Answer : The value of activation energy for this reaction is 108.318 kJ/mol
Explanation :
The Arrhenius equation is written as:
[tex]K=A\times e^{\frac{-Ea}{RT}}[/tex]
Taking logarithm on both the sides, we get:
[tex]\ln k=-\frac{Ea}{RT}+\ln A[/tex] ............(1)
where,
k = rate constant = [tex]2.95\times 10^{-3}L/mol.s[/tex]
Ea = activation energy = ?
T = temperature = 435 K
R = gas constant = 8.314 J/K.mole
A = pre-exponential factor = [tex]3.00\times 10^{+10}L/mol.s[/tex]
Now we have to calculate the value of rate constant by putting the given values in equation 1, we get:
[tex]\ln (2.95\times 10^{-3}L/mol.s)=-\frac{Ea}{8.314J/K.mol\times 435K}+\ln (3.00\times 10^{10}L/mol.s)[/tex]
[tex]Ea=108318.365J/mol=108.318kJ/mol[/tex]
Therefore, the value of activation energy for this reaction is 108.318 kJ/mol
