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4 - Region of zone decomposition in t h e system ammonium nitrate-ammonium dihydrogen phosphatepotassium chloride. HTJYGEN a n d P E R B A L . grams such as t h a t shown in Figure 4 for the ammonium nitrate-ammo nium phosphate-potassium chloride system. The main conclusion from both is t h a t a solid matrix a t the decomposition temperature is an impor t a n t factor in governing whether and a t what rate t h e self-sustaining reac tion will propagate. The greater the tendency for the fertilizer to become 46 molten, or to contain large amounts of liquid phase, before the decom position temperature is reached, the less likely is the material to propagate the decomposition reaction.
33 kcals/mole. The solid solution can also react with potassium chloride (equation 8). 43 kcals (8) I t is this reaction, and/or the simple reversion of the solid solution to the stable form t h a t results in the self-heating of fertilizers in the pre sence of urea. The thermochemistry of the above process has been investi gated at Levington Research Station . I t will be seen t h a t the heat evolved from reaction  is greater than t h a t from the straightforward ionic exchange reaction (7).
1955, 23, 693.  M. A . COOK a n d T. A B E G G , " I n d . E n g . ", 1956, 48, 1090.  R . D . SMITH, "Trans. Faraday S o c " , 1957, 53, 1341.  W . A . R O S S E R , S. H . I N A M I a n d H . W I S E , " J . P h y s . ", 1963, 67, 1753.  B . ROZMAN and L. BORODKINA, " J . Applied Chem. ", 1959, 32, 291.  T. L . D A V I S a n d A . J . J . A B R A M S , " J . Amer. Chem. S o c " , 1925, 47, 1043.  L . F R I E D M A N N a n d J . B I G E L E I S E N , " J . Chem. P h y s " , 1950, 18, 1325.