A 9.00 L tank at 4.22 °C is filled with 3.83 g of sulfur tetrafluoride gas and 7.58 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. mole fraction: sulfur tetrafluoride partial pressure: || atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm

A 9.00 L tank at 4.22 °C is filled with 3.83 g of sulfur tetrafluoride gas and 7.58 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. mole fraction: sulfur tetrafluoride partial pressure: || atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter6: The Gaseous State

Section: Chapter Questions

Problem 6.17QE

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