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One mole of water is placed in surroundings at -3 °C, but at first it does not freeze (it remains as supercooled water). Suddenly it freezes. Calculate the entropy change in the system during the freezing, making use of the following data: C,(water)=75 3JK mol C, (ice)=37.7JK mol A,H(icewater)=6.02kJ mol at 0 °C The two Cp values can be assumed to be independent of temperature. Also, calculate the entropy change in the surroundings, and the net entropy change in the system and surroundings.

One mole of water is placed in surroundings at -3 °C, but at first it does not freeze (it remains as supercooled water). Suddenly it freezes. Calculate the entropy change in the system during the freezing, making use of the following data: C,(water)=75 3JK mol C, (ice)=37.7JK mol A,H(icewater)=6.02kJ mol at 0 °C The two Cp values can be assumed to be independent of temperature. Also, calculate the entropy change in the surroundings, and the net entropy change in the system and surroundings.

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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. One mole of water is placed in surroundings at -3 °C, but at first it does not freeze (it remains as supercooled water) Suddenly it freezes. Calculate the entropy change in the system during the freezing, making use of the following data: C (water)=753JK mol C, (ice)=37.7JK mol A,H(ice-water)=6.02kJ mol at 0 °C The two Cp values can be assumed to be independent of temperature. Also, calculate the entropy change in the surroundings, and the net entropy change in the system and surroundings.
Transcribed Image Text:. One mole of water is placed in surroundings at -3 °C, but at first it does not freeze (it remains as supercooled water) Suddenly it freezes. Calculate the entropy change in the system during the freezing, making use of the following data: C (water)=753JK mol C, (ice)=37.7JK mol A,H(ice-water)=6.02kJ mol at 0 °C The two Cp values can be assumed to be independent of temperature. Also, calculate the entropy change in the surroundings, and the net entropy change in the system and surroundings.
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