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 The rate coefficient (k) for a particular  reactions is 1.3\times10-4 M-1 s-1 at 1000C,  and 1.3\times10-3 M-1 s-1 at 1500C. What  
is the energy of activation (EA) (in kJ) for this reaction ?   (R=molar gas constant =8.314 JK-1 mol-1)            

 

  • Option 1)

    16

  • Option 2)

    60

  • Option 3)

    99

  • Option 4)

    132

 

Answers (1)

best_answer

As we have learnt,

 

Arrhenius Equation -

Arrhenius gave the quantitative dependence of rate constant on temperature by the Arrhenius equation.

- wherein

k = A e^{-E_{a}/RT}

In k=InA-\frac{E_{a}}{RT}

k = Rate constant

 

 

 

As we know the relation,

\\*\ln\left(\frac{K_1}{K_2} \right ) = \frac{E_A}{R}\left[\frac{1}{T_2} - \frac{1}{T_1}\right ]\\*\ln\left(\frac{1.3\times 10^{-4}}{1.3\times 10^{-3}} \right ) = \frac{E_A}{8.314}\left[\frac{1}{423} - \frac{1}{373}\right ] \\*\\*\ln(10^{-1}) = \frac{E_A}{8.314}\times \left [0.000316\right ] \Rightarrow E_A \cong 60 kJ


Option 1)

16

Option 2)

60

Option 3)

99

Option 4)

132

Posted by

SudhirSol

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