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Properties of substance:

ammonium nitrate



skc-file

Group of substances:

inorganic

Physical appearance:

colorless rhombic crystals

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

H4N2O3

Structural formula as text:

NH4NO3

Molar/atomic mass: 80.04

Melting point (°C):

169.6

Boiling point (°C):

235

Decomposition temperature (°C):

210

Solubility (g/100 g of solvent):

acetic acid: 0.284 (17.7°C) [Ref.]
acetic acid: 0.326 (21.4°C) [Ref.]
acetic acid: 0.3931 (27°C) [Ref.]
acetic acid: 0.517 (33.6°C) [Ref.]
acetic acid: 0.8822 (45.8°C) [Ref.]
acetic acid: 1.661 (61.2°C) [Ref.]
acetic acid: 2.707 (69°C) [Ref.]
acetic acid: 4.94 (78.3°C) [Ref.]
acetic acid: 20.7 (101°C) [Ref.]
acetone: soluble [Ref.]
ammonia liquid : 391 (25°C) [Ref.]
benzonitrile: insoluble [Ref.]
dimethylformamide: 55.1 (25°C) [Ref.]
dimethylsulfoxide: 73 (25°C) [Ref.]
ethanol: 2.5 (20°C) [Ref.]
ethanol: 5 (40°C) [Ref.]
ethanol: 7.5 (60°C) [Ref.]
hydrazine: 78 (18°C) [Ref.]
methanol: 14.6 (14°C) [Ref.]
methanol: 16.3 (18.5°C) [Ref.]
methanol: 17.1 (20°C) [Ref.]
methyl acetate: insoluble [Ref.]
nitric acid: 26.7 (8°C) [Ref.]
nitric acid: 40.3 (23°C) [Ref.]
nitric acid: 63.4 (29.5°C) [Ref.]
nitric acid: 213.5 (79°C) [Ref.]
pyridine: 23.35 (25°C) [Ref.]
water: 119 (0°C) [Ref.]
water: 150 (10°C) [Ref.]
water: 212 (25°C) [Ref.]
water: 346 (50°C) [Ref.]
water: 600 (80°C) [Ref.]

Multicomponent solubility (in wt%):

water 34.8%, ammonium nitrate 65.2%, calcium nitrate 0.%, 20 °C, separating phase: NH4NO3 [Ref.]
water 34.6%, ammonium nitrate 58.%, calcium nitrate 7.4%, 20 °C, separating phase: NH4NO3 [Ref.]
water 33.6%, ammonium nitrate 37.4%, calcium nitrate 39.%, 20 °C, separating phase: NH4NO3 [Ref.]
water 24.9%, ammonium nitrate 29.5%, calcium nitrate 45.6%, 20 °C, separating phase: Ca(NO3)2 * NH4NO3 * 2H2O + 5Ca(NO3)2 * NH4NO3 * 10H2O [Ref.]
water 35.4%, ammonium nitrate 13.3%, calcium nitrate 51.3%, 20 °C, separating phase: Ca(NO3)2 * 4H2O [Ref.]
water 45.3%, ammonium nitrate 0.%, calcium nitrate 54.7%, 20 °C, separating phase: Ca(NO3)2 * 4H2O [Ref.]

Properties of solutions:

1% (wt.), solvent - water
  Density (g/cm3) = 1.0023 (20°)
2% (wt.), solvent - water
  Density (g/cm3) = 1.0064 (20°)
4% (wt.), solvent - water
  Density (g/cm3) = 1.0147 (20°)
6% (wt.), solvent - water
  Density (g/cm3) = 1.023 (20°)
8% (wt.), solvent - water
  Density (g/cm3) = 1.0313 (20°)
10% (wt.), solvent - water
  Density (g/cm3) = 1.0397 (20°)
20% (wt.), solvent - water
  Density (g/cm3) = 1.0828 (20°)
28% (wt.), solvent - water
  Density (g/cm3) = 1.1186 (20°)
35% (wt.), solvent - water
  Density (g/cm3) = 1.1512 (20°)
40% (wt.), solvent - water
  Density (g/cm3) = 1.1754 (20°)
50% (wt.), solvent - water
  Density (g/cm3) = 1.2258 (20°)
55% (wt.), solvent - water
  Density (g/cm3) = 1.252 (20°)
68,3% (wt.), solvent - water
  Density (g/cm3) = 1.32 (25°)

Hygroscopic:

yes

Numerical data:

Year of discovery: 1659
Heat of Explosion (kJ/kg): 1600
Detonation velocity (m/s): 2750
Detonation velocity (m/s): 1400
Critical relative humidity (%): 48.4
Critical relative humidity (%): 52.5
Critical relative humidity (%): 59.4
Critical relative humidity (%): 61.8
Critical relative humidity (%): 66.9
Critical relative humidity (%): 69.8
Critical relative humidity (%): 75.3

Density:

1.725 (20°C, g/cm3)
1.436 (170°C, g/cm3)
1.414 (220°C, g/cm3)

Reactions:

  1. [Ref.1]
    NH4NO3 → N2O + 2H2O
  2. [Ref.1]
    2NH4NO3 → 2N2 + O2 + 4H2O

Viscosity (mPa·s):

5.71 (170°C)
3.23 (220°C)

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

-365.7 (s)

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

-184 (s)

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

151.1 (s)

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

139.4 (s)

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

5.86

References:

  1. Milne G.W.A. Gardner's Commercially Important Chemicals. - Wiley-Interscience, 2005. - pp. 34
  2. Patnaik P. Handbook of inorganic chemicals. - McGraw-Hill, 2003. - pp. 39-42
  3. Perry D.L. Handbook of Inorganic Compounds. - 2nd ed. - CRC Press, 2011. - pp. 29
  4. Seidell A. Solubilities of inorganic and metal organic compounds. - 3ed., vol.1. - New York: D. Van Nostrand Company, 1940. - pp. 1105-1115
  5. Urbanski T. Chemistry and technology of explosives. - vol.2. - Warszawa, 1965. - pp. 450-464
  6. Вредные вещества в промышленности: Справочник для химиков, инженеров и врачей. - 7-е изд., Т.3. - Л.: Химия, 1976. - pp. 118-119 [Russian]
  7. Дубнов Л.В., Бахаревич Н.С., Романов А.И. Промышленные взрывчатые вещества. - 3-е изд. - М.: Недра, 1988. - pp. 227-252 [Russian]
  8. Позин М.Е. Технология минеральных солей (удобрений, пестицидов, промышленных солей, окислов и кислот). - Ч.2. - Л.: Химия, 1974. - pp. 1178-1208 [Russian]
  9. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 53 [Russian]
  10. Справочник азотчика. - М.: Химия, 1987. - pp. 142-201 [Russian]
  11. Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961. - pp. 217-218, 744-745 [Russian]
  12. Технология аммиачной селитры. - Под ред. Олевского В.М. - М.: Химия, 1978 [Russian]
  13. Химическая технология неорганических веществ. - Кн.1, под ред. Ахметова Т.Г. - М.: Высшая школа, 2002. - pp. 549-558 [Russian]
  14. Химическая энциклопедия. - Т. 1. - М.: Советская энциклопедия, 1988. - pp. 153 [Russian]

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    © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru