AMMONIUM NITRITE 409 



The density is not known. 



3. The dry salt may explode when suddenly heated, even 

 below 80. 



4. It is decomposed principally into water and nitrogen, 

 N0 2 HNH 3 = N 2 + 2H 2 O, which yields 22'32 litres of permanent 

 gases, or, for 1 kgm., 349 litres. 



5. The same reaction liberates -f 73'2 Gal. at constant 

 pressure and -f- 734 Cal. at constant volume, or, for 1 kgm., 

 1144 Cal. at constant pressure, 1153 Cal. at constant volume. 



6. At the temperature of the explosion the water is gaseous, 

 which trebles the volume of the gases. The latter therefore 

 occupy 



66-96 litres (l + 



On the other hand, the heat developed must be referred to 

 the formation of gaseous water, which reduces it to 4- 5 3 '8 Cal. 



7. The theoretical temperature of the products is obtained by 

 dividing 53,800 by 19'2, which gives 2800. 



8. The permanent pressure is obtained by subtracting from 

 the fixed capacity the volume of the water, or 562 c.c. for 

 1 kgm. 



For the density of charge, , it will therefore be 



349 atm. 361 kgm. 

 n - 0-5625 r n - 0'56 



for n = 1 : 820 kgm. per square centimetre. 



9. At the theoretical temperature of decomposition the 

 pressure becomes, the water being gaseous 



1147 \ l + 273J 12961 atm. 13393 kgm. 

 - = _ _ or - -, 



n n n 



which makes for n = 1 : 13,393 kgm. per square centimetre. 



6. AMMONIUM NITRATE: N0 3 HNH 3 . 



1. Equivalent = 80 grms. 



2. Composition 



Nitrogen ......... 350 



Hydrogen ......... 50 Water ... 450 



Oxygen ......... 600 Excess of oxygen 200 



1000 



3. Density, 1'707. 



4. Heat of formation from the elements 



N 2 + H 4 + O 3 = N0 3 HNH 3 + 87'9 Cal. 



