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2Ararr4B+D , in this reaction, concentr...

`2Ararr4B+D` , in this reaction, concentration of B increases to `2xx10^(-3)"mol.L"^(-1)` after 10s from the start of the reaction . Calculate : rate of formation of B

Text Solution

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Rate of formation of B , `(Delta[B])/(Deltat)=(2xx10^(3))/(10)=2xx10^(-4)"mol.L"^(-1).s^(-1)`
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2Ararr4B+D , in this reaction, concentration of B increases to 2xx10^(-3)"mol.L"^(-1) after 10s from the start of the reaction . Calculate : rate of disappearance of A.

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Knowledge Check

  • After 200s of the initiation of the reaction, 2Ararr4B+(1)/(2)D, the concentration of B is 4xx10^(-2)"mol.L"^(-1) . At the particular time , the rate of the reaction is -

    A
    `10^(-4)"mol.L"^(-1).s^(-1)`
    B
    `2xx10^(-4)"mol.L"^(-1)`
    C
    `5xx10^(-5)"mol.L"^(-1).s^(-1)`
    D
    `2.5xx10^(-4)"mol.L"^(-1).s^(-1)`

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