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In the catalysed decomposition of benzen...

In the catalysed decomposition of benzene diazonium chloride,

half-life period is found to be independent of the initial concentration of the reactant. After 10 minutes, the volume of `N_(2)` gas collected is 10 L and after the reaction is complete, it is 50 L. Hence, rate constant of the reaction (in `"min"^(-1)`) is

A

`(2.303)/(10)log""(10)/(50)`

B

`(2.303)/(10)log""(50)/(50-10)`

C

`(2.303)/(10)log""(50)/(10)`

D

`(2.303)/(10)log""(10)/(50-10)`

Text Solution

Verified by Experts

The correct Answer is:
B
As half-life period is independent of initial concentration, hence it is a reaction of 1st order.
`therefore k = (2*303)/(t) log ""(a)/(a-x)`
But `V_(oo) prop a and V_(t) prop x.`
Hence, `k = (2*303)/(10) log""(50)/(50-10).`
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Knowledge Check

  • Half life id independent of the concentration of A . After 10 mi n volume of N_(2) gas is 10 L and after complete reaction is 50 L . Hence, the rate constant is

    A
    `(2.303)/(10) log 5 mi n^(-1)`
    B
    `(2.303)/(10) log 1.25 mi n^(-1)`
    C
    `(2.303)/(10) log 2 mi n^(-1)`
    D
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  • Half-life period of a first order reaction is 10 min. Starting with initial concentration 12 M, the rate after 20 min is

    A
    `0.693 "M min"^(-1)`
    B
    `0.693xx3 "M min"^(-1)`
    C
    `0.0693xx3 "M min"^(-1)`
    D
    `0.0693xx4 "M min"^(-1)`

  • The half-life period of a first order reaction is 10 minutes. Starting with initial concentration 12 M, the rate after 20 minutes is

    A
    `0.693 xx 3 M min^(-1)`
    B
    `0.0693 xx 4 M min^(-1)`
    C
    `0.0693 M min^(-1)`
    D
    `0.0693 xx 3 M min^(-1)`
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