I was checking my answers for a chem test and came across a solution for a problem where the ∆S was pos, ∆H was neg and ∆G was neg. I believed it was only favorable at low temps, as reactions with a negative ∆H and negative ∆S are spontaneous at low temperatures. I was incorrect and the reaction was favorable at higher temps like 90 C as well.
Is a reaction always favorable if the ∆G is negative (at all temps)? What about when the ∆S is positive? If it's not favorable in all situations, what temps would cause it to be favorable? What role does ∆H play in determining the favorability of a reaction?
PLS HELP I WILL GIVE 30 POINTS AND NAME BRAINLIEST
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