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Properties of substance:

hydrogen

Group of substances:

inorganic

Physical appearance:

colorless gas

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

H2

Structural formula as text:

H2

Molar/atomic mass: 2.01565

Melting point (°C):

-259.19

Boiling point (°C):

-252.77

Decomposition temperature (°C):

1700-5000

Solubility (g/100 g of solvent):

acetic acid: 0.000486 (20°C) [Ref.]
acetone: 0.00102 (20.9°C) [Ref.]
aluminum fused: soluble [Ref.]
benzene: 0.00066 (22.9°C) [Ref.]
carbon tetrachloride: 0.000365625 (0°C) [Ref.]
carbon tetrachloride: 0.000414562 (20.9°C) [Ref.]
chloroform: 0.000353 (18.7°C) [Ref.]
copper liquid: 0.00054 (1083°C) [Ref.]
copper liquid: 0.00124 (1550°C) [Ref.]
dimethylformamide: 0.0004 (25°C) [Ref.]
dimethylsulfoxide: insoluble [Ref.]
ethanol: 0.000624 (0°C) [Ref.]
ethyl acetate: 0.000762 (21°C) [Ref.]
i-butanol: 0.00105 (20°C) [Ref.]
methanol: 0.00103 (20°C) [Ref.]
methyl acetate: 0.000809 (20.9°C) [Ref.]
monochlorbenzene: 0.000452 (21.2°C) [Ref.]
perfluoro-n-heptane: 0.000522 (-25°C) [Ref.]
perfluoro-n-heptane: 0.0006204 (0°C) [Ref.]
perfluoro-n-heptane: 0.0007287 (25°C) [Ref.]
perfluoro-n-heptane: 0.0007763 (35°C) [Ref.]
tin liquid: 0.04 (1000°C) [Ref.]
tin liquid: 0.036 (1300°C) [Ref.]
water: 0.000194 (0°C) [Ref.]
water: 0.000175 (10°C) [Ref.]
water: 0.000164 (20°C) [Ref.]
water: 0.000157 (25°C) [Ref.]
water: 0.000153 (30°C) [Ref.]
water: 0.000147 (40°C) [Ref.]
water: 0.000145 (50°C) [Ref.]
water: 0.000144 (60°C) [Ref.]
water: 0.000144 (100°C) [Ref.]

Numerical data:

Year of discovery: 1766
Thermal conductivity (W/m·K): 0.1866
Polarizability of molecules (nm3): 0.00079
Magnetic susceptibility (mm3/kg): -1.9867


Density:

0.0763 (-260°C, g/cm3)
0.0768 (-253°C, g/cm3)
0.07081 (-252.68°C, g/cm3)
0.00008988 (20°C, g/cm3)

Reactions of synthesis:

  1. [Ref.1]
    2K + 2H2O → 2KOH + H2
  2. [Ref.1]
    2Na + 2H2O → 2NaOH + H2
  3. [Ref.1, Ref.2]
    Fe + H2O → FeO + H2
  4. [Ref.1]
    Mg + 2H2O → Mg(OH)2 + H2
  5. [Ref.1, Ref.2]
    2NaCl + 2H2O → 2NaOH + H2 + Cl2
  6. [Ref.1]
    Zn + 2NaOH + 2H2O → Na2[Zn(OH)4] + H2
  7. [Ref.1]
    Zn + 2HCl → ZnCl2 + H2
  8. [Ref.1, Ref.2]
    Zn + H2SO4 → ZnSO4 + H2
  9. [Ref.1]
    C + H2O → CO + H2
  10. [Ref.1]
    2H2O → 2H2 + O2

Reactions:

  1. [Ref.1]
    2H2 + O2 → 2H2O
  2. [Ref.1, Ref.2]
    H2 + F2 → 2HF
  3. [Ref.1]
    2K + H2 → 2KH
  4. [Ref.1]
    2Na + H2 → 2NaH
  5. [Ref.1]
    Ca + H2 → CaH2
  6. Yeild 70-80%. [Ref.1, Ref.2aster, Ref.3]

  7. Yeild 86%. [Ref.1aster, Ref.2aster]
    C6H5CH3 + 3H2 → C6H11CH3
  8. Yeild 75%. [Ref.1aster, Ref.2]
    C6H5OH + 3H2 → C6H11OH
  9. [Ref.1]
    CuO + H2 → Cu + H2O
  10. [Ref.1aster]
    MoO3 + 3H2 → Mo + 3H2O
  11. [Ref.1]
    NOCl + 3H2 → NH4Cl + H2O
    2NOCl + 3H2 → N2 + 2H2O + 2HCl
  12. Yeild 8%. [Ref.1]
    2C + H2 → C2H2
  13. [Ref.1]
    S2Cl2 + H2 → 2S + 2HCl
  14. [Ref.1]
    S + H2 → H2S
  15. [Ref.1]
    VCl4 + H2 → VCl2 + 2HCl
  16. [Ref.1, Ref.2]
    2Na2O + H2 → 2NaOH + 2Na
  17. [Ref.1, Ref.2]
    N2 + 3H2 → 2NH3
  18. [Ref.1]
    H2 + PdCl2 → Pd + 2HCl
  19. [Ref.1aster, Ref.2aster, Ref.3aster, Ref.4aster, Ref.5aster, Ref.6]
    H2 + I2 → 2HI
  20. [Ref.1, Ref.2]
    H2 + Cl2 → 2HCl
  21. [Ref.1]
    C2H5OOC2H5 + H2 → 2C2H5OH
  22. [Ref.1]
    (CH3)3COOC(CH3)3 + H2 → 2(CH3)3COH
  23. [Ref.1]
    2CuCl + H2 → 2Cu + 2HCl
  24. [Ref.1]
    2NOCl + H2 → 2HCl + 2NO
  25. [Ref.1aster]
    H2 + Br2 → 2HBr
  26. [Ref.1]
    ((CH3)3C6H2)2PC6F4B(C6F5)2 + H2 → ((CH3)3C6H2)2PHC6F4BH(C6F5)2
  27. [Ref.1aster, Ref.2, Ref.3aster, Ref.4aster, Ref.5aster]
    Fe2O3 + 3H2 → 2Fe + 3H2O

Half-life:

11H = stable (mass excess 7288,9705 keV (isotopic abundance 99,985%))
21H = stable (mass excess 13135,7216 keV (isotopic abundance 0,015%))
31H = 12.33 y (β- (100%); mass excess 14949,806 keV)
41H = 139 ys (n (100%); mass excess 25900 keV)
51H = 86 ys (2n (100%); mass excess 32890 keV)
61H = 294 ys (mass excess 41880 keV)
71H = 652 ys (mass excess 49140 keV)

Vapour pressure (Torr):

1 (-263.6°C)
10 (-261.4°C)
100 (-258.1°C)

Electrode potential:

H2 + 2e- → 2H-, E = -2.251 V (water, 25°C)
2H+ + 2e- → H2, E = 0 V (water, 25°C)
H1 + H+ + e- → H2, E = 2.106 V (water, 25°C)

Dissociation:

pKa (1) = 39 (25°C, water)

Permittivity (dielectric constant):

1.000252 (25°C)

Dipole moment (D):

0 (20°C)

Viscosity (mPa·s):

0.0085 (0°C)
0.0103 (100°C)
0.0121 (200°C)
0.0154 (400°C)
0.0183 (600°C)
0.0087 (-253°C)

Speed sound (m/s):

1284 (0°C, aggregative state - gas)
1301 (18°C, aggregative state - gas)
1463 (100°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)):

130.52 (g)

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

28.83 (g)

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

0.117

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

0.916

Enthalpy (heat) of dissociation ΔdissH (kJ/mol)

435.88 (g) [Ref.]

Critical temperature (°C):

-239.91

Critical pressure (MPa):

1.297

Critical density (g/cm3):

0.031

References:

  1. Handbook of Chemistry and Physics. - CRC Press, Inc., 2002. - pp. 11-51
  2. Holleman A.F., Wiberg E., Wiberg N. Lehrbuch der Anorganischen Chemie. - Berlin: Walter de Gruyter, 1995. - pp. 238
  3. Nuclear Physics A. - 2003. - vol.729, Issue 1, 1 December. - pp. 27
  4. Seidell A. Solubilities of inorganic and metal organic compounds. - 3ed., vol.1. - New York: D. Van Nostrand Company, 1940. - pp. 553-567
  5. The Merck Index 11th ed., Merck & Company, 1989. - pp. 759
  6. Варгафтик Н.Б. Справочник по теплофизическим свойствам газов и жидкостей. - М.: Наука, 1972. - pp. 7-43 [Russian]
  7. Взаимодействие водорода с металлами. - Авторы: Агеев В.Н., Бекман И.Н. и др., Бурмистрова О.П. - М.: Наука, 1987 [Russian]
  8. Гидриды переходных металлов. - М.: Мир, 1975. - pp. 9-15 [Russian]
  9. Гринвуд Н., Эрншо А. Химия элементов. - Т.1. - М.: БИНОМ. Лаборатория знаний, 2008. - pp. 39-53 [Russian]
  10. Гурвич Я.А. Справочник молодого аппаратчика-химика. - М.: Химия, 1991. - pp. 50 [Russian]
  11. Иванова М.А., Кононова М.А. Химический демонстрационный эксперимент. - М.: Высшая школа, 1969. - pp. 12-21 [Russian]
  12. Карапетьянц М.Х., Дракин С.И. Общая и неорганическая химия. - М.: Химия, 1981. - pp. 465 [Russian]
  13. Корольченко А.Я., Корольченко Д.А. Пожаровзрывоопасность веществ и материалов и средства их тушения. - 2 изд, Ч.1. - М.: Ассоциация Пожнаука, 2004. - pp. 311-312 [Russian]
  14. Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973. - pp. 79-82, 115-122 [Russian]
  15. Неорганическая химия. - Под ред. Третьякова Ю.Д., Т.2. - М.: Academa, 2004. - pp. 5-13 [Russian]
  16. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 59 [Russian]
  17. Реми Г. Курс неорганической химии. - Т.1. - М., 1963. - pp. 42-48, 55, 60-65 [Russian]
  18. Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961. - pp. 536-553 [Russian]
  19. Справочник химика. - Т. 3. - М.-Л.: Химия, 1965. - pp. 742 [Russian]
  20. Физические величины. - Под ред. Григорьева И.С., Мейлихова Е.З. - М.: Энергоатомиздат, 1991. - pp. 994 [Russian]
  21. Химическая энциклопедия. - Т. 1. - М.: Советская энциклопедия, 1988. - pp. 400-402 [Russian]
  22. Химический энциклопедический словарь. - Под ред. Кнунянц И.Л. - М.: Советская энциклопедия, 1983. - pp. 104 [Russian]
  23. Химмотология ракетных и реактивных топлив. - Под ред. Браткова А.А. - М.: Химия, 1987. - pp. 81-86 [Russian]

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    © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru