Energy can be removed from water as heat at and even below the normal freezing point (0.00 ?C at atmospheric pressure) without causing the water to freeze; the water is then said to be supercooled. Suppose a 1.70 g water drop is supercooled until its temperature is that of the surrounding air, which is at -7.93 ?C. The drop then suddenly and irreversibly freezes, transferring energy to the air as heat. What is the entropy change for the drop? The specific heat of ice is 2220 J/kg•K; the specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg.