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A reaction has a Gibbs free energy change (AG) of +5.3 kcal/mol. Indicate whether each of the following is true (T) or false (F): A. This reaction needs to be coupled to an exergonic reaction. [Select] B. This reaction is spontaneous. [Select]

A reaction has a Gibbs free energy change (AG) of +5.3 kcal/mol. Indicate whether each of the following is true (T) or false (F): A. This reaction needs to be coupled to an exergonic reaction. [Select] B. This reaction is spontaneous. [Select]

Biochemistry
Biochemistry
9th Edition
ISBN:9781319114671
Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.
Chapter1: Biochemistry: An Evolving Science
Section: Chapter Questions
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**Question:** A reaction has a Gibbs free energy change (ΔG) of +5.3 kcal/mol. Indicate whether each of the following is true (T) or false (F): A. This reaction needs to be coupled to an exergonic reaction. - [ Select ] B. This reaction is spontaneous. - [ Select ] **Explanation:** In thermodynamics, the Gibbs free energy change (ΔG) indicates the spontaneity of a reaction. A positive ΔG (+5.3 kcal/mol in this case) means the reaction is non-spontaneous under standard conditions and requires energy input. To make such a reaction occur, it often needs to be coupled to an exergonic reaction, which releases energy and has a negative ΔG. - Therefore, option A is true as this reaction requires coupling to proceed. - Option B is false because the reaction is not spontaneous with a positive ΔG.
Transcribed Image Text:**Question:** A reaction has a Gibbs free energy change (ΔG) of +5.3 kcal/mol. Indicate whether each of the following is true (T) or false (F): A. This reaction needs to be coupled to an exergonic reaction. - [ Select ] B. This reaction is spontaneous. - [ Select ] **Explanation:** In thermodynamics, the Gibbs free energy change (ΔG) indicates the spontaneity of a reaction. A positive ΔG (+5.3 kcal/mol in this case) means the reaction is non-spontaneous under standard conditions and requires energy input. To make such a reaction occur, it often needs to be coupled to an exergonic reaction, which releases energy and has a negative ΔG. - Therefore, option A is true as this reaction requires coupling to proceed. - Option B is false because the reaction is not spontaneous with a positive ΔG.
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