Hw.91. At 1 atm, how much energy is required to heat 75.0 g H₂O(s) at-18.0 °C to H₂O(g) at 159.0 °C? Use the heat transfer constantsfound in this table.9=TextHeat-transfer constants for H₂O at 1 atmQuantityper gramEnthalpy of fusion at 0°C333.6 J/g2257 J/gEnthalpy of vaporization at 100°CSpecific heat of solid H₂O (ice)2.087 J/(g°C)*37.60 J/(mol-°C) *Specific heat of liquid H₂O (water)4.184 J/(g-°C)* 75.37 J/(mol-°C) *Specific heat of gaseous H₂O (steam) 2.000 J/(g°C)* 36.03 J/(mol-°C)per mole6010. J/mol40660 J/molkJ

Given data, Mass of H2O=75.0gInitial temperature of H2O=-18.0oCFinal temperature of H2O=159.0oC

Answered: At 1 atm, how much energy is required…

At 1 atm, how much energy is required to heat 75.0 g H₂O(s) at-18.0 °C to H₂O(g) at 159.0 °C? Use the heat transfer constants found in this table.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Hw.91.

At 1 atm, how much energy is required to heat 75.0 g H₂O(s) at-18.0 °C to H₂O(g) at 159.0 °C? Use the heat transfer constants
found in this table.
9=
Text
Heat-transfer constants for H₂O at 1 atm
Quantity
per gram
Enthalpy of fusion at 0°C
333.6 J/g
2257 J/g
Enthalpy of vaporization at 100°C
Specific heat of solid H₂O (ice)
2.087 J/(g°C)*37.60 J/(mol-°C) *
Specific heat of liquid H₂O (water)
4.184 J/(g-°C)* 75.37 J/(mol-°C) *
Specific heat of gaseous H₂O (steam) 2.000 J/(g°C)* 36.03 J/(mol-°C)
per mole
6010. J/mol
40660 J/mol
kJ

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