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If the products of a certain reaction are favored (i.e., the Δ G value of the reaction is negative), one would expect a significant amount of product to form when the reactants are combined. Which of the choices could explain why such a reaction might produce very little product?

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Answer:

B. high Ea

The available choices are as below:

A. low Ea

B. high Ea

C. positive AH

D. negative AS

Explanation:

ΔG is a measure of how favorable a reaction is, it also relates to the equilibrium constant.  It is also the measure of spontaneity of a chemical reaction.

A reaction with a negative  ΔG, is very favorable.

A reaction with a positive  ΔG is not favorable.

A reaction with  ΔG = 0 is at equilibrium.

Now a molecule must acquire sufficient activation energy before they can react. However, the higher the activation energy, the slower the chemical reaction will be which leads to production of very little product.

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