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Problem 2: A 100 g ice cube, initially at 0 C, is placed on a table in a room at 20 C. The ice cube melts, and the water eventually comes into thermal equilibrium with the room. Assume that the temperature of the room doesn't change during this process. (a) How much heat is absorbed by the ice cube in order to melt it? (The "latent heat" of ice is 333 J/g every gram of ice.) (b) What is the entropy change of the ice as it melts? (c) How much heat is absorbed by the water as it comes into thermal equilibrium with the room? (The specific heat of water is 4.2 J/g/ °C) - that is, 333 J are required to melt -

Problem 2: A 100 g ice cube, initially at 0 C, is placed on a table in a room at 20 C. The ice cube melts, and the water eventually comes into thermal equilibrium with the room. Assume that the temperature of the room doesn't change during this process. (a) How much heat is absorbed by the ice cube in order to melt it? (The "latent heat" of ice is 333 J/g every gram of ice.) (b) What is the entropy change of the ice as it melts? (c) How much heat is absorbed by the water as it comes into thermal equilibrium with the room? (The specific heat of water is 4.2 J/g/ °C) - that is, 333 J are required to melt -

College Physics
College Physics
11th Edition
ISBN:9781305952300
Author:Raymond A. Serway, Chris Vuille
Publisher:Raymond A. Serway, Chris Vuille
Chapter1: Units, Trigonometry. And Vectors
Section: Chapter Questions
Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...
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Problem 2: A 100 g ice cube, initially at 0 C, is placed on a table in a room at 20 C. The ice cube melts, and the water eventually comes into thermal equilibrium with the room. Assume that the temperature of the room doesn't change during this process. (a) How much heat is absorbed by the ice cube in order to melt it? (The "latent heat" of ice is 333 J/g every gram of ice.) (b) What is the entropy change of the ice as it melts? (c) How much heat is absorbed by the water as it comes into thermal equilibrium with the room? (The specific heat of water is 4.2 J/g/ °C) (d) What is the entropy change of the water as it comes to thermal equilibrium? (e) What is the entropy change of the room as it melts the ice then heats the water? (f) What is the total change in entropy of the universe during this process? Is it in accordance with the second law? Explain. that is, 333 J are required to melt -
Transcribed Image Text:Problem 2: A 100 g ice cube, initially at 0 C, is placed on a table in a room at 20 C. The ice cube melts, and the water eventually comes into thermal equilibrium with the room. Assume that the temperature of the room doesn't change during this process. (a) How much heat is absorbed by the ice cube in order to melt it? (The "latent heat" of ice is 333 J/g every gram of ice.) (b) What is the entropy change of the ice as it melts? (c) How much heat is absorbed by the water as it comes into thermal equilibrium with the room? (The specific heat of water is 4.2 J/g/ °C) (d) What is the entropy change of the water as it comes to thermal equilibrium? (e) What is the entropy change of the room as it melts the ice then heats the water? (f) What is the total change in entropy of the universe during this process? Is it in accordance with the second law? Explain. that is, 333 J are required to melt -
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