Gibbs Free Energy Question Regarding Favorable Processes

[Rita Tran 2B]

On page 41 of the course reader where the Gibbs free energy is used to calculate the boiling point, I am confused as to why (endothermic) "does not favor the forward process". How can you determine this? I thought that according to the Le Châtelier's principle, endothermic reactions favor the forward process.

So does this mean that always favors the forward process and always favors the reverse process? And that always favors the reverse process and favors the forward reaction? Or does it depend on each reaction?

[Chem_Mod]

delta G= delta H - T delta S. Since delta G is negative for spontaneous processes, this happens at lower temperatures when delta H is negative. In this case, it is just saying that enthalpy alone will not spontaneously push this reaction at the given temperature. It would require some heat.