Carbonyl Sulfide - Wikipedia

Carbonyl sulfide

Names
IUPAC names Carbonyl sulfide[1] Oxidosulfidocarbon[1]
Systematic IUPAC name Thioxomethanone
Identifiers
CAS Number	463-58-1 Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:16573 Y
ChemSpider	9644 Y
ECHA InfoCard	100.006.674
EC Number	207-340-0
KEGG	C07331 Y
PubChem CID	10039
UNII	871UI0ET21 Y
UN number	2204
CompTox Dashboard (EPA)	DTXSID6023949
InChI InChI=1S/COS/c2-1-3 YKey: JJWKPURADFRFRB-UHFFFAOYSA-N Y InChI=1/COS/c2-1-3Key: JJWKPURADFRFRB-UHFFFAOYAF
SMILES O=C=S
Properties
Chemical formula	COS
Molar mass	60.075 g/mol
Appearance	colorless gas
Odor	sulfide-like
Density	2.51 g/L
Melting point	−138.8 °C (−217.8 °F; 134.3 K)
Boiling point	−50.2 °C (−58.4 °F; 223.0 K)
Critical point (T, P)	101.85 °C (215.3 °F; 375.0 K), 58.03 standard atmospheres (5,879.9 kPa; 852.8 psi)[2]
Solubility in water	0.376 g/100 mL (0 °C) 0.125 g/100 mL (25 °C)
Solubility	very soluble in KOH, CS2 soluble in alcohol, toluene
Magnetic susceptibility (χ)	−32.4×10−6 cm3/mol
Dipole moment	0.65 D
Thermochemistry
Heat capacity (C)	41.5 J/(mol⋅K)
Std molarentropy (S⦵298)	231.5 J/(mol⋅K)
Std enthalpy offormation (ΔfH⦵298)	−141.8 kJ/mol
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H220, H315, H319, H331, H335
Precautionary statements	P210, P261, P264, P271, P280, P302+P352, P304+P340, P305+P351+P338, P311, P312, P321, P332+P313, P337+P313, P362, P377, P381, P403, P403+P233, P405, P410+P403, P501
NFPA 704 (fire diamond)	3 4 1
Explosive limits	12–29%
Safety data sheet (SDS)	Carbonyl sulfide MSDS
Related compounds
Related compounds	Carbon dioxideCarbon disulfideCarbonyl selenide
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

Chemical compound

Carbonyl sulfide is the chemical compound with the linear formula O=C=S. It is a colorless flammable gas with an unpleasant odor. It is a linear molecule consisting of a carbonyl double bonded to a sulfur atom. Carbonyl sulfide can be considered to be intermediate between carbon dioxide and carbon disulfide, both of which are valence isoelectronic with it.

Occurrence

[edit]

Carbonyl sulfide is the most abundant sulfur compound naturally present in the atmosphere, at 0.5±0.05 ppb, because it is emitted from oceans, volcanoes and deep sea vents. As such, it is a significant compound in the global sulfur cycle. Measurements on the Antarctica ice cores and from air trapped in snow above glaciers (firn air) have provided a detailed picture of OCS concentrations from 1640 to the present day and allow an understanding of the relative importance of anthropogenic and non-anthropogenic sources of this gas to the atmosphere.[3] Some carbonyl sulfide that is transported into the stratospheric sulfate layer is oxidized to sulfuric acid.[4] Sulfuric acid forms particulate which affects energy balance due to light scattering.[5] The long atmospheric lifetime of COS makes it the major source of stratospheric sulfate, though sulfur dioxide from volcanic activity can be significant too.[5] Carbonyl sulfide is also removed from the atmosphere by terrestrial vegetation by enzymes associated with the uptake of carbon dioxide during photosynthesis, and by hydrolysis in ocean waters.[6][7][8] Loss processes, such as these, limit the persistence (or lifetime) of a molecule of COS in the atmosphere to a few years.

The largest man-made sources of carbonyl sulfide release include its primary use as a chemical intermediate and as a byproduct of carbon disulfide production; however, it is also released from automobiles and their tire wear,[9] coal-fired power plants, coking ovens, biomass combustion, fish processing, combustion of refuse and plastics, petroleum manufacture, and manufacture of synthetic fibers, starch, and rubber.[10] The average total worldwide release of carbonyl sulfide to the atmosphere has been estimated[when?] at about 3 million tons per year, of which less than one third was related to human activity.[10] It is also a significant sulfur-containing impurity in many fuel gases such as synthesis gas, which are produced from sulfur-containing feedstocks.[11]

Carbonyl sulfide is present in foodstuffs, such as cheese and prepared vegetables of the cabbage family. Traces of COS are naturally present in grains and seeds in the range of 0.05–0.1 mg/kg.

Carbonyl sulfide has been observed in the interstellar medium (see also List of molecules in interstellar space), in comet 67P[12] and in the atmosphere of Venus, where, because of the difficulty of producing COS inorganically, it is considered a possible indicator of life.[13]

Reactions and applications

[edit]

Carbonyl sulfide is used as an intermediate in the production of thiocarbamate herbicides.[14]

The hydrolysis of carbonyl sulfide is promoted by chromium-based catalysts:[11]

COS + H2O → CO2 + H2S

This conversion is catalyzed in solution by carbonic anhydrase enzymes in plants and mammals. Because of this chemistry, the release of carbonyl sulfide from small organic molecules has been identified as a strategy for delivering hydrogen sulfide, which is gaseous signaling molecule.[15][16]

This compound is found to catalyze the formation of peptides from amino acids. This finding is an extension of the Miller–Urey experiment, and it is suggested that carbonyl sulfide played a significant role in the origin of life.[17]

In ecosystem science,[18] are increasingly being used to describe the rate of photosynthesis.[19][20]

Synthesis

[edit]

Carbonyl sulfide was first described in 1841,[21] but was apparently mischaracterized as a mixture of carbon dioxide and hydrogen sulfide. Carl von Than first characterized the substance in 1867. It forms when carbon monoxide reacts with molten sulfur:

CO + ⁠1/8⁠ S8 → COS

This reaction reverses above 1200 K (930 °C; 1700 °F).

A laboratory synthesis entails the reaction potassium thiocyanate and sulfuric acid:

KSCN + 2 H2SO4 + H2O → KHSO4 + NH4HSO4 + COS

The resulting gas contains significant amounts of byproducts and requires purification.[22]

Hydrolysis of isothiocyanates in hydrochloric acid solution also affords COS.

Toxicity

[edit]

Carbonyl sulfide has the "rotten egg" odor characteristic of sulfides, although some sources suggest that the associated odor is due to impurities, and not present in the pure compound.[23] The detectability threshold is estimated at 135μg/m 3 {\displaystyle ^{3}} .[23]

As of 1994, limited information existed on the acute toxicity of carbonyl sulfide in humans and in animals.[14] High concentrations (above 1000 ppm) can cause sudden collapse, convulsions, and death from respiratory paralysis.[10][14] Occasional fatalities have been reported, practically without local irritation or olfactory warning.[14] In tests with rats, 50% animals died when exposed to 1400 ppm of COS for 90 minutes, or at 3000 ppm for 9 minutes.[14] Limited studies with laboratory animals also suggest that continued inhalation of low concentrations (around 50 ppm for up to 12 weeks) does not affect the lungs or the heart.[14]

Carbonyl sulfide is a potential alternative fumigant[24] to methyl bromide and phosphine. In some cases, however, residues on the grain result in flavours that are unacceptable to consumers, such as in barley used for brewing.

References

[edit]

1. ^ a b International Union of Pure and Applied Chemistry (2005). Nomenclature of Inorganic Chemistry (IUPAC Recommendations 2005). Cambridge (UK): RSC–IUPAC. ISBN 0-85404-438-8. p. 292. Electronic version.
2. ^ Lide, David R.; Kehiaian, Henry V. (1994). CRC Handbook of Thermophysical and Themochemical Data (PDF). CRC Press. p. 32.
3. ^ Montzka, S. A.; Aydin, M.; Battle, M.; Butler, J. H.; Saltzman, E. S.; Hall, B. D.; Clarke, A. D.; Mondeel, D.; Elkins, J. W. (2004). "A 350-year atmospheric history for carbonyl sulfide inferred from Antarctic firn air and air trapped in ice" (PDF). Journal of Geophysical Research. 109 (D18): 22302. Bibcode:2004JGRD..10922302M. doi:10.1029/2004JD004686. S2CID 1261238. eid D22302.
4. ^ Crutzen, P. (1976). "The possible importance of COS for the sulfate layer of the stratosphere". Geophysical Research Letters. 3 (2): 73–76. Bibcode:1976GeoRL...3...73C. doi:10.1029/GL003i002p00073.
5. ^ a b Seinfeld, J. (2006). Atmospheric Chemistry and Physics. London: J. Wiley. ISBN 978-1-60119-595-1.
6. ^ Campbell, J. E.; Carmichael, G. R.; Chai, T.; Mena-Carrasco, M.; Tang, Y.; Blake, D. R.; Blake, N. J.; Vay, S. A.; Collatz, G. J.; Baker, I.; Berry, J. A.; Montzka, S. A.; Sweeney, C.; Schnoor, J. L.; Stanier, C. O. (2008). "Photosynthetic Control of Atmospheric Carbonyl Sulfide During the Growing Season". Science. 322 (5904): 1085–1088. Bibcode:2008Sci...322.1085C. doi:10.1126/science.1164015. PMID 19008442. S2CID 206515456.
7. ^ Kettle, A. J.; Kuhn, U.; von Hobe, M.; Kesselmeier, J.; Andreae, M. O. (2002). "Global budget of atmospheric carbonyl sulfide: Temporal and spatial variations of the dominant sources and sinks". Journal of Geophysical Research. 107 (D22): 4658. Bibcode:2002JGRD..107.4658K. doi:10.1029/2002JD002187.
8. ^ Montzka, S. A.; Calvert, P.; Hall, B. D.; Elkins, J. W.; Conway, T. J.; Tans, P. P.; Sweeney, C. (2007). "On the global distribution, seasonality, and budget of atmospheric carbonyl sulfide (COS) and some similarities to CO2". Journal of Geophysical Research. 112 (D9): 9302. Bibcode:2007JGRD..112.9302M. doi:10.1029/2006JD007665. eid D09302.
9. ^ Pos W, Berreshein B (1993). "Automotive tire wear as a source for atmospheric OCS and CS2". Geophysical Research Letters. 1 (9): 815–818. Bibcode:1993GeoRL..20..815P. doi:10.1029/93GL00972.
10. ^ a b c "Carbonyl Sulfide CASRN: 463-58-1". Hazardous Substances Data Bank. National Library of Medicine.
11. ^ a b Hiller, Heinz; Reimert, Rainer; Marschner, Friedemann; Renner, Hans-Joachim; Boll, Walter; Supp, Emil; Brejc, Miron; Liebner, Waldemar; Schaub, Georg; Hochgesand, Gerhard; Higman, Christopher; Kalteier, Peter; Müller, Wolf-Dieter; Kriebel, Manfred; Schlichting, Holger; Tanz, Heiner; Stönner, Hans-Martin; Klein, Helmut; Hilsebein, Wolfgang; Gronemann, Veronika; Zwiefelhofer, Uwe; Albrecht, Johannes; Cowper, Christopher J.; Driesen, Hans Erhard (2006). "Gas Production". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a12_169.pub2. ISBN 3527306730.
12. ^ Rosetta Blog. "OMET'S FIREWORK DISPLAY AHEAD OF PERIHELION". blogs.esa.int. European Space Agency. Retrieved 11 August 2015.
13. ^ Landis, G. A. (2003). "Astrobiology: the Case for Venus" (PDF). Journal of the British Interplanetary Society. 56 (7–8): 250–254. Bibcode:2003JBIS...56..250L.
14. ^ a b c d e f "Chemical Summary for Carbonyl Sulfide". U.S. Environmental Protection Agency. 2013-07-19. Archived from the original on 2015-07-01.
15. ^ Steiger, Andrea K.; Pardue, Sibile; Kevil, Christopher G.; Pluth, Michael D. (2016-06-15). "Self-Immolative Thiocarbamates Provide Access to Triggered H2S Donors and Analyte Replacement Fluorescent Probes". Journal of the American Chemical Society. 138 (23): 7256–7259. Bibcode:2016JAChS.138.7256S. doi:10.1021/jacs.6b03780. ISSN 0002-7863. PMC 4911618. PMID 27218691.
16. ^ Protoschill-Krebs, G.; Wilhelm, C.; Kesselmeier, J. (1996). "Consumption of carbonyl sulphide (COS) by higher plant carbonic anhydrase (CA)". Atmospheric Environment. 30 (18): 3151–3156. Bibcode:1996AtmEn..30.3151P. doi:10.1016/1352-2310(96)00026-X.
17. ^ Leman, L.; Orgel, L.; Ghadiri, M. R. (2004). "Carbonyl sulfide-mediated prebiotic formation of peptides". Science. 306 (5694): 283–6. Bibcode:2004Sci...306..283L. doi:10.1126/science.1102722. PMID 15472077. S2CID 11819295.
18. ^ What Carbonyl Sulfide Teaches Us About Earth's Biosphere on YouTube.
19. ^ Campbell, J. E.; Berry, J. A.; Seibt, U.; Smith, S. J.; Montzka, S. A.; Launois, T.; Belviso, S.; Bopp, L.; Laine, M. (April 2017). "Large historical growth in global terrestrial gross primary production". Nature. 544 (7648): 84–87. Bibcode:2017Natur.544...84C. doi:10.1038/nature22030. OSTI 1398774. PMID 28382993. S2CID 205255121.
20. ^ Yakir, Dan; Montzka, Stephen A.; Uri Dicken; Tatarinov, Fyodor; Rotenberg, Eyal; Asaf, David (March 2013). "Ecosystem photosynthesis inferred from measurements of carbonyl sulphide flux". Nature Geoscience. 6 (3): 186–190. Bibcode:2013NatGe...6..186A. doi:10.1038/ngeo1730. ISSN 1752-0908.
21. ^ Couërbe, J. P. (1841). "Ueber den Schwefelkohlenstoff". Journal für Praktische Chemie. 23 (1): 83–124. doi:10.1002/prac.18410230105.
22. ^ Ferm R. J. (1957). "The Chemistry of Carbonyl Sulfide". Chemical Reviews. 57 (4): 621–640. doi:10.1021/cr50016a002.
23. ^ a b CDC, Hydrogen Sulfide and Carbonyl Sulfide, 4. Chemical and Physical Information, p. 139. Retrieved 20 April 2025.
24. ^ Bartholomaeus, Andrew; Haritos, Victoria (2005). "Review of the toxicology of carbonyl sulfide, a new grain fumigant". Food and Chemical Toxicology. 43 (12): 1687–1701. doi:10.1016/j.fct.2005.06.016. PMID 16139940.

Further reading

[edit]

• Beck, M. T.; Kauffman, G. B. (1985). "COS and C3S2: The Discovery and Chemistry of Two Important Inorganic Sulfur Compounds". Polyhedron. 4 (5): 775–781. doi:10.1016/S0277-5387(00)87025-4.
• J. Elliott Campbell; Jürgen Kesselmeier; Dan Yakir; Joe A. Berry; Philippe Peylin; Sauveur Belviso; Timo Vesala; Kadmiel Maseyk; Ulrike Seibt; Huilin Chen; Mary E. Whelan; Timothy W. Hilton; Stephen A. Montzka; Max B. Berkelhammer; Sinikka T. Lennartz; Le Kuai; Georg Wohlfahrt; Yuting Wang; Nicola J. Blake; Donald R. Blake; James Stinecipher; Ian Baker; Stephen Sitch (2017). "Assessing a New Clue to How Much Carbon Plants Take Up". EOS. 98. doi:10.1029/2017EO075313. hdl:10871/31921.
• Svoronos P. D. N.; Bruno T. J. (2002). "Carbonyl sulfide: A review of its chemistry and properties". Industrial & Engineering Chemistry Research. 41 (22): 5321–5336. doi:10.1021/ie020365n.

External links

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• Carbonyl sulfide and origins of life
• Carbonyl sulfide as a potential fumigant
• Carbonyl sulfide in the atmosphere

v t e Inorganic compounds of carbon and related ions
Compounds	CF CO CO2 CO3 CO4 CO5 CO6 COS CS C2S2 CS2 CSe2 C3O2 C3S2 SiC
Carbon ions	Carbides [:C≡C:]2−, [::C::]4−, [:C=C=C:]4− Cyanide [:C≡N:]− Cyanate [:O−C≡N:]− Thiocyanate [:S−C≡N:]− Fulminate [:C≡N−O:]− Thiofulminate [:C≡N−S:]−
Nanostructures	Graphite intercalation compounds Fullerides
Oxides and related	Oxides Nitrides Metal carbonyls Carbonic acid Bicarbonates Carbonates

v t e Molecules detected in outer space
Molecules	Diatomic Aluminium monochloride Aluminium monofluoride Aluminium(II) oxide Argonium Carbon cation Carbon monophosphide Carbon monosulfide Carbon monoxide Cyano radical Diatomic carbon Fluoromethylidynium Helium hydride ion Hydrogen chloride Hydrogen fluoride Hydrogen (molecular) Hydroxyl radical Imidogen Iron(II) oxide Magnesium monohydride Methylidyne radical Nitric oxide Nitrogen (molecular) Oxygen (molecular) Phosphorus monoxide Phosphorus mononitride Potassium chloride Silicon carbide Silicon monoxide Silicon monosulfide Sodium chloride Sodium iodide Sulfanyl Sulfur mononitride Sulfur monoxide Titanium(II) oxide Triatomic Aluminium(I) hydroxide Aluminium isocyanide Amino radical Carbon dioxide Carbonyl sulfide CCP radical Chloronium Diazenylium Dicarbon monoxide Disilicon carbide Ethynyl radical Formyl radical Hydrogen cyanide (HCN) Hydrogen isocyanide (HNC) Hydrogen sulfide Hydroperoxyl Iron cyanide Isoformyl Magnesium cyanide Magnesium isocyanide Methylene Methylidynephosphane N2H+ Nitrous oxide Nitroxyl Ozone Potassium cyanide Sodium cyanide Sodium hydroxide Silicon carbonitride c-Silicon dicarbide SiNC Sulfur dioxide Thioformyl Thioxoethenylidene Titanium dioxide Tricarbon Trihydrogen cation Water Fouratoms Acetylene Ammonia Cyanoethynyl Formaldehyde Fulminic acid HCCN Hydrogen peroxide Hydromagnesium isocyanide Isocyanic acid Isothiocyanic acid Ketenyl Methyl cation Methyl radical Methylene amidogen Propynylidyne Protonated carbon dioxide Protonated hydrogen cyanide Silicon tricarbide Thiocyanic acid Thioformaldehyde Tricarbon monosulfide Tricarbon monoxide Fiveatoms Ammonium ion Butadiynyl Carbodiimide Cyanamide Cyanoacetylene Cyanoformaldehyde Cyanomethyl Cyclopropenylidene Formic acid Isocyanoacetylene Ketene Methane Methoxy radical Methylenimine Propadienylidene Protonated formaldehyde Silane Silicon-carbide cluster Sixatoms Acetonitrile Cyanobutadiynyl radical Cyclopropenone Diacetylene E-Cyanomethanimine Ethylene Formamide HC4N Ketenimine Methanethiol Methanol Methyl isocyanide Pentynylidyne Propynal Protonated cyanoacetylene Sevenatoms Acetaldehyde Acrylonitrile Vinyl cyanide Cyanodiacetylene Ethylene oxide Glycolonitrile Hexatriynyl radical Methyl isocyanate Methylamine Propyne Vinyl alcohol Eightatoms Acetic acid Acrolein Aminoacetonitrile Cyanoallene Ethanimine Glycolaldehyde Hexapentaenylidene Methyl formate Methylcyanoacetylene Nineatoms Acetamide Cyanohexatriyne Dimethyl ether Ethanethiol Ethanol Methyldiacetylene N-Methylformamide Octatetraynyl radical Propene Propionitrile Tenatomsor more Acetone Benzene Benzonitrile Buckminsterfullerene (C60, C60+, fullerene, buckyball) Butyronitrile C70 fullerene Cyanodecapentayne Ethyl formate Ethylene glycol Heptatrienyl radical Methyl acetate Methyl-cyano-diacetylene Methyltriacetylene Propionaldehyde Pyrimidine
Deuteratedmolecules	Ammonia Ammonium ion Formaldehyde Formyl radical Heavy water Hydrogen cyanide Hydrogen deuteride Hydrogen isocyanide N2D+ Propyne Trihydrogen cation
Unconfirmed	Anthracene Dihydroxyacetone Glycine Graphene H2NCO+ Hemolithin Linear C5 Methoxyethane Naphthalene cation Phosphine Pyrene Silylidyne
Related	Abiogenesis Astrobiology Astrochemistry Atomic and molecular astrophysics Chemical formula Circumstellar dust Circumstellar envelope Cosmic dust Cosmic ray Cosmochemistry Diffuse interstellar band Earliest known life forms Extraterrestrial life Extraterrestrial liquid water Forbidden mechanism Homochirality Intergalactic dust Interplanetary medium Interstellar medium Iron–sulfur world theory Kerogen Molecules in stars Nexus for Exoplanet System Science Organic compound Outer space PAH world hypothesis Photodissociation region Polycyclic aromatic hydrocarbon (PAH) Pseudo-panspermia RNA world hypothesis Spectroscopy Tholin
Category:Astrochemistry Outer space portal Astronomy portal Chemistry portal

v t e Sulfur compounds
Sulfides and disulfides	Al2S3 As2S2 As2S3 As2S5 As4S4 Au2S Au2S3 B2S3 BaS BeS Bi2S3 CS2 C3S2 C6S6 CaS CdS CeS CoS Cr2S3 CSSe CSTe CuFeS2 CuS D2S Dy2S3 Er2S3 EuS FeS2 GaS H2S HfS2 HgS In2S3 K2S LaS LiS MgS MoS2 MoS3 NaHS Na2S NH4HS NiS P4Sx PbS PbS2 PSCl3 PSI3 PtS ReS2 Re2S7 SiS SrS TlS VS SeS2 S2U WS2 WS3 Sb2S3 Sb2S5 Sb4S3O3 Sm2S3 Y2S3 ZrS2 La2O2S Gd2O2S
Sulfur halides	S2Br2 SBr2 S2Cl2 SCl2 SCl4 S2F2 SF2 SF4 S2F10 SF6 S2I2
Sulfur oxides and oxyhalides	BrSO3F S2O5Cl2 F2S5O2 FClO5S2 F2OS3 ISO3F F2O6S2 SO2 SO3 SOBr2 SOCl2 SOF2 SOF4 H2S3O6 I3SO3F S3O8Cl2 S3O8F2 H2SO3 H2SO4 H2S2O7 H2SO5 Sulfites CdSO3 K2SO3 Sulfates Ag2SO4 CaSO4 CuSO4 Cs2SO4 Er2(SO4)3 Eu2(SO4)3 HgSO4 K2SO4 KAl(SO4)2 NaAl(SO4)2 RaSO4 SnSO4 SrSO4 Ti(SO4)2 Tm2(SO4)3 Yb2(SO4)3 Zr(SO4)2
Sulfur nitrides	SN S2N2 S4N4
Thiocyanates	HSCN KSCN Co(SCN)2
Organic compounds	C2H4S C2H6S3 C4H4S C32H66S2 CHCl3S C2H3SN

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