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It is also considered as the anhydride of thiocarbonic acid. 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. In , the German chemist Wilhelm August Lampadius — first prepared carbon disulfide by heating pyrite with moist charcoal.
Small amounts of carbon disulfide are released by volcanic eruptions and marshes. The reaction is analogous to the combustion of methane. Carbon disulfide can dissolve a variety of nonpolar chemicals including phosphorus , sulfur, selenium , bromine , iodine , fats , resins , rubber , and asphalt.
Combustion of CS 2 affords sulfur dioxide according to this ideal stoichiometry:. For example, amines afford dithiocarbamates : [ 18 ]. Xanthates form similarly from alkoxides : [ 18 ]. 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 CS 2 with sodium thiolates are used as flotation agents in mineral processing.
Upon treatment with sodium sulfide , carbon disulfide affords trithiocarbonate : [ 18 ]. Carbon disulfide does not hydrolyze readily, although the process is catalyzed by an enzyme carbon disulfide hydrolase. Compared to the isoelectronic carbon dioxide , CS 2 is a weaker electrophile. 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.
