The second law of thermodynamics is almost obviously false for chemical systems. Consider the (valid) argument that, if catalysts can shift chemical equilibrium, the second law would be violated:

https://www.boundless.com/chemistry/...lyst-447-3459/
"In the presence of a catalyst, both the forward and reverse reaction rates will speed up equally, thereby allowing the system to reach equilibrium faster. However, it is very important to keep in mind that the addition of a catalyst has no effect whatsoever on the final equilibrium position of the reaction. It simply gets it there faster. (...) To reiterate, catalysts do not affect the equilibrium state of a reaction. In the presence of a catalyst, the same amounts of reactants and products will be present at equilibrium as there would be in the uncatalyzed reaction. To state this in chemical terms, catalysts affect the kinetics, but not the thermodynamics, of a reaction. If the addition of catalysts could possibly alter the equilibrium state of the reaction, this would violate the second rule of thermodynamics...."

It is evident that, for the dissociation-association reaction

A - B + C,

a catalyst cannot speed up both the forward and reverse reaction rates equally, due to the entirely different forward and reverse catalytic mechanisms.. In the forward (dissociation) reaction, the catalyst should just meet and split A. In the reverse (association) reaction, the catalyst should first get together B and C, which, if the diffusion factor is predominant, could be highly improbable.

Catalysts do shift chemical equilibrium, in violation of the second law of thermodynamics.

I have started the same discussion (and it has developed in an interesting way) he

https://www.youtube.com/watch?v=aL_iNGh8CNo
Chemical Thermodynamics - Second Law / Entropy Review

Pentcho Valev