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It is possible, with care, to cool water below its freezing point without causing the water to freeze. This is referred to as supercooling. Suppose that you did this, and had 93.1 g of supercooled water at -6.12 oC (6.12 oC below the freezing point) in a perfectly insulated container.

Now suppose that the supercooled water suddenly and spontaneously changes to a mixture of ice and water (that is, it partially freezes). Assume a constant volume, a constant pressure of 1 atm, and no gain or loss of heat to or from the container. How much of the water freezes?
Specific Heat of water = 4.184 JK-1g-1
Heat of fusion of ice = 333 Jg-1

Find the mass of ice formed and the entropy change.

What I know of this problem is that heat is added to the water so -1.62 would become 0 degress as the system goes to equilibrium. also, this is a phase transition since some water is converted to ice, therefore heat is also removed. But I dont know How should I begin to solve this problem.