| Identification | Back Directory | [Name]
Nitric acid chlorine salt | [CAS]
14545-72-3 | [Synonyms]
Chloronitrate
Nitroxychloride
Nitrooxy chloride
Nitryl hypochlorite
Nitric acid chlorine salt
Nitryl hypochlorite ((NO2)(ClO)) (9CI) | [Molecular Formula]
ClNO3 | [MOL File]
14545-72-3.mol | [Molecular Weight]
97.46 |
| Chemical Properties | Back Directory | [Definition]
A compound that slows the rate of destruction of
ozone. | [Melting point ]
-107°C | [Boiling point ]
18°C | [form ]
Colorless to pale yellow, mobile liquid | [Henry's Law Constant]
7.0×10-2 mol/(m3Pa) at 25℃, Robinson et al. (1997) |
| Hazard Information | Back Directory | [Hazard]
Explosive reaction with metals, metal chlorides, alcohols, ethers, and most organic materials. | [Production Methods]
A refrigerated pocket-shaped receiver is used to sublime an excess of N2O5 directly onto Cl2O in a high vacuum. The receiver containing the Cl2O (equivalent to 5 ml of liquid) is placed in liquid nitrogen so that only the portion holding the Cl2O is cooled, and the N2O5 thus deposits on the Cl2O as a solid. After releasing the vacuum, the receiver is removed from the high-vacuum apparatus, closed off using a drying tube, and placed in a refrigerating bath at —78°C. While the bath is slowly warmed to between —20 and 0°C (over 15 hours), the components react slowly. The ClNO3 thus formed is still contaminated with chlorine (an impurity of the Cl2O) and excess N2O5. To eliminate the chlorine, which is difficult to separate, the reaction product is heated to 30°C in a water bath and refluxed for one hour. The upper half of the reaction vessel (serving as a condenser) is cooled by a ring-shaped cup filled with Dry Ice. The chlorine is volatilized in this procedure, while the excess N2O5 is decomposed to NO2 and O2. The ClNO3 is then distilled at — 90°C in a high vacuum, leaving behind the NO2.
Cl2O+N2O5=2ClNO3
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