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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-1miL-1

            I

    1.0 x 10-3

    1.0 x 10-3

    10-4

            II

    0.2 x 10-2

    2.0 x 10-3

    4 x 10-4

            III

    0.2 x 10-2

    1.0 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]^2[B] \\ }


Option: 2

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


Option: 3

\mathrm{\text { Rate }=K[A][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 A is doubled, the rate increases by 2 times. Hence, order of reaction is 1 wrt A.

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

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

Posted by

Ritika Harsh

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