An insulated Thermos contains 130 g of water at 84.5 ˚C. You put in a 7.00 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?
An insulated Thermos contains 130 g of water at 84.5 ˚C. You put in a 7.00 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?
Chapter4: The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 59P: Two hundred grams of water at 0 is brought into contact into thermal equilibrium successively with...
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An insulated Thermos contains 130 g of water at 84.5 ˚C. You put in a 7.00 g ice cube at 0.00 ˚C to form a system of ice + original water. The specific heat of liquid water is 4190 J/kg•K; and the heat of fusion of water is 333 kJ/kg. What is the net entropy change of the system from then until the system reaches the final (equilibrium) temperature?
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