Reaction- 2-methyl-2-butene + H20 + H3O
When this reaction was run at room temperature (298 K) it was found that the major product made up 83% of the product distribution vs 17% of the minor product. If the temperature of the reaction was increased to 355K the same compound was the major product, but the product distribution had changed significantly (55% major product vs 45% minor product). Which of the following statements explains these results?
A. 2-methyl-2-butanol is the major product in both examples because it formed from the more stable tertiary carbocation
B. The difference in energies of the possible intermediate species accounts for the formation of major and minor products in this reaction
C. The energy of the reactants, products, and intermediates will not change at low or high temperature
D. Formation of the minor intermediate has the higher activation energy, so at the higher temperature a greater percentage of minor intermediates can be formed relative to the reaction at room temperature (Because more collisions now have sufficient energy). This leads to the formation of a greater percentage of minor product
E. At higher temperature the major product is less stable, so it will not form as readily
I have the answers I want the explanation behind these.
**For E also tell me if at higher temperatures the major INTERMEDIATES are less stable. Does temperature have any effect on stability at all??
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