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For superheated water at 112.4°C and 1.0 atm, solve for the enthalpy, entropy and free energy changes when 44.4g vaporizes at 1.00 atm and a) 100 °C   ΔH =  kJ ΔS =  J/K ΔG = 0 kJ b) 112.4°C ΔH =  kJ ΔS =  J/K ΔG =  kJ Hints: Superheated water is liquid water. Use the Chapter 2 data and appendix data tables and set up a thermodynamic cycle for part b.

For superheated water at 112.4°C and 1.0 atm, solve for the enthalpy, entropy and free energy changes when 44.4g vaporizes at 1.00 atm and a) 100 °C   ΔH =  kJ ΔS =  J/K ΔG = 0 kJ b) 112.4°C ΔH =  kJ ΔS =  J/K ΔG =  kJ Hints: Superheated water is liquid water. Use the Chapter 2 data and appendix data tables and set up a thermodynamic cycle for part b.

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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For superheated water at 112.4°C and 1.0 atm, solve for the enthalpy, entropy and free energy changes when 44.4g vaporizes at 1.00 atm and
a) 100 °C  
ΔH =  kJ
ΔS =  J/K
ΔG = 0 kJ
b) 112.4°C
ΔH =  kJ
ΔS =  J/K
ΔG =  kJ
Hints: Superheated water is liquid water. Use the Chapter 2 data and appendix data tables and set up a thermodynamic cycle for part b.  

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