Question: Liquid water can be cooled to a temperature of -10 C and stay a liquid. As it is below its freezing point it is thermodynamically unstable and will eventually turn into solid water. If you put 100 g of supercooled water at -10 C into an insulated thermos (adiabatic) it will eventually freeze into a mixture of solid ice and liquid water at 0 C. How much of the water is solid? What is the entropy change of the universe for this process? (Assume the heat capacities of solid and liquid water are independent of temperature.) I have to admit, I have very little clue as to where to even begin with this question. Normally, every time I ask a question, I like to have some answer or idea to let people know I at least thought about it, but I simply cannot decipher this problem. I tried working with absolute entropies of the water in solid and ice forms at 263 and 273 K, but I am getting nowhere. Any advice is appreciated.