An insulated Thermos contains 135 g of water at 86.7 °C. You put in a 13.9 g ice cube at 0.00 °C (273.15 K) 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? Number i Units

An insulated Thermos contains 135 g of water at 86.7 °C. You put in a 13.9 g ice cube at 0.00 °C (273.15 K) 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? Number i Units

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

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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