CHEMISTRY COMMUNITY

Is it true that when H and S are both negative that decreasing the temperature increases spontaneity? If so, could someone explain why this is the case? I know it has to do with the equation G=H-TS, but beyond the math, what is the explanation?

If both delta H and delta S are negative, the reaction is only spontaneous at low temperatures since the T delta S part of the equation will be overall positive. In order for a reaction to be spontaneous, then, the negative delta H needs to be of larger magnitude than the positive T delta S so that delta G is negative.

The chart we went over in lecture goes:
Delta S (+) and Delta H (-) means spontaneous at all temperatures
Delta S (+) and Delta H (+) means spontaneous at high temperatures
Delta S (-) and Delta H (-) means spontaneous at low temperatures
Delta S (-) and Delta H (+) means not spontaneous at any temperatures, however, the reverse process is spontaneous