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Properties of substance:

hydrazoic acid

Synonyms:

hydrogen azide

Group of substances:

inorganic

Physical appearance:

colorless mobile liquid

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

HN3

Structural formula as text:

HN=N≡N

Molar/atomic mass: 43.03

Melting point (°C):

-80

Boiling point (°C):

36

Solubility (g/100 g of solvent):

ethanol: miscible [Ref.]
hydrogen fluoride : insoluble [Ref.]
water: miscible [Ref.]

Properties of solutions:

70% (wt.), solvent - water
  Detonation velocity (m/s) = 7300.

Interatomic distances and bond angles:

Interatomic distances (in pm): 124 (N(1)-N(2))
Interatomic distances (in pm): 113 (N(2)-N(3))
Interatomic distances (in pm): 98 (H-N)
Bond angles (in degrees): 114 (H-N-N)

Numerical data:

Year of discovery: 1890
Detonation velocity (m/s): 8100

Density:

1.13 (20°C, g/cm3)

Vapour pressure (Torr):

1 (-72.8°C)
10 (-44.9°C)
100 (-8.1°C)

    Electrode potential:

    3N2 + 2H+ + 2e- → 2HN3, E = -3.1 V (water, 25°C)
    HN3 + 3H+ + 2e- → NH4+ + N2, E = 1.96 V (water, 25°C)

    Dissociation:

    pKBH+ (1) = -7.02 (°C, water)
    pKa (1) = 4.59 (25°C, water)

    Dipole moment (D):

    0.85 (20°C)

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

    294 (g)

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

    328 (g)

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

    238.8 (g)

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

    43.68 (g)

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

    30

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

    264 (l)

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

    327.3 (l)

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

    140.6 (l)

    LD50 (mg/kg):

    22 (mice, intraperitoneal)

    References:

    1. CRC Handbook of Chemistry and Physics. - 90ed. - CRC Press, 2010. - pp. 5-13
    2. Encyclopedia of inorganic chemistry. - editor R. Bruce King, 2 Ed., 10 volume set. - 2005
    3. Holleman A.F., Wiberg E., Wiberg N. Lehrbuch der Anorganischen Chemie. - Berlin: Walter de Gruyter, 1995. - pp. 680-682
    4. Inorganic Syntheses. - Vol. 1. - New York and London, 1939. - pp. 77-79
    5. Matyas R., Pachman J. Primary Explosives. - Springer, 2013. - pp. 71-72
    6. Багал Л.И. Химия и технология инициирующих взрывчатых веществ. - М., 1975. - pp. 136-153 [Russian]
    7. Волынец В.Ф., Волынец М.П. Аналитическая химия азота. - М.: Наука, 1977. - pp. 19, 24 [Russian]
    8. Вредные вещества в промышленности: Справочник для химиков, инженеров и врачей. - 7-е изд., Т.3. - Л.: Химия, 1976. - pp. 98-99 [Russian]
    9. Гринвуд Н., Эрншо А. Химия элементов. - Т.1. - М.: БИНОМ. Лаборатория знаний, 2008. - pp. 405-406 [Russian]
    10. Досон Р., Эллиот Д., Эллиот У., Джонс К. Справочник биохимика. - М.: Мир, 1991. - pp. 251 [Russian]
    11. Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973. - pp. 405 [Russian]
    12. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 51 [Russian]
    13. Справочник химика. - 2 изд., Т.1. - Л.-М.: Химия, 1966. - pp. 607 [Russian]
    14. Физер Л., Физер М. Реагенты для органического синтеза. - Т. 1: А-Е. - М., 1970. - pp. 25-28 [Russian]
    15. Химическая энциклопедия. - Т. 1. - М.: Советская энциклопедия, 1988. - pp. 61 [Russian]
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      © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru