How much heat energy is required to convert 76.9 g of solid ethanol at –114.5 °C to gasesous ethanol at 150.7 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of –114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45J/g · °C, and that of gaseous ethanol is 1.43J/g · °C. 137.5 q = kJ Incorrect

How much heat energy is required to convert 76.9 g of solid ethanol at –114.5 °C to gasesous ethanol at 150.7 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of –114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45J/g · °C, and that of gaseous ethanol is 1.43J/g · °C. 137.5 q = kJ Incorrect

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 97E: The molar heat of fusion of sodium metal is 2.60 kJ/mol, whereas its heat of vaporization is 97.0...

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The molar heat of fusion of sodium metal is 2.60 kJ/mol, whereas its heat of vaporization is 97.0 kJ/mol. a. Why is the heat of vaporization so much larger than the heat of fusion? b. What quantity of heat would be needed to melt 1.00 g sodium at its normal melting point? c. What quantity of heat would be needed to vaporize 1.00 g sodium at its normal boiling point? d. What quantity of heat would be evolved if 1.00 g sodium vapor condensed at its normal boiling point?
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