the GABAA receptor. Excessive exposure may result in sedation and amnesia, progressing to coma and death in a mechanism equivalent to benzodiazepine overdose. Intentional inhalation may also result in death via asphyxiation (sudden inhalant death).

See also


  1. ^ Collins Discovery Encyclopedia, 1st edition © HarperCollins Publishers, 2005
  2. ^ "Spacecraft finds propylene on Saturn moon, Titan". 2013-09-30. Retrieved 2013-11-12. 
  3. ^ "Cassini finds ingredient of household plastic on Saturn moon". Retrieved 2013-11-12. 
  4. ^ a b c d e "Product Safety Assessment(PSA): Propylene". Dow Chemical Co. 
  5. ^ a b "Propylene Production via Metathesis, Technology Economics Program". by Intratec, ISBN 978-0-615-61145-7, Q2 2012. 
  6. ^ Ashford’s Dictionary of Industrial Chemicals, Third edition, 2011, ISBN 978-0-9522674-3-0, pages 7766-9
  7. ^ Giovanni Maggini (2012-06-28). "Technology Economics: Propylene via Propane Dehydrogenation". Retrieved 2013-11-12. 
  8. ^ Giovanni Maggini (2013-04-17). "Technology Economics: Propylene via Propane Dehydrogenation, Part 3". Retrieved 2013-11-12. 
  9. ^ Giovanni Maggini (2012-05-31). "Technology Economics: Propylene from Methanol". Retrieved 2013-11-12. 
  10. ^ Organic Chemistry 6th edition, McMurry,J., Brooks/Cole Publishing, Pacific Grove USA (2005)
  11. ^ "Market Study: Propylene (2nd edition), Ceresana, December 2014". Retrieved 2015-02-03. 
  12. ^ Budavari, Susan, ed. (1996). "8034. Propylene". The Merck Index, Twelfth Edition. New Jersey: Merck & Co. pp. 1348–1349 
  13. ^ For example, "MAPP-Pro"[2]
  14. ^ Encyclopedia of Chemical Technology, Fourth edition, 1996, ISBN 0471-52689-4 (v.20), page 261
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