Gibbs Free Energy and Thermodynamic Favorability
All of the following statements are true regarding the relationship between ∆G, ∆H, and ∆S except
A
The sign of ∆G can change depending on the temperature for certain ∆H and ∆S combinations.
B
A negative ∆H and a positive ∆S always result in a thermodynamically favored process.
C
A process is always thermodynamically favored if ∆H is positive and ∆S is negative.
D
∆G° = ∆H° - T∆S°, where T is the temperature in Kelvin.
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