Problem: The rate constant of a reaction is measured at different temperatures. A plot of the natural log of the rate constant as a function of the inverse of the temperature (in kelvins) yields a straight line with a slope of -8500 K-1 . What is the activation energy (Ea) for the reaction?

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ln k=-EaR 1T + ln A  y  =     m    x  +   b

We are given the slope (m) = -8500 K-1. We shall compute activation energy (Ea) from this slope:

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Problem Details

The rate constant of a reaction is measured at different temperatures. A plot of the natural log of the rate constant as a function of the inverse of the temperature (in kelvins) yields a straight line with a slope of -8500 K-1 . What is the activation energy (Ea) for the reaction?

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Our tutors have indicated that to solve this problem you will need to apply the Arrhenius Equation concept. You can view video lessons to learn Arrhenius Equation. Or if you need more Arrhenius Equation practice, you can also practice Arrhenius Equation practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Bindell's class at UCF.