This reaction has an activation energy of zero in the gas phase:
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Question

This reaction has an activation energy of zero in the gas phase:
CH3 + CH3¡C2H6
a. Would you expect the rate of this reaction to change very
much with temperature?

Accepted Answer

hey everyone in this example, we need to identify the relationship between the reaction rate and temperature. So we want to recall our formula where our rate constant K. Is equal to our frequency factor represented by a here, which is then multiplied by Euler number which is raised to our activation energy divided by r gas constant times the temperature. We can also interpret this equation by saying that we can take the L. N. Of the rate constant for a single reaction At different absolute temperatures. So we would therefore have to rate constants K. one And then that is going to be placed over K two. So just to be clear, these are the rate constants for a single reaction at two absolute, We can say two different absolute temperatures and now we can set this equal to our activation energy divided by r gas constant. R. Where now we're going to multiply by the inverse values of our initial temperature. T one Subtracted from the inverse value of our final temperature T. two. And so here it's clear that our rate constant K. Is directly related to temperature. And so we can say that therefore if we increase our rate constant or we can say if we increase our temperature, we would also increase our rate constant. So the answer here is that they have a direct relationship. So this would be our final answer. To complete this example. If you have any questions please leave them down below and I will see everyone in the next practice video

This reaction has an activation energy of zero in the gas phase: CH3 + CH3¡C2H6 a. Would you expect the rate of this reaction to change very much with temperature?

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