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.

The half time of first order decomposition of nitramide is `2.1` hour

1.	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.
Answer» `(i) k=(0693)/(t_(1//2))=(0.693)/(2.1)=0.33hr^(-1)` Applying kinetic eqution of rist order reaction, `k=(2.303)/(t)log_(10).(a)/((a-x))` `or t=(2.303)/(0.33)log_(10).(100)/((10099))=13.96hrs` (ii) No. of moles of `NH_(2)NO_(2)` decomposed `=0.99xx(6.2)/(62)=0.099` No. of moels of `N_(2)O` formed =0.099 Volume f `N_(2)O` at STP `=0.099xx225400 mL=2217.6mL`

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