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Properties of substance:

CL

Synonyms:

chlorine

Group of substances:

inorganic

Physical appearance:

gas

Empirical formula (Hill's system for organic substances):

Cl2

Structural formula as text:

Cl2

Molar/atomic mass: 70.91

Melting point (°C):

-101.03

Boiling point (°C):

-34.1

CAS №: 7782-50-5

Solubility (g/100 g of solvent):

benzene: 32.8 (10°C) [Ref.]
benzene: 22.7 (20°C) [Ref.]
boron trichloride: soluble [Ref.]
carbon tetrachloride: 31.4 (0°C) [Ref.]
carbon tetrachloride: 17.61 (19°C) [Ref.]
carbon tetrachloride: 11 (40°C) [Ref.]
chloroform: 8.28 (25°C) [Ref.]
hydrogen chloride liquid anhydrous: very soluble [Ref.]
methylene chloride: 10.44 (25°C) [Ref.]
perfluoro-n-heptane: 3.585 (0°C) [Ref.]
perfluoro-n-heptane: 2.2608 (19.8°C) [Ref.]
perfluoro-n-heptane: 2.146 (25°C) [Ref.]
potassium chloride fused: 0.005503 (820°C) [Ref.]
water: 1.48 (0°C) [Ref.]
water: 0.96 (20°C) [Ref.]
water: 0.65 (25°C) [Ref.]
water: 0.46 (40°C) [Ref.]
water: 0.38 (60°C) [Ref.]
water: 0.22 (80°C) [Ref.]
water: 0.13 (90°C) [Ref.]

Numerical data:

Year of discovery: 1774

Density:

1.9 (-102°C, d4)
1.6552 (-70°C, d4)
0.00321 (20°C, g/cm3)

Reactions of synthesis:

  1. [Ref.1, Ref.2]
    2NaCl + 2H2O → 2NaOH + H2 + Cl2
  2. [Ref.1]
    K2Cr2O7 + 14HCl → 2KCl + 2CrCl3 + 3Cl2 + 7H2O

Reactions:

  1. Yeild 90%. [Ref.1, Ref.2]
    Cl2 + F2 → 2ClF
  2. [Ref.1]
    Si + Cl2 → SiCl4
  3. [Ref.1]
    2S + Cl2 → S2Cl2
  4. [Ref.1aster]
    S8 + Cl2 → S8Cl2
  5. [Ref.1]
    MoO2 + Cl2 → MoO2Cl2
  6. [Ref.1, Ref.2aster, Ref.3]
    2Au + 3Cl2 → 3AuCl3
  7. [Ref.1]
    2K + Cl2 → 2KCl
  8. [Ref.1]
    Fe + Cl2 → FeCl2
    2FeCl2 + Cl2 → 2FeCl3
  9. [Ref.1, Ref.2, Ref.3]
    CH2Cl2 + Cl2 → CHCl3 + HCl
    CHCl3 + Cl2 → CCl4 + HCl
  10. Yeild 18,5%. [Ref.1]
    Cl2 + AgF → ClF + AgCl
  11. Yeild 68%. [Ref.1]
    24(NH2)2CO + 9Cl2 → 18NH4Cl + 3N2 + 8(CONH)3
  12. Yeild 95%. [Ref.1]
    ClF3 + Cl2 → 3ClF
  13. Yeild 85%. [Ref.1aster]
    PCl3 + Cl2 → PCl5
  14. Yeild 80%. [Ref.1aster]
    2Re + 5Cl2 → 2ReCl5
  15. [Ref.1, Ref.2]
    Pd + Cl2 → PdCl2
  16. [Ref.1]
    2NaN3 + 3F2 + Cl2 → 2NF2Cl + 2NaF + 2N2
  17. [Ref.1]
    2Na2O + Cl2 → 2NaCl + Na2O2
  18. [Ref.1]
    (C2H5)2O + 4Cl2 → 4C + 8HCl + H2O
  19. [Ref.1aster]
    (NH4)2SO4 + 3Cl2 → NCl3 + NH4HSO4 + 3HCl
  20. [Ref.1, Ref.2]
    H2 + Cl2 → 2HCl
  21. [Ref.1, Ref.2]
    CH4 + Cl2 → CH3Cl + HCl
    CH3Cl + Cl2 → CH2Cl2 + HCl
    CH2Cl2 + Cl2 → CHCl3 + HCl
    CHCl3 + Cl2 → CCl4 + HCl
  22. [Ref.1]
    (CH3)3COOC(CH3)3 + SO2 + Cl2 → (CH3)3COOC(CH3)2CH2SO2Cl + HCl
  23. [Ref.1aster]
    2VO + 3Cl2 → 2VOCl3
  24. [Ref.1aster]
    SO2 + Cl2 → SO2Cl2
  25. [Ref.1]
    Ag2S + Cl2 → 2AgCl + S
  26. [Ref.1]
    2P + 3Cl2 → 2PCl3
  27. [Ref.1aster]
    I2 + Cl2 → 2ICl
  28. [Ref.1aster]
    I2 + 3Cl2 → 2ICl3
  29. [Ref.1aster]
    NaIO3 + 4NaOH + Cl2 → Na3H3IO6 + 2NaCl + H2O
  30. [Ref.1]
    Ni + Cl2 → NiCl2
  31. [Ref.1, Ref.2aster]
    2Cl2 + HgO → Cl2O + HgCl2
  32. [Ref.1, Ref.2]
    2K4[Fe(CN)6] + Cl2 → 2K3[Fe(CN)6] + 2KCl

Vapour pressure (Torr):

1 (-118°C)
10 (-101.5°C)
100 (-71.9°C)

Electrode potential:

Cl2 + 2e- → 2Cl-, E = 0.58 V (acetonitrile, 25°C)
Cl2 + 2e- → 2Cl-, E = 0.99 V (formic acid, 25°C)
Cl2 + 2e- → 2Cl-, E = 1.048 V (ethanol, 25°C)
Cl2 + 2e- → 2Cl-, E = 1.116 V (methanol, 25°C)
Cl2 + 2e- → 2Cl-, E = 1.34 V (water, 25°C)
Cl2 + 2e- → 2Cl-, E = 2.03 V (ammonia liquid , -50°C)

Viscosity (mPa·s):

0.00133 (20°C)
0.00188 (150°C)

Speed sound (m/s):

206 (0°C, aggregative state - gas)

Standard molar enthalpy (heat) of formation ΔfH0 (298.15 K, kJ/mol):

0 (g)

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

0 (g)

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

222.9 (g)

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

34.94 (g)

Molar enthalpy (heat) of fusion ΔfusH (kJ/mol):

6.406

Enthalpy (heat) of vaporization ΔvapH (kJ/mol):

20.41

Critical temperature (°C):

144

Critical pressure (MPa):

7.71

Critical density (g/cm3):

0.573

References:

  1. Hoenig S.L. Compendium of chemical warfare agents. - 2007. - pp. 57-60
  2. Seidell A. Solubilities of inorganic and metal organic compounds. - 3ed., vol.1. - New York: D. Van Nostrand Company, 1940. - pp. 396-399
  3. Вредные вещества в промышленности: Справочник для химиков, инженеров и врачей. - 7-е изд., Т.3. - Л.: Химия, 1976. - pp. 20-23 [Russian]
  4. Герасимов Я.И., Древинг В.П., Еремин Е.Н.. Киселев А.В., Лебедев В.П., Панченков Г.М., Шлыгин А.И. Курс физической химии. - Т.2. - М.: Химия, 1973. - pp. 528 [Russian]
  5. Гурвич Я.А. Справочник молодого аппаратчика-химика. - М.: Химия, 1991. - pp. 47, 52, 229 [Russian]
  6. Промышленные хлорорганические продукты: Справочник. - М.: Химия, 1978. - pp. 634-636 [Russian]
  7. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 109 [Russian]
  8. Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961. - pp. 617-621 [Russian]
  9. Химическая энциклопедия. - Т. 5. - М.: Советская энциклопедия, 1999. - pp. 280-281 [Russian]
  10. Якименко Л.М. Производство хлора, каустической соды и неорганических хлорпродуктов. - М.: Химия, 1974. - pp. 309-365 [Russian]
  11. Якименко Л.М., Пасманик М.И. Справочник по производству хлора, каустической соды и соновных хлорпродуктов. - 2 изд. - М.: Химия, 1976. - pp. 152-189 [Russian]

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    © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru