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At 0 °C 20 g of ice are added to 50 g of water at 30 °C in a vessel that has a water equivalent of 10 g. Calculate the entropy changes in the system and in the surroundings. The heat of fusion of ice at 0 °C is 6.02 kJ mol, and the specific heat capacities of water and ice may be taken as constant at 4.184 and 2.094JK -1 g, respectively, and independent of temperature.

At 0 °C 20 g of ice are added to 50 g of water at 30 °C in a vessel that has a water equivalent of 10 g. Calculate the entropy changes in the system and in the surroundings. The heat of fusion of ice at 0 °C is 6.02 kJ mol, and the specific heat capacities of water and ice may be taken as constant at 4.184 and 2.094JK -1 g, respectively, and independent of temperature.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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At 0 °C 20 g of ice are added to 50 g of water at 30 °C in a vessel that has a water equivalent of 10 g. Calculate the entropy changes in the system and in the surroundings. The heat of fusion of ice at 0 °C is 6.02 kJ mol, and the specific heat capacities of water and ice may be taken as constant at 4.184 and 2.094 J K -1 g, respectively, and independent of temperature.
Transcribed Image Text:At 0 °C 20 g of ice are added to 50 g of water at 30 °C in a vessel that has a water equivalent of 10 g. Calculate the entropy changes in the system and in the surroundings. The heat of fusion of ice at 0 °C is 6.02 kJ mol, and the specific heat capacities of water and ice may be taken as constant at 4.184 and 2.094 J K -1 g, respectively, and independent of temperature.
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