The following questions are based on the reaction A B C D Assume that the reacti

Question

The following questions are based on the reaction A B C D Assume that the reaction has a ?G of-5.6 kcal/mol. Which of the following would be true? Select one: O a. The reaction could be coupled to power an exergonic reaction with a AG of +8.8 kcal/mol O b. The reaction could be coupled to power an endergonic reaction with a AG of +6.2 kcal/mol O C. The reaction would result in a decrease in entropy (9 and an increase in the total energy content (H) of the system O d. The reaction could be coupled to power an endergonic reaction with a AG of +3.4kcal/mol. e. The reaction would result in products (C+ D) with a greater free-energy content than in the initial reactants (A+B) O

Explanation / Answer

First of all, since delta G is negative, therefore, your reaction is exergonic and the reaction is also spontaneous. For spontaneous reactions there is always an increase in Entropy. Hence your option (c) is wrong.

Now, Since reaction is exergonic (spontaneous), therefore, energy of reactants will be higher than energy of products. Therefore, your option (e) is laso wrong.

Now, your option (a) is also wrong because all the exergonic reaction have negative deltaG.

Therefore, you are now left with option (b) and (d). Since the deltaG of the reaction is given as -5.6 kcal/mol hence it can only power an endergonic reaction of either the same or lower deltaG. Hence option (b) is also wrong.

Therefore, the right answer is option (d)

Thanks!

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