The question is incomplete; the complete question is;
The normal boiling point of acetic acid is 118.1°C. If a sample of the acetic acid is at 125.2°C, predict the
signs of ∆H, ∆S, and ∆G for the boiling process at this temperature.
A. ∆H > 0, ∆S > 0, ∆G < 0
B. ∆H > 0, ∆S > 0, ∆G > 0
C. ∆H > 0, ∆S < 0, ∆G < 0
D. ∆H < 0, ∆S > 0, ∆G > 0
E. ∆H < 0, ∆S < 0, ∆G > 0
Answer:
∆H > 0, ∆S > 0, ∆G < 0
Step-by-step explanation:
If we look at the question carefully, we will observe that it deals with a phase change from liquid to vapour phase.
Energy is required to break the intermolecular bonds in the liquid as it changes into vapour hence the process is endothermic, ∆H>0.
Also, the entropy of the vapour phase is greater than that of the liquid phase hence there is a positive change in entropy, ∆S>0.
Lastly, the process is spontaneous, hence the change in free energy ∆G is less than zero.