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a) Ethanol (C2H:OH) melts at -114°C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g.K and 2.3 JigK, respectively. Determine the heat required to convert 42.0 g of ethanol at 35 °C to the vapor phase at 78 °C.

a) Ethanol (C2H:OH) melts at -114°C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g.K and 2.3 JigK, respectively. Determine the heat required to convert 42.0 g of ethanol at 35 °C to the vapor phase at 78 °C.

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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a) Ethanol (C2H5OH) melts at -114°C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g.K and 2.3 J/gK, respectively. Determine the heat required to convert 42.0 g of ethanol at 35 °C to the vapor phase at 78 °C.
Transcribed Image Text:a) Ethanol (C2H5OH) melts at -114°C and boils at 78 °C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g.K and 2.3 J/gK, respectively. Determine the heat required to convert 42.0 g of ethanol at 35 °C to the vapor phase at 78 °C.
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