Difluoromethane

Difluoromethane

Names
Preferred IUPAC name Difluoromethane[1]
Other names Carbon fluoride hydride Methylene difluoride Methylene fluoride Freon-32
Identifiers
CAS Number	75-10-5 Y
3D model (JSmol)	Interactive image
Abbreviations	HFC-32 R-32 FC-32
Beilstein Reference	1730795
ChEBI	CHEBI:47855 Y
ChEMBL	ChEMBL115186 Y
ChemSpider	6105 Y
ECHA InfoCard	100.000.764
EC Number	200-839-4
Gmelin Reference	259463
MeSH	Difluoromethane
PubChem CID	6345
RTECS number	PA8537500
UNII	77JW9K722X N
UN number	3252
CompTox Dashboard (EPA)	DTXSID6029597
InChI InChI=1S/CH2F2/c2-1-3/h1H2 Y Key: RWRIWBAIICGTTQ-UHFFFAOYSA-N Y InChI=1/CH2F2/c2-1-3/h1H2 Key: RWRIWBAIICGTTQ-UHFFFAOYAC
SMILES FCF
Properties
Chemical formula	CH2F2
Molar mass	52.024 g·mol−1
Appearance	Colorless gas
Density	1.1 g cm−3(in liquid form)
Melting point	−136 °C (−213 °F; 137 K)
Boiling point	−52 °C (−62 °F; 221 K)
log P	-0.611
Vapor pressure	1518.92 kPa (at 21.1 °C)
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H220, H221, H280
Precautionary statements	P210, P377, P381, P403, P410+P403
NFPA 704 (fire diamond)	1 4 0
Autoignition temperature	648 °C (1,198 °F; 921 K)
Safety data sheet (SDS)	MSDS at Oxford University
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references

Difluoromethane, also called difluoromethylene, HFC-32 Methylene Fluoride or R-32, is an organic compound of the dihalogenoalkane variety. It has the formula of CH₂F₂. It is a colorless gas in the ambient atmosphere and is slightly soluble in water, with a high thermal stability.^{[2][failed verification]} Due to the low melting and boiling point, (-136.0 °C and -51.6 °C respectively) contact with this compound may result in frostbite.^{[2][failed verification]} In the United States, the Clean Air Act Section 111 on Volatile Organic Compounds (VOC) has listed difluoromethane as an exception (since 1997) from the definition of VOC due to its low production of tropospheric ozone.^[3] Difluoromethane is commonly used in endothermic processes such as refrigeration or air conditioning.

Synthesis

Difluoromethane is primarily synthesized via batch processes, by the reaction of dichloromethane and hydrogen fluoride (HF), in the liquid phase using SbCl₅ as a catalyst.^[4] Due to hydrogen fluoride's hazardous properties, a new synthesis was developed. The new synthesis allows for constant flow of difluoromethane production through an isolated chamber.^[4]

Applications

Difluoromethane is often used as a fire extinguishant due to its ability to undergo endothermic processes.^[5] Atmospheric concentration of difluoromethane at various latitudes since the year 2009 are shown to the left.

Difluoromethane is a molecule used as refrigerant that has prominent heat transfer and pressure drop performance, both in condensation and vaporization.^[6] It has a 100-year global warming potential (GWP) of 675 times that of carbon dioxide, and an atmospheric lifetime of nearly 5 years.^[7] It is classified as A2L - slightly flammable by ASHRAE,^[8] and has zero ozone depletion potential (ODP).^[9] Difluoromethane is thus a relatively low-risk choice among HFC refrigerants, most of which have higher GWP and longer persistence when leaks occur.

The common refrigerant R-410A is a zeotropic, 50/50-mass-percent mixture of difluoromethane and pentafluoroethane (R-125). Pentafluoroethane is a common replacement for various chlorofluorocarbons (i.e Freon) in new refrigerant systems, especially for air-conditioning. The zeotropic mix of difluoromethane with pentafluoroethane (R-125) and tetrafluoroethane (R-134a) is known as R-407A through R-407F depending on the composition. Likewise, R-504 is the azeotropic (48.2/51.8 mass%) mixture of difluoromethane and chlorotrifluoromethane (R13). In 2011 17,949,893 metric tons of difluoromethane were emitted into the atmosphere in the United States alone.^[10]

Difluoromethane is currently used by itself in residential and commercial air-conditioners in Japan, China, and India as a substitute for R-410A. In order to reduce the residual risk associated with its mild flammability, this molecule should be applied in heat transfer equipment with low refrigerant charge such as brazed plate heat exchangers (BPHE), or shell and tube heat exchangers and tube and plate heat exchangers with tube of small diameter.^[11] Many applications confirmed that difluoromethane exhibits heat transfer coefficients higher than those of R-410A under the same operating conditions but also higher frictional pressure drops.^[11]

Other uses of difluoromethane include its use as aerosol propellants, blowing agents, and solvents.^[3]

Environmental Effects

Every year, approximately 15 kilotons of difluoromethane are produced.^[3] In gas form, the compound will degrade in the atmosphere by reaction with photochemically-produced hydroxyl radicals. This process will form carbonyl difluoride. The half-life for this process is estimated to be 4 years.^[3] Difluoromethane tends to enter the environment via the gas phase and accumulates there more commonly than in soils or sediments. Volatilization half-lives of this compound are about 45 minutes for rivers and 69 hours for lakes, difluoromethane does not bioaccumulate in aquatic areas well.^[3]

HFC-32 released into the environment gets broken down into CF as an intermediate product. This goes on to create HF and CO₂ by hydrolysis in atmospheric water.^[3]

The global warming potential (GWP) of HFC-32 is estimated at 677 on a 100-year time window.^[12] This is far lower than the GWP for HFC refrigerants it is replacing, but remains sufficiently high to spur continued research into using lower-GWP refrigerants.

Difluoromethane is excluded from the list of VOCs supplied in the United States Clean Air Act due to the ODP being zero. Therefore, tropospheric ozone is not likely to be produced from this molecule. Tropospheric ozone may lead to adverse health effects such as respiratory, cardiac or neurological damage.^[3] Additionally, ozone can affect plant and vegetation by inducing the bronzing of leaves.^[3]

Toxicity

Difluoromethane shows slight maternal and developmental toxicity at concentrations of approximately 50,000 ppm in rats, but not in rabbits. The exposure limitations set on difluoromethane for human use are 1,000 ppm, making exposure to dangerous levels unlikely.^[3]

References

See also

• R-410A, a refrigerant that is being phased out, and which R-32 is a popular replace for
• R-454B, another R-410A replacement
• List of refrigerants

External links

• Flammability Measurements of Difluoromethane in Air at 100 °C Archived 2016-09-20 at the Wayback Machine
• Difluoromethane at Gas Encyclopaedia Archived 2016-03-03 at the Wayback Machine
• IR absorption spectra Archived 2006-10-13 at the Wayback Machine
• SDS Data sheet