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Given the following data, calculate ΔH and ΔS of the process when 2.3 mole of substance was heated from 0 °C to 50 °C.            ΔHfus = 23.7 kJ/mol; Tfus = 289.6 K; ΔHvap = 39.1 kJ/mol; Tvap = 360.0 K under 1 atm.            Cp(gas) = 63.4 J/mol·K; Cp(liq) = 139.7 J/mol·K; Cp(solid) = 86.6 J/mol·K

Given the following data, calculate ΔH and ΔS of the process when 2.3 mole of substance was heated from 0 °C to 50 °C.            ΔHfus = 23.7 kJ/mol; Tfus = 289.6 K; ΔHvap = 39.1 kJ/mol; Tvap = 360.0 K under 1 atm.            Cp(gas) = 63.4 J/mol·K; Cp(liq) = 139.7 J/mol·K; Cp(solid) = 86.6 J/mol·K

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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 Given the following data, calculate ΔH and ΔS of the process when 2.3 mole of substance was heated from 0 °C to 50 °C.

           ΔHfus = 23.7 kJ/mol; Tfus = 289.6 K; ΔHvap = 39.1 kJ/mol; Tvap = 360.0 K under 1 atm.

           Cp(gas) = 63.4 J/mol·K; Cp(liq) = 139.7 J/mol·K; Cp(solid) = 86.6 J/mol·K 

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