Difference between revisions of "Dinitrogen pentoxide"
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===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=20272 N2O5 from UV-light on NO2] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=20272 N2O5 from UV-light on NO2] | ||
| + | *[http://www.sciencemadness.org/talk/viewthread.php?tid=157356 N2O5 from NO2 and Ozone?] | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=7600 Nitronium ion, Dinitrogen Pentoxide] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=7600 Nitronium ion, Dinitrogen Pentoxide] | ||
Latest revision as of 20:28, 5 May 2021
| Names | |
|---|---|
| IUPAC name
Dinitrogen pentaoxide
| |
| Other names
Anhydrous nitric acid
Dinitrooxidane DNPO Nitric anhydride Nitroether Nitronium nitrate Nitryl nitrate | |
| Properties | |
| N2O5 | |
| Molar mass | 108.01 g/mol |
| Appearance | White-yellowish solid |
| Odor | Nitrogen dioxide |
| Density | 2.05 g/cm3 (0 °C) 1.99 g/cm3 (16 °C) 1.642 g/cm3 (18 °C) |
| Melting point | 41 °C (106 °F; 314 K) |
| Boiling point | 47 °C (117 °F; 320 K) (sublimes) |
| Reacts | |
| Solubility | Soluble in 1,1-dichloroethane, 1,2-dichloroethane, allyl chloride, bromine, chloroform, CCl4, dinitrogen tetroxide, nitric acid, nitromethane, pentachloroethane, POCl3, liq. SO2 |
| Solubility in carbon tetrachloride | 51.6288 g/100 ml (15 °C)[1] |
| Solubility in nitric acid | 9 g/100 ml |
| Solubility in nitromethane | 47.3084 g/100 ml (15 °C) |
| Vapor pressure | 279 mmHg at 20 °C |
| Thermochemistry | |
| Std molar
entropy (S |
178.2 J·mol-1·K-1 (s) 355.6 J·mol-1·K-1 (g) |
| Std enthalpy of
formation (ΔfH |
−43.1 kJ/mol (s) +11.3 kJ/mol (g) |
| Hazards | |
| Safety data sheet | None |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Nitrogen dioxide Dinitrogen trioxide Dinitrogen tetroxide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Dinitrogen pentoxide is the chemical compound with the formula N2O5, an unstable nitrogen oxide, used as oxidizer in various chemical reactions, though now largely replaced by nitronium tetrafluoroborate.
Contents
Properties
Chemical
Dinitrogen pentoxide can nitrate organic compounds, similar to the nitrating mixture.
- N2O5 + Ar–H → HNO3 + Ar–NO2
While not explosive on its own, N2O5 can form explosive mixtures with various organic compounds.
Physical
Dinitrogen pentoxide is a white to slight yellowish solid. It reacts exothermically with water to give nitric acid, but it is soluble in chloroform and nitromethane.
Availability
Dinitrogen pentoxide is not sold by any supplier and has to be made.
Preparation
Dinitrogen pentoxide can be obtained via dehydration of conc. nitric acid with conc. sulfuric acid or oleum, though phosphorus pentoxide gives better results. The N2O5 obtained this way however, is difficult to separate from the reaction product.
A very simple way of obtaining nitrogen pentoxide involves the reaction of nitrogen dioxide or dinitrogen tetroxide with ozone, reaction which takes place at low temperatures (-11 °C). A good solvent for the reaction is trifluoroacetic acid.
Another route involves the reaction between lithium nitrate with nitryl fluoride, at -196 °C in a passivated stainless steel cylinder.[2]
Projects
- Synthesis of various energetic materials[3]
Handling
Safety
Dinitrogen pentoxide is a very poweful oxidizer and must be kept away from any combustible material.
Storage
Dinitrogen pentoxide should be used as soon as possible. At room temp it has a half-life of about 9 h, at 0 °C 2 weeks and at -60 °C around one year.
Disposal
Dissolution in large amounts of water will give nitric acid. Addition of a base will convert the acid to nitrate salt, which is easy to safely dispose of.
References
- ↑ Eyring, H.; Daniels, F.; J. Am. Chem. Soc., 1930, 52 (4), pp 1472–1486
- ↑ Jochims, H.-W.; Denzer, W.; Baumgaertel, H.; Loesking, O.; Willner, H.; Berichte der Bunsen-Gesellschaft; vol. 96; nb. 4; (1992); p. 573 - 578
- ↑ http://www.sciencemadness.org/talk/files.php?pid=219365&aid=15690
