JEE Main & Advanced JEE Main Paper (Held On 9 April 2017)

  • question_answer
    The rate of a reaction quadruples when the temperature changes from 300 to 310 K. The activation energy of this reaction is: (Assume activation energy and pre-exponential factor are independent of temperature;  [JEE Online 09-04-2017]\[\ln \,2=\,0.693;\,\,R=8.314\,J\,\,mo{{l}^{-1}}\,{{K}^{-1}}\])

    A)  \[53.6\,kJ\,mo{{l}^{-1}}\]           

    B)  \[214.4\,\,kJ\,mo{{l}^{-1}}\]

    C)  \[107.2\,kJ\,mo{{l}^{-1}}\]         

    D)  \[26.8\,kJ\,mo{{l}^{-1}}\]

    Correct Answer: C

    Solution :

                    \[4=\,{{e}^{\frac{Ea}{R}\left\{ \frac{1}{300}-\frac{1}{310} \right\}}}\]                 \[\ln \,(4)=\frac{Ea}{R}\left\{ \frac{10}{300\,\times 310} \right\}\]                 \[Ea\,=\frac{0.693\,\times 2\times 8.314\,\times 300\,\times 310}{10}\]                 \[=107165.79\,J\,=107.\,165\,kJ\]


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