- #1
Eureka99
- 32
- 3
Hi everybody!
While I was studying the Pourbaix diagram of chlorine ( and its disproportionation), I got stuck in a conceptual problem about the potential E. The diagram, as I understood, it's supposed to represent the equilibrium between the various species, but knowing that at equilibrium the ΔG of the reaction is zero, E have to be zero as well. But I kinda feel that this concept isn't applicable to half-reactions (like this case, in which the equilibrium is between Cl- / Cl2 , Cl2/HClO and so on). If it's not applicable, then why is it so? And then, what does the equilibrium mean in this case?
Thanks in advance
While I was studying the Pourbaix diagram of chlorine ( and its disproportionation), I got stuck in a conceptual problem about the potential E. The diagram, as I understood, it's supposed to represent the equilibrium between the various species, but knowing that at equilibrium the ΔG of the reaction is zero, E have to be zero as well. But I kinda feel that this concept isn't applicable to half-reactions (like this case, in which the equilibrium is between Cl- / Cl2 , Cl2/HClO and so on). If it's not applicable, then why is it so? And then, what does the equilibrium mean in this case?
Thanks in advance