Good day!

I study hydrogenation reactions with organometallic catalyst. The software used is Orca.

If we calculate energy difference (see attached Figure with PES Scan final single point energy) or enthalpy change between 2 reactants and intermediate (~4 A), intermediate - reactants = -15 kJ/mol, so the intermediate is 15 kJ/mol lower on the figure. We understand this local minima at 4A as a stabilization of molecule with hydrogen bonds near the catalyst.

However, if we calculate Gibbs free energy change (which includes entropic contribution), the intermediate is 53 kJ/mol higher than reactants.

What energy difference we should consider if we want to speak about the energy barriers and rate-determining step (we compare multiple mechanisms)?

Reading the articles, I noticed the Gibbs free energy change is used everywhere. In my case, I'm embrassed by the fact that this hydrogen-bond formation is assisted with the big barrier 53 kJ/mol, and this reaction becomes the rate-determining step in the whole mechanism if we calculate Gibbs free energy energy barriers for all reactions.

Also, Orca (and me) usually watch total energy values from PES Scan to locate TS, and it is often useful. There is no TS for hydrogen bonding according to PES Scan (please, see Figure). How can it be: big Gibbs free energy barrier, and no TS? Please, shed some light on it.

Regards, Ivan.

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