A certain reaction has k = 8.79 x 10-4 s-1 at 373 K and k = 3.27 Ă— 10-3 s-1 at 401 K. What is the numerical value of the activation energy (in kJ/mol) for this reaction? give your answer to three sig figs do not include units or use scientific notation
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Step 1
The Arrhenius equation relates the rate constant (k) of a reaction to the temperature (T) and the activation energy (Ea). It is given by: k = A * e^(-Ea/RT) where: - k is the rate constant - A is the pre-exponential factor (also known as the frequency factor) - Show more…
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