Concept explainers
A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases.
Interpretation:
The partial pressures of the given gases have to be calculated.
Concept Introduction:
A mole fraction is the unit less proportion of the number of moles of a mixture constituent and the total number of moles in the mixture.
The number of molecules of gases is known. Since the mole fraction is:
- In a mixture of gases, every gas has an incomplete pressure which is the theoretical stress of that gas if it alone engaged the entire volume of the original combination at the same temperature.
- The sum pressure of an ideal gas mixture is the amount of the partial pressures of the gases in the mixture.
Answer to Problem 5.67QP
The partial pressure of
The partial pressure of
The partial pressure of
Explanation of Solution
First, we calculate the mole fraction Methane from the mixture. Then, we can calculate the partial pressure of each component.
The number of moles of the combined gases is:
The partial pressure of
The partial pressure of
Second, we calculate the mole fraction Ethane from the mixture. Then, we can calculate the partial pressure of each component.
The partial pressure of
The partial pressure of
Third, we calculate the mole fraction Propane from the mixture. Then, we can calculate the partial pressure of each component.
The partial pressure of
The partial pressure of
The partial pressures of the given gases were calculated.
Want to see more full solutions like this?
Chapter 5 Solutions
CHEMISTRY LOOSELEAF WITH ALEKS>IC<
- A mixture at 33 °C contains H2at 325 torr. N;at 475 tore and O2at 650. torr. What is the total pressure of the gases in the system? Which gas contains the greatest number of moles?arrow_forwardA 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_forwardHydrogen gas is used in weather balloon because it is less expensive than Helium. Assume that 5.57 g of H2 is used to fill a weather balloon to an initial volume of 67 L at 1.04 atm. If the ballloon rises to an altitude where the pressure is 0.047 atm, what is its new volume? Assume that the temperature remains constant.arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781285199030Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning