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JEE Main & Advanced JEE Main Paper (Held On 12 April 2014)

  • question_answer
    The rate coefficient (k) for a particular reactions is \[1.3\times {{10}^{-4}}{{M}^{-1}}\]\[{{s}^{-1}}\] at \[100{}^\circ C\], and \[1.3\times {{10}^{-3}}\] at \[150{}^\circ C\]. What is the energy of activation (EA) (in kJ) for this reaction? (R = molar gas constant\[=8.31J{{K}^{-1}}kJ\])   [JEE Main Online Paper ( Held On 12 Apirl  2014 )

    A) 16                                          

    B) 60

    C) 99                                          

    D) 132

    Correct Answer: B

    Solution :

                    According to Arrhenius equation \[\log \frac{{{k}_{2}}}{{{k}_{1}}}=\frac{{{E}_{a}}}{2.303R}\left( \frac{1}{{{T}_{1}}}-\frac{1}{{{T}_{2}}} \right)\] \[\log \frac{1.3\times {{10}^{-3}}}{1.3\times {{10}^{-4}}}=\frac{{{E}_{a}}}{2.303\times 8.314}\left[ \frac{1}{373}-\frac{1}{423} \right]\] \[1=\frac{{{E}_{a}}}{2.303\times 8.314}\left[ \frac{1}{373}-\frac{1}{423} \right]\]\[{{E}_{a}}=60\text{kJ/mole}\]


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