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### Topic: Why does lower activation energy mean faster reaction, other things equal?  (Read 4971 times)

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#### sodium.dioxid

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##### Why does lower activation energy mean faster reaction, other things equal?
« on: May 10, 2012, 05:55:01 PM »
Note I said other things equal. Assume a temperature such that ALL the molecules have abundant energy, satisfying the energy requirements of either reaction (the one with lower activation energy and the one with higher activation energy).

#### ramboacid

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##### Re: Why does lower activation energy mean faster reaction, other things equal?
« Reply #1 on: May 10, 2012, 06:29:15 PM »
If all the molecules had sufficient energy to overcome the activation energy in both reactions, then theoretically there shouldn't be any difference if they have the same steric factors, molecular size, etc.

However, real reactions don't work that way, because there will never be a state in which absolutely all molecules will have sufficient energy. For gases, the proportion of molecules with sufficient energy to have a reaction can be found using the Maxwell-Boltzmann Distribution of Speeds:
http://en.wikipedia.org/wiki/Maxwellâ€“Boltzmann_distribution
Don't worry about the math - it's a little dense. See what you can make out from the graphs on that page though, keeping in mind that only the molecules with sufficient kinetic energy will participate in a reaction.
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#### fledarmus

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##### Re: Why does lower activation energy mean faster reaction, other things equal?
« Reply #2 on: May 10, 2012, 09:04:33 PM »
You are exactly right. If all molecules in a mixture have enough energy to react, then they all react. If the energy available for the molecules to react is far higher than the energy necessary for either pathway, then you do not see selectivity between the pathways. The reaction will be very fast, and you will see a mixture of products.

This is one reason why you control the temperature in a reaction. The idea is to give enough energy for the reaction pathway that you desire to take place at a reasonable rate, without giving so much energy that other, higher energy pathways become available.

One example where this is sometimes critical is in SN2 reactions. If you have two different functional groups that could both act as nucleophiles present on a molecule, it can be tricky getting the reaction selective for only one of the two functional groups to add. However, the stronger nucleophile will react faster (that reaction has a lower activation energy), and at lower temperatures you may see selectivity while at higher temperatures you see none.

This is also useful in selecting between the kinetic and the thermodynamic products of a reaction, but that is a whole new lecture.

#### sodium.dioxid

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##### Re: Why does lower activation energy mean faster reaction, other things equal?
« Reply #3 on: May 10, 2012, 11:18:57 PM »
Thank you both. I like the answers.