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The half time of first order decompositi...

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.

Text Solution

Verified by Experts

`:' t=2.303/K"log"_(10)a/((a-x))`
If `t=t/2, x=a/2`,
`:. t_(1//2)=2.303/K"log"_(10)a/(a-a/2) …(1)`
If `t=t_(99%), x=(99a)/(100)`
`t_(99%)=2.303/K"log"_(10) a/(a-(99a)/100) …(2)`
By eqs. (1) and (2)
`t_(99%)=(log_(10) 100)/(log_(10)2)xxt_(1//2)=2/0.3010xx2.1`
`=13.95 hour`
Also mole of `N_(2)O` formed
`=99/100xx"mole of" NH_(2)NO_(2)` taken
`=99/100xx6.2/62=0.099`
`:.` Volume of `N_(2)O` formed at `STP`
`=0.099xx22.4=2.217 litre`
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Knowledge Check

  • The half-time of the following first order decomposition of nitramide is 2.1 h at 15^(@)C : NH_(2)NO_(2)(aq)rarrN_(2)O(g)+H_(2)O(l) If 6.2 g of nitramide is allowed to decompose then time taken for it to decompose 99%, will be

    A
    2.1 h
    B
    12 h
    C
    13.96 h
    D
    33 h

  • The half-life of first order decomposition of NH_(4)NO_(3) is 2.10 hr at 288 K temperature NH_(4)NO_(3)(aq)toN_(2)O(g)+2H_(2)O(l) . If 6.2 of NH_(4)NO_(3) is allowed to decompose, the required for NH_(4)NO_(3) to decompose 90 % is :

    A
    6.978 hr
    B
    0.319
    C
    0.319 hr
    D
    None of these

  • NH_(4)NO_(3) overset(Delta) to N_(2)O+H_(2)O

    A
    For disproportionation reaction.
    B
    For comproportionation reaction.
    C
    For either intermolecular redox reaction or displacement reaction
    D
    For either thermal combination redox reaction or thermal decomposition redox reaction.