NEET NEET SOLVED PAPER 2017

  • question_answer
    Mechanism of a hypothetical reaction\[{{X}_{2}}+{{Y}_{2}}\to 2XY\] is given below:                        
    (i) \[{{X}_{2}}\to X+X(fast)\]
    (ii) \[X+{{Y}_{2}}XY+Y(slow)\]
    (iii)\[X+Y\to XY(fast)\]
                    The overall order of the reaction will be

    A)                  1.5                        

    B)         1

    C)                  2                                            

    D)  0

    Correct Answer: A

    Solution :

                     The solution of this question is given by assuming step (i) to be reversible which is not given in question                 Overall rate = Rate of slowest step (ii)                                 \[=k[X][{{Y}_{2}}]\]                                         ?(1)                 K=rate constant of step (ii) Assuming step (i) to be reversible, its equilibrium constant, \[{{k}_{eq}}=\frac{{{[X]}^{2}}}{[{{X}_{2}}]}\Rightarrow [X]={{k}_{eq}}^{\frac{1}{2}}{{[{{X}_{2}}]}^{\frac{1}{2}}}\]                                ?(2) Put (2) in (1) \[Rate=k{{k}_{eq}}^{\frac{1}{2}}{{[{{X}_{2}}]}^{\frac{1}{2}}}[{{Y}_{1}}]\] Overall order \[=\frac{1}{2}+1=\frac{3}{2}\]


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