BCECE Medical BCECE Medical Solved Papers-2014

  • question_answer
    The activation energy for a reaction at the temperature T K was found to be\[2.303\,\,RT\,\,J\,mo{{l}^{-1}}\]. The ratio of the rate constant to Arrhenius factor is

    A)  \[{{10}^{-1}}\]

    B)  \[{{10}^{-2}}\]

    C)  \[2\times {{10}^{-3}}\]

    D)  \[2\times {{10}^{-2}}\]

    Correct Answer: A

    Solution :

    Arrhenius equation is, rate constant, \[k=A{{e}^{-{{E}_{a}}/RT}}\] \[k=A{{e}^{-2.303\,RT/RT}}\Rightarrow \frac{k}{A}={{e}^{-2.303}}\] on solving, we get \[\frac{k}{A}={{10}^{-1}}\]


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