A 6.00 L tank at 26. °C is filled with 11.1 g of boron trifluoride gas and 6.48 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. Be sure your answers have the correct number of significant digits. boron trifluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: atm atm atm X

A 6.00 L tank at 26. °C is filled with 11.1 g of boron trifluoride gas and 6.48 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. Be sure your answers have the correct number of significant digits. boron trifluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: atm atm atm X

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter5: Gases

Section: Chapter Questions

Problem 70QAP: Given that 1.00 mol of neon and 1.00 mol of hydrogen chloride gas are in separate containers at the...

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