Problem: A certain reaction has an activation energy of 32.89 kJ/mol. At what Kelvin temperature will the reaction proceed 7.00 times faster than it did at 287 K?  

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A certain reaction has an activation energy of 32.89 kJ/mol. At what Kelvin temperature will the reaction proceed 7.00 times faster than it did at 287 K?  

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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 Dixon's class at UCF.