Consider the freezing of liquid water at -10°C.For this process what are the signs for $\Delta$H,$\Delta$S,and$\Delta$G?

Question

Quizplus · Accepted Answer

For freezing of liquid water at -10°C, the system releases heat (exothermic process) and the entropy of the system decreases (since liquid water has higher entropy than solid ice). Therefore, we have:
F1F1F1S1F1F1F10H = -
F1F1F1S1F1F1F10S = -
F1F1F1S1F1F1F10G = - -
Thus, the correct choice is E (- - -).

Consider the Freezing of Liquid Water at -10°C Δ\DeltaΔ H Δ\DeltaΔ S,and Δ\DeltaΔ

Consider the Freezing of Liquid Water at -10°C $\Delta$ H $\Delta$ S,and $\Delta$