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BVP Medical BVP Medical Solved Paper-2012

  • 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, \[k=A{{e}^{-{{E}_{a}}/RT}}\]                 \[k=A{{e}^{-2.303RT/RT}}\]                 \[k=A{{e}^{-2.303RT/RT}}\] On solving, we get                 \[\frac{k}{A}={{10}^{-1}}\]


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