NEET Chemistry NEET PYQ-Haloalkanes and Haloarenes

  • question_answer
    For the reaction \[RX+Mg\xrightarrow[{}]{{}}RMgX\]products it is observed that 
    (1) On doubling the initial concentration of A only the rate of reaction is also doubled and.
    (2) On doubling the initial concentrations of both A and B there is a change by a factor of 8 in the rate of the reaction.
    The rate of this reaction is given by                                                    [AIPMT (S) 2009]

    A) rate\[\text{mo}{{\text{l}}^{\text{-1}}}\]

    B) rate\[\text{mo}{{\text{l}}^{\text{-1}}}\]

    C) rate\[\text{mo}{{\text{l}}^{\text{-1}}}\]

    D) rate\[\text{mo}{{\text{l}}^{\text{-1}}}\]

    Correct Answer: B

    Solution :

    [b] For the reaction, \[\underset{\begin{smallmatrix}  \text{ }\!\!|\!\!\text{ } \\  \text{H} \end{smallmatrix}}{\overset{\begin{smallmatrix}  \text{H} \\  \text{ }\!\!|\!\!\text{ } \end{smallmatrix}}{\mathop{\text{C}}}}\,=\underset{\begin{smallmatrix}  \text{ }\!\!|\!\!\text{ } \\  \text{H} \end{smallmatrix}}{\overset{\begin{smallmatrix}  \text{H} \\  \text{ }\!\!|\!\!\text{ } \end{smallmatrix}}{\mathop{\text{C}}}}\,+\text{H}-\xrightarrow[{}]{{}}\text{H}-\underset{\begin{smallmatrix}  \text{ }\!\!|\!\!\text{ } \\  \text{H} \end{smallmatrix}}{\overset{\begin{smallmatrix}  \text{H} \\  \text{ }\!\!|\!\!\text{ } \end{smallmatrix}}{\mathop{\text{C}}}}\,-\underset{\begin{smallmatrix}  \text{ }\!\!|\!\!\text{ } \\  \text{H} \end{smallmatrix}}{\overset{\begin{smallmatrix}  \text{H} \\  \text{ }\!\!|\!\!\text{ } \end{smallmatrix}}{\mathop{\text{C}}}}\,-\text{H}\]Products
    On doubling the initial concentration of A only, the rate of reaction is also doubled, therefore
    Rat\[\text{mo}{{\text{l}}^{\text{-1}}}\]                                                ...(i)
    Let initially rate law is
    Rate\[\text{mo}{{\text{l}}^{\text{-1}}}\]                                               ...(ii)
    If concentration of A and B both are doubled, the rate gets changed by a factor of 8.
    \[\text{mo}{{\text{l}}^{\text{-1}}}\]                             …(iii)
    \[\text{mo}{{\text{l}}^{\text{-1}}}\]
    Dividing Eq. (iii) by Eq. (ii),
    \[1.77\times {{10}^{-5}}\]
    \[5.65\times {{10}^{-10}}\]
    \[6.50\times {{10}^{-12}}\]\[5.65\times {{10}^{-13}}\]
    Hence, rate law is, rate\[5.65\times {{10}^{-12}}\]


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