Answer: The energy of activation for the chirping process is 283.911 kJ/mol
Explanation:
According to the Arrhenius equation,
[tex]K=A\times e^{\frac{-Ea}{RT}}[/tex]
The expression used with catalyst and without catalyst is,
[tex]\log (\frac{K_2}{K_1})=\frac{Ea}{2.303\times R}[\frac{1}{T_1}-\frac{1}{T_2}][/tex]
where,
[tex]K_2[/tex] = rate of reaction at [tex]28^0C[/tex] = 194/min
[tex]K_1[/tex] = rate of reaction at [tex]5^0C[/tex] = 47.6 /min
[tex]Ea[/tex] = activation energy
R = gas constant = 8.314 J/Kmol
tex]T_1[/tex] = initial temperature = [tex]5^oC=273+5=278K[/tex]
tex]T_1[/tex] = final temperature = [tex]28^oC=273+28=301K[/tex]
Now put all the given values in this formula, we get
[tex]\frac{194}{47.6}=\frac{E_a}{2.303\times 8.314}[\frac{1}{278}-\frac{1}{301}][/tex]
[tex]{E_a}=283911J/mol=283.911kJ/mol[/tex]
Thus the energy of activation for the chirping process is 283.911 kJ/mol
