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JIPMER Jipmer Medical Solved Paper-2014

  • question_answer
    Observe the following reaction \[2A+B\xrightarrow{{}}C\] The rate of formation of C is \[2.2\times {{10}^{-3}}\,mol\,{{L}^{-1}}\,mi{{n}^{-1}}.\] What is the value of\[-\frac{d[A]}{dt}(in\,mol\,{{L}^{-1}}\,mi{{n}^{-1}})?\]

    A)  \[2.2\times {{10}^{-3}}\]             

    B)     \[1.1\times {{10}^{-3}}\]                             

    C)     \[4.4\times {{10}^{-3}}\]             

    D)     \[5.5\times {{10}^{-3}}\]

    Correct Answer: C

    Solution :

    From rate of reaction \[-\frac{1}{2}\frac{d\,[A]}{dt}=-\frac{d\,[B]}{dt}=\frac{d\,[C]}{dt}\Rightarrow \frac{d\,[A]}{dt}=2\cdot \frac{d\,[C]}{dt}\]   \[=2\times 2.2\times {{10}^{-3}}=4.4\times {{10}^{-3}}\]


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