Which of the following sets of conditions is true for an exothermic reaction that is spontaneous at all temperatures?

Question

∆H < 0 , ∆S < 0 , ∆G < 0

∆H > 0 , ∆S < 0 , ∆G < 0

∆H < 0 , ∆S < 0 , ∆G > 0

∆H > 0 , ∆S < 0 , ∆G < 0

∆H < 0 , ∆S > 0 , ∆G < 0

Answer 1

∆H < 0 , ∆S > 0 , ∆G < 0

The is because ∆G = ∆H - T ∆S, therefore if ∆H is negative and ∆S is positive, ∆G will always be negative as -T∆S will always be negative.