Nitrogen explosives

Heating must be terminated when two-thirds of the nitrate has decomposed since explosive nitrogen trichloride may be formed from traces of ammonium chloride impurity. 

A liquid chlorine tank was kept cool by a refrigeration system that used CFCs. In 1976 the local management decided to use ammonia instead. Management w as unaware that ammonia and chlorine react to form explosive nitrogen trichloride. Some of the armnonia leaked into the chlorine, and the nitrogen trichloride that was formed exploded in a pipeline... 

Urea reacts with sodium hypochlorite or calcium hypochlorite to form explosive nitrogen trichloride. 

Electrolysis of sodium chloride in presence of nitrogenous compounds to produce chlorine may lead to formation of explosive nitrogen trichloride. Precautions are detailed. 

During the reductive cleavage of cyclopolyenes with potassium in liquid ammonia, the intermediate anionic species are quenched with iodine-pentane mixtures. The possibility of formation of explosive nitrogen triiodide and the need for precautions are stressed. 

R Based on sodium hypochlorite solution MSDS. Generates heat and toxic vapors can form explosive nitrogen trichloride under certain conditions... 

Accidental contact via a cracked glass trap caused a violent explosion. Nitrogen is a safer coolant. 

In one of J. S. Stas processes, the iodine was dissolved in a soln. of potassium iodide. The soln. was diluted with water until a precipitate began to form, and then three-fourths of the amount of water required to precipitate all the iodine were added. The separated iodine was washed free from potassium iodide by decantation, the crystals, after draining, were dried over calcium nitrate in vacuo, and then distilled twice from barium oxide. In another process, J. S. Stas purified the iodine by first treating the iodide with ammonia which converts about 95 per cent, of it into the explosive nitrogen iodide. The washed nitrogen iodide decomposes quietly when warmed with an excess of water. J. S. Stas thus describes the procedure ... 

The reaction is 8NH3+3Br,=6NH4Br+Na. The liquid should remain strongly ammoniacal during the addition of the bromine, and it should be continually shaken. If the bromine is run in too rapidly, or if the liquid becomes acid, the explosive nitrogen bromide may be formed. Heat the liquid nntil all the free ammonia is driven off, and evaporate the soln. to enable the ammonium bromate to crystallize. Dry the aihmonium salt by warming the dish over a flame. The yield is 220 grms. of ammonium bromate. 

Khattak, M. A., Engineering Horizons (Pakistan), 1991, (Aug.), 33 Chlorine reacts with ammonia and compounds to form the treacherously explosive nitrogen trichloride. A change was made to ammonia as refrigerant in the production of liquid chlorine some months later minor explosions when transferring the chlorine... 

Contact above 0°C of excess chlorine or a chlorinating agent with aqueous ammonia, ammonium salts or a compound containing a hydrolysable amino-derivative, or electrolysis of ammonium chloride solution produces the highly endothermic (AHf (g) +230.1 kJ/mol, 1.91 kJ/g) and explosive nitrogen trichloride as a water-insoluble yellow oil [1,2,3]. Detonation at constant volume generates 5,500 Bar maximum pressure and 2,100°C maximum temperature. As a vapour it decomposes explosively at pressures as low as 1 mBar and may sensitise flammable gas mixtures even as a... 

Where two or more elements or compounds are involved in a reactive hazard, and an intermediate or product of reaction is identifiable as being responsible for the hazard, both reacting substances are normally cross-referred to the identified product. The well-known reaction of ammonia and iodine to give explosive nitrogen triodide-ammonia is an example of this type. The two entries Ammonia Halogens, p. 1730 Iodine Ammonia, p. 1794... 

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