Ammonium nitrate can decompose with explosion by the following reaction `:`
`NH_(4)NO_(3(s)) rarr N_(2)O_((g))+2H_(2)O_((g)),DeltaH=-37.0kJ` Calculate the heat produced when `2.50g` of `NH_(4)NO_(3)` decomposes.

Write the expression of K_(c) for the reactions: NH_(4)NO_(3)(s)hArrN_(2)O(g)+2H_(2)O(g)

The equilibrium constant for the reaction NH_(4)NO_(2)(s)hArr N_(2)(g)+2H_(2)O(g) , is given by

Identify whether the following reactions are redox reactions or not : NH_(4)NO_(2)(s)toN_(2)(g)+2H_(2)O(g)

The molar heat ofreaction of NH_(4)NO_(3(s)) rarr N_(2)O_((g)) + 2H_(2)O_((l))," is "-122.55 KJ" at "25^(@)C and 1.0 atmospheric pressure. Delta U for the reaction :

The half time of first order decomposition of nitramide is 2.1 hour at 15^(@)C . NH_(2)NO_(2(aq.))rarr N_(2)O_((g))+H_(2)O_((l)) If 6.2 g of NH_(2)NO_(2) is allowed to decompose, calculate: (i) Time taken for NH_(2)NO_(2) is decompose 99% . (ii) Volume of dry N_(2)O produced at this point measured at STP.

Identify the following reactions at disproportionation a comproportionations reactions- 2NH_(4)NO_(3)(s)toN_(2)(g)+4H_(2)O_(g)+O_(2)(g)

Decomposition of NH_(4)NO_(2)(aq into N_(2)(g) and 2H_(2)O(l) is first order reaction.