JEE Main & Advanced Chemistry Chemical Kinetics / रासायनिक बलगतिकी Question Bank Critical Thinking Chemical Kinetics

  • question_answer
    The activation energy for a reaction is \[9.0\,K\,cal/mol.\] The increase in the rate constant when its temperature is increased from 298K to 308K is   [JIPMER 2000]

    A)                 63%       

    B)                 50%

    C)                 100%    

    D)                 10%

    Correct Answer: A

    Solution :

               \[2.303\log \frac{{{K}_{2}}}{{{K}_{1}}}=\frac{{{E}_{a}}}{R}\left[ \frac{{{T}_{2}}-{{T}_{1}}}{{{T}_{1}}{{T}_{2}}} \right]\]                    \[\log \frac{{{K}_{2}}}{{{K}_{1}}}=\frac{9.0\times {{10}^{3}}}{2.303\times 2}\,\,\left[ \frac{308-298}{308\times 298} \right]\]                 \[\frac{{{K}_{2}}}{{{K}_{1}}}=1.63\,;\,\,{{K}_{2}}=1.63\,{{K}_{1}};\,\frac{1.63{{K}_{1}}-{{K}_{1}}}{{{K}_{1}}}\times 100=63.0%\]


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