Principles of Physics 11th ISV Edition · Entropy and the Second Law of Thermodynamics · Problem 33
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Walker, Halliday & Resnick — Entropy and the Second Law of Thermodynamics: Problem 33
33 A mixture of 1773 g of water and 513 g of ice is in an initial equilibrium state at $0.000^\circ\text{C}$. 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 $0.000^\circ\text{C}$. (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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주어진 조건: 33 A, 1773 g, 513 g, , in, 333 kJ
구하는 것: (a) Calculate the entropy change of the system during this proce; (b) The system is then returned to the initial equilibrium state; (c) Are your answers consistent with the second law of thermodyn
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Principles of Physics · 11th ISV Edition
저자: Walker, Halliday & Resnick
출판사: Wiley
단원: Entropy and the Second Law of Thermodynamics