A 7.00 L tank at 3.16 °C is filled with 2.08 g of boron trifluoride gas and 6.38 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. moie fraction: boron trifluoride partial pressure atm mole fraction sulfur hexafuoride partial pressure: atm Total pressure in tank Latm

A 7.00 L tank at 3.16 °C is filled with 2.08 g of boron trifluoride gas and 6.38 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. moie fraction: boron trifluoride partial pressure atm mole fraction sulfur hexafuoride partial pressure: atm Total pressure in tank Latm

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

ChapterC: Mathematics For General Chemistry

Section: Chapter Questions

Problem 2P

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Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
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