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EC number: 216-600-2
CAS number: 1623-05-8
PPVE is used as a monomer in polymer manufacture. PPVE is a liquid at
room temperature with a vapor pressure of 410 mm Hg at 20°C. The water
solubility is 1.8 mg/L at 22.3 °C. The measured Henry’s Law constant
(HLC) is 78.3 atm·m³/mole. The vapor pressure, water solubility and high
Henry’s law constant combine to move PPVE from any terrestrial
compartment into the atmosphere. Evaporation of PPVE from surfaces is
rapid. Fugacity modeling indicates that distribution from soil to air
dominates over all other processes, and therefore that release to soils
would result in rapid volatilization to the atmospheric compartment.
Given identified uses (manufacturing and polymerization) and technical
processes during use, essentially all releases are to the atmospheric
compartment. Assuming 100% release to the atmospheric compartment,
99.996% of substance remains in the gas phase of the air compartment,
with 0.0036% in gas-filled pore paces, and 0.00020% sorbed to soil
solids. Therefore, this compound will remain in the atmosphere when
released from industrial applications. Degradation in the environment
is by indirect photolysis, with a half-life of approximately 4.8 days.
The pathway for decay (1) is expected to be addition of hydroxyl radical
to the vinylic group followed by decay of the radical adduct. The
ultimate degradation products are expected to be perfluoropropionic acid
(PFPA) and hydrofluoric acid (HF). These acids are miscible in water and
are completely ionized in rainwater. They are expected to undergo wet
deposition with no further significant transformation. Degradation is
expected to take place after atmospheric mixing, and production of PFPA
would occur over a distributed area leading to trace levels in
terrestrial and aquatic systems.
USEPA states flatly that fluorocarbons do not deplete ozone because they
lack chlorine or bromine. Fluorine radicals do not contribute to ozone
depletion because of fast quenching of F* by water or hydrogen donors,
slow reaction of FO* radicals with oxygen, and obligate reformation of
F* in the pathway (3). F* radicals are rapidly and irreversibly removed
from the atmosphere after quenching as HF. Therefore, neither PPVE nor
any of its acidic photodegradation products contribute to ozone
PPVE is not expected to partition to moist soils or surface waters. Upon
accidental, direct release to the aquatic compartment, the chemical is
expected to volatilize rapidly. In closed-bottle (OECD301D) assays, ≤7%
biodegradation was observed. PPVE has a measured log n-octanol:water
partition coefficient of 4.0 and is expected to have little potential to
bioaccumulate. The calculated log Koa of PPVE is 0.46. This log Koa
value indicates that PPVE has a low potential to partition from air to
the lipid rich tissues of air-breathing organisms. Given its extremely
short half-life due to volatilization, it would not remain in aquatic
environments or organisms for a sufficient time to allow partitioning
into lipid tissues or to permit meaningful testing of bioconcentration.
Distribution of PFPA and HF in the environment is driven by the fact
that these acids are completely ionized at environmental pH values, are
miscible in water, and are not likely to bind with organic matter based
on low Koc values and low log Kow values. PFPA and HF will be associated
with the aqueous phase of any environment where they are released, and
will be highly mobile in soils. PFPA and HF that have deposited in
aquatic compartments are expected to remain in the aquatic compartment.
The registrant has assessed PFPA in ready biodegradation tests and
demonstrated that essentially no biodegradation occurs. The registrant
has completed a bioconcentration study of PFPA in carp. The BCF at
steady state was found to be 1.2 - ≤4.8. PFPA is not subject to
bioaccumulation in aquatic organisms.
HF is an inorganic mineral acid. It is not subject to biodegradation.
1) D. Amedro, L. Vereecken, J.N. Crowley. 2015. Kinetics and mechanism
of the reaction of perfluoro propyl vinyl ether (PPVE, C3F7OCF=CF2) with
OH: assessment of its fate in the atmosphere. Phys. Chem. Chem. Phys.
Vol. 17, pp. 18558–18566.
2) A.J. Colussi, M.A. Crela. 1994. Rate of the reaction between oxygen
monofluoride and ozone. Implications for the atmospheric role of
fluorine. Chem. Phys. Lett. Vol. 229, pp. 134-138.
Information on Registered Substances comes from registration dossiers which have been assigned a registration number. The assignment of a registration number does however not guarantee that the information in the dossier is correct or that the dossier is compliant with Regulation (EC) No 1907/2006 (the REACH Regulation). This information has not been reviewed or verified by the Agency or any other authority. The content is subject to change without prior notice.Reproduction or further distribution of this information may be subject to copyright protection. Use of the information without obtaining the permission from the owner(s) of the respective information might violate the rights of the owner.
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