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Properties of substance:
perchloryl fluoride
Group of substances:
inorganic
Physical appearance:
colorless gas
Empirical formula (Hill's system for organic substances):
ClFO
3
Structural formula as text:
ClO3F
Molar/atomic mass: 102.45
Melting point (°C):
-147.8
Boiling point (°C):
-46.7
Decomposition temperature (°C):
400
Solubility (g/100 g of solvent):
acetone
: 4.44 (25°C) [
Ref.
]
acetonitrile
: 2.29 (25°C) [
Ref.
]
carbon tetrachloride
: 2.49 (25°C) [
Ref.
]
dimethylformamide
: 2.05 (25°C) [
Ref.
]
fluorosulfuric acid
: soluble [
Ref.
]
hydrogen fluoride
: insoluble [
Ref.
]
methanol
: 3.13 (25°C) [
Ref.
]
monoglyme
: 2.62 (25°C) [
Ref.
]
phosphorus trichloride
: soluble [
Ref.
]
phosphorus(V) trichloride oxide
: soluble [
Ref.
]
sulfuryl chloride
: soluble [
Ref.
]
tetrachlorosilane
: soluble [
Ref.
]
tetrahydrofuran
: 5.89 (25°C) [
Ref.
]
thionyl chloride
: soluble [
Ref.
]
titan tetrachloride
: soluble [
Ref.
]
water
: 0.158 (5°C) [
Ref.
]
water
: 0.127 (10°C) [
Ref.
]
water
: 0.103 (15°C) [
Ref.
]
water
: 0.084 (20°C) [
Ref.
]
water
: 0.069 (25°C) [
Ref.
]
water
: 0.04 (40°C) [
Ref.
]
Interatomic distances and bond angles:
Interatomic distances (in pm): 161,9 (Cl-F) [gas]
Interatomic distances (in pm): 140,4 (Cl-O) [gas]
Bond angles (in degrees): 100,8 (O-Cl-F) [gas]
Bond angles (in degrees): 116,6 (O-Cl-O) [gas]
Numerical data:
Year of discovery: 1951
Density:
2.19 (-190°C, g/cm
3
)
1.989 (-141.84°C, g/cm
3
)
Reactions:
[
Ref.1
,
Ref.2
]
FClO
3
+ 8KI + 3H
2
SO
4
→ 4I
2
+ KCl + KF + 3K
2
SO
4
+ 3H
2
O
Vapour pressure (Torr):
0.1 (-145.1°C)
1 (-129.8°C)
10 (-109.8°C)
100 (-82.2°C)
Permittivity (dielectric constant):
2.194 (-123°C)
Dipole moment (D):
0.023 (20°C)
Viscosity (mPa·s):
0.55 (-73°C)
Standard molar enthalpy (heat) of formation Δ
f
H
0
(298.15 K, kJ/mol):
-23.8 (g)
Standard molar Gibbs energy of formation Δ
f
G
0
(298.15 K, kJ/mol):
48.2 (g)
Standard molar entropy S
0
(298.15 K, J/(mol·K)):
279 (g)
Molar heat capacity at constant pressure C
p
(298.15 K, J/(mol·K)):
64.9 (g)
References:
Advances in Inorganic Chemistry and Radiochemistry. - 1963. - Vol. 5. - pp. 66-70
Journal of Fluorine Chemistry. - 1978. - Vol. 11, №3-4. - pp. 225-241
Journal of Inorganic and Nuclear Chemistry. - 1956. - Vol. 2, No. 5-6. - pp. 348-357 [DOI:
10.1016/0022-1902(56)80089-4
]
Simons J.H. Fluorine Chemistry. - Vol. 5. - New York: Academic Press, 1964. - pp. 84-85
Urbanski T. Chemistry and technology of explosives. - vol.2. - Warszawa, 1965. - pp. 488-489
Гринвуд Н., Эрншо А. Химия элементов. - Т.2. - М.: БИНОМ. Лаборатория знаний, 2008. - pp. 221-222 [Russian]
Исикава Н., Кобаяси Ё. Фтор: химия и применение. - М.: Мир, 1982. - pp. 78-80 [Russian]
Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973. - pp. 265 [Russian]
Никитин И.В. Фториды и оксифториды галогенов. - М.: Наука, 1989. - pp. 69-77 [Russian]
Росоловский В.Я. Химия безводной хлорной кислоты. - М.: Наука, 1966. - pp. 130-135 [Russian]
Рысс И.Г. Химия фтора и его неорганических соединений. - М., 1956. - pp. 155-156 [Russian]
Справочник химика. - 2 изд., Т.1. - Л.-М.: Химия, 1966. - pp. 606 [Russian]
Успехи химии. - 1967. - Т.36, №3. - pp. 377-398 [Russian]
Химмотология ракетных и реактивных топлив. - Под ред. Браткова А.А. - М.: Химия, 1987. - pp. 79 [Russian]
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© Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru