JEE Main & Advanced Chemistry Chemical Kinetics / रासायनिक बलगतिकी Question Bank Collision theory, Energy of activation and Arrhenius equation

  • question_answer
    The rate constant is doubled when temperature increases from 27°C to 37°C. Activation energy in kJ is     [JEE Orissa 2004]

    A)                 34          

    B)                 54

    C)                 100        

    D)                 50

    Correct Answer: B

    Solution :

               \[\log \frac{{{K}_{2}}}{{{K}_{1}}}=\frac{{{E}_{a}}}{2.303R}\left[ \frac{1}{{{T}_{1}}}-\frac{1}{{{T}_{2}}} \right]\]                    If \[\frac{{{K}_{2}}}{{{K}_{1}}}=2\]                    \[\log 2=\frac{{{E}_{a}}}{2.303\times 8.314}\left[ \frac{1}{300}-\frac{1}{310} \right]\]                    \[{{E}_{a}}=.3010\times 2.303\times 8.314\left( \frac{300\times 310}{10} \right)\]                       \[=53598.59\ Jmo{{l}^{-1}}\] \[=54\ kJ\].


You need to login to perform this action.
You will be redirected in 3 sec spinner