Chemistry - Thermodynamics - II Question with Solution | TestHub

At $-1℃$, liquid water is supercooled and freezes spontaneously to form ice. During freezing, the entropy of the system decreases because ice is more ordered than liquid water. However, freezing is an exothermic process, so heat is released to the surroundings, causing the entropy of the surroundings to increase. According to the second law of thermodynamics, for a spontaneous process, $\Delta S_{universe}>0$. Therefore, the increase in entropy of the surroundings is greater than the decrease in entropy of the system.