JEE Main & Advanced Sample Paper JEE Main - Mock Test - 31

  • question_answer
    The activation energy for a reaction is 9.0 kcal/mol. The increase in the rate constant when its temperature is increased from 298K to 308K is

    A) \[63 %\]            

    B)        \[50 %\]

    C) \[100 %\]

    D) \[10 %\]

    Correct Answer: A

    Solution :

    \[2.303\,\,\log \,\frac{{{k}_{2}}}{{{k}_{1}}}=\frac{{{E}_{a}}}{R}\left[ \frac{{{T}_{2}}-{{T}_{1}}}{{{T}_{1}}{{T}_{2}}} \right]\] \[\log \frac{{{k}_{2}}}{{{k}_{1}}}=\frac{9.0\times {{10}^{3}}}{2.303\times 2}\left[ \frac{308-298}{308\times 298} \right]\] \[\frac{{{k}_{2}}}{{{k}_{1}}}=\frac{9.0\times {{10}^{3}}}{2.303\times 2}\left[ \frac{308-298}{308\times 298} \right]\] \[\frac{{{k}_{2}}}{{{k}_{1}}}=1.63;\,\,{{k}_{2}}=1.63\,{{k}_{1}};\,\,\frac{1.63{{k}_{1}}-{{k}_{1}}}{{{k}_{1}}}\times 100=63\,%\]


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