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Properties of substance:

ethylene glycol

Group of substances:

organic

Physical appearance:

colorless liquid

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

C2H6O2

Structural formula as text:

HOCH2CH2OH

Molar/atomic mass: 62.07

Melting point (°C):

-12.6

Boiling point (°C):

197.85

Decomposition temperature (°C):

500-550

Solubility (g/100 g of solvent):

1-butanol: miscible (20°C) [Ref.]
2-propanol: miscible (20°C) [Ref.]
acetic acid: miscible (20°C) [Ref.]
acetone: miscible (20°C) [Ref.]
ammonia liquid : miscible [Ref.]
aniline: miscible (20°C) [Ref.]
benzene: 6 (25°C) [Ref.]
benzylic alcohol: miscible (20°C) [Ref.]
carbon tetrachloride: 6.6 (25°C) [Ref.]
chloroform: insoluble [Ref.]
cyclohexanone: miscible (20°C) [Ref.]
diethyl ether: 7.89 (20°C) [Ref.]
ethanol: miscible [Ref.]
formamide: miscible (20°C) [Ref.]
glycerol: miscible (20°C) [Ref.]
heptane: 0.062 (67.9°C) [Ref.]
methanol: miscible (20°C) [Ref.]
petroleum ether: insoluble [Ref.]
water: miscible [Ref.]

Properties of solutions:

2% (wt.), solvent - water
  Density (g/cm3) = 1.0007 (20°)
  Freezing point (°C) = -0.6
4% (wt.), solvent - water
  Density (g/cm3) = 1.0032 (20°)
  Freezing point (°C) = -1.3
6% (wt.), solvent - water
  Density (g/cm3) = 1.0057 (20°)
  Freezing point (°C) = -2.
8% (wt.), solvent - water
  Density (g/cm3) = 1.0082 (20°)
  Freezing point (°C) = -2.7
10% (wt.), solvent - water
  Density (g/cm3) = 1.0108 (20°)
  Freezing point (°C) = -3.5
  Boiling point (°C) = 101.1
12% (wt.), solvent - water
  Freezing point (°C) = -4.4
14% (wt.), solvent - water
  Freezing point (°C) = -5.3
16% (wt.), solvent - water
  Freezing point (°C) = -6.3
18% (wt.), solvent - water
  Freezing point (°C) = -7.3
20% (wt.), solvent - water
  Density (g/cm3) = 1.0241 (20°)
  Freezing point (°C) = -8.
  Boiling point (°C) = 102.2
22% (wt.), solvent - water
  Freezing point (°C) = -9.
24% (wt.), solvent - water
  Freezing point (°C) = -11.
26% (wt.), solvent - water
  Freezing point (°C) = -12.
28% (wt.), solvent - water
  Freezing point (°C) = -13.
30% (wt.), solvent - water
  Freezing point (°C) = -15.
  Boiling point (°C) = 103.3
32% (wt.), solvent - water
  Density (g/cm3) = 1.0405 (20°)
  Freezing point (°C) = -17.
34% (wt.), solvent - water
  Freezing point (°C) = -18.
36% (wt.), solvent - water
  Dynamic viscosity (mPa·s) = 2.537 (20°)
  Density (g/cm3) = 1.046 (20°)
  Index of refraction = 1.3687 (20°)
  Freezing point (°C) = -19.82
38% (wt.), solvent - water
  Freezing point (°C) = -22.
40% (wt.), solvent - water
  Density (g/cm3) = 1.0514 (20°)
  Freezing point (°C) = -24.
  Boiling point (°C) = 105.
42% (wt.), solvent - water
  Freezing point (°C) = -26.
44% (wt.), solvent - water
  Freezing point (°C) = -28.
45,6% (wt.), solvent - water
  Freezing point (°C) = -30.
46% (wt.), solvent - water
  Freezing point (°C) = -31.
48% (wt.), solvent - water
  Density (g/cm3) = 1.0619 (20°)
  Freezing point (°C) = -33.
50% (wt.), solvent - water
  Freezing point (°C) = -36.
  Boiling point (°C) = 107.2
52% (wt.), solvent - water
  Freezing point (°C) = -38.
54% (wt.), solvent - water
  Freezing point (°C) = -41.
56% (wt.), solvent - water
  Freezing point (°C) = -44.
58% (wt.), solvent - water
  Freezing point (°C) = -48.
60% (wt.), solvent - water
  Density (g/cm3) = 1.0765 (20°)
  Boiling point (°C) = 110.
63,1% (wt.), solvent - water
  Freezing point (°C) = -60.
66,7% (wt.), solvent - water
  Freezing point (°C) = -75.
70% (wt.), solvent - water
  Boiling point (°C) = 114.4
72,1% (wt.), solvent - water
  Freezing point (°C) = -60.
78,4% (wt.), solvent - water
  Freezing point (°C) = -50.
80% (wt.), solvent - water
  Freezing point (°C) = -47.
  Boiling point (°C) = 122.2
82% (wt.), solvent - water
  Freezing point (°C) = -43.
84% (wt.), solvent - water
  Freezing point (°C) = -40.
86% (wt.), solvent - water
  Freezing point (°C) = -36.
88% (wt.), solvent - water
  Freezing point (°C) = -33.
90% (wt.), solvent - water
  Freezing point (°C) = -29.
  Boiling point (°C) = 137.2
91% (wt.), solvent - water
  Boiling point (°C) = 140.
92% (wt.), solvent - water
  Freezing point (°C) = -26.
  Boiling point (°C) = 142.8
93% (wt.), solvent - water
  Boiling point (°C) = 145.6
94% (wt.), solvent - water
  Freezing point (°C) = -23.
  Boiling point (°C) = 149.4
95% (wt.), solvent - water
  Boiling point (°C) = 153.9
96% (wt.), solvent - water
  Freezing point (°C) = -19.
  Boiling point (°C) = 159.4
97% (wt.), solvent - water
  Boiling point (°C) = 165.6
98% (wt.), solvent - water
  Freezing point (°C) = -16.
  Boiling point (°C) = 173.9
99% (wt.), solvent - water
  Boiling point (°C) = 183.9

Numerical data:

Sweetness potency сompared with a 2% (w/v) aqueous solution of sucrose: 0.49

Density:

1.134 (-10°C, g/cm3)
1.127 (0°C, g/cm3)
1.12 (10°C, g/cm3)
1.113 (20°C, g/cm3)
1.106 (30°C, g/cm3)
1.093 (50°C, g/cm3)
1.078 (70°C, g/cm3)
1.055 (100°C, g/cm3)
1.014 (150°C, g/cm3)
0.985 (180°C, g/cm3)

Reactions:

  1. Yeild 60%. [Ref.1, Ref.2aster]
    HOCH2CH2OH + 2Cl2O7 → O3ClOCH2CH2OClO3 + 2HClO4

Refractive index (nD):

1.43192 (20°C)

Vapour pressure (Torr):

0.06 (20°C)
0.7 (50°C)
1.3 (60°C)
5 (80°C)
12 (95°C)
25 (109°C)
43 (120°C)
75 (132.2°C)
219 (160°C)
312 (170°C)
435 (180°C)
605 (190°C)
820 (200°C)

Dissociation:

pKa (1) = 15.1 (25°C, water)

Viscosity (mPa·s):

20.9 (20°C)

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

-454.3 (l)

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

-322.7 (l)

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

166.9 (l)

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

11.23

Flash point (°C):

111

Autoignition temperature (°C):

410

Heat of combustion (kJ/mol):

1179.5

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

-392.2 (g)

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

303.8 (g)

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

82.7 (g)

LD50 (mg/kg):

8050 (white mice, oral)
5000 (rabbits, oral)
13000 (rats, oral)
11150 (guinea pig, oral)

References:

  1. CRC Handbook of Chemistry and Physics. - 90ed. - CRC Press, 2010. - pp. 5-22
  2. Flick E.W. Industrial solvent handbook. - 5ed. - 1998. - pp. 359-367
  3. Seidell A. Solubilities of organic compounds. - 3ed., vol.2. - New York: D. Van Nostrand Company, 1941. - pp. 156-158
  4. Альберт А., Сержент Е. Константы ионизации кислот и оснований. - М.-Л.: Химия, 1964. - pp. 124 [Russian]
  5. Волков А.И., Жарский И.М. Большой химический справочник. - Минск: Современная школа, 2005. - pp. 386 [Russian]
  6. Дымент О.Н., Казанский К.С., Мирошников А.М. Гликоли и другие производные окисей этилена и пропилена. - М.: Химия, 1976 [Russian]
  7. Корольченко А.Я., Корольченко Д.А. Пожаровзрывоопасность веществ и материалов и средства их тушения. - 2 изд, Ч.2. - М.: Ассоциация Пожнаука, 2004. - pp. 717 [Russian]
  8. Краткая химическая энциклопедия. - Т. 5: Т-Я. - М.: Советская энциклопедия, 1967. - pp. 1033-1034 [Russian]
  9. Мономеры для поликонденсации. - М.: Мир, 1976. - pp. 232 [Russian]
  10. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 198 [Russian]
  11. Справочник по растворимости. - Т.1, Кн.2. - М.-Л.: ИАН СССР, 1962. - pp. 1262-1263 [Russian]
  12. Справочник по химии. Для учащихся средней школы. - М.: Просвещение, 1970. - pp. 158 [Russian]
  13. Справочник химика. - 2 изд., Т.1. - Л.-М.: Химия, 1966. - pp. 1057 [Russian]
  14. Хёрд Ч.Д. Пиролиз соединений углерода. - Л.-М.: ГОНТИ РКТП СССР, 1938. - pp. 163 [Russian]
  15. Химическая энциклопедия. - Т. 5. - М.: Советская энциклопедия, 1999. - pp. 496-497 [Russian]
  16. Химический энциклопедический словарь. - Под ред. Кнунянц И.Л. - М.: Советская энциклопедия, 1983. - pp. 718 [Russian]

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    © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru