According with the Arrhenius equation the activation energy can be estimated determining the rate constant. Why often we see Arrhenius plots with the ln (reaction rate) as a funtion ln(1/T)?
Arrhenius plots is the ln (reaction rate) as a function of 1/T for the apparent activation energy
Eyring plot is the ln(rate/T) versus 1/T is for the apparent enthalpy of activation.
I'm always wondering, why the people ask the question and don't look at answers.
Thank you for your answer, Yurii V Geletii . Could you explain further why do you mention for Arrhenius plots the ln (reaction rate) instead the ln(rate constant)? I think that's where relies my doubt mainly.
Thank you in advance.
The reaction rate constant is the characteristic of an elementary reaction. A reaction proceeding through a complex mechanism may follow a simple reaction rate law. From this law, one can calculate the apparent reaction rate constant, k(ap), which can be plotted as the ln (k(ap)) as a function of 1/T to determine apparent Arrhenius activation energy. In numerous studies people determine the dependence of the rate as a function of temperature and plot ln (reaction rate) versus of 1/T. Thus calculated apparent activation energy does not make much sense, but often used in chemical engineering.
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