Trichlorofluoromethane

Trichlorofluoromethane

Names
Preferred IUPAC name Trichloro(fluoro)methane
Other names Trichlorofluoromethane Fluorotrichloromethane Fluorochloroform Freon 11 CFC 11 R 11 Arcton 9 Freon 11A Freon 11B Freon HE Freon MF
Identifiers
CAS Number	75-69-4 Y
3D model (JSmol)	Interactive image Interactive image
ChEBI	CHEBI:48236 Y
ChEMBL	ChEMBL348290 Y
ChemSpider	6149 Y
ECHA InfoCard	100.000.812
EC Number	200-892-3
PubChem CID	6389
RTECS number	PB6125000
UNII	990TYB331R Y
CompTox Dashboard (EPA)	DTXSID5021384
InChI InChI=1S/CCl3F/c2-1(3,4)5 Y Key: CYRMSUTZVYGINF-UHFFFAOYSA-N Y InChI=1/CCl3F/c2-1(3,4)5
SMILES C(F)(Cl)(Cl)Cl ClC(Cl)(Cl)F
Properties
Chemical formula	CCl3F
Molar mass	137.36 g·mol−1
Appearance	Colorless liquid/gas
Odor	nearly odorless[1]
Density	1.494 g/cm3
Melting point	−110.48 °C (−166.86 °F; 162.67 K)
Boiling point	23.77 °C (74.79 °F; 296.92 K)
Solubility in water	1.1 g/L (at 20 °C)
log P	2.53
Vapor pressure	89 kPa at 20 °C 131 kPa at 30 °C
Thermal conductivity	0.0079 W m−1 K−1 (gas at 300 K, ignoring pressure dependence)[2][verification needed]
Hazards
GHS labelling:[4]
Pictograms
Signal word	Warning
Hazard statements	H420
Precautionary statements	P502
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LCLo (lowest published)	26,200 ppm (rat, 4 hr) 100,000 ppm (rat, 20 min) 100,000 ppm (rat, 2 hr)[3]
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 1000 ppm (5600 mg/m3)[1]
REL (Recommended)	C 1000 ppm (5600 mg/m3)[1]
IDLH (Immediate danger)	2000 ppm[1]
Safety data sheet (SDS)	ICSC 0047
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is YN ?) Infobox references

Trichlorofluoromethane, also called freon-11, CFC-11, or R-11, is a chlorofluorocarbon (CFC). It is a colorless, faintly ethereal, and sweetish-smelling liquid that boils around room temperature.^[5] CFC-11 is a Class 1 ozone-depleting substance which damages Earth's protective stratospheric ozone layer.^[6] Also R-11 is not flammable at ambient temperature and pressure but it can become very combustible if heated and ignited by a strong ignition source.

Trichlorofluoromethane was first widely used as a refrigerant. Because of its high boiling point compared to most refrigerants, it can be used in systems with a low operating pressure, making the mechanical design of such systems less demanding than that of higher-pressure refrigerants R-12 or R-22.

Trichlorofluoromethane is used as a reference compound for fluorine-19 NMR studies.

Trichlorofluoromethane was formerly used in the drinking bird novelty, largely because it has a boiling point of 23.77 °C (74.79 °F). The replacement, dichloromethane, boiling point 39.6 °C (103.3 °F), requires a higher ambient temperature to work.

Prior to the knowledge of the ozone depletion potential of chlorine in refrigerants and other possible harmful effects on the environment, trichlorofluoromethane was sometimes used as a cleaning/rinsing agent for low-pressure systems.^[7]

Trichlorofluoromethane can be obtained by reacting carbon tetrachloride with hydrogen fluoride at 435 °C and 70 atm, producing a mixture of trichlorofluoromethane, tetrafluoromethane and dichlorodifluoromethane in a ratio of 77:18:5. The reaction can also be carried out in the presence of antimony(III) chloride or antimony(V) chloride:^[8]

${\displaystyle {\ce {CCl4 + HF -> CCl3F + CF4 + CCl2F2}}}$

Trichlorofluoromethane is also formed as one of the byproducts when graphite reacts with chlorine and hydrogen fluoride at 500 °C.^[8]

Sodium hexafluorosilicate under pressure at 270 °C, titanium(IV) fluoride, chlorine trifluoride, cobalt(III) fluoride, iodine pentafluoride, and bromine trifluoride are also suitable fluorinating agents for carbon tetrachloride.^[8][9]

${\displaystyle {\ce {CCl4 + Na2SiF6 -> CCl3F + CCl2F2 + CCl3F + NaCl + SiF4}}}$

${\displaystyle {\ce {CCl4 + BrF3 -> BrF + CCl2F2 + CCl3F}}}$

Trichlorofluoromethane was included in the production moratorium in the Montreal Protocol of 1987. It is assigned an ozone depletion potential of 1.0, and U.S. production was ended on January 1, 1996.^[6]

In 2018, the atmospheric concentration of CFC-11 was noted by researchers to be declining more slowly than expected,^[10][11] and it subsequently emerged that it remains in widespread use as a blowing agent for polyurethane foam insulation in the construction industry of China.^[12] In 2021, researchers announced that emissions declined by 20,000 U.S. tons from 2018 to 2019, which mostly reversed the previous spike in emissions.^[13] In 2022, the European Commission announced an updated regulation that mandates the recovery and prevention of emissions of CFC-11 blowing agents from foam insulation in demolition waste, which is still emitted at significant scale.^[14]

R11, like most chlorofluorocarbons, forms phosgene gas when exposed to a naked flame.^[15]

• 
  CFC-11 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.
• 
  Hemispheric and Global mean concentrations of CFC-11 (NOAA/ESRL)
• 
  Time-series of atmospheric concentrations of CFC-11 (Walker et al., 2000)
• 
  "Present day" (1990s) sea surface CFC-11 concentration
• 
  "Present day" (1990s) CFC-11 oceanic vertical inventory

• List of refrigerants
• IPCC list of greenhouse gases

• CFC-11 NOAA/ESRL Global measurements
• Public health goal for trichlorofluoromethane in drinking water
• Names at webbook.nist.gov
• Data sheet at speclab.com Archived 2007-06-09 at the Wayback Machine
• International Chemical Safety Card 0047
• NIOSH Pocket Guide to Chemical Hazards. "#0290". National Institute for Occupational Safety and Health (NIOSH).
• Phase change data at webbook.nist.gov
• Thermochemistry data at chemnet.ru
• ChemSub Online: Trichlorofluoromethane - CFC-11
• materialsproject.org