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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 1.76 g water drop is supercooled until its temperature is that of the surrounding air, which is at -7.50 *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. Number Units V K C Hint J/K mol Save for Later Attempts: 0 of 1 used Submit Answer J / kg-K J/mol.K kJ/kg kg/mole /C or (Co) 4-1 Co/s J/K.S J/mol J/K.m