Which of the following statements is not true?
A) The position of the equilibrium for an exergonic reaction favors products
B) The products of an exergonic reaction have a higher Gibbs free energy than the reactants.
C) The equilibrium constant of a reaction for which ΔG° = 0 is 1.
D) ΔG° = ΔH° − TΔS°

Question

Quizplus · Accepted Answer

The products of an exergonic reaction have a lower Gibbs free energy than the reactants, not higher. This is what makes the reaction energetically favorable and allows it to proceed spontaneously.

Which of the Following Statements Is Not True