Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter12: Thermodynamic Processes And Thermochemistry
Section: Chapter Questions
Problem 15P
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Transcribed Image Text:d. How much energy is needed to boil 87.0 g H₂O(1) if its enthalpy of vaporization is 2257 J/g?
energy:
e. Going from the boling point of H₂O (100 °C) to 135.0 °C is a temperature change of 35.0 °C.
How much energy is needed to heat 87.0 g H₂O(g) by 35.0 °C if its specific heat is 2.000 J/(g° C)?
energy:
Transcribed Image Text:At 1 atm, how much energy is required to heat 87.0 g H₂O(s) at -18.0 °C to H₂O(g) at 135.0 °C?
STRATEGY:
1. Calculate the energy needed for each temperature change or phase change individually.
a. the energy needed to heat 87.0 g H₂O(s) from-18.0 °C to its melting point.
b. the energy needed to melt 87.0 g H₂O(s) at its melting point.
c. the energy needed to heat 87.0 g H₂O(1) from the melting point to the boiling point.
d. the energy needed to boil 87.0 g H₂O(1) at its boiling point.
e. the energy needed to heat 87.0 g H₂O(g) from the boiling point to 135.0 °C.
2. Sum the energies from each step and convert to kilojoules.
Step 1.
a. Going from -18.0 °C to the melting point of H₂O (0 °C) is a temperature change of 18.0 °C.
How much energy is needed to heat 87.0 g H₂O(s) by 18.0 °C if its specific heat is 2.087 J/(gx °C)?
energy:
b. How much energy is needed to melt 87.0 g H₂O(s) if its enthalpy of fusion is 333.6 J/g?
energy:
c. For H₂O, going from the melting point (0 °C) to the boiling point (100 °C) is a temperature change of 100 °C. How much
energy is needed to heat 87.0 g H₂O(1) by 100 °C if its specific heat is 4.184 J/(g -* C)?
energy:
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