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From the data below, calculate the total heat (in J) needed to convert 30.00 g of ice at -7.00°C to liquid water at 0.400°C: AH° : 6.02 kJ/mol fus m.p. at 1 atm: 0.0°C C liquid: 4.184 J/g•°C Csolid: 2.09 J/g.°C J

From the data below, calculate the total heat (in J) needed to convert 30.00 g of ice at -7.00°C to liquid water at 0.400°C: AH° : 6.02 kJ/mol fus m.p. at 1 atm: 0.0°C C liquid: 4.184 J/g•°C Csolid: 2.09 J/g.°C J

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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From the data below, calculate the total heat (in J) needed to convert 30.00 g of ice at -7.00°C to liquid water at 0.400°C: m.p. at 1 atm: 0.0°C : 6.02 kJ/mol fus C liquid: 4.184 J/g.°C Csolid: 2.09 J/g-°C
Transcribed Image Text:From the data below, calculate the total heat (in J) needed to convert 30.00 g of ice at -7.00°C to liquid water at 0.400°C: m.p. at 1 atm: 0.0°C : 6.02 kJ/mol fus C liquid: 4.184 J/g.°C Csolid: 2.09 J/g-°C
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