CMC Medical CMC-Medical VELLORE Solved Paper-2008

  • question_answer
    The rate constant for a first order reaction becomes six times when the temperature is raised from 350 K to 400 K. Calculate the activation energy for the reaction. \[(R=8.314\,\,J{{K}^{-1}}mo{{l}^{-1}})\]

    A)  \[41.7\,kJ\,mo{{l}^{-1}}\]           

    B)  \[4.17\,kJ\,mo{{l}^{-1}}\]

    C)  \[417\,kJ\,mo{{l}^{-1}}\]                             

    D)  \[0.417\,kJ\,mo{{l}^{-1}}\]

    E)  \[4170\,kJ\,mo{{l}^{-1}}\]

    Correct Answer: A

    Solution :

                    \[\log \frac{{{k}_{2}}}{{{k}_{1}}}=\frac{{{E}_{a}}}{2.303R}\left[ \frac{{{T}_{2}}-{{T}_{1}}}{{{T}_{1}}\cdot {{T}_{2}}} \right]\] \[\frac{{{k}_{2}}}{{{k}_{1}}}=6,\] \[{{T}_{1}}=350K,\,{{T}_{2}}=400\,K\] \[\log 6=\frac{{{E}_{a}}}{2.303\times 8.314}\left[ \frac{400-350}{400\times 350} \right]\] \[0.7782=\frac{{{E}_{a}}}{2.303\times 8.314}\times \frac{50}{400\times 350}\] \[{{E}_{a}}=41721\,J\,mo{{l}^{-1}}\]       \[=41.721\,kJ\,mo{{l}^{-1}}\]


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