The discussion centers on the relationship between ΔG′° and equilibrium in exergonic reactions, specifically addressing whether the negative ΔG′° is the sole determinant of product favorability at equilibrium. It concludes that ΔG° and the equilibrium constant K are intrinsically linked through the equation ΔG° = -RT ln K, indicating that any changes to ΔG° will directly influence K and vice versa. The conversation emphasizes that one cannot attribute equilibrium to ΔG° while simultaneously considering other factors without creating confusion, as both concepts convey the same information.
PREREQUISITESBiochemists, students of biochemistry, and researchers interested in thermodynamics and reaction dynamics in biochemical processes.
thanks a lot !mjc123 said:Given the relation between ΔG° and equilibrium, ΔG° = -RT ln K, anything that affects ΔG° also affects K and vice versa. They both contain the same information. It makes no sense to talk about equilibrium being determined by ΔG° and "other factors". Either you can say that ΔG° fully determines K, with no other factors involved, or you can say that both ΔG° and K (which are just different ways of saying the same thing) are fully determined by the "other factors". You can't mix the explanations, in a way that suggests that there can be factors that affect K but not ΔG°, or vice versa.