Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Chapter 10, Problem 32P
Helium condenses to a liquid at 4.224 K under atmospheric pressure and remains a liquid down to the absolute zero of temperature. (It is used as a coolant to reach very low temperatures.) The vapor pressure of liquid helium at 2.20 K is 0.05256 atm. Calculate the volume occupied by 1.000 mol helium vapor under these conditions and compare it with the volume of the same amount of helium at standard temperature and pressure.
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Helium condenses to a liquid at 4.224 K under atmospheric pressure and remains a liquid down to the absolute zero of temperature. (It is used as a coolant to reach very low temperatures.) The vapor pressure of liquidhelium at 2.20 K is 0.05256 atm. Calculate the volume occupied by 1.000 mol helium vapor under these conditions and compare it with the volume of the same amount of helium at standard temperature and pressure.
A sample of gas collected over water at 42 degrees Celsius occupies a volume of one liter. The wet gas has a pressure of 0.986 atm. The gas is dried and the dry gas occupies 1.04 L with a pressure of 1.00 atm at 90 degrees Celsius. Using this information, calculate the vapor pressure of water at 42 degrees Celsius.
Argon at a pressure of 1 atm condenses to a liquid at 87.4 K and
solidifies at 83.9 K. The vapor pressure of liquid argon is 0.912 atm at
86.5 K. Calculate the volume of 1.00 mol of Ar vapor under these
conditions and compare it with the volume of 1.00 mol of Ar at STP (0 °C,
1 atm).
Volume 1 mol vapor at 86.5 K:
Volume 1 mol gas at STP:
The volume of 1.00 mol gas at STP is
L
mol vapor at 86.5 K.
L
✓than the volume of 1.00
Chapter 10 Solutions
Principles of Modern Chemistry
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