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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):

ClFO3

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/cm3)
1.989 (-141.84°C, g/cm3)

Reactions:

  1. [Ref.1, Ref.2]
    FClO3 + 8KI + 3H2SO4 → 4I2 + KCl + KF + 3K2SO4 + 3H2O

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 ΔfH0 (298.15 K, kJ/mol):

-23.8 (g)

Standard molar Gibbs energy of formation ΔfG0 (298.15 K, kJ/mol):

48.2 (g)

Standard molar entropy S0 (298.15 K, J/(mol·K)):

279 (g)

Molar heat capacity at constant pressure Cp (298.15 K, J/(mol·K)):

64.9 (g)

References:

  1. Advances in Inorganic Chemistry and Radiochemistry. - 1963. - Vol. 5. - pp. 66-70
  2. Journal of Fluorine Chemistry. - 1978. - Vol. 11, №3-4. - pp. 225-241
  3. Journal of Inorganic and Nuclear Chemistry. - 1956. - Vol. 2, No. 5-6. - pp. 348-357 [DOI: 10.1016/0022-1902(56)80089-4]
  4. Simons J.H. Fluorine Chemistry. - Vol. 5. - New York: Academic Press, 1964. - pp. 84-85
  5. Urbanski T. Chemistry and technology of explosives. - vol.2. - Warszawa, 1965. - pp. 488-489
  6. Гринвуд Н., Эрншо А. Химия элементов. - Т.2. - М.: БИНОМ. Лаборатория знаний, 2008. - pp. 221-222 [Russian]
  7. Исикава Н., Кобаяси Ё. Фтор: химия и применение. - М.: Мир, 1982. - pp. 78-80 [Russian]
  8. Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973. - pp. 265 [Russian]
  9. Никитин И.В. Фториды и оксифториды галогенов. - М.: Наука, 1989. - pp. 69-77 [Russian]
  10. Росоловский В.Я. Химия безводной хлорной кислоты. - М.: Наука, 1966. - pp. 130-135 [Russian]
  11. Рысс И.Г. Химия фтора и его неорганических соединений. - М., 1956. - pp. 155-156 [Russian]
  12. Справочник химика. - 2 изд., Т.1. - Л.-М.: Химия, 1966. - pp. 606 [Russian]
  13. Успехи химии. - 1967. - Т.36, №3. - pp. 377-398 [Russian]
  14. 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