Question

If a reaction has a very low activation energy, the products would be expected to form quickly at high temperatures. Select the reason why such a reaction might form products very slowly, or not at alla. negative delta G
b. lack of a catalyst
c. positive delta G

Answer 1

Answer: Option (c) is the correct answer.

Explanation:

It is known that when Gibb's free energy, that is, $\Delta G$ has a negative value then the reaction will be spontaneous and the formation of products is favored more rapidly.  

Activation energy is defined as the minimum amount of energy required to initiate a chemical reaction.

So, when reactants of a chemical reaction are unable to reach towards its activation energy then a catalyst is added to lower the activation energy barrier so the reaction can take place rapidly.

Since, the given reaction has low activation energy. Therefore, there is no need to add a catalyst.

And, when value of $\Delta G$ is positive then the reaction is spontaneous in nature and formation of products is less favored.

Thus, we can conclude that for the given situation positive delta G is the reason that a reaction might form products very slowly, or not at all.

Answer 2

Answer:

c

Explanation:

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