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Dimethyl sulfide
From Wikipedia, the free encyclopedia
| Dimethyl sulfide | |
|---|---|
 |
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| IUPAC name | Dimethyl sulfide |
| Identifiers | |
| CAS number | |
| SMILES | CSC |
| Properties | |
| Molecular formula | C2H6S |
| Molar mass | 62.13 g/mol |
| Density | 0.840 g/cm³ |
| Melting point |
-98 °C |
| Boiling point |
37 °C |
| Hazards | |
| MSDS | OSHA MSDS |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Dimethyl sulfide (DMS) or methylthiomethane is a sulfur containing organic chemical compound with formula: (CH3)2S. Dimethyl sulfide in concentrated liquid form is flammable and insoluble with a boiling point of 37°C and a disagreeable odor. In vapor form it is produced by cooking of certain vegetables, notably corn and cabbage, and seafoods. It is also an indication of bacterial infection in malt production and brewing. It is a breakdown product of dimethylsulfoniopropionate (DMSP), and is also produced by the bacterial metabolism of methanethiol.
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DMS is the most abundant biological sulfur compound emitted to the atmosphere.[1] Emission occurs over the oceans by phytoplankton. While Andrew Johnston, of the University of East Anglia, has characterized DMS as being the "smell of the sea",[2] it would be more accurate to say that DMS is a component of the "smell of the sea," another being pheromones of algae called dictyopterenes. DMS is also produced naturally by bacterial transformation of dimethyl sulfoxide (DMSO) waste that is disposed of into sewers, where it can cause environmental odor problems.[3].
DMS is oxidized in the marine atmosphere to various sulfur-containing compounds, such as sulfur dioxide, dimethyl sulfoxide (DMSO), dimethyl sulfone, methane sulfonic acid and sulfuric acid. [4] Among these compounds, sulfuric acid has the potential to create new aerosols which act as cloud condensation nuclei. Through this interaction with cloud formation, the massive production of atmospheric DMS over the oceans may have a significant impact on the Earth's climate.[5]
Recent research suggests that marine bacteria are reducing the amount of this important climate cooling gas given off from our seas.[citation needed]
In industry it is used in petroleum refining and in petrochemical production processes to control the formation of coke and carbon monoxide. In addition it is used to control dusting in steel mills. It is also used in a range of organic syntheses, also being a side product of Swern oxidation. It also has a use as a food flavoring component. It can also be oxidized by natural or artificial means to dimethyl sulfoxide, (DMSO), which has several important solvent properties.
The largest single commercial producer of DMS in the world is Gaylord Chemical Corporation, which is a significant economic component of the paper industry of Bogalusa, Louisiana.
Dimethyl sulfide is flammable and an irritant. Dimethyl sulfide has an unpleasant odor at even extremely low concentrations.
- ^ Simpson, David; Winiwarter, Wilfried; Börjesson, Gunnar; Cinderby, Steve; Ferreiro, Antonio; Guenther, Alex; Hewitt, C. Nicholas; Janson, Robert; Khalil, M. Aslam K.; Owen, Susan; Pierce, Tom E.; Puxbaum, Hans; Shearer, Martha; Skiba, Ute; Steinbrecher, Rainer; Tarrasón, Leonor; Öquist, Mats G. (1999). "Inventorying emissions from nature in Europe". Journal of Geophysical Research. 104 (D7): 8113-8152. doi:10.1029/98JD02747.
- ^ University of East Anglia press release, Cloning the smell of the seaside, February 2, 2007
- ^ Glindemann, D., Novak, J., Witherspoon, J. (2006). "Dimethyl Sulfoxide (DMSO) Waste Residues and Municipal Waste Water Odor by Dimethyl Sulfide (DMS): the North-East WPCP Plant of Philadelphia.". Environmental Science and Technology 40 (1): 202-207. doi:S0013-936X(05)01312-X 10.1021/es051312a S0013-936X(05)01312-X.
- ^ Lucas, DD; Prinn, RG (2005). "Parametric sensitivity and uncertainty analysis of dimethylsulfide oxidation in the clear-sky remote marine boundary layer.". Atmospheric Chemistry and Physics 5: 1505-1525.
- ^ Malin, G; Turner, SM; Liss, PS (1992). "Sulfur: The plankton/climate connection.". Journal of Phycology 28 (5): 590-597.