Tetrachloro-1,1-difluoroethane or 1,1,1,2-tetrachloro-2,2-difluoroethane, Freon 112a, R-112a, or CFC-112a is an asymmetric chlorofluorocarbon isomer of tetrachloro-1,1-difluoroethane with formula CClF2CCl3. It contains ethane substituted by four chlorine atoms and two fluorine atoms. With a boiling point of 91.5°C it is the freon with second highest boiling point.
It can also be made in a reaction with hydrogen fluoride with hexachloroethane or tetrachloroethane with extra chlorine. This reaction occurs with an aluminium fluoride catalyst at 400°C. unsymmetrical trichlorotrifluoroethane (CCl2FCClF2) is also produced along with other chlorofluorocarbons. Separation of the symmetrical and unsymmetrical isomer is difficult.[4]
Properties
Tetrachloro-1,1-difluoroethane is non-combustible.
It has a critical pressure of 4.83MPa and a critical temperature of 279.2°C.[clarification needed] At the critical point the density is 0.754 g/cm3.[5]
Tetrachloro-1,1-difluoroethane in liquid form is miscible with perfluorocarbons.[6]
Tetrachlorodifluoroethane (CFC-112a), as with most high boiling point CFCs, has various uses as a non-flammable and clean agent solvent. It has historically been used as an extractant in liquid-liquid extraction and dry cleaning processes. CFC-112 and CFC-112a have also been used as feedstock chemicals in the manufacturing of fluorovinyl ethers.[8] CFC-112a and its isomers are attractive organic solvents, as they have many important properties: they are nonflammable, clean drying, and have lower toxicity than common chlorinated organic solvents.[9]
Tetrachlorodifluoroethane (mixture of isomers) has a niche application as a veterinary medicine to treat parasites (Fasciola hepatica).[10]
Atmosphere
Tetrachloro-1,1-difluoroethane was first detected in air collected from Cape Grim, Tasmania in the Cape Grim Air Archive, and later from air bubbles in snow from Greenland. The substance made its first appearance around 1965, and increased in level until around 2000.[11] In 2000 Earth's atmosphere contained 0.08 parts per trillion of Freon 112a.[12] Level slightly declined to 0.07 ppt by 2012.[11] Estimated lifetime in the stratosphere is 44 years.[12] By 2014 3,600 tons of Freon 112a had been put into the atmosphere.[11] As of 2023, levels have been rising in the Earth's atmosphere.[13]
As a greenhouse gas its radiative efficiency is 0.25 Wm−2ppb−1.[12]
1 2 3 Miller, William T.; Fager, Edward W.; Griswald, Paul H. (February 1950). "The Rearrangement of Chlorofluorocarbons by Aluminum Chloride 1". Journal of the American Chemical Society. 72 (2): 705–707. Bibcode:1950JAChS..72..705M. doi:10.1021/ja01158a013.
↑ Gallagher, C. H.; Boray, J. C.; Koch, J. H. (June 1965). "Toxicity of Samples of Tetrachlorodifluoroethane". Australian Veterinary Journal. 41 (6): 167–172. doi:10.1111/j.1751-0813.1965.tb01814.x. PMID14337687.
↑ Vecchio, M; Groppelli, G; Tatlow, J. C. (1 July 1974). "Studies on a vapour-phase process for the manufacture of chlorofluoroethanes". Journal of Fluorine Chemistry. 4 (2): 117–139. Bibcode:1974JFluC...4..117V. doi:10.1016/S0022-1139(00)82507-5.
Sládek, Petr; Navrátil, Oldřich; Linhart, Petr (1992). "Extraction of Selected Lanthanoids and Scandium with Bis(2-ethylhexyl)hydrogenphosphate in 1,1,2,2-Tetrachlorodifluoroethane". Collection of Czechoslovak Chemical Communications. 57 (8): 1647–1654. doi:10.1135/cccc19921647.
Sládek, Petr; Navrátil, Oldřich; Linhart, Petr (1992). "Extraction of Ce, Pm, Eu, Tm and Sc Using Di-n-butylhydrogenphosphate in 1,1,2,2-Tetrachlorodifluoroethane". Collection of Czechoslovak Chemical Communications. 57 (8): 1639–1646. doi:10.1135/cccc19921639.
Kakáč, B.; Hudlický, M. (1965). "Organic compounds of fluorine. VII. Spectrophotometric study in the series of halofluoroethanes". Collection of Czechoslovak Chemical Communications. 30 (3): 745–751. doi:10.1135/cccc19650745.
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