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Dimethyl sulfide



Dimethyl sulfide
IUPAC name Dimethyl sulfide
Identifiers
CAS number 75-18-3
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

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.

Additional recommended knowledge

Contents

Natural sources and link with climate

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]

Industrial uses

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.

Safety

Dimethyl sulfide is flammable and an irritant. Dimethyl sulfide has an unpleasant odor at even extremely low concentrations.

See also

References

  1. ^ 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.
  2. ^ University of East Anglia press release, Cloning the smell of the seaside, February 2, 2007
  3. ^ 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.
  4. ^ 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.
  5. ^ Malin, G; Turner, SM; Liss, PS (1992). "Sulfur: The plankton/climate connection.". Journal of Phycology 28 (5): 590-597.
 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Dimethyl_sulfide". A list of authors is available in Wikipedia.
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