Question

Which of the following is true concerning exergonic reactions? (Select all that apply)

Group of answer choices

LaTeX: \Delta Δ G°’ is negative.

The reaction proceeds spontaneously.

Energy is released.

LaTeX: \Delta Δ G°’is positive.

The reaction does not proceed spontaneously.

Answer 1

Solution:

In exergonic reactions the  Δ G is negative and the reaction proceeds spontaneosly. A reaction cannot occur spontaneously if Δ G is positive. An input of free energy is required to drive such a reaction. These reactions are termed endergonic reactions. The criterion for the spontaneity of a reaction is Δ G, not Δ G ° . This point is important because reactions that are not spontaneous based on Δ G ° can be made spontaneous by adjusting the concentrations of reactants and products in a reaction.

eg; Generally bond breakages are considered as exergonic and bond formation as endergonic. Hydrolysis of acyl bond releases huge energy (spontaneous and Δ G is negative) is coupled to the formation of peptide bond (non-spontaneous and Δ G is positive) during protein synthesis.