|Jmol-3D images||Image 1|
|Molar mass||76.139 g/mol|
|Melting point||−110.8 °C (−167.4 °F; 162.3 K)|
|Boiling point||46.3 °C (115.3 °F; 319.4 K)|
|Solubility in water||2.9 g/kg (20 °C)|
|Solubility||soluble in alcohol, ether, benzene, oil. chloroform, CCl4|
|Refractive index (nD)||1.6295|
|EU classification||T, Xi, F|
|R-phrases||R11, R36/38, R48/23, R62, R63|
|S-phrases||(S1/2), S16, S33, S36/37, S45|
|Flash point||−30 °C (−22 °F; 243 K)|
|Related compounds||Carbon dioxide
|Supplementary data page|
|n, εr, etc.|
Solid, liquid, gas
|Spectral data||UV, IR, NMR, MS|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Carbon disulfide is a colorless volatile liquid with the formula CS2. The compound is used frequently as a building block in organic chemistry as well as an industrial and chemical non-polar solvent. It has an "ether-like" odor, but commercial samples are typically contaminated with foul-smelling impurities, such as carbonyl sulfide.
Occurrence and manufacture
Small amounts of carbon disulfide are released by volcanic eruptions and marshes. CS2 once was manufactured by combining carbon (or coke) and sulfur at high temperatures. A lower temperature reaction, requiring only 600 °C utilizes natural gas as the carbon source in the presence of silica gel or alumina catalysts:
- 2CH4 + S8 → 2CS2 + 4H2S
- CS2 + 3O2 → CO2 + 2SO2
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. USA production in 2007 was 56,000 tonnes.
Compared to CO2, CS2 is more reactive toward nucleophiles and more easily reduced. These differences in reactivity can be attributed to the weaker π donor-ability of the sulfido centers, which renders the carbon more electrophilic. It is widely used in the synthesis of organosulfur compounds such as metham sodium, a soil fumigant and is commonly used in the production of the soft fabric viscose.
Addition of nucleophiles
Nucleophiles such as amines afford dithiocarbamates:
- 2R2NH + CS2 → [R2NH2+][R2NCS2−]
- RONa + CS2 → [Na+][ROCS2−]
This reaction is the basis of the manufacture of regenerated cellulose, the main ingredient of viscose, rayon and cellophane. Both xanthates and the related thioxanthates (derived from treatment of CS2 with sodium thiolates) are used as flotation agents in mineral processing.
Sodium sulfide affords trithiocarbonate:
- Na2S + CS2 → [Na+]2[CS32−]
This conversion proceeds via the intermediacy of thiophosgene, CSCl2.
Carbon disulfide hydrolase
Carbon disulfide is naturally formed in the mudpots of volcanic solfataras. It serves as a source of hydrogen sulfide, which is an electron donor for certain organisms that oxidize it into sulphuric acid or related sulfur oxides. The hyperthermophilic Acidianus strain was found to convert CS2 into H2S and CO2. The enzyme responsible for this conversion is termed carbon disulfide hydrolase.
The mechanism by this hydrolase converts CS2 into H2S is similar to that of how carbonic anhydrase hydrates CO2 to HCO3−. This similarity points to a likely mechanism.
CS2 polymerizes upon photolysis or under high pressure to give an insoluble material called "Bridgman's black", named after the discoverer of the polymer, P. W. Bridgman. Trithiocarbonate (-S-C(S)-S-) linkages comprise, in part, the backbone of the polymer, which is a semiconductor.
At high levels, carbon disulfide may be life-threatening because it affects the nervous system. Significant safety data comes from the viscose rayon industry, where both carbon disulfide as well as small amounts of H2S may be present.
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- Australian National Pollutant Inventory: Carbon disulfide
- CDC - NIOSH Pocket Guide to Chemical Hazards - Carbon Disulfide
- Inno Motion Engineering