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Hot water volume ,V1 = 100 mL Hot water initial temperature, T1 = 43. 0°c Final water volume, V2 = 125 mL Final water temperature, T2 = 15.0°C Molar heat of fusion (True value) = 6.01 kJ/mol SHOW COMPLETE CALCULATIONS / SOLUTIONS. FOLLOW THE SIGNIFICANT FIGURES CONVENTION AND SHOW UNITS FOR ALL QUAI Hot water mass g Total water mass g Melt water mass Hot water temperature change °C Melt water temperature change Heat lost by hot water Heat gained by melt water AHfus kJ/mol

Hot water volume ,V1 = 100 mL Hot water initial temperature, T1 = 43. 0°c Final water volume, V2 = 125 mL Final water temperature, T2 = 15.0°C Molar heat of fusion (True value) = 6.01 kJ/mol SHOW COMPLETE CALCULATIONS / SOLUTIONS. FOLLOW THE SIGNIFICANT FIGURES CONVENTION AND SHOW UNITS FOR ALL QUAI Hot water mass g Total water mass g Melt water mass Hot water temperature change °C Melt water temperature change Heat lost by hot water Heat gained by melt water AHfus kJ/mol

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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Calculations or Solution Hot water mass: m hot = V1.p43 or ( volume 1) (density at 43°C) Total water mass: m total = V2.p4 or ( volume 2 ) ( density at 4°C) Melt water mass: m melt = m total – m hot Hot water temperature change: AT hot = T2 - T1 Melt water temperature change: AT melt = T2 – 0.0 °C Heat lost by hot water: q hot = -[CP m hot · AT hot ] Heat gained by melt water: q melt = CP m melt · AT melt Heat absorbed by melting ice: q fusion = -(g hot + gmelt) wwww afusion Heat absorbed per mole: molar Haision molesmelt True value-Experimental value % difference from accepted value= x 100% true value
Transcribed Image Text:Calculations or Solution Hot water mass: m hot = V1.p43 or ( volume 1) (density at 43°C) Total water mass: m total = V2.p4 or ( volume 2 ) ( density at 4°C) Melt water mass: m melt = m total – m hot Hot water temperature change: AT hot = T2 - T1 Melt water temperature change: AT melt = T2 – 0.0 °C Heat lost by hot water: q hot = -[CP m hot · AT hot ] Heat gained by melt water: q melt = CP m melt · AT melt Heat absorbed by melting ice: q fusion = -(g hot + gmelt) wwww afusion Heat absorbed per mole: molar Haision molesmelt True value-Experimental value % difference from accepted value= x 100% true value
Hot water volume , V1 = 100 mL Hot water initial temperature, T1 = 43. O°C Final water volume, V2 = 125 mL Final water temperature, T2 = 15.0°c Molar heat of fusion (True value) = 6.01 kJ/mol SHOW COMPLETE CALCULATIONS / SOLUTIONS. FOLLOW THE SIGNIFICANT FIGURES CONVENTION AND SHOW UNITS FOR ALL QUAN Hot water mass g Total water mass Melt water mass Hot water temperature change |°C Melt water temperature change °C Heat lost by hot water Heat gained by melt water J AHfus kJ/mol
Transcribed Image Text:Hot water volume , V1 = 100 mL Hot water initial temperature, T1 = 43. O°C Final water volume, V2 = 125 mL Final water temperature, T2 = 15.0°c Molar heat of fusion (True value) = 6.01 kJ/mol SHOW COMPLETE CALCULATIONS / SOLUTIONS. FOLLOW THE SIGNIFICANT FIGURES CONVENTION AND SHOW UNITS FOR ALL QUAN Hot water mass g Total water mass Melt water mass Hot water temperature change |°C Melt water temperature change °C Heat lost by hot water Heat gained by melt water J AHfus kJ/mol
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