Organic Reaction Mechanisms

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Organic Reaction Mechanisms

Postby Lubna_Abdulmajeed_2A » Mon Mar 06, 2017 8:17 pm

In the introduction to Organic Chemistry book, on page 161, there is an equation that states the following:
G*=H*-TS* (standard gibbs free energy of activation = standard enthalpy of activation - temperature*standard entropy of activation) and below it, there is a statement that says in this case delta G* is always unfavorable, meaning positive. However, why are we considering the gibbs free energy of activation to be unfavorable? why cant it be favorable for the transition state?


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Joined: Fri Jul 15, 2016 3:00 am

Re: Organic Reaction Mechanisms

Postby kara_kremer_2N » Mon Mar 06, 2017 9:03 pm

If you look at a PEDD diagram(graph), the energy in the transition state is always higher than the reactants. This means that from the reactants to the transition state, G standard will always be positive and unfavorable. If this were not the case, the transition state would not be the transition state because the transition state is the peak of the energy barrier.

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