I am studying the dehydrogenation of a cyclohexane ring containing $\ce{B-N}$ on the adjacent position. or simply we can think about $\ce{H3N-BH3}$. If we release one $\ce{H2}$ molecule from it then the Gibbs free energy and the enthalpy of dehydrogenation are negative (See Scheme 1 under Fig. 1 here: https://pubs.acs.org/doi/10.1021/ja9106622 ). If we calculate simple dehydrogenation energy for $\ce{H3N-BH3}$ then it is also negative.
Negative dehydrogenation energy means it's a spontaneous reaction and we do not need anything to release the $\ce{H2}$ molecule from the system. My concern is "How the system is stable in its pristine condition if its dehydrogenation enthalpy/energy is negative"?
Under the scheme 3rd of Fig. 1 in the above-mentioned paper. If we release $\ce{1H2}$ from the ring then the dehydrogenation energy is negative. I do not understand how I can explain this negative value of dehydrogenation energy.
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. Also, is your question about an completely experimental study, or is there a theoretical modelling somewhere? $\endgroup$