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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

(i) `k=(0.693)/(t_(1//2))=(0.693)/(2.1" hr")=0.33" hr"^(-1)`
`x=99%" of "a=0.99" a"`
`t=(2.303)/(k)log""(a)/(a-x)=(2.303)/(0.33" hr"^(-1))log""(a)/(a-0.99a)=(2.303)/(0.33)log10^(2)=13.96" hours"`
(ii) Amount decomposed `=99%" of "6.2" g "=(99)/(100)xx6.2" g "=6.138" g"`
1 mol `NH_(2)NO_(2)(62" g")" produce "N_(2)O" at STP"=22.4" L"`
6.138 g will produce `N_(2)O` at STP `=(22.4)/(62)xx6.138" L"=2.2176" L"`
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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

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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.