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  • During the kinetic study of the reaction, A + B→ C, following results were obtained:

During the kinetic study of the reaction, A + B→ C, following results were obtained:

    Run

    [A] mol L-1

    [B] mol L-1

    Rate of appearance of C mol L-1min-1

    I

    1.0 x 10-3

    1.0 x 10-3

    10-4

    II

    2.0 x 10-3

    2.0 x 10-3

    4 x 10-4

    III

    1.0 x 10-3

    2.0 x 10-3

    4 x 10-4

 

Based on the above data, which one of the following is correct rate law for the reaction?

Option: 1

\mathrm{ Rate =K[A]^2[B] }


Option: 2

\mathrm{Rate =K[A][B] }


Option: 3

\mathrm{ Rate =K[A]^2[B]^2 \\ }


Option: 4

\mathrm{ Rate =K[A]^0[B]^2 }


Answers (1)

best_answer

On observing the given data, it appears that at Run III while the concentration of B is doubled, the rate increases by 4 times. Hence, order of reaction is 2 wrt B.

During Run II while the concentration of both A and B is doubled, the rate increases by 4 times. Since the 4 times rate increase is expected by doubling the rate of B. Hence, it can be said, rate variation has remained unaffected due to change in concentration of A. 

\mathrm{\ Rate =\mathrm{K}[\mathrm{A}]^0[\mathrm{~B}]^2}.

 

Posted by

himanshu.meshram

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