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Ammonium nitrate
Ammonium nitrate
Ammonium-nitrate-xtal-3D-balls-A.png
IUPAC name
Identifiers
CAS number 6484-52-2 Yes check.svgY
UN number 0222with > 0.2% combustible substances
1942with <= 0.2% combustible substances
2067fertilizers
2426liquid
RTECS number BR9050000
Properties
Molecular formula (NH4)(NO3)
Molar mass 80.043 g/mol
Appearance white solid
Density 1.725 g/cm3 (20 °C)
Melting point

169.6 °C

Boiling point

approx. 210 °C decomp.

Solubility in water 118 g/100 ml (0 °C)
150 g/100 ml (20 °C)
297 g/100 ml (40 °C)
410 g/100 ml (60 °C)
576 g/100 ml (80 °C)
1024 g/100 ml (100 °C) [1]
Explosive data
Shock sensitivity very low
Friction sensitivity very low
Explosive velocity 5270 m/s
Hazards
MSDS ICSC 0216
EU Index not listed
Main hazards Explosive
NFPA 704
NFPA 704.svg
0
2
3
OX
LD50 2085–5300 mg/kg (oral in rats, mice)[2]
Related compounds
Other anions Ammonium nitrite
Other cations Sodium nitrate
Potassium nitrate
Hydroxylammonium nitrate
Related compounds Ammonium perchlorate
 Yes check.svgY (what is this?)  (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

The chemical compound ammonium nitrate, the nitrate of ammonia with the chemical formula NH4NO3, is a white crystalline solid at room temperature and standard pressure. It is commonly used in agriculture as a high-nitrogen fertilizer, and it has also been used as an oxidizing agent in explosives, including improvised explosive devices. It is the main component of ANFO, a very popular explosive.

Ammonium nitrate is used in cold packs, as hydrating the salt is an endothermic process.

Contents

Production

The processes involved in the production of ammonium nitrate in industry, although chemically simple, are technologically challenging. The acid-base reaction of ammonia with nitric acid gives a solution of ammonium nitrate:[3] HNO3(aq) + NH3(g) → NH4NO3(aq). For industrial production, this is done using anhydrous ammonia gas and concentrated nitric acid. This reaction is violent and very exothermic. After the solution is formed, typically at about 83% concentration, the excess water is evaporated to an ammonium nitrate (AN) content of 95% to 99.9% concentration (AN melt), depending on grade. The AN melt is then made into "prills" or small beads in a spray tower, or into granules by spraying and tumbling in a rotating drum. The prills or granules may be further dried, cooled, and then coated to prevent caking. These prills or granules are the typical AN products in commerce.

The Haber process combines nitrogen and hydrogen to produce ammonia, part of which can be oxidised to nitric acid and combined with the remaining ammonia to produce the nitrate. Another production method is used in the so-called Odda process.

Ammonium nitrate is also manufactured by amateur explosive enthusiasts by metathesis reactions:

(NH4)2SO4 + 2 NaNO3 → Na2SO4 + 2 NH4NO3
Ca(NO3)2 + (NH4)2SO4 → 2 NH4NO3 + CaSO4

Sodium sulfate is removed by lowering the temperature of the mixture. Since sodium sulfate is much less water-soluble than ammonium nitrate, it precipitates, and may be filtered off. For the reaction with calcium nitrate, the calcium sulfate generated is quite insoluble, even at room temperature.

Crystalline phases

Transformations of the crystal states due to changing conditions (temperature, pressure) affect the physical properties of ammonium nitrate. The following crystalline states have been identified:

System Temperature (°C) State Volume Change (%)
- >169.6 liquid -
I 169.6 to 125.2 cubic +2.1
II 125.2 to 84.2 tetragonal -1.3
III 84.2 to 32.3 α-rhombic +3.6
IV 32.3 to −16.8 β-rhombic −2.9
V −16.8 tetragonal -

The type V crystal is a quasi-cubic form which is related to caesium chloride, the nitrogens of the nitrates and the ammoniums are at the sites in a cubic array where Cs and Cl would be in the CsCl lattice. See C.S. Choi and H.J. Prask, Acta Crystallographica B, 1983, 39, 414-420.

Disasters

Ammonium nitrate decomposes into gases including oxygen when heated (non-explosive reaction); however, ammonium nitrate can be induced to decompose explosively by detonation. Large stockpiles of the material can be a major fire risk due to their supporting oxidation, and may also detonate, as happened in the Texas City disaster of 1947, which led to major changes in the regulations for storage and handling.

There are two major classes of incidents resulting in explosions:

  • In the first case, the explosion happens by the mechanism of shock to detonation transition. The initiation happens by an explosive charge going off in the mass, by the detonation of a shell thrown into the mass, or by detonation of an explosive mixture in contact with the mass. The examples are Kriewald, Morgan (present-day Sayreville, New Jersey) Oppau, Tessenderlo and Traskwood.
  • In the second case, the explosion results from a fire that spreads into the ammonium nitrate itself (Texas City, Brest, Oakdale), or from a mixture of ammonium nitrate with a combustible material during the fire (Repauno, Cherokee, Nadadores). The fire must be confined at least to a degree for successful transition from a fire to an explosion (a phenomenon known as "deflagration to detonation transition", or DDT). Pure, compact AN is stable and very difficult to ignite, and there are numerous cases when even impure AN did not explode in a fire.

Ammonium nitrate based explosives were used in the Oklahoma City bombing.

Ammonium nitrate decomposes in temperatures normally well above 200°C. However the presence of impurities (organic and/or inorganic) will often reduce the temperature point when heat is being generated. Once the AN has started to decompose then a runaway reaction will normally occur as the heat of decomposition is very large. AN evolves so much heat that this runaway reaction is not normally possible to stop. This is a well-known hazard with some types of N-P-K Fertilizers, and is responsible for the loss of several cargo ships.

References

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
  2. ^ Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook. Butterworth–Heinemann. pp. 362. ISBN 1903996651.  
  3. ^ http://www.google.com/patents/pdf/Process_of_producing_concentrated_soluti.pdf?id=XronAAAAEBAJ&output=pdf&sig=ACfU3U0iYFRDUxltKLaVind-3wwP_JYPxg
  • Properties: UNIDO and International Fertilizer Development Center (1998), Fertilizer Manual, Kluwer Academic Publishers, ISBN 0-7923-5032-4.

External links

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Simple English

File:Ammonium nitrate
Ammonium nitrate

Ammonium nitrate is a chemical compound. Its chemical formula is NH4NO3. It contains ammonium and nitrate ions. The nitrogen is in the -3 and +5 oxidation states.

Contents

Properties

Ammonium nitrate is a colorless solid. It dissolves in water. It makes water cold when it dissolves. It is an oxidizing agent. When it is heated gently, it turns into water and nitrous oxide. It can detonate when heated strongly. There were several disasters where ammonium nitrate exploded. Ammonium nitrate fertilizers were banned in some places because they were used to make explosives.

Preparation

Ammonium nitrate is made by reacting ammonia with nitric acid. This reaction is very violent. It can be made by reacting sodium nitrate with ammonium sulfate. This makes a solution of ammonium nitrate and sodium sulfate. When the mixture is cooled, the sodium sulfate is crystallized and can be filtered.

Uses

Ammonium nitrate is used as a fertilizer. It contains more nitrogen than most fertilizers. It is also used in explosives used by terrorists. It can be used as an oxidizer in rockets.

See also


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