JEE Main & Advanced AIEEE Solved Paper-2013

  • question_answer
    The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation of such a reaction will be: (\[R=8.314\text{ }J{{K}^{-1}}\]and\[log2=0.301\])     AIEEE Solevd Paper-2013

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

    B) \[48.6\text{ }kJ\text{ }mo{{l}^{-1}}\]      

    C) \[58.5\text{ }kJ\text{ }mo{{l}^{-1}}\]

    D)        \[60.5\text{ }kJ\text{ }mo{{l}^{-1}}\]

    Correct Answer: A

    Solution :

    \[0.3010=\frac{Ea}{2.303R}\left[ \frac{{{T}_{2}}-{{T}_{1}}}{{{T}_{1}}{{T}_{2}}} \right]\] \[\Rightarrow \]\[0.3010=\frac{Ea}{2.303\times 8.314\times {{10}^{-3}}}\left( \frac{310-300}{310\times 300} \right)\] \[{{E}_{a}}=53.6\text{ }kJ\text{ }mol\]


You need to login to perform this action.
You will be redirected in 3 sec spinner