A 7.00 L tank at 27.3 °C is filled with 16.4 g of sulfur hexafluoride gas and 15.7 g of sulfur tetrafluoride 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. sulfur hexafluoride sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm atm atm X S
A 7.00 L tank at 27.3 °C is filled with 16.4 g of sulfur hexafluoride gas and 15.7 g of sulfur tetrafluoride 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. sulfur hexafluoride sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm atm atm X S
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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The given data is as follows:
The mass of sulfur hexafluoride gas = 16.4 g
The mass of sulfur tetrafluoride gas = 15.7 g
Volume of tank = 7.00 L
The temperature =
Mole fraction, partial pressure of each gas and total pressure of tank = ?
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