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 -

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter1: Temperature And Heat

Section: Chapter Questions

Problem 80P: How many grams of coffee must evaporate from 350 g of coffee in a 100-g glass cup to cool the coffee...

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