Answer:
0.023
Explanation:
The Arrhenius' equation states that:
[tex]k = A*e^{\frac{-Ea}{RT}[/tex]
Where k is the velocity constant of the reaction, A is the constant of the collisions, Ea is the activation energy (the energy necessary to the molecules have so the reaction will happen), R is the gas constant (8.314 J/molK) and T is the temperature.
This equation is derivated of:
k = pZf
Where
p=fraction of collisions that occur with reactant molecules properly oriented
f=fraction of collisions having energy greater than the activation energy
Z=frequency of collisions
Thus, p*Z = A, and
f = [tex]e^{\frac{-Ea}{RT} }[/tex]
So, if the energy of the molecules is 12.5 kJ/mol = 12500 J/mol, thus the fraction will be:
f = [tex]e^{\frac{-12500}{8.314*400} }[/tex]
f = 0.023
