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If a given reaction has a rate constant of 2.0×103rnsrn-1rn, the activation energy is 15.0kj/mol. What rnis the value of the rate constant at 75°c?
Accepted Answer
The Arrhenius equation relates the rate constant to the activation energy and temperature:
k = A * e^(-Ea/RT)
where:
* k is the rate constant
* A is the pre-exponential factor
* Ea is the activation energy
* R is the gas constant (8.314 J/mol*K)
* T is the temperature in Kelvin
We can use this equation to solve for the rate constant at 75°C (348K):
k = 2.0×103
s
-1
* e^(-15.0kJ/mol / (8.314 J/mol*K * 348K))
k = 5.6×105
s
-1
Therefore, the value of the rate constant at 75°C is 5.6×105
s
-1
.
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