Vinyl chloride

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Vinyl chloride
Vinyl-chloride-2D.png
Structural formula of vinyl chloride Vinyl-chloride-3D-balls.png
Structural formula of vinyl chloride
Space-filling model Vinyl-chloride-3D-vdW.png
Space-filling model
Names
Preferred IUPAC name
Chloroethene
Other names
Vinyl chloride monomer
VCM
Chloroethylene
Refrigerant-1140
Identifiers
3D model (JSmol)
1731576
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.000.756 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 200-831-0
100541
KEGG
PubChem CID
RTECS number
  • KU9625000
UNII
UN number 1086
  • InChI=1S/C2H3Cl/c1-2-3/h2H,1H2 Yes check.svgY
    Key: BZHJMEDXRYGGRV-UHFFFAOYSA-N Yes check.svgY
  • InChI=1/C2H3Cl/c1-2-3/h2H,1H2
    Key: BZHJMEDXRYGGRV-UHFFFAOYAW
  • ClC=C
Properties
C2H3Cl
Molar mass 62.50 g·mol−1
AppearanceColorless gas
Odor pleasant [1]
Density 0.911 g/cc
Melting point −153.8 °C (−244.8 °F; 119.3 K)
Boiling point −13.4 °C (7.9 °F; 259.8 K)
2.7 g/L (0.0432 mol/L)
Vapor pressure 2580 mmHg at 20 °C (68 °F)
-35.9·10−6 cm3/mol
Thermochemistry
0.8592 J/K/g (gas)
0.9504 J/K/g (solid)
−94.12 kJ/mol (solid)
Hazards
GHS labelling:
GHS-pictogram-flamme.svg GHS-pictogram-silhouette.svg
Danger
H220, H350
P201, P202, P210, P281, P308+P313, P377, P381, P403, P405, P501
NFPA 704 (fire diamond)
NFPA 704.svgHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneInstability 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
4
2
Flash point −61 °C (−78 °F; 212 K)
Explosive limits 3.6–33% [1]
NIOSH (US health exposure limits):
PEL (Permissible)
TWA 1 ppm C 5 ppm [15-minute] [1]
REL (Recommended)
Ca [1]
IDLH (Immediate danger)
Ca [N.D.] [1]
Related compounds
Related chloroethenes
 dichloroethylenes, trichloroethylene, tetrachloroethylene, allyl chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Yes check.svgY  verify  (what is  Yes check.svgYX mark.svgN ?)

Vinyl chloride is an organochloride with the formula H2C=CHCl. It is also called vinyl chloride monomer (VCM) or chloroethene. This colorless compound is an important industrial chemical chiefly used to produce the polymer polyvinyl chloride (PVC). Vinyl chloride monomer is among the top twenty largest petrochemicals (petroleum-derived chemicals) in world production. [2] The United States remains the largest vinyl chloride manufacturing region because of its low-production-cost position in chlorine and ethylene raw materials. China is also a large manufacturer and one of the largest consumers of vinyl chloride. [3] Vinyl chloride is a flammable gas that has a sweet odor and is carcinogenic. It can be formed in the environment when soil organisms break down chlorinated solvents. Vinyl chloride that is released by industries or formed by the breakdown of other chlorinated chemicals can enter the air and drinking water supplies. Vinyl chloride is a common contaminant found near landfills. [4] Before the 1970s, vinyl chloride was used as an aerosol propellant and refrigerant. [5] [6]

Contents

Uses

Poly(vinyl chloride) (PVC), the main end-product of vinyl chloride, is used extensively in sewage pipes due to its low cost, chemical resistance, and ease of jointing. Laying sewer hi res (2).jpg
Poly(vinyl chloride) (PVC), the main end-product of vinyl chloride, is used extensively in sewage pipes due to its low cost, chemical resistance, and ease of jointing.

Vinyl chloride, also called vinyl chloride monomer (VCM), is exclusively used as a precursor to PVC. Due to its toxic nature, vinyl chloride is not found in other products. Poly(vinyl chloride) (PVC) is very stable, storable and not toxic. [2]

Until 1974, vinyl chloride was used in aerosol spray propellant. [7] Vinyl chloride was briefly used as an inhalational anaesthetic, in a similar vein to ethyl chloride, though its toxicity forced this practice to be abandoned. [8] [9]

Production

Globally, approximately 40 million tonnes of PVC resin are produced per year, [10] requiring a corresponding amount of vinyl chloride monomer. [11]

History

Vinyl chloride was first synthesized in 1835 by Justus von Liebig and his student Henri Victor Regnault. They obtained it by treating 1,2-dichloroethane with a solution of potassium hydroxide in ethanol. [12]

Acetylene-based routes

In 1912, Fritz Klatte, a German chemist working for Griesheim-Elektron, patented a means to produce vinyl chloride from acetylene and hydrogen chloride using mercuric chloride as a catalyst. Acetylene reacts with hydrogen chloride over a mercuric chloride catalyst to give vinyl chloride:

C2H2 + HCl → CH2=CHCl

The reaction is exothermic and highly selective. Product purity and yields are generally very high. [2]

This route to vinyl chloride was common before ethylene became widely distributed. When vinyl chloride producers shifted to using the thermal cracking of EDC described below, some used byproduct HCl in conjunction with a colocated acetylene-based unit. The hazards of storing and shipping acetylene meant that the vinyl chloride facility needed to be located very close to the acetylene generating facility. [2]

In view of mercury's toxicity, gold- and platinum-based catalysts have been proposed. [13] [14]

The mercury-based technology is the main production method in China due to low price on coal from which acetylene is produced, [3] [2] with over 80% of national capacity as of 2018, even though the resulting PVC contains residues and is only suitable for low-end products like pipes. [15]

Ethylene-based routes

In the United States and Europe, mercury-catalyzed routes widely used in the 20th century have been superseded by more economical and greener processes based on ethylene. Ethylene is made by cracking ethane. Two steps are involved, chlorination and dehydrochlorination:

H2C=CH2 + Cl2 → H2ClC−CH2Cl
H2ClC−CH2Cl → H2C=CHCl + HCl

Possible routes from ethane

Numerous attempts have been made to convert ethane directly to vinyl chloride. [2] Ethane, which is even more readily available than ethylene, is a potential precursor to vinyl chloride. The conversion of ethane to vinyl chloride has been demonstrated by various routes: [2]

High-temperature chlorination:

H3C−CH3 + 2 Cl2 → H2C=CHCl + 3 HCl

High-temperature oxychlorination, which uses oxygen and hydrogen chloride in place of chlorine:

H3C−CH3 + O2 + HCl → H2C=CHCl + 2 H2O

High-temperature oxidative chlorination: 4 H3C−CH3 + 3 O2 + 2 Cl2 → 4 H2C=CHCl + 6 H2O

Thermal decomposition of dichloroethane

1,2-Dichloroethane, ClCH2CH2Cl (also known as ethylene dichloride, EDC), can be prepared by halogenation of ethane or ethylene, inexpensive starting materials. EDC thermally converts into vinyl chloride and anhydrous HCl. This production method has become the major route to vinyl chloride since the late 1950s. [2]

ClCH2−CH2Cl → CH2=CHCl + HCl

The thermal cracking reaction is highly endothermic, and is generally carried out in a fired heater. Even though residence time and temperature are carefully controlled, it produces significant quantities of chlorinated hydrocarbon side products. In practice, the yield for EDC conversion is relatively low (50 to 60 percent). The furnace effluent is immediately quenched with cold EDC to minimize undesirable side reactions. The resulting vapor-liquid mixture then goes to a purification system. Some processes use an absorber-stripper system to separate HCl from the chlorinated hydrocarbons, while other processes use a refrigerated continuous distillation system. [2]

Storage and transportation

Vinyl chloride is stored as a liquid. The accepted upper limit of safety as a health hazard is 500 ppm. Often, the storage containers for the product vinyl chloride are high capacity spheres. The spheres have an inside sphere and an outside sphere. Several inches of space separate the inside sphere from the outside sphere. The interstitial space between the spheres is purged with an inert gas such as nitrogen. As the nitrogen purge gas exits the interstitial space it passes through an analyzer that detects whether any vinyl chloride is leaking from the internal sphere. If vinyl chloride starts to leak from the internal sphere or if a fire is detected on the outside of the sphere then the contents of the sphere are automatically dumped into an emergency underground storage container. Containers used for handling vinyl chloride at atmospheric temperature are always under pressure. Inhibited vinyl chloride may be stored at normal atmospheric conditions in suitable pressure vessels. Uninhibited vinyl chloride may be stored either under refrigeration or at normal atmospheric temperature in the absence of air or sunlight but only for a duration of a few days. If stored for longer periods, regular checks must be made to confirm no polymerization has taken place. [16] [ better source needed ]

In addition to its toxicity risk, transporting vinyl chloride also presents the same risks as transporting other flammable gases such as propane, butane, or natural gas. [17] Examples of incidents in which this danger was observed include the 2023 Ohio train derailment, [18] [19] in which derailed tank cars dumped 100,000 gallons of hazardous materials, including vinyl chloride. [20] [21]

Fire and explosion hazard

In the U.S., OSHA lists vinyl chloride as a Class IA Flammable Liquid, with a National Fire Protection Association Flammability Rating of 4. Because of its low boiling point, liquid vinyl chloride will undergo flash evaporation (i.e., autorefrigerate) upon its release to atmospheric pressure. The portion vaporized will form a dense cloud (more than twice as heavy as the surrounding air). The risk of subsequent explosion or fire is significant. According to OSHA, the flash point of vinyl chloride is −78 °C (−108.4 °F). [22] Its flammable limits in air are: lower 3.6 volume% and upper 33.0 volume%. The explosive limits are: lower 4.0%, upper 22.05% by volume in air. Fire may release toxic hydrogen chloride (HCl) and carbon monoxide (CO) and trace levels of phosgene. [23] [24] Vinyl chloride can polymerise rapidly due to heating and under the influence of air, light and contact with a catalyst, strong oxidisers and metals such as copper and aluminium, with fire or explosion hazard. As a gas mixed with air, vinyl chloride is a fire and explosion hazard. On standing[ clarification needed ], vinyl chloride can form peroxides, which may then explode. Vinyl chloride will react with iron and steel in the presence of moisture. [6] [25]

Health effects

Since it is a gas under most ambient conditions, primary exposure is via inhalation, as opposed to the consumption of contaminated food or water, with occupational hazards being highest. Prior to 1974, workers were commonly exposed to 1,000 ppm vinyl chloride, causing "vinyl chloride illness" such as acroosteolysis and Raynaud's Phenomenon. The symptoms of vinyl chloride exposure are classified by ppm levels in ambient air with 4,000  ppm having a threshold effect. [26] The intensity of symptoms varies from acute (1,000–8,000 ppm), including dizziness, nausea, visual disturbances, headache, and ataxia, to chronic (above 12,000 ppm), including narcotic effect, cardiac arrhythmias, and fatal respiratory failure. [27] RADS (Reactive Airway Dysfunction Syndrome) may be caused by acute exposure to vinyl chloride. [28]

Vinyl chloride is a mutagen having clastogenic effects which affect lymphocyte chromosomal structure. [27] [29] Vinyl chloride is a IARC group 1 Carcinogen posing elevated risks of rare angiosarcoma, brain and lung tumors, and malignant haematopoeitic lymphatic tumors. [30] Chronic exposure leads to common forms of respiratory failure (emphysema, pulmonary fibrosis) and focused hepatotoxicity (hepatomegaly, hepatic fibrosis). Continuous exposure can cause CNS depression including euphoria and disorientation. Decreased male libido, miscarriage, and birth defects are known major reproductive defects associated with vinyl chloride.

Vinyl chloride can have acute dermal and ocular effects. Dermal exposure effects are thickening of skin, edema, decreased elasticity, local frostbites, blistering, and irritation. [27] The complete loss of skin elasticity expresses itself in Raynaud's Phenomenon. [29]

Liver toxicity

The hepatotoxicity of vinyl chloride has long been established since the 1930s when the PVC industry was just in its early stages. In the very first study about the dangers of vinyl chloride, published by Patty in 1930, it was disclosed that exposure of test animals to just a single short-term high dose of vinyl chloride caused liver damage. [31] In 1949, a Russian publication discussed the finding that vinyl chloride caused liver injury among workers. [32] In 1954, B.F. Goodrich Chemical stated that vinyl chloride caused liver injury upon short-term exposures. Almost nothing was known about its long-term effects. They also recommended long-term animal toxicology studies. The study noted that if a chemical did justify the cost of testing, and its ill-effects on workers and the public were known, the chemical should not be made. [33] In 1963, research paid for in part by Allied Chemical found liver damage in test animals from exposures below 500 parts per million (ppm). [34] Also in 1963, a Romanian researcher published findings of liver disease in vinyl chloride workers. [35] In 1968, Mutchler and Kramer, two Dow researchers, reported their finding that exposures as low as 300 ppm caused liver damage in vinyl chloride workers thus confirming earlier animal data in humans. [36] In a 1969 presentation given in Japan, P. L. Viola, a European researcher working for the European vinyl chloride industry, indicated, "every monomer used in V.C. manufacture is hazardous....various changes were found in bone and liver. Particularly, much more attention should be drawn to liver changes. The findings in rats at the concentration of 4 to 10 ppm are shown in pictures." In light of the finding of liver damage in rats from just 4–10 ppm of vinyl chloride exposure, Viola added that he "should like some precautions to be taken in the manufacturing plants polymerizing vinyl chloride, such as a reduction of the threshold limit value of monomer." [37] Vinyl chloride was first reported to induce angiosarcoma of the liver in 1974 [38] and further research has demonstrated the carcinogenicity of VC to other organs and at lower concentrations, [39] [40] with evidence now extending to jobs associated with poly(vinyl chloride) exposure, indicating the need for prudent control of PVC dust in the industrial setting. [41]

Vinyl chloride is now an IARC group 1 carcinogen known to cause hepatic angiosarcoma (HAS) in highly exposed industrial workers. [42] Vinyl chloride monomer, a component in the production of poly(vinyl chloride) (PVC) resins, is a halogenated hydrocarbon with acute toxic effects, as well as chronic carcinogenic effects. [43]

Cancerous tumors

Animals exposed to 30,000 ppm of vinyl chloride developed cancerous tumors. Studies on vinyl chloride workers were a "red flag" to B.F. Goodrich and the industry. [44] In 1972, Maltoni, another Italian researcher for the European vinyl chloride industry, found liver tumors (including angiosarcoma) from vinyl chloride exposures as low as 250 ppm for four hours a day. [45]

In 1997 the U.S. Centers for Disease Control and Prevention (CDC) concluded that the development and acceptance by the PVC industry of a closed loop polymerization process in the late 1970s "almost completely eliminated worker exposures" and that "new cases of hepatic angiosarcoma in vinyl chloride polymerization workers have been virtually eliminated." [46]

The Houston Chronicle claimed in 1998 that the vinyl industry manipulated vinyl chloride studies to avoid liability for worker exposure and hid extensive and severe chemical spills in local communities. [47]

Environment pollution

According to the U.S. EPA, "vinyl chloride emissions from poly(vinyl chloride) (PVC), ethylene dichloride (EDC), and vinyl chloride monomer (VCM) plants cause or contribute to air pollution that may reasonably be anticipated to result in an increase in mortality or an increase in serious irreversible, or incapacitating reversible illness. Vinyl chloride is a known human carcinogen that causes a rare cancer of the liver." [48] EPA's 2001 updated Toxicological Profile and Summary Health Assessment for vinyl chloride in its Integrated Risk Information System (IRIS) database lowers EPA's previous risk factor estimate by a factor of 20 and concludes that "because of the consistent evidence for liver cancer in all the studies...and the weaker association for other sites, it is concluded that the liver is the most sensitive site, and protection against liver cancer will protect against possible cancer induction in other tissues." [49]

Mechanism

The carcinogenicity of VC is attributed to the action of two metabolites, chloroethylene oxide and chloroacetaldehyde. The former is produced by the action of cytochrome P-450 on VC. Both chloroethylene oxide and chloroacetaldehyde are alkylating agents.

Microbial remediation

The bacteria species Nitrosomonas europaea can degrade a variety of halogenated compounds including trichloroethylene, and vinyl chloride. [50]

See also

Related Research Articles

<span class="mw-page-title-main">Polyvinyl chloride</span> Common synthetic polymer

Polyvinyl chloride (alternatively: poly(vinyl chloride), colloquial: vinyl or polyvinyl; abbreviated: PVC) is the world's third-most widely produced synthetic polymer of plastic (after polyethylene and polypropylene). About 40 million tons of PVC are produced each year.

The compound hydrogen chloride has the chemical formula HCl and as such is a hydrogen halide. At room temperature, it is a colorless gas, which forms white fumes of hydrochloric acid upon contact with atmospheric water vapor. Hydrogen chloride gas and hydrochloric acid are important in technology and industry. Hydrochloric acid, the aqueous solution of hydrogen chloride, is also commonly given the formula HCl.

<span class="mw-page-title-main">Tetrachloroethylene</span> Chemical compound in very wide use

Tetrachloroethylene, also known as perchloroethylene or under the systematic name tetrachloroethene, and abbreviations such as perc, and PCE, is a chlorocarbon with the formula Cl2C=CCl2. It is a non-flammable, stable, colorless and heavy liquid widely used for dry cleaning of fabrics, hence it is sometimes called "dry-cleaning fluid". It also has its uses as an effective automotive brake cleaner. It has a mild sweet, sharp odor, detectable by most people at a concentration of 50 ppm.

<span class="mw-page-title-main">Dichloromethane</span> Chemical compound

Dichloromethane is an organochlorine compound with the formula CH2Cl2. This colorless, volatile liquid with a chloroform-like, sweet odor is widely used as a solvent. Although it is not miscible with water, it is slightly polar, and miscible with many organic solvents.

<span class="mw-page-title-main">Trichloroethylene</span> C2HCl3, widely used industrial solvent

Trichloroethylene (TCE) is a halocarbon with the formula C2HCl3, commonly used as an industrial metal degreasing solvent. It is a clear, colourless, non-flammable, volatile liquid with a chloroform-like pleasant mild smell and sweet taste. Its IUPAC name is trichloroethene. Trichloroethylene has been sold under a variety of trade names. Industrial abbreviations include TCE, trichlor, Trike, Tricky and tri. Under the trade names Trimar and Trilene, it was used as a volatile anesthetic and as an inhaled obstetrical analgesic. It should not be confused with the similar 1,1,1-trichloroethane, which was commonly known as chlorothene.

Organochlorine chemistry is concerned with the properties of organochlorine compounds, or organochlorides, organic compounds containing at least one covalently bonded atom of chlorine. The chloroalkane class includes common examples. The wide structural variety and divergent chemical properties of organochlorides lead to a broad range of names, applications, and properties. Organochlorine compounds have wide use in many applications, though some are of profound environmental concern, with TCDD being one of the most notorious.

In chemistry, trihalomethanes (THMs) are chemical compounds in which three of the four hydrogen atoms of methane are replaced by halogen atoms. Trihalomethanes with all the same halogen atoms are called haloforms. Many trihalomethanes find uses in industry as solvents or refrigerants. Some THMs are also environmental pollutants, and a few are considered carcinogenic.

<span class="mw-page-title-main">1,4-Dioxane</span> Chemical compound

1,4-Dioxane is a heterocyclic organic compound, classified as an ether. It is a colorless liquid with a faint sweet odor similar to that of diethyl ether. The compound is often called simply dioxane because the other dioxane isomers are rarely encountered.

<span class="mw-page-title-main">Ethylbenzene</span> Hydrocarbon compound; precursor to styrene and polystyrene

Ethylbenzene is an organic compound with the formula C6H5CH2CH3. It is a highly flammable, colorless liquid with an odor similar to that of gasoline. This monocyclic aromatic hydrocarbon is important in the petrochemical industry as a reaction intermediate in the production of styrene, the precursor to polystyrene, a common plastic material. In 2012, more than 99% of ethylbenzene produced was consumed in the production of styrene.

<span class="mw-page-title-main">Chloroprene</span> Chemical compound

Chloroprene (IUPAC name 2-chlorobuta-1,3-diene) is a chemical compound with the molecular formula CH2=CCl−CH=CH2. Chloroprene is a colorless volatile liquid, almost exclusively used as a monomer for the production of the polymer polychloroprene, better known as neoprene, a type of synthetic rubber.

The chemical compound 1,2-dichloroethane, commonly known as ethylene dichloride (EDC), is a chlorinated hydrocarbon. It is a colourless liquid with a chloroform-like odour. The most common use of 1,2-dichloroethane is in the production of vinyl chloride, which is used to make polyvinyl chloride (PVC) pipes, furniture and automobile upholstery, wall coverings, housewares, and automobile parts. 1,2-Dichloroethane is also used generally as an intermediate for other organic chemical compounds, and as a solvent. It forms azeotropes with many other solvents, including water and other chlorocarbons.

<span class="mw-page-title-main">Vinylacetylene</span> Chemical compound

Vinylacetylene is the organic compound with the formula C4H4. The colourless gas was once used in the polymer industry. It is composed of both alkyne and alkene groups and is the simplest enyne.

<span class="mw-page-title-main">Hexachloroethane</span> Chemical compound

Hexachloroethane (perchloroethane) is an organochlorine compound with the chemical formula (CCl3)2. It is a white or colorless solid at room temperature with a camphor-like odor. It has been used by the military in smoke compositions, such as base-eject smoke munitions.

<span class="mw-page-title-main">Benzotrichloride</span> Chemical compound

Benzotrichloride (BTC), also known as α,α,α-trichlorotoluene, phenyl chloroform or (trichloromethyl)benzene, is an organic compound with the formula C6H5CCl3. Benzotrichloride is an unstable, colorless or somewhat yellowish, viscous, chlorinated hydrocarbon with a penetrating odor. Benzotrichloride is used extensively as a chemical intermediate for products of various classes, i.e. dyes and antimicrobial agents.

<span class="mw-page-title-main">Ethyl acrylate</span> Chemical compound

Ethyl acrylate is an organic compound with the formula CH2CHCO2CH2CH3. It is the ethyl ester of acrylic acid. It is a colourless liquid with a characteristic acrid odor. It is mainly produced for paints, textiles, and non-woven fibers. It is also a reagent in the synthesis of various pharmaceutical intermediates.

<span class="mw-page-title-main">1,1,2,2-Tetrachloroethane</span> Chemical compound

1,1,2,2-tetrachloroethane (TeCA), also known by the brand names Bonoform, Cellon and Westron, is an organic compound. It is colorless liquid and has a sweet odor. It is used as an industrial solvent and as a separation agent. TeCA is toxic and it can be inhaled, consumed or absorbed through the skin. After exposure, nausea, dizziness or even liver damage may occur.

<span class="mw-page-title-main">Hexachlorobutadiene</span> Chemical compound

Hexachlorobutadiene, (often abbreviated as "HCBD") Cl2C=C(Cl)C(Cl)=CCl2, is a colorless liquid at room temperature that has an odor similar to that of turpentine. It is a chlorinated aliphatic diene with niche applications but is most commonly used as a solvent for other chlorine-containing compounds. Structurally, it has a 1,3-butadiene core, but fully substituted with chlorine atoms.

<span class="mw-page-title-main">Chloroacetaldehyde</span> Chemical compound

Chloroacetaldehyde is an organic compound with the formula ClCH2CHO. Like some related compounds, it is highly electrophilic reagent and a potentially dangerous alkylating agent. The compound is not normally encountered in the anhydrous form, but rather as the hemiacetal (ClCH2CH(OH))2O.

<span class="mw-page-title-main">Pentachloroethane</span> Chemical compound

Pentachloroethane is a chemical compound of chlorine, hydrogen, and carbon with the chemical formula C2HCl5. It is a colourless non-flammable liquid that is used as a solvent for oil and grease, in metal cleaning, and in the separation of coal from impurities.

In chemistry, oxychlorination is a process for generating the equivalent of chlorine gas (Cl2) from hydrogen chloride and oxygen. This process is attractive industrially because hydrogen chloride is less expensive than chlorine.

References

Additional references for environmental pollution

Inline citations

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  30. ↑ International Agency for Research on Cancer (IARC). "Vinyl chloride, polyvinyl chloride, and vinyl chloride-vinyl acetate copolymers." Vol 19, 1979. IARC. "Vinyl chloride." Supplement 7, 1987. Lyon.
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  32. ↑ Tribukh, S L et al. "Working Conditions and Measures for Their Improvement in Production and Use of Vinylchloride Plastics" (1949)
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  34. ↑ Lester, D.; Greenberg, L. A.; Adams, W. Robert (May 1963). "Effects of Single and Repeated Exposures of Humans and Rats to Vinyl Chloride". American Industrial Hygiene Association Journal. 24 (3): 265–275. doi:10.1080/00028896309342963. ISSN   0002-8894. PMID   13929916. Archived from the original on 2023-02-18. Retrieved 2023-02-07.
  35. ↑ Suciu, I.; Prodan, L.; Ilea, Elena; Păduraru, A.; Pascu, Livia (January 1975). "Clinical Manifestations in Vinyl Chloride Poisoning" . Annals of the New York Academy of Sciences. 246 (1): 53–69. Bibcode:1975NYASA.246...53S. doi:10.1111/j.1749-6632.1975.tb51080.x. ISSN   0077-8923. PMID   1054970. S2CID   30706677.
  36. ↑ Kramer, G.C., M.D. "The Correlation of Clinical and Environmental Measurements for Workers Exposed to Vinyl Chloride." The Dow Chemical Company. Midland Michigan.
  37. ↑ Viola, P.L. "Pathology of Vinyl Chloride" International Congress on Occupational Health. Japan. 1969.
  38. ↑ Wagoner, Joseph K. (1983). "Toxicity of Vinyl Chloride and Poly(Vinyl Chloride): A Critical Review". Environmental Health Perspectives. 52: 61–66. doi:10.2307/3429651. ISSN   0091-6765. JSTOR   3429651. PMC   1569348 . PMID   6360677.
  39. ↑ Winsten, Jay A.; Watson, James D.; Hiatt, Howard H.; Cold Spring Harbor Laboratory, eds. (1977). Origins of human cancer. Cold Spring Harbor conferences on cell proliferation. Vol. Book A. Incidence of cancer in humans. Cold Spring Harbor, N.Y.: Cold Spring Harbor Laboratory. p. 119. ISBN   978-0-87969-119-6.
  40. ↑ Maltoni, C.; Lefemine, G.; Ciliberti, A.; Cotti, G.; Carretti, D. (1981-10-01). "Carcinogenicity bioassays of vinyl chloride monomer: a model of risk assessment on an experimental basis". Environmental Health Perspectives. 41: 3–29. doi:10.1289/ehp.81413. ISSN   0091-6765. PMC   1568874 . PMID   6800782.
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  42. ↑ Sass, Jennifer Beth; Castleman, Barry; Wallinga, David (2005-07-01). "Vinyl chloride: a case study of data suppression and misrepresentation". Environmental Health Perspectives. 113 (7): 809–812. doi:10.1289/ehp.7716. ISSN   1552-9924. PMC   1257639 . PMID   16002366.
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  45. ↑ Maltoni, C. "Cancer Detection and Prevention" (1972) Presented at the Second International Symposium on Cancer Detection and Prevention. Bologna, April 9–12, 1973.
  46. ↑ Epidemiologic Notes and Reports Angiosarcoma of the Liver Among Polyvinyl Chloride Workers – Kentucky Archived 2010-09-16 at the Wayback Machine . Centers for Disease Control and Prevention. 1997.
  47. ↑ Jim Morris, "In Strictest Confidence. The chemical industry's secrets," Houston Chronicle. Part One: "Toxic Secrecy," June 28, 1998, pp. 1A, 24A–27A; Part Two: "High-Level Crime," June 29, 1998, pp. 1A, 8A, 9A; and Part Three: "Bane on the Bayou," July 26, 1998, pgs. 1A, 16A.
  48. ↑ National Emission Standards for Hazardous Air Pollutants (NESHAP) for Vinyl Chloride Subpart F, OMB Control Number 2060-0071, EPA ICR Number 0186.09 (Federal Register: September 25, 2001 (Volume 66, Number 186) Archived March 22, 2003, at the Wayback Machine )
  49. ↑ EPA Toxicological Review of Vinyl Chloride in Support of Information on the IRIS. May 2000
  50. ↑ "Home – Nitrosomonas europaea". genome.jgi-psf.org. Archived from the original on 3 July 2009. Retrieved 5 April 2018.

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