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 $\Delta$G^$\circ$ = 0 is 1." D)"$\Delta$G^$\circ$ = $\Delta$H^$\circ$-T$\Delta$S^$\circ$"

Question

Quizplus · Accepted Answer

The statement "The products of an exergonic reaction have a higher Gibbs free energy than the reactants" is not true. In fact, exergonic reactions release energy and therefore have products with lower Gibbs free energy than the reactants.

Which of the Following Statements Is Not True? A)"The Position Δ\DeltaΔ

Which of the Following Statements Is Not True?
A)"The Position $\Delta$