Styrene

Styrene (/ˈstʌɪriːn/)[5] is an organic compound with the chemical formula C6H5CH=CH2. This derivative of benzene is a colorless oily liquid, although aged samples can appear yellowish. The compound evaporates easily and has a sweet smell, although high concentrations have a less pleasant odor. Styrene is the precursor to polystyrene and several copolymers. Approximately 25 million tonnes of styrene were produced in 2010,[6] increasing to around 35 million tonnes by 2018.

Styrene
Names
Preferred IUPAC name
Ethenylbenzene[1]
Other names
Styrene[1]
Vinylbenzene
Phenylethene
Phenylethylene
Cinnamene
Styrol
Diarex HF 77
Styrolene
Styropol
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.002.592
KEGG
RTECS number
  • WL3675000
UNII
Properties
C8H8
Molar mass 104.15 g/mol
Appearance colorless oily liquid
Odor sweet, floral[2]
Density 0.909 g/cm3
Melting point −30 °C (−22 °F; 243 K)
Boiling point 145 °C (293 °F; 418 K)
0.03% (20 °C)[2]
log P 2.70[3]
Vapor pressure 5 mmHg (20 °C)[2]
−6.82×10−5 cm3/mol
1.5469
Viscosity 0.762 cP at 20 °C
Structure
0.13 D
Hazards
Main hazards flammable, toxic, probably carcinogenic
Safety data sheet MSDS
R-phrases (outdated) R10 R36
S-phrases (outdated) S38 S20 S23
NFPA 704 (fire diamond)
Flammability code 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g. gasolineHealth code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformReactivity code 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazards (white): no code
3
2
2
Flash point 31 °C (88 °F; 304 K)
Explosive limits 0.9%-6.8%[2]
Lethal dose or concentration (LD, LC):
2194 ppm (mouse, 4 hr)
5543 ppm (rat, 4 hr)[4]
10,000 ppm (human, 30 min)
2771 ppm (rat, 4 hr)[4]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 100 ppm C 200 ppm 600 ppm (5-minute maximum peak in any 3 hours)[2]
REL (Recommended)
 TWA 50 ppm (215 mg/m3) ST 100 ppm (425 mg/m3)[2]
IDLH (Immediate danger)
 700 ppm[2]
Related compounds
Related styrenes;
related aromatic compounds
 Polystyrene, Stilbene;
Ethylbenzene
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Natural occurrence

Styrene is named after storax balsam, the resin of Liquidambar trees of the Altingiaceae plant family. Styrene occurs naturally in small quantities in some plants and foods (cinnamon, coffee beans, balsam trees and peanuts)[7] and is also found in coal tar.

History

In 1839, the German apothecary Eduard Simon isolated a volatile liquid from the resin (called storax or styrax (Latin)) of the American sweetgum tree (Liquidambar styraciflua). He called the liquid "styrol" (now styrene).[8][9] He also noticed that when styrol was exposed to air, light, or heat, it gradually transformed into a hard, rubber-like substance, which he called "styrol oxide".[10] By 1845, the German chemist August Hofmann and his student John Blyth had determined styrene's empirical formula: C8H8.[11] They had also determined that Simon's "styrol oxide" – which they renamed "metastyrol" – had the same empirical formula as styrene.[12] Furthermore, they could obtain styrene by dry-distilling "metastyrol".[13] In 1865, the German chemist Emil Erlenmeyer found that styrene could form a dimer,[14] and in 1866 the French chemist Marcelin Berthelot stated that "metastyrol" was a polymer of styrene (i.e. polystyrene).[15] Meanwhile, other chemists had been investigating another component of storax, namely, cinnamic acid. They had found that cinnamic acid could be decarboxylated to form "cinnamene" (or "cinnamol"), which appeared to be styrene. In 1845, French chemist Emil Kopp suggested that the two compounds were identical,[16] and in 1866, Erlenmeyer suggested that both "cinnamol" and styrene might be vinylbenzene.[17] However, the styrene that was obtained from cinnamic acid seemed different from the styrene that was obtained by distilling storax resin: the latter was optically active.[18] Eventually, in 1876, the Dutch chemist van 't Hoff resolved the ambiguity: the optical activity of the styrene that was obtained by distilling storax resin was due to a contaminant.[19]

Industrial production

From ethylbenzene

The vast majority of styrene is produced from ethylbenzene,[20] and almost all ethylbenzene produced worldwide is intended for styrene production. As such, the two production processes are often highly integrated. Ethylbenzene is produced via a Friedel–Crafts reaction between benzene and ethylene; originally this used aluminum chloride as a catalyst, but in modern production this has been replaced by zeolites.

By dehydrogenation

Around 80% of styrene is produced by the dehydrogenation of ethylbenzene. This is achieved using superheated steam (up to 600 °C) over an iron(III) oxide catalyst.[21] The reaction is highly endothermic and reversible, with a typical yield of 88–94%.

The crude ethylbenzene/styrene product is then purified by distillation. As the difference in boiling points between the two compounds is only 9 °C at ambient pressure this necessitates the use of a series of distillation columns. This is energy intensive and is further complicated by the tendency of styrene to undergo thermally induced polymerisation into polystyrene,[22] requiring the continuous addition of polymerization inhibitor to the system.

Via ethylbenzene hydroperoxide

Styrene is also co-produced commercially in a process known as POSM (Lyondell Chemical Company) or SM/PO (Shell) for styrene monomer / propylene oxide. In this process, ethylbenzene is treated with oxygen to form the ethylbenzene hydroperoxide. This hydroperoxide is then used to oxidize propylene to propylene oxide, which is also recovered as a co-product. The remaining 1-phenylethanol is dehydrated to give styrene:

Other industrial routes

Pyrolysis gasoline extraction

Extraction from pyrolysis gasoline is performed on a limited scale.[20]

From toluene and methanol

Styrene can be produced from toluene and methanol, which are cheaper raw materials than those in the conventional process. This process has suffered from low selectivity associated with the competing decomposition of methanol.[23] Exelus Inc. claims to have developed this process with commercially viable selectivities, at 400–425 °C and atmospheric pressure, by forcing these components through a proprietary zeolitic catalyst. It is reported[24] that an approximately 9:1 mixture of styrene and ethylbenzene is obtained, with a total styrene yield of over 60%.[25]

From benzene and ethane

Another route to styrene involves the reaction of benzene and ethane. This process is being developed by Snamprogetti and Dow. Ethane, along with ethylbenzene, is fed to a dehydrogenation reactor with a catalyst capable of simultaneously producing styrene and ethylene. The dehydrogenation effluent is cooled and separated and the ethylene stream is recycled to the alkylation unit. The process attempts to overcome previous shortcomings in earlier attempts to develop production of styrene from ethane and benzene, such as inefficient recovery of aromatics, production of high levels of heavies and tars, and inefficient separation of hydrogen and ethane. Development of the process is ongoing.[26]

Laboratory synthesis

A laboratory synthesis of styrene entails the decarboxylation of cinnamic acid:[27]

C6H5CH=CHCO2H → C6H5CH=CH2 + CO2

Styrene was first prepared by this method.[28]

Polymerization

The presence of the vinyl group allows styrene to polymerize. Commercially significant products include polystyrene, ABS, styrene-butadiene (SBR) rubber, styrene-butadiene latex, SIS (styrene-isoprene-styrene), S-EB-S (styrene-ethylene/butylene-styrene), styrene-divinylbenzene (S-DVB), styrene-acrylonitrile resin (SAN), and unsaturated polyesters used in resins and thermosetting compounds. These materials are used in rubber, plastic, insulation, fiberglass, pipes, automobile and boat parts, food containers, and carpet backing.

Hazards

Explosive autopolymerisation

Styrene will polymerise spontaneously to polystyrene, without the need of external initiators.[29] This is known as autopolymerisation, and will take place at ambient temperatures and above. At 100 °C it will polymerise at a rate of ~2% per hour, and more rapidly than this at higher temperatures.[22] The polymerisation reaction is exothermic; hence, there is a real risk of thermal runaway and explosion. An example is the 2019 explosion of the tanker Stolt Groenland; in this incident 5,250 metric tons of styrene monomer detonated while the ship was docked in Ulsan, Republic of Korea. The autopolymerisation reaction can only be kept in check by the continuous addition of polymerisation inhibitors.

Health effects

Styrene is regarded as a "known carcinogen", especially in case of eye contact, but also in case of skin contact, of ingestion and of inhalation, according to several sources.[20][30][31][32] Styrene is largely metabolized into styrene oxide in humans, resulting from oxidation by cytochrome P450. Styrene oxide is considered toxic, mutagenic, and possibly carcinogenic. Styrene oxide is subsequently hydrolyzed in vivo to styrene glycol by the enzyme epoxide hydrolase.[33] The U.S. Environmental Protection Agency (EPA) has described styrene to be "a suspected toxin to the gastrointestinal tract, kidney, and respiratory system, among others".[34][35] On 10 June 2011, the U.S. National Toxicology Program has described styrene as "reasonably anticipated to be a human carcinogen".[36][37] However, a STATS author describes[38] a review that was done on scientific literature and concluded that "The available epidemiologic evidence does not support a causal relationship between styrene exposure and any type of human cancer".[39] Despite this claim, work has been done by Danish researchers to investigate the relationship between occupational exposure to styrene and cancer. They concluded, "The findings have to be interpreted with caution, due to the company based exposure assessment, but the possible association between exposures in the reinforced plastics industry, mainly styrene, and degenerative disorders of the nervous system and pancreatic cancer, deserves attention".[40] In 2012, the Danish EPA concluded that the styrene data do not support a cancer concern for styrene.[41] The U.S. EPA does not have a cancer classification for styrene,[42] but it has been the subject of their Integrated Risk Information System (IRIS) program.[43] The National Toxicology Program of the U.S. Department of Health and Human Services has determined that styrene is "reasonably anticipated to be a human carcinogen".[44] Various regulatory bodies refer to styrene, in various contexts, as a possible or potential human carcinogen. The International Agency for Research on Cancer considers styrene to be "probably carcinogenic to humans".[45][46]

The neurotoxic[47] properties of styrene have also been studied and reported effects include effects on vision[48] (although unable to reproduce in a subsequent study[49]) and on hearing functions.[50][51][52][53] Studies on rats have yielded contradictory results,[51][52] but epidemiologic studies have observed a synergistic interaction with noise in causing hearing difficulties.[54][55][56]

Industrial accident
Main article: Visakhapatnam gas leak

On 7 May 2020, a gas, reported to be styrene, leaked from a tank at the LG Chem (LG Polymers India Private Limited) plant at RR Venkatapuram, Visakhapatnam, Andra Pradesh, India. The leak occurred in the early morning hours while workers were preparing to reopen the plant, which was closed due to the COVID-19 pandemic. Thirteen people including a child reportedly died and over 200 people were hospitalized.[57][58]

gollark: Hmm. Perhaps it would be best to write the indexer thing in superior Rust.
gollark: Yes.
gollark: Possibly.
gollark: Nope. UEFI.
gollark: Horse = bee neuron data (78EB)

References
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  11. See:
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