Problem: Suppose that a certain biologically important reaction is quite slow at physiological temperature (37 oC) in the absence of a catalyst.Assuming that the collision factor remains the same, by how much must an enzyme lower the activation energy of the reaction in order to achieve a 4×105-fold increase in the reaction rate?

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k = A·e-EaRTk = A·e-E8.314×310.15kcat = A·e-Ecat8.314×310.15


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Problem Details

Suppose that a certain biologically important reaction is quite slow at physiological temperature (37 oC) in the absence of a catalyst.

Assuming that the collision factor remains the same, by how much must an enzyme lower the activation energy of the reaction in order to achieve a 4×105-fold increase in the reaction rate?

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What scientific concept do you need to know in order to solve this problem?

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 Gilman's class at LSU.