with all due respect, I don't agree with your textbook's definition of "spontaneity"
as I already pointed out , there's an abundance of situations (i.e. "systems") where ΔG is negative, though nothing happens at all
consider a coal mine, air: this is a stable situation, has been so for hundreds of millions of years, though there's a huge negative ΔG
in fact, even your life depends on this "kinetic hindrance" , as the system "human being, air" is of negative ΔG , too.
btw.: reactions with a negative ΔG will be called "exergonic", those with a positive ΔG endergonic
I want to know of an example of a reaction for which ΔH<0 and ΔS>0, i.e., a reaction that is always spontaneous. In other words, a reaction for which ΔG<0, regardless of the value of T.
there is no such thing as a
complete independence of T , as I already pointed out earlier
however, talking of ambient temperatures, one of many examples that comes to mind where ΔH is negative, ΔS is positive over a broad temperature range would be the formation of Al
2O
3 from the elements :
4 Al + 3 O
2 2 Al
2O
3 ; ΔH
of −1669,8 kJ/mol , ΔS
of 52.3 J/molK
pls. also note, that this reaction by no means is spontaneous
regards
Ingo