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Sagot :
Answer: The activation energy, Ea, of the reaction is 89195 Joules
Explanation:
The effect of temperature on rate constant is given by Arrhenius equation:
[tex]ln \frac{k_{2}}{k_{1}} = \frac{-E_{a}}{R}[\frac{1}{T_{2}} - \frac{1}{T_{1}}][/tex]
where
[tex]k_2[/tex] = rate constant at temperature [tex]T_2[/tex]
[tex]k_1[/tex] = rate constant at temperature [tex]T_1[/tex]
[tex]E_a[/tex]= activation energy
R= gas constant
[tex]T[/tex] = temperature
[tex]ln \frac{17k_1}{k_{1}} = \frac{-E_{a}}{8.314}[\frac{1}{300} - \frac{1}{278}][/tex]
[tex]2.83=\frac{-E_{a}}{8.314}[\frac{1}{300} - \frac{1}{278}][/tex]
[tex]E_a=89195J[/tex]
The activation energy, Ea, of the reaction is 89195 Joules
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