A 9.00 L tank at 9.44 °C is filled with 5.94 g of boron trifluoride gas and 17.9 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: boron trifluoride partial pressure: atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm
A 9.00 L tank at 9.44 °C is filled with 5.94 g of boron trifluoride gas and 17.9 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: boron trifluoride partial pressure: atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter1: Gases And The Zeroth Law Of Thermodynamics
Section: Chapter Questions
Problem 1.21E: Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He...
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![Calculating partial pressure in a gas mixture
A 9.00 L tank at 9.44 °C is filled with 5.94 g of boron trifluoride gas and 17.9 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases
under these conditions.
Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
mole fraction:
boron trifluoride
partial pressure:
atm
mole fraction:
sulfur hexafluoride
partial pressure:
atm
Total pressure in tank:
atm](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F89d12a3e-fa9d-40d1-bbf3-8602c6a6217f%2F5aed45a5-400b-412d-a370-aa339de1037a%2Fh76pi88_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Calculating partial pressure in a gas mixture
A 9.00 L tank at 9.44 °C is filled with 5.94 g of boron trifluoride gas and 17.9 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases
under these conditions.
Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
mole fraction:
boron trifluoride
partial pressure:
atm
mole fraction:
sulfur hexafluoride
partial pressure:
atm
Total pressure in tank:
atm
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