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Problem 5i13 part c for reference, asks to determine which dissociation reaction is more thermodynamically stable, dichloride to chlorine vs difluorine to fluorine. I know that a reaction reaches its equilibrium constant so that its ratio of products to reactant is as stable as possible, but how can you tell between separate reactions which of the two is more stable?
A large equilibrium constant favors the products of dissociation, which means F2 would tend to split apart into two F and is therefore unstable. So, in comparison, Cl2 is more stable.
I haven't done the exact problem yet but if you know the equilibrium concentrations of dichloride and chlorine or difluorine and fluorine, the one with the higher equilibrium concentration is more stable because the reactions proceeds to the more stable molecules.
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