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How is the rate of a reaction related to the stability of the intermediate? In other...

How is the rate of a reaction related to the stability of the intermediate? In other words, why does the free-radical bromination of 2-methylpropane proceed faster than the free-radical bromination of propane?

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Answer #1

Rate of reaction is directly proportional to the stability of intermediate formed.

In case of 2-methylpropane, intermediate formed is tertiary carbon with unpaired electron but in the case of propane, intermediate formed is secondary carbon with unpaired electron. Unpaired electroin is more stable on tertiarty carbon than on secondary carbon. This is the reason free-radical bromination of 2-methylpropane proceed faster than the free-radical bromination of propane

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