Which reaction is faster, one with ΔG^†=+45 kJ / mol or one with ΔG^†=+70 kJ / mol ?

Name: Problem 12, Chapter 6: Organic Chemistry
Uploaded: 2020-05-07T21:10:03-08:00
Duration: 1 min 55 s
Channel: Jil Modi
Description: Which reaction is faster, one with ΔG^†=+45 kJ / mol or one with ΔG^†=+70 kJ / mol ?

step 1 So in this question, we're asked to determine which reaction is faster, and we're given two acti

Which reaction is faster, one with ΔG^†=+45 kJ / mol or...

Key Concepts

Activation Energy

Activation energy is the minimum energy barrier that must be overcome for reactants to transform into products. A lower activation energy generally implies that more reactant molecules have sufficient energy to react, leading to a faster reaction rate.

Transition State Theory

Transition state theory connects the free energy of activation to the reaction rate. It postulates that the reaction rate depends on the population of molecules that reach the high-energy transition state; hence, a lower ?G‡ (free energy of activation) corresponds to a larger population of molecules in the transition state and results in a faster reaction.

Reaction Rate

Reaction rate is determined by how quickly a chemical reaction proceeds, which is strongly influenced by the activation energy. In general, reactions with lower activation energies, such as a ?G‡ of +45 kJ/mol compared to +70 kJ/mol, occur faster because more molecules can overcome the energy barrier at a given temperature.

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