| |||
| Names | |||
|---|---|---|---|
| Preferred IUPAC name 1,1,2-Trichloro-1,2,2-trifluoroethane | |||
| Other names Arklone P CFC-113 Freon 113 Frigen 113 TR Freon TF Valclene 1,1,2-trichlorotrifluoroethane TCTFE Solvent 113 | |||
| Identifiers | |||
| |||
3D model (JSmol) | |||
| ChEMBL | |||
| ChemSpider |
| ||
| ECHA InfoCard | 100.000.852 | ||
| UNII | |||
| |||
| |||
| Properties | |||
| CClF2CCl2F | |||
| Molar mass | 187.37 g·mol−1 | ||
| Appearance | Colorless liquid | ||
| Odor | likecarbon tetrachloride[1] | ||
| Density | 1.56 g/mL | ||
| Melting point | −35 °C (−31 °F; 238 K) | ||
| Boiling point | 47.7 °C (117.9 °F; 320.8 K) | ||
| 170 mg/L | |||
| Vapor pressure | 285 mmHg (20 °C)[1] | ||
| Thermal conductivity | 0.0729 W m−1 K−1 (300 K)[2] | ||
| Hazards | |||
| Lethal dose or concentration (LD, LC): | |||
LCLo (lowest published) | 250,000 ppm (mouse, 1.5 hr) 87,000 (rat, 6 hr)[3] | ||
| NIOSH (US health exposure limits): | |||
PEL (Permissible) | TWA 1000 ppm (7600 mg/m3)[1] | ||
REL (Recommended) | TWA 1000 ppm (7600 mg/m3) ST 1250 ppm (9500 mg/m3)[1] | ||
IDLH (Immediate danger) | 2000 ppm[1] | ||
| Hazards | |||
| GHS labelling:[4] | |||
  | |||
| Warning | |||
| NFPA 704 (fire diamond) | |||
| Safety data sheet (SDS) | https://datasheets.scbt.com/sc-251541.pdf | ||
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |||
1,1,2-Trichloro-1,2,2-trifluoroethane, also called simplytrichlorotrifluoroethane (often abbreviated asTCTFE) orCFC-113, is achlorofluorocarbon. It has the formulaCl2FC−CClF2. This colorless, volatile liquid was a versatile solvent[5] used in various precise cleaning operations until it was phased out due its impact on the ozone layer.
CFC-113 can be prepared fromhexachloroethane andhydrofluoric acid:[6]
This reaction may require catalysts such asantimony,chromium,iron andalumina at high temperatures.[7]
Another synthesis method uses HF ontetrachloroethylene instead.[8] Industrial production of CFC-113 began in the early 1940s.[9]
CFC-113 was one of the three most popular CFCs, along withCFC-11 andCFC-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 asprinted 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 adry-cleaning solvent, as an alternative to perchloroethylene, introduced byDuPont in March 1961 as "Valclene"[13] (former designated trade name was "Fasclene"[14] but it was later changed toValclene in the same year for legal reasons)[15][16] and was also marketed as the "solvent of the future" byImperial Chemical Industries in the 1970s under the tradename "Arklone". Others from this series werePerklone (Tetrachloroethylene),Triklone (Trichloroethylene),Methoklone (Dichloromethane) andGenklene (1,1,1-Trichloroethane).[17][18] Its use in dry-cleaning peaked around 1971, and dry-cleaners using CFC-113 were known asValclenerías 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]
Reduction of CFC-113 with zinc giveschlorotrifluoroethylene:[5]
When inhaled in large concentrations, trichlorotrifluoroethane can cause loss of consciousness.
CFC-113 is a very unreactive chlorofluorocarbon. It may remain in theatmosphere up to 90 years,[22] sufficiently long that it will cycle out of thetroposphere and into thestratosphere. In the stratosphere, CFC-113 can be broken up byultraviolet radiation (UV, sunlight in the 190-225 nm range), generating chlorine radicals (Cl•), which initiate degradation of ozone requiring only a few minutes:[23][24]
This reaction is followed by:
The process regenerates Cl• to destroy moreO3. The Cl• will destroy an average of 100,000O3 molecules during its atmospheric lifetime of 1–2 years.[11]
Aside from its immense environmental impacts, trichlorotrifluoroethane, like most chlorofluoroalkanes, formsphosgene gas when exposed to a naked flame.[25]
