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Sagot :
The activation energy for this reaction is - 55.5 kJ/mol
Calculation,
Given data,
First temperature [tex]T_{1}[/tex] = 302°C = 302+273 = 575 K
Second temperature [tex]T_{2}[/tex] = 508°C = 508+273 = 781 K
rate constant at 302°C = 2. 45 × [tex]10^{-4}[/tex] lit/mol s
rate constant at 508°C = 0. 0965 lit/mol s.
Value of universal gas constant = 8.3145 J/k mol.
Apply Arrhenius equation,
㏒[tex]K_{1} /K_{2}[/tex] = [tex]E_{a}/2.203R[/tex] [1/ 575 K - 1/781 K]
㏒2. 45×[tex]10^{-4}[/tex] lit/mol s/0.0965 lit/mol s = [tex]E_{a}[/tex] /2.303×8.3145 J/k mol[781-575/575K×781 K]
[tex]E_{a}[/tex] = - 55.5 kJ/mol
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