Energy can be removed from water as heat at and even below the normal freezing point (0.0oC at atmospheric pressure) without causing the water to freeze; the water is then said to be super cooled. Suppose a 1.00 g water drop is super cooled until its temperature is that of the surrounding air, which is at – 5.00oC. 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.