A sketch of the free energy for a hypothetical chemical equilibrium is shown here. What part of the plot on the axis representing the relative quantities of reactants and products corresponds to a value of$\Delta$G that is greater than zero?

Question

Quizplus · Accepted Answer

According to the definition of free energy, a positive value of ∆G represents a non-spontaneous reaction. Therefore, a positive value of ∆G corresponds to a range where the reaction is not favorable, and the required energy input would be significant for the reaction to occur. Looking at the plot, the range of ∆G > 0 corresponds to the region from point c to point d, where the concentration of product is greater than the concentration of reactants. In this region, the reaction is not thermodynamically favored, and the equilibrium constant (K) for this reaction would be less than 1, indicating that the reaction in the forward direction is unfavorable.

A Sketch of the Free Energy for a Hypothetical Chemical Δ\DeltaΔ

A Sketch of the Free Energy for a Hypothetical Chemical $\Delta$