BVP Medical BVP Medical Solved Paper-2009

  • question_answer
    The rate of a gaseous reaction triples when temperature is increased by \[{{10}^{o}}C\] from \[{{25}^{o}}C\]. The energy of activation of the reaction (in \[kJ\,\,mo{{l}^{-1}}\]) will be

    A)  \[40\]                                  

    B)  \[70\]

    C)  \[83.8\]                              

    D)  \[200\]

    Correct Answer: C

    Solution :

                    Given, \[{{T}_{1}}={{25}^{o}}C=25+273=298K\] \[{{T}_{2}}=(25+{{10}^{o}}C)={{35}^{o}}C=308K\] Rate \[\propto \]k \[\Rightarrow \]                \[\frac{{{(Rate)}_{{{25}^{o}}}}}{{{(Rate)}_{{{35}^{o}}}}}=\frac{{{k}_{{{25}^{o}}}}}{{{k}_{{{35}^{o}}}}}\]                 \[\frac{{{k}_{{{25}^{o}}}}}{{{k}_{{{35}^{o}}}}}=\frac{1}{3}\] From Arrhenius equation,                 \[\log \frac{{{k}_{{{35}^{o}}}}}{{{k}_{{{25}^{o}}}}}=\frac{{{E}_{a}}}{2.303R}\left[ \frac{1}{{{T}_{1}}}-\frac{1}{{{T}_{2}}} \right]\] \[\log 3=\frac{{{E}_{a}}}{2.303\times 8.314\times {{10}^{-3}}}\left[ \frac{1}{298}-\frac{1}{308} \right]\] \[0.477=\frac{{{E}_{a}}}{2.303\times 8.314\times {{10}^{-3}}}\left[ \frac{10}{298\times 308} \right]\] \[\therefore \]  \[{{E}_{a}}=83.8kJ\,mo{{l}^{-1}}\]


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