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

During the kinetic study of the reaction, A + B→ C, the 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

    0.5 x 10-3

    2.0 x 10-3

    4 x 10-4

        III

    1.0 x 10-3

    2.0 x 10-3

    2 x 10-4

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

 

Option: 1

\mathrm{ \text { Rate }=K[A]^{-1}[B] \\ }


Option: 2

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


Option: 3

\mathrm{\text { Rate }=K[A]^{-1}[B]^2 \\ }


Option: 4

\mathrm{ \text { 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 2 times. Hence, order of reaction is 1 wrt B.

During Run II while the concentration of B is doubled while A is halved, the rate increases by 4 times. Since the 2 times rate increase is expected by doubling the rate of B. It can be said, rate has doubled due to halving the concentration of A. Thus, order of reaction is -1 wrt A.

\mathrm{ \text { Rate }=K[A]^{-1}[B] \\ }

Posted by

Suraj Bhandari

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