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What fraction of collisions will have sufficient energy to react for a gas whose activation energy is 80kj/mol at 25°c
Accepted Answer
To calculate the fraction of collisions with sufficient energy, we can use the Arrhenius equation. However, we need the pre-exponential factor (A) for this calculation. Without it, we can't determine the exact fraction. The Arrhenius equation is:
k = A
exp(-Ea/RT)
where:
k is the rate constant
A is the pre-exponential factor
Ea is the activation energy (80 kJ/mol)
R is the ideal gas constant (8.314 J/mol
K)
T is the temperature (25°C = 298 K)
The exponential term, exp(-Ea/RT), represents the fraction of collisions with sufficient energy to overcome the activation energy barrier. Let me know if you have the pre-exponential factor (A) and I can calculate the fraction!
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