Cs2 polarity11/25/2023 ![]() Reduction of carbon disulfide with sodium affords sodium 1,3-dithiole-2-thione-4,5-dithiolate together with sodium trithiocarbonate: 4 Na + 4 CS 2 → Na 2C 3S 5 + Na 2CS 3 Chlorination Ĭhlorination of CS 2 provides a route to carbon tetrachloride: CS 2 + 3 Cl 2 → CCl 4 + S 2Cl 2 While, however, reactions of nucleophiles with CO 2 are highly reversible and products are only isolated with very strong nucleophiles, the reactions with CS 2 are thermodynamically more favored allowing the formation of products with less reactive nucleophiles. Upon treatment with sodium sulfide, carbon disulfide affords trithiocarbonate: Na 2S + CS 2 → 2Ĭarbon disulfide does not hydrolyze readily, although the process is catalyzed by an enzyme carbon disulfide hydrolase.Ĭompared to the isoelectronic carbon dioxide, CS 2 is a weaker electrophile. Both xanthates and the related thioxanthates (derived from treatment of CS 2 with sodium thiolates) are used as flotation agents in mineral processing. This reaction is the basis of the manufacture of regenerated cellulose, the main ingredient of viscose, rayon, and cellophane. Xanthates form similarly from alkoxides: RONa + CS 2 → ![]() Reactions Ĭombustion of CS 2 affords sulfur dioxide according to this ideal stoichiometry:ĬS 2 + 3 O 2 → CO 2 + 2 SO 2 With nucleophiles įor example, amines afford dithiocarbamates: 2 R 2NH + CS 2 → Solvent Ĭarbon disulfide is a solvent for phosphorus, sulfur, selenium, bromine, iodine, fats, resins, rubber, and asphalt. United States production in 2007 was 56,000 tonnes. 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. The reaction is analogous to the combustion of methane. C + 2S → CS 2Ī lower-temperature reaction, requiring only 600 ☌, utilizes natural gas as the carbon source in the presence of silica gel or alumina catalysts: 2 CH 4 + S 8 → 2 CS 2 + 4 H 2S CS 2 once was manufactured by combining carbon (or coke) and sulfur at 800–1000 ☌. Small amounts of carbon disulfide are released by volcanic eruptions and marshes. Their analysis was consistent with an empirical formula of CS 2. The composition of carbon disulfide was finally determined in 1813 by the team of the Swedish chemist Jöns Jacob Berzelius (1779–1848) and the Swiss-British chemist Alexander Marcet (1770–1822). He called it "liquid sulfur" ( flüssig Schwefel). In 1796, the German chemist Wilhelm August Lampadius (1772–1842) first prepared carbon disulfide by heating pyrite with moist charcoal. Pure carbon disulfide has a pleasant, ether- or chloroform-like odor, but commercial samples are usually yellowish and are typically contaminated with foul-smelling impurities. It is a colorless, flammable, neurotoxic liquid that is used as a building block in organic synthesis. Carbon disulfide (also spelled as carbon disulphide) is an inorganic compound with the chemical formula CS 2 and structure S=C=S.
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