If the activation energy for a given compound is found to be 22.0 kJ/mol, with a frequency factor of 8.0 × 1010 s-1, what is the rate constant for this reaction at 298 K?
Given:
T= 298 K
A = 8.0*10^10 s-1
Ea = 22.0 KJ/mol
= 22000 J/mol
R = 8.314 J/mol.K
use:
K = A*e^(-Ea/RT)
= 8.0*10^10*e^(-22000/(8.314*298))
= 8.*10^10*e^(-8.8797)
= 8.0*10^10*1.392*10^-4
= 1.1*10^7 s-1
Answer: 1.1*10^7 s-1
If the activation energy for a given compound is found to be 22.0 kJ/mol, with a...
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