Concept explainers
(a)
Interpretation:
A
When the real gas molecules occupy a relatively small volume and have large intermolecular attractions, the pressure of the two gases has to be compared.
Concept Introduction:
Ideal
The ideal gas equation is:
Where,
P is the pressure
V is the volume
T is the temperature
R is molar gas constant
n is the mole
(b)
Interpretation:
A
When the real gas molecules occupy a relatively large volume and have negligible intermolecular attractions, the pressure of the two gases has to be compared.
Concept Introduction:
Ideal Gas Law:
The ideal gas equation is:
Where,
P is the pressure
V is the volume
T is the temperature
R is molar gas constant
n is the mole
(c)
Interpretation:
A
When the real gas molecules occupy a relatively large volume and have large intermolecular attractions, the pressure of the two gases has to be compared.
Concept Introduction:
Ideal Gas Law:
The ideal gas equation is:
Where,
P is the pressure
V is the volume
T is the temperature
R is molar gas constant
n is the mole
Want to see the full answer?
Check out a sample textbook solutionChapter 5 Solutions
General Chemistry - Standalone book (MindTap Course List)
- A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O2, is then added so that the final volume of the balloon is 26 L with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is 21.5 C. (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of O2 in the balloon? (d) What is the mole fraction of each gas?arrow_forwardUnder which of the following sets of conditions does a real gas behave most like an ideal gas, and for which conditions is a real gas expected to deviate from ideal behavior? Explain. (a) high pressure, small volume (b) high temperature, low pressure (c) low temperature, high pressurearrow_forwardShown below are three containers of an ideal gas (A, B, and C), each equipped with a movable piston (assume that atmospheric pressure is 1.0 atm). a How do the pressures in these containers compare? b Are all the gases at the same temperature? If not, compare the temperatures. c If you cooled each of the containers in an ice-water bath to 0.0C, describe how the volumes and pressures of the gases in these containers would compare.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781285199023Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning