NEET Sample Paper NEET Sample Test Paper-91

  • question_answer
    For a reaction of type \[A+B\xrightarrow{{}}\] products, it is observed that doubling concentration of A causes the reaction rate to be four times as great, but doubling amount of B does not affect the rate. The rate equation is

    A) Rate\[=K[A][B]\]

    B)        Rate\[=\frac{K}{4}{{[A]}^{2}}\]

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

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

    Correct Answer: C

    Solution :

    [c] Let the rate law equation be \[r=k{{[A]}^{x}}{{[B]}^{y}}\]                                   ...(1) when A = 2A, \[4r=k{{[2A]}^{x}}{{[B]}^{y}}\]                                ...(2) Divide (2) by(1) \[\frac{4r}{r}=\frac{k{{[2A]}^{x}}{{[B]}^{y}}}{k{{[A]}^{x}}{{[B]}^{y}}}\] \[\therefore \] \[4={{(2)}^{x}},\]Hence \[x=2\] when B = 2B, \[r=k{{[A]}^{x}}{{[2B]}^{y}}\]                                  ...(3) \[\therefore \] 1 = Divide (3) by (1) \[\frac{r}{r}=\frac{k{{[A]}^{x}}{{[2B]}^{y}}}{k{{[A]}^{x}}{{[B]}^{y}}}{{(2)}^{y}}\] \[\therefore \]\[y=0\] \[\therefore \] Rate \[=k{{[A]}^{2}}{{[B]}^{0}}\]


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