1,1,2-Trichloro-1,2,2-trifluoroethane, also called simply trichlorotrifluoroethane (often abbreviated as TCTFE) or CFC-113, is a chlorofluorocarbon. It has the formula Cl2FC−CClF2. This colorless, volatile liquid was a versatile solvent[5] used in various precision cleaning operations until it was phased out due its impact on the ozone layer.
Another synthesis method uses HF on tetrachloroethylene instead.[8] Industrial production of CFC-113 began in the early 1940s.[9]
Uses
CFC-113 was one of the three most popular CFCs, along with CFC-11 and CFC-12.[10] In 1989, an estimated 250,000 tons were produced.[5] It has been used as a cleaning agent for electrical and electronic components.[11] CFC-113’s low flammability and low toxicity made it ideal for use as a cleaner for delicate electrical-electronic equipment such as printed circuit boards, fabrics, and metals. It would not harm the product it was cleaning, ignite with a spark or react with other chemicals.[12]
It was used as a dry-cleaning solvent, as an alternative to perchloroethylene, introduced by DuPont in March 1961 as "Valclene"[13] (former designated trade name was "Fasclene"[14] but it was later changed to Valclene in the same year for legal reasons)[15][16] and was also marketed as the "solvent of the future" by Imperial Chemical Industries in the 1970s under the tradename "Arklone". Others from this series were Perklone (Tetrachloroethylene), Triklone (Trichloroethylene), Methoklone (Dichloromethane) and Genklene (1,1,1-Trichloroethane).[17][18] Its use in dry-cleaning peaked around 1971, and dry-cleaners using CFC-113 were known as Valclenerías in Spanish.[19] In 1986, 489 dry-cleaning facilities (about 2.2% of 21,787 dry-cleaning facilities) in the US were using CFC-113 as their main solvent.[20] It was seen as the perfect dry-cleaning solvent until its environmental effects were discovered.
CFC-113 in laboratory analytics and industry has been replaced by other solvents.[21]
When inhaled in large concentrations, trichlorotrifluoroethane can cause loss of consciousness.
CFC-113 measured by the Advanced Global Atmospheric Gases Experiment (AGAGE) in the lower atmosphere (troposphere) at stations around the world. Abundances are given as pollution free monthly mean mole fractions in parts-per-trillion.Atmospheric concentration of CFC-113 since year 1992.
CFC-113 is a very unreactive chlorofluorocarbon. It may remain in the atmosphere up to 90 years,[22] sufficiently long that it will cycle out of the troposphere and into the stratosphere. In the stratosphere, CFC-113 can be broken up by ultraviolet radiation (UV, sunlight in the 190-225nm range), generating chlorine radicals (Cl•), which initiate degradation of ozone requiring only a few minutes:[23][24]
CClF2CCl2F → C2F3Cl2 + Cl•
Cl• + O3 → ClO• + O2
This reaction is followed by:
ClO• + O → Cl• + O2
The process regenerates Cl• to destroy more O3. The Cl• will destroy an average of 100,000 O3 molecules during its atmospheric lifetime of 1–2 years.[11]
Aside from its immense environmental impacts, trichlorotrifluoroethane, like most chlorofluoroalkanes, forms phosgene gas when exposed to a naked flame.[25]
↑Touloukian, Y.S., Liley, P.E., and Saxena, S.C. Thermophysical properties of matter - the TPRC data series. Volume 3. Thermal conductivity - nonmetallic liquids and gases. Data book. 1970.
↑Kirk-Othmer Encyclopedia of Chemical Technology. 4th ed. Volumes 1: New York, NY. John Wiley and Sons, 1991-Present., p. V11 507 (1994)
↑Robert D. Ashford: Ashford's Dictionary of Industrial Chemicals, p. 1131. 2nd Edition. Wavelength Publications, 2001
↑Use and application of CFC-11, CFC-12, CFC-113 and SF6 as environmental tracers of groundwater residence time: A review Geoscience Frontiers Volume 10, Issue 5, September 2019, Pages 1643-1652; L.A. Chambers, D.C. Gooddy, A.M. Binley
