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Values of the rate constant for the decomposition of N2O5 at four different temperatures are as...

Values of the rate constant for the decomposition of N2O5 at four different temperatures are as follows: T(K) k(s^-1) 658 2.14 x 10^5 673 3.23 x 10^5 688 4.81 x 10^5 703 7.03 x 10^5 Determine the activation energy of the decomposition reaction: _____kJ/mol Calculate the value of the rate constant at 300 K. _____s^-1

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Answer #1

Temperature k value given are

1) 658 2.14 x 10-5

2) 673 3.23 x1o-5

3) 688 4.81 x 10-5

4) 703 7.03x 10-5

Using the Arhenius equation log(k2/k1) = Ea/R [1/T1 -1/T2]

calculating for different sets 1,2,3 and 4 , we get the valuesfor activation energy like 43858 , 44371, 44088 etc. the average of which can be taken as the activation energy for the reaction .

Thus activation energy = 44105 j = 44.1 kJ /mol

Using the same expression, using the value of Ea already calculated, we can calculate the k at 300K.

log (2.14x 10-5/ k ) = 44105/8.314[1/300 -1/658]

Solving for k we get k = 2.49 x 10-12 M/s

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