A 9.00 L tank at 2.08 °C is filled with 9.55 g of boron trifluoride gas and 14.3 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. boron trifluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm atm atm 0 x10 X S

A 9.00 L tank at 2.08 °C is filled with 9.55 g of boron trifluoride gas and 14.3 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. boron trifluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm atm atm 0 x10 X S

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5.93PAE: 93 The complete combustion of octane can be used as a model for the burning of gasoline:...

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