The rate constant of a chemical reaction is a temperature dependent quantity.
The relation between the rate constant and temperature is quantified by the Arrhenius equation.
We have the following data:
k1 = 4.6x10-2 s-1 at T1 = 0 oC
k2 = 8.1x10-2 s-1 20 °C
R = 8.314 J/mol/K
Ea = ?
A first-order reaction has rate constants of 4.6 x 10 -2 s-1 and 8.1 x 10-2 s-1 at 0°C and 20.°C, respectively. What is the value of the activation energy?
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