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The decomposition of NO2 follows a second order rate equation. Data at different temperatures are as follows:
T (K) 592 603 627 651.5 656
k (cm3/gmol.sec) 522 755 1700 4020 5030
Compute the energy of activation Energy from the data. The reaction is 2NO2 à 2NO + O2
Activation energy is found from the Arrhenius' relation
k = ko e-E/RT
ln k vs. 1/T is a straight line with a slope of -E/R
where, E is the activation energy; and
R is the universal gas constant.
From the above data, the following graph is drawn, and the slope is = -13622
E/R = 13622
E = 13622 x 8314 = 113253.3 kJ/kmol
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