| Revision as of 13:04, 15 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 472721116 of page Carbon_disulfide for the Chem/Drugbox validation project (updated: 'KEGG'). |
Latest revision as of 15:34, 23 October 2024 edit Mondtaler (talk | contribs)182 edits Updated data and sourceTag: 2017 wikitext editor |
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{{Short description|1=Neurotoxic compound with formula S=C=S}} |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{chembox |
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{{chembox |
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| Verifiedfields = changed |
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| Watchedfields = changed |
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| Watchedfields = changed |
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| verifiedrevid = 460018440 |
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| verifiedrevid = 476998332 |
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| Name = '''Carbon disulfide''' |
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| Name = Carbon disulfide |
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| ImageFile_Ref = {{chemboximage|correct|??}} |
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| ImageFile_Ref = {{chemboximage|correct|??}} |
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| ImageFile = Carbon-disulfide-2D-dimensions.png |
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| ImageFile = Carbon-disulfide-2D-dimensions.png |
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| ImageSize = 150px |
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| ImageSize = 150px |
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| ImageFile1 = Carbon-disulfide-3D-vdW.png |
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| ImageFile1 = Carbon-disulfide-3D-vdW.png |
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| ImageSize1 = 150px |
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| ImageSize1 = 150px |
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| ImageName = Carbon disulfide |
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| ImageName = Carbon disulfide |
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| IUPACName = Carbon disulfide |
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| IUPACName = Carbon disulfide |
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| OtherNames = Carbon bisulfide<br/>Dithiocarbonic anhydride<ref>{{Cite web|title=Carbon disulfide chemistry |url=https://webbook.nist.gov/cgi/cbook.cgi?ID=C75150&Mask=80:~:text=Dithiocarbonic%20Anhydride |access-date=August 24, 2022|publisher=]}}</ref> |
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| OtherNames = |
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| SystematicName = Methanedithione |
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| Section1 = {{Chembox Identifiers |
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| Section1 = {{Chembox Identifiers |
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| CASNo = 75-15-0 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| Beilstein = 1098293 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI = 23012 |
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| ChEBI = 23012 |
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| SMILES = C(=S)=S |
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| ChEMBL = 1365180 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 6108 |
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| ChemSpiderID = 6108 |
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| KEGG_Ref = {{keggcite|correct|kegg}} |
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| KEGG = C19033 |
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| PubChem = 6348 |
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| EINECS = 200-843-6 |
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| RTECS = FF6650000 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = S54S8B99E8 |
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| UNII = S54S8B99E8 |
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| UNNumber = 1131 |
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| InChI = 1/CS2/c2-1-3 |
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| InChI = 1/CS2/c2-1-3 |
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| InChIKey = QGJOPFRUJISHPQ-UHFFFAOYAS |
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| InChIKey = QGJOPFRUJISHPQ-UHFFFAOYAS |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = QGJOPFRUJISHPQ-UHFFFAOYSA-N |
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| StdInChIKey = QGJOPFRUJISHPQ-UHFFFAOYSA-N |
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| CASNo = 75-15-0 |
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| SMILES = S=C=S |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| PubChem = 6348 |
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| EINECS = 200-843-6 |
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| RTECS = FF6650000 |
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| UNNumber = 1131 |
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| KEGG_Ref = {{keggcite|changed|kegg}} |
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| KEGG = <!-- blanked - oldvalue: C19033 --> |
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}} |
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| Section2 = {{Chembox Properties |
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| Formula = CS<sub>2</sub> |
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| MolarMass = 76.139 g/mol |
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| ExactMass = 75.944141 |
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| Appearance = colorless liquid<br/>impure: light-yellow |
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| Odor = ] (pure) <br> foul (commerical) |
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| Density = 1.261 g/cm<sup>3</sup> |
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| MeltingPtC = -110.8 |
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| BoilingPtC = 46.3 |
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| Solubility = 2.9 g/kg (20 °C) |
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| SolubilityOther = soluble in ], ], ], ]. ], ] |
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| RefractIndex = 1.6295 |
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| Viscosity = 0.363 |
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}} |
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}} |
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| Section3 = {{Chembox Structure |
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| Section2 = {{Chembox Properties |
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| C=1 | S=2 |
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| Appearance = Colorless liquid<br />Impure: light-yellow |
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| Odor = Pleasant, ]- or ]-like<br />Commercial: Foul, like rotten ] |
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| Density = 1.539 g/cm<sup>3</sup> (−186°C)<br />1.2927 g/cm<sup>3</sup> (0 °C)<br />1.266 g/cm<sup>3</sup> (25 °C)<ref name="chemister" /> |
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| MeltingPtC = −111.61 |
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| MeltingPt_notes = |
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| BoilingPtC = 46.24 |
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| Solubility = 2.58 g/L (0 °C)<br />2.39 g/L (10 °C)<br />2.17 g/L (20 °C)<ref name="sioc">{{cite book |last1=Seidell |first1=Atherton |last2=Linke |first2=William F. |year=1952 |title=Solubilities of Inorganic and Organic Compounds |publisher=Van Nostrand }}</ref><br /> 0.14 g/L (50 °C)<ref name="chemister" /> |
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| RefractIndex = 1.627<ref name="sigma" /> |
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| Viscosity = 0.436 ] (0 °C)<br /> 0.363 cP (20 °C) |
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| SolubleOther = Soluble in ], ], ], ], ], ] |
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| Solubility1 = 4.66 g/100 g<ref name="chemister" /> |
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| Solvent1 = formic acid |
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| Solubility2 = 45 g/100 g (20.3 °C)<ref name="chemister" /> |
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| Solvent2 = dimethyl sulfoxide |
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| VaporPressure = 48.1 kPa (25 °C)<br /> 82.4 kPa (40 °C)<ref name="nist">{{nist |name=Carbon disulfide |id=C75150 |accessdate=2014-05-27 |mask=FFFF |units=SI }}.</ref> |
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| MagSus = −42.2·10<sup>−6</sup> cm<sup>3</sup>/mol |
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}} |
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| Section3 = {{Chembox Structure |
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| MolShape = Linear |
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| MolShape = Linear |
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| Dipole = zero |
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| Dipole = 0 D (20 °C)<ref name="chemister" /> |
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}} |
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| Section5 = {{Chembox Thermochemistry |
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| DeltaHf = 88.7 kJ/mol<ref name="chemister">{{cite web |url=http://chemister.ru/Database/properties-en.php?dbid=1&id=1955 |website=chemister.ru |title=Properties of substance: carbon disulfide}}</ref> |
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| DeltaGf = 64.4 kJ/mol<ref name="chemister" /> |
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| Entropy = 151 J/(mol·K)<ref name="chemister" /> |
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| HeatCapacity = 75.73 J/(mol·K)<ref name="chemister" /> |
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| DeltaHc = 1687.2 kJ/mol<ref name="nist" /> |
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}} |
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| Section7 = {{Chembox Hazards |
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| Section7 = {{Chembox Hazards |
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| ExternalSDS = |
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| ExternalMSDS = |
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| GHSPictograms = {{GHS02}} {{GHS07}} {{GHS08}} |
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| EUIndex = 006-003-00-3 |
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| GHS_ref = <ref name="sigma">], . Retrieved on 2024-10-23.</ref> |
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| EUClass = Extremely Flammable ('''F+''')<br/>Repr. Cat. 3<br/>Toxic ('''T''')<br/>Irritant ('''Xi''') |
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| GHSSignalWord = Danger |
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| RPhrases = {{R11}}, {{R36/38}}, {{R48/23}}, {{R62}}, {{R63}} |
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| HPhrases = {{H-phrases|225|315|319|332|361fd|372}} |
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| SPhrases = {{S1/2}}, {{S16}}, {{S33}}, {{S36/37}}, {{S45}} |
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| PPhrases = {{P-phrases|202|210|281|303+361+353|304+340+312|305+351+338|308+313}}<br/> |
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| NFPA-H = 3 |
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| NFPA-H = 3 |
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| NFPA-F = 4 |
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| NFPA-F = 4 |
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| NFPA-R = 0 |
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| NFPA-R = 0 |
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| FlashPt = -30 °C |
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| FlashPtC = −43 |
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| FlashPt_ref = <ref name="chemister" /> |
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| Autoignition = 90 °C |
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| AutoignitionPtC = 102 |
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| ExploLimits = 1.3–50% |
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| AutoignitionPt_ref = <ref name="chemister" /> |
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| LD50 = 3188 mg/kg |
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| ExploLimits = 1.3–50%<ref name="PGCH" /> |
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| LD50 = 3188 mg/kg (rat, oral) |
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| EyeHazard = Irritant |
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| SkinHazard = Irritant |
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| InhalationHazard = Irritant; neurotoxic |
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| PEL = TWA 20 ppm C 30 ppm 100 ppm (30-minute maximum peak)<ref name="PGCH">{{PGCH|0104}}</ref> |
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| REL = TWA 1 ppm (3 mg/m<sup>3</sup>) ST 10 ppm (30 mg/m<sup>3</sup>) <ref name="PGCH" /> |
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| IDLH = 500 ppm<ref name="PGCH" /> |
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| LC50 = >1670 ppm (rat, 1 h)<br />15500 ppm (rat, 1 h)<br />3000 ppm (rat, 4 h)<br />3500 ppm (rat, 4 h)<br />7911 ppm (rat, 2 h)<br />3165 ppm (mouse, 2 h)<ref name="IDLH">{{IDLH|75150|Carbon disulfide}}</ref> |
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| LCLo = 4000 ppm (human, 30 min)<ref name="IDLH" /> |
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}} |
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| Section8 = {{Chembox Related |
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| Section8 = {{Chembox Related |
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| OtherCpds = ]<br/>]<br/>] |
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| OtherCompounds = ]<br />]<br />] |
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'''Carbon disulfide''' (also spelled as '''carbon disulphide''') is an ] with the ] {{chem2|CS2}} and ] {{chem2|S\dC\dS}}. It is also considered as the anhydride of ].<ref>{{Cite web |last=Informatics |first=NIST Office of Data and |title=Carbon disulfide |url=https://webbook.nist.gov/cgi/cbook.cgi?ID=C75150&Mask=80 |access-date=2024-05-07 |website=webbook.nist.gov |language=en}}</ref> It is a colorless, flammable, ] liquid that is used as a building block in organic synthesis. Pure carbon disulfide has a pleasant, ]- or ]-like odor, but commercial samples are usually yellowish and are typically contaminated with foul-smelling impurities.<ref name="Holleman">{{Holleman&Wiberg}}.</ref> |
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== History == |
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In 1796, the German chemist ] (1772–1842) first prepared carbon disulfide by heating ] with moist charcoal. He called it "liquid sulfur" (''flüssig Schwefel'').<ref>{{cite journal |last1=Lampadius |title=Etwas über flüssigen Schwefel, und Schwefel-Leberluft |journal=Chemische Annalen für die Freunde der Naturlehre, Arzneygelährtheit, Haushaltungskunst und Manufacturen (Chemical Annals for the Friends of Science, Medicine, Economics, and Manufactures)|date=1796 |issue=2 |pages=136–137 |url=https://books.google.com/books?id=gqk5AAAAcAAJ&pg=PA136 |trans-title=Something about liquid sulfur and liver-of-sulfur gas (i.e., hydrogen sulfide) |language=de}}</ref> The composition of carbon disulfide was finally determined in 1813 by the team of the Swedish chemist ] (1779–1848) and the Swiss-British chemist ] (1770–1822).<ref>{{cite journal |last1=Berzelius |first1=J. |last2=Marcet |first2=Alexander |title=Experiments on the alcohol of sulphur, or sulphuret of carbon |journal=Philosophical Transactions of the Royal Society of London |date=1813 |volume=103 |pages=171–199 |doi=10.1098/rstl.1813.0026 |s2cid=94745906 |doi-access=free }}</ref> Their analysis was consistent with an ] of CS<sub>2</sub>.<ref>(Berzelius and Marcet, 1813), p. 187.</ref> |
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==Occurrence, manufacture, properties== |
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Small amounts of carbon disulfide are released by ] eruptions and ]es. CS<sub>2</sub> once was manufactured by combining ] (or ]) and ] at 800–1000 °C.<ref>{{cite journal | last=Warnecke | first=Friedrich | title=Die gewerbliche Schwefelkohlenstoffvergiftung | journal=Archiv für Gewerbepathologie und Gewerbehygiene | publisher=Springer Science and Business Media LLC | volume=11 | issue=2 | year=1941 | issn=0340-0131 | doi=10.1007/bf02122927 | pages=198–248 | bibcode=1941IAOEH..11..198W | s2cid=72106188 | language=de}}</ref> |
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:C + 2S → CS<sub>2</sub> |
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A lower-temperature reaction, requiring only 600 °C, utilizes ] as the carbon source in the presence of ] or ] ]s:<ref name="Holleman" /> |
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:2 CH<sub>4</sub> + S<sub>8</sub> → 2 CS<sub>2</sub> + 4 H<sub>2</sub>S |
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The reaction is analogous to the combustion of ]. |
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Global production/consumption of carbon disulfide is approximately one million tonnes, with China consuming 49%, followed by India at 13%, mostly for the production of rayon fiber.<ref>{{cite web |url=http://www.ihs.com/products/chemical/planning/ceh/carbon-disulfide.aspx |title=Carbon Disulfide report from IHS Chemical |access-date= June 15, 2013 }}</ref> United States production in 2007 was 56,000 tonnes.<ref>{{cite web |url=http://www.icis.com/Articles/2008/09/08/9154319/chemical-profile-carbon-disulfide.html |title=Chemical profile: carbon disulfide from ICIS.com |access-date= June 15, 2013 }}</ref> |
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===Solvent=== |
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Carbon disulfide can dissolve a variety of ] chemicals including ], sulfur, ], ], ], ]s, ]s, ], and ].<ref>{{cite web |url=http://www.akzonobel.com/sulfurderivatives/products/carbon_disulfide/ |title=Carbon Disulfide |publisher=Akzo Nobel |access-date=2010-12-16 |archive-date=2017-09-03 |archive-url=https://web.archive.org/web/20170903211829/https://www.akzonobel.com/sulfurderivatives/products/carbon_disulfide/ |url-status=dead }}</ref> |
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=== Extraterrestrial === |
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In March 2024, traces of CS<sub>2</sub> were likely detected in the atmosphere of the temperate ] planet ] by the ].<ref >{{Citation |last1=Benneke |first1=Björn |title=JWST Reveals CH$_4$, CO$_2$, and H$_2$O in a Metal-rich Miscible Atmosphere on a Two-Earth-Radius Exoplanet |date=2024-03-05 |last2=Roy |first2=Pierre-Alexis |last3=Coulombe |first3=Louis-Philippe |last4=Radica |first4=Michael |last5=Piaulet |first5=Caroline |last6=Ahrer |first6=Eva-Maria |last7=Pierrehumbert |first7=Raymond |last8=Krissansen-Totton |first8=Joshua |last9=Schlichting |first9=Hilke E.|arxiv=2403.03325 }}</ref> |
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==Reactions== |
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Combustion of CS<sub>2</sub> affords ] according to this ideal stoichiometry: |
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:CS<sub>2</sub> + 3{{nbsp}}O<sub>2</sub> → CO<sub>2</sub> + 2{{nbsp}}SO<sub>2</sub> |
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===With nucleophiles=== |
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For example, amines afford ]s:<ref name=":0">{{cite journal | last1=Yokoyama | first1=Masataka | last2=Imamoto | first2=Tsuneo | title=Organic Reactions of Carbon Disulfide | journal=Synthesis | publisher=Georg Thieme Verlag KG | volume=1984 | issue=10 | year=1984 | issn=0039-7881 | doi=10.1055/s-1984-30978 | pages=797–824}}</ref> |
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:2{{nbsp}}R<sub>2</sub>NH + CS<sub>2</sub> → |
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]s form similarly from ]s:<ref name=":0"/> |
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:RONa + CS<sub>2</sub> → |
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This reaction is the basis of the manufacture of regenerated ], the main ingredient of ], ], and ]. Both xanthates and the related ]s (derived from treatment of CS<sub>2</sub> with sodium ]s) are used as ] in mineral processing. |
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Upon treatment with ], carbon disulfide affords ]:<ref name=":0"/> |
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:Na<sub>2</sub>S + CS<sub>2</sub> → <sub>2</sub> |
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Carbon disulfide does not hydrolyze readily, although the process is catalyzed by an ] ]. |
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Compared to the ] ], CS<sub>2</sub> is a weaker ]. While, however, reactions of ]s with CO<sub>2</sub> are highly reversible and products are only isolated with very strong nucleophiles, the reactions with CS<sub>2</sub> are thermodynamically more favored allowing the formation of products with less reactive nucleophiles.<ref>{{Cite journal|last1=Li|first1=Zhen|last2=Mayer|first2=Robert J.|last3=Ofial|first3=Armin R.| last4=Mayr|first4=Herbert|date=2020-04-27|title= From Carbodiimides to Carbon Dioxide: Quantification of the Electrophilic Reactivities of Heteroallenes|journal=Journal of the American Chemical Society|volume=142|issue=18|pages=8383–8402|doi=10.1021/jacs.0c01960|pmid=32338511|s2cid=216557447}}</ref> |
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===Reduction=== |
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Reduction of carbon disulfide with ] affords ] together with sodium ]:<ref>{{cite journal|journal=Org. Synth.|year=1996|volume=73|page=270|doi=10.15227/orgsyn.073.0270|title=4,5-Dibenzoyl-1,3-dithiole-1-thione}}</ref> |
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: 4{{nbsp}}Na + 4{{nbsp}}CS<sub>2</sub> → Na<sub>2</sub>C<sub>3</sub>S<sub>5</sub> + Na<sub>2</sub>CS<sub>3</sub> |
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===Chlorination=== |
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] of CS<sub>2</sub> provides a route to ]:<ref name="Holleman" /> |
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:CS<sub>2</sub> + 3 ] → CCl<sub>4</sub> + ] |
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This conversion proceeds via the intermediacy of ], CSCl<sub>2</sub>. |
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===Coordination chemistry=== |
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CS<sub>2</sub> is a ligand for many metal complexes, forming pi complexes. One example is ]Co(]-CS<sub>2</sub>)(P]<sub>3</sub>).<ref>{{cite journal |last=Werner |first=Helmut |title=Novel Coordination Compounds formed from CS<sub>2</sub> and Heteroallenes |journal=Coordination Chemistry Reviews |year=1982 |volume=43 |pages=165–185 |doi=10.1016/S0010-8545(00)82095-0 }}</ref> |
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==Polymerization== |
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CS<sub>2</sub> polymerizes upon photolysis or under high pressure to give an insoluble material called car-sul or "Bridgman's black", named after the discoverer of the polymer, ].<ref>{{cite journal |last1=Bridgman |first1=P.W. |title=Explorations toward the limit of utilizable pressures |journal=Journal of Applied Physics |date=1941 |volume=12 |issue=6 |pages=461–469|doi=10.1063/1.1712926 |bibcode=1941JAP....12..461B }}</ref> Trithiocarbonate (-S-C(S)-S-) linkages comprise, in part, the backbone of the polymer, which is a ].<ref>{{cite journal |title=Carbon dioxide and carbon disulfide as resources for functional polymers |first1=Bungo |last1=Ochiai |first2=Takeshi |last2=Endo |journal=Progress in Polymer Science |volume=30 |issue=2 |pages=183–215 |doi=10.1016/j.progpolymsci.2005.01.005 |year=2005 }}</ref> |
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==Uses== |
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The principal industrial uses of carbon disulfide, consuming 75% of the annual production, are the manufacture of ] and ] film.<ref name="Ullmann" /> |
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It is also a valued intermediate in chemical synthesis of ]. It is widely used in the synthesis of ] such as ]s, which are used in ], a method for extracting metals from their ores. Carbon disulfide is also a precursor to ], which are used as drugs (e.g. ]) and ]. |
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===Niche uses=== |
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] |
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It can be used in ] of airtight storage warehouses, airtight flat storage, bins, ], railroad ], ship holds, ], and cereal mills.<ref>{{Greenwood&Earnshaw2nd|page=}}</ref> Carbon disulfide is also used as an ] for the fumigation of grains, nursery stock, in fresh fruit conservation, and as a ] against insects and ].<ref>{{cite book |last1=Worthing |first1=Charles R. |last2=Hance |first2=Raymond J. |title=The Pesticide Manual, A World Compendium |publisher=British Crop Protection Council |year=1991 |edition=9th |isbn=9780948404429 |url-access=registration |url=https://archive.org/details/pesticidemanualw0000unse }}</ref> |
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It can also be used for the ]. |
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==Health effects== |
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Carbon disulfide has been linked to both ] and chronic forms of ], with a diverse range of symptoms.<ref>{{Cite web|url=https://www.atsdr.cdc.gov/phs/phs.asp?id=472&tid=84#bookmark05|title=ATSDR - Public Health Statement: Carbon Disulfide|website=www.atsdr.cdc.gov|access-date=2020-01-17}}</ref> |
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Concentrations of 500–3000 mg/m<sup>3</sup> cause acute and subacute poisoning. These include a set of mostly neurological and psychiatric symptoms, called encephalopathia sulfocarbonica. Symptoms include acute ] (manic ], ]), ] ideas, loss of appetite, gastrointestinal and sexual disorders, ], ], and mood changes (including irritability and anger). Effects observed at lower concentrations include neurological problems (], psychomotor and psychological disturbances, ], abnormalities in nerve conduction), ] problems, vision problems (burning eyes, abnormal light reactions, increased ]<!--blurred vision{{cn}}-->), heart problems (increased deaths for heart disease, ], ]), reproductive problems (increased ], ] or ] sperm), and decreased immune response.<ref name="WHO">{{cite book |title=Air Quality Guidelines |date=2000 |publisher=WHO Regional Office for Europe, Copenhagen, Denmark |edition=2 |url=https://www.euro.who.int/__data/assets/pdf_file/0019/123058/AQG2ndEd_5_4carbodisulfide.PDF |access-date=31 July 2021 |chapter=Chapter 5.4 : Carbon disulfide |archive-date=18 October 2022 |archive-url=https://web.archive.org/web/20221018194943/https://www.euro.who.int/__data/assets/pdf_file/0019/123058/AQG2ndEd_5_4carbodisulfide.PDF |url-status=dead }}</ref><ref>{{Cite report |url=https://www.cdc.gov/niosh/docs/2018-124/ |title=Preventing hearing loss caused by chemical (ototoxicity) and noise exposure. |date=2018-03-01 |publisher=U.S. Department of Health and Human Services, Public Health Service, Centers for Disease Control and Prevention, National Institute for Occupational Safety and Health |doi=10.26616/nioshpub2018124 |language=en|doi-access=free }}</ref><!--cramps, muscle weakness, pain, ] impairment, ], ], ], ], and death by ]{{cn}}<ref name="Ullmann">Lay, Manchiu D. S.; Sauerhoff, Mitchell W.; Saunders, Donald R.; "Carbon Disulfide", in ''Ullmann's Encyclopedia of Industrial Chemistry'', Wiley-VCH, Weinheim, 2000 {{DOI| 10.1002/14356007.a05_185}}</ref><ref>{{Cite book|title=The Golden Thread: How Fabric Changed History|last=St. Clair|first=Kassia|publisher=John Murray|year=2018|isbn=978-1-4736-5903-2|location=London|pages=213–215|oclc=1057250632}}</ref><ref>{{cite book |last1=Blanc, M.D. |first1=Paul David |title=Fake Silk / The Lethal History of Viscose Rayon |date=15 November 2016 |publisher=Yale University Press |isbn=9780300204667 |page=79 |url=https://yalebooks.yale.edu/book/9780300204667/fake-silk |access-date=17 December 2020 |quote=in 1915,... carbon disulfide poisoning cases....one worker had been briefly committed to an asylum and several others had experienced nervous system complaints...}}</ref>--> |
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] to carbon disulfide is also associated with ], particularly ].<ref name="SBU2017">{{cite web |url=http://www.sbu.se/en/publications/sbu-assesses/occupational-health-and-safety--chemical-exposure/ |title=Occupational health and safety – chemical exposure |publisher=] (SBU) |website=www.sbu.se |language=en |access-date=2017-06-07 |archive-url=https://web.archive.org/web/20170606093333/http://www.sbu.se/en/publications/sbu-assesses/occupational-health-and-safety--chemical-exposure/ |archive-date=2017-06-06 |url-status=dead }}</ref> |
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In 2000, the WHO believed that health harms were unlikely at levels below 100 μg/m<sup>3</sup>, and set this as a guideline level.{{needs update|date=November 2023}} Carbon disulfide can be smelled at levels above 200 μg/m<sup>3</sup>, and the WHO recommended a sensory guideline of below 20 μg/m<sup>3</sup>. Exposure to carbon disulfide is well-established to be harmful to health in concentrations at or above 30 mg/m<sup>3</sup>. Changes in the function of the central nervous system have been observed at concentrations of 20–25 mg/m<sup>3</sup>. There are also reports of harms to health at 10 mg/m<sup>3</sup>, for exposures of 10–15 years, but the lack of good data on past exposure levels make the association of these harms with concentrations of 10 mg/m<sup>3</sup> findings uncertain. The measured concentration of 10 mg/m<sup>3</sup> may be equivalent to a concentration in the general environment of 1 mg/m<sup>3</sup>.<ref name="WHO"/> |
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===Environmental sources=== |
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The primary source of carbon disulfide in the environment is ] factories.<ref name="WHO"/> Most global carbon disulfide emissions come from rayon production, as of 2008.<ref name=dir/> Other sources include the production of ], ],<ref name=dir>{{cite web |url=https://www.dir.ca.gov/dosh/DoshReg/CarbonDisulfide5155-4-08.doc|type=DOC|title=Carbon Disulfide Health Effects Assessment for HEAC Discussion April 2008|date=April 2008|website=Division of Occupational Safety and Health|publisher=State of California Department of Industrial Relations|access-date=24 March 2023}}</ref> ], and sulfur recovery. Carbon disulfide production also emits hydrogen sulfide.<ref name=large-scale/> |
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{{as of|2004}}, about 250 g of carbon disulfide is emitted per kilogram of rayon produced. About 30 g of carbon disulfide is emitted per kilogram of carbon black produced. About 0.341 g of carbon disulfide is emitted per kilogram of sulfur recovered.<ref name=large-scale/> |
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Japan has reduced carbon disulfide emissions per kilogram of rayon produced, but in other rayon-producing countries, including China, emissions are assumed to be uncontrolled (based on global modelling and large-scale free-air concentration measurements). Rayon production is steady or decreasing except in China, where it is increasing, {{as of|lc=yes|2004}}.<ref name=large-scale>{{cite journal |last1=Blake |first1=Nicola J. |title=Carbonyl sulfide and carbon disulfide: Large-scale distributions over the western Pacific and emissions from Asia during TRACE-P |journal=Journal of Geophysical Research |date=2004 |volume=109 |issue=D15 |pages=D15S05 |doi=10.1029/2003JD004259|bibcode=2004JGRD..10915S05B |s2cid=43793469 |url=https://scholars.unh.edu/cgi/viewcontent.cgi?article=1072&context=earthsci_facpub |doi-access=free }}</ref> Carbon black production in Japan and Korea uses incinerators to destroy about 99% of the carbon disulfide that would otherwise be emitted.<ref name=large-scale/> When used as a ], Japanese emissions are about 40% of the carbon disulfide used; elsewhere, the average is about 80%.<ref name=large-scale/> |
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Most rayon production uses carbon sulfide.<ref name=SwanBlanc>{{cite news |last1=Swan |first1=Norman |last2=Blanc |first2=Paul |title=The health burden of viscose rayon |url=http://www.abc.net.au/radionational/programs/healthreport/the-health-burden-of-viscose-rayon/8286870 |work=ABC Radio National |date=20 February 2017 |language=en|access-date=24 March 2023}}</ref><ref name="scientificamerican.com">{{cite magazine|title=Bamboo Boom: Is This Material for You?|author=Nijhuis, Michelle |magazine=Scientific American Special Editions|volume=19|issue=2|pages=60–65|url=https://www.scientificamerican.com/article/bamboo-boom/|access-date=24 March 2023|year=2009|bibcode=2009SciAm..19f..60N}}</ref> One exception is rayon made using the ] process, which uses a different solvent; {{as of|lc=yes|2018}} the lyocell process is not widely used, because it is more expensive than the viscose process.<ref name=brief>{{cite journal |title=Regenerated cellulose by the Lyocell process, a brief review of the process and properties :: BioResources |journal=BioRes |url=https://bioresources.cnr.ncsu.edu/resources/regenerated-cellulose-by-the-lyocell-process-a-brief-review-of-the-process-and-properties/ |date=2018}}</ref><ref name=thesis>{{cite thesis |last1=Tierney |first1=John William |title=Kinetics of Cellulose Dissolution in N-MethylMorpholine-N-Oxide and Evaporative Processes of Similar Solutions |date=2005 |url=https://trace.tennessee.edu/cgi/viewcontent.cgi?referer=&httpsredir=1&article=3796&context=utk_gradthes}}</ref> ] also does not use carbon disulfide. |
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===Historic and current exposure=== |
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Industrial workers working with carbon disulfide are at high risk. Emissions may also harm the health of people living near rayon plants.<ref name="WHO"/> |
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Concerns about carbon disulfide exposure have a long history.<ref name="Ullmann">Lay, Manchiu D. S.; Sauerhoff, Mitchell W.; Saunders, Donald R.; "Carbon Disulfide", in ''Ullmann's Encyclopedia of Industrial Chemistry'', Wiley-VCH, Weinheim, 2000 {{doi| 10.1002/14356007.a05_185}}</ref><ref>{{Cite book|title=The Golden Thread: How Fabric Changed History|last=St. Clair|first=Kassia|publisher=John Murray|year=2018|isbn=978-1-4736-5903-2|location=London|pages=213–215|oclc=1057250632}}</ref><ref name="Blanc 2016">{{cite book |last1=Blanc, M.D. |first1=Paul David |title=Fake Silk / The Lethal History of Viscose Rayon |date=15 November 2016 |publisher=Yale University Press |isbn=9780300204667 |url=https://yalebooks.yale.edu/book/9780300204667/fake-silk |access-date=17 December 2020 |quote=in 1915,... carbon disulfide poisoning cases....one worker had been briefly committed to an asylum and several others had experienced nervous system complaints...}}</ref>{{rp|79}} Around 1900, carbon disulfide came to be widely used in the production of ]. The ] produced by high exposures was immediately apparent (it has been reported with 6 months of exposure<ref name="WHO"/>). ] told a story about a ] that put bars on its windows so that the workers would not ].<ref name="Blanc 2016"/>{{rp|17|\}} Carbon disulfide's use in the US as a heavier-than-air burrow poison for ] also led to reports of psychosis. No systematic medical study of the issue was published, and knowledge was not transferred to the rayon industry.<ref name=SwanBlanc/> |
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The first large epidemiological study of rayon workers was done in the US in the late 1930s, and found fairly severe effects in 30% of the workers. Data on increased risks of heart attacks and strokes came out in the 1960s. ], a major ], worked hard to prevent publication of this data in the UK.<ref name=SwanBlanc/> Average concentrations in sampled rayon plants were reduced from about 250 mg/m<sup>3</sup> in 1955–1965 to about 20–30 mg/m<sup>3</sup> in the 1980s (US figures only?{{globalize inline|US|date=October 2021}}).<ref name="WHO"/> Rayon production has since largely moved to the developing world, especially China, Indonesia and India.<ref name="scientificamerican.com"/><ref name=SwanBlanc/> |
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Rates of ] in modern factories are unknown, {{as of|lc=yes|2016}}.<ref name="scientificamerican.com"/><ref name="Monosson">{{cite journal |doi= 10.1126/science.aak9834|pmid=27884997|title=Toxic textiles|year= 2016 |last1= Monosson |first1= Emily |journal= Science|volume= 354|issue= 6315 |page=977|bibcode= 2016Sci...354..977M|s2cid=45869497}}</ref> Current manufacturers using the ] process do not provide any information on harm to their workers.<ref name=SwanBlanc/><ref name="scientificamerican.com"/> |
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==See also== |
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* ] |
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* ] |
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* ] |
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* ] |
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* ] |
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* ], accident with truck carrying carbon disulfide. |
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==References== |
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{{reflist}} |
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==External links== |
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{{Commons category|Carbon disulfide}} |
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{{EB1911 poster|Carbon Bisulphide}} |
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* |
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* |
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* Agency for Toxic Substances & Disease Registry , 1996. |
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* by the ] |
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* {{cite book |last1=Blanc |first1=Paul David |title=Fake silk : the lethal history of viscose rayon |date=2016 |publisher=Yale University Press |location=New Haven |isbn=9780300204667 |pages=328 |url=https://yalebooks.yale.edu/book/9780300204667/fake-silk}} |
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{{Carbon compounds}} |
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{{Sulfides}} |
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{{Authority control}} |
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{{DEFAULTSORT:Carbon Disulfide}} |
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] |
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] |
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] |
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] |
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