A mixture of 1773 g of water and 227 g of ice is in an initial equilibrium state at 0.000°C. The mixture is then, in a reversible process, brought to a second equilibrium state where the water- ice ratio, by mass, is 1.00 1.00 at 0.000°C. (a) Calculate the entropy change of the system during this process. (The heat of fusion for water is 333 kJ/kg.) (b) The system is then returned to the initial equilibrium state in an irreversible process (say, by using a Bunsen burner). Calculate the entropy change of the system during this process. (c) Are your answers consistent with the second law of thermodynamics?
A mixture of 1773 g of water and 227 g of ice is in an initial equilibrium state at 0.000°C. The mixture is then, in a reversible process, brought to a second equilibrium state where the water- ice ratio, by mass, is 1.00 1.00 at 0.000°C. (a) Calculate the entropy change of the system during this process. (The heat of fusion for water is 333 kJ/kg.) (b) The system is then returned to the initial equilibrium state in an irreversible process (say, by using a Bunsen burner). Calculate the entropy change of the system during this process. (c) Are your answers consistent with the second law of thermodynamics?
Elements Of Electromagnetics
7th Edition
ISBN:9780190698614
Author:Sadiku, Matthew N. O.
Publisher:Sadiku, Matthew N. O.
ChapterMA: Math Assessment
Section: Chapter Questions
Problem 1.1MA
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Transcribed Image Text:A mixture of 1773 g of water and 227 g of ice is in an initial
equilibrium state at 0.000°C. The mixture is then, in a reversible
process, brought to a second equilibrium state where the water-
ice ratio, by mass, is 1.00 1.00 at 0.000°C. (a) Calculate the
entropy change of the system during this process. (The heat of
fusion for water is 333 kJ/kg.) (b) The system is then returned to
the initial equilibrium state in an irreversible process (say, by
using a Bunsen burner). Calculate the entropy change of the
system during this process. (c) Are your answers consistent with
the second law of thermodynamics?
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