1,1,2-Trichloro-1,2,2-trifluoroethane

CFC-113 can be prepared from hexachloroethane and hydrofluoric acid:[6]

${\displaystyle {\ce {C2Cl6 + 3HF -> CF2Cl-CFCl2 + 3HCl}}}$

This reaction may require catalysts such as antimony, chromium, iron and alumina at high temperatures.[7]

Another synthesis method uses HF on tetrachloroethylene instead.[8]

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 remains in the atmosphere about 90 years,[9] 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 (where sunlight in the 190-225 nm (UV) range), generating chlorine radicals (Cl•), which initiate degradation of ozone requiring only a few minutes:[10][11]

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. In some parts of the world, these reactions have significantly thinned the Earth's natural stratospheric ozone layer that shields the biosphere against solar UV radiation; increased UV levels at the surface can cause skin cancer or even blindness.[12]

CFC-113 was one of the most heavily produced CFCs. In 1989, an estimated 250,000 tons were produced.[5] It has been used as a cleaning agent for electrical and electronic components.[12] CFC-113’s low flammability and low toxicity made it ideal for use as a cleaner for delicate electrical equipment, fabrics, and metals. It would not harm the product it was cleaning, ignite with a spark or react with other chemicals.[13] It was used as a dry-cleaning solvent and was 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).[14][15]

CFC-113 is one of the three most popular CFCs, along with CFC-11 and CFC-12.[16]

CFC-113 in laboratory analytics has been replaced by other solvents.[17]

Reduction of CFC-113 with zinc gives chlorotrifluoroethylene:[5]

CFCl₂−CClF₂ + Zn → CClF=CF₂ + ZnCl₂

Aside from its immense environmental impacts, Freon 113, like most chlorofluoroalkanes, forms phosgene gas when exposed to a naked flame.[18]

• 1,1,1-Trichloro-2,2,2-trifluoroethane