A 10.0 L tank at 12.5 °C is filled with 3.91 g of sulfur tetrafluoride gas and 6.79 g of dinitrogen monoxide 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: dinitrogen monoxide partial pressure: atm Total pressure in tank: atm

A 10.0 L tank at 12.5 °C is filled with 3.91 g of sulfur tetrafluoride gas and 6.79 g of dinitrogen monoxide 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: dinitrogen monoxide partial pressure: atm Total pressure in tank: atm

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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Exhaled air contains 74.5% N2, 15.7% O2, 3.6% CO2, and 6.2% H2O (mole percent). (a) Calculate the molar mass of exhaled air. (b) Calculate the density of exhaled air at 37C and 757 mm Hg and compare the value you obtained with that of ordinary air (MM=29.0g/mol) under the same conditions.
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