10.0L tank at 1.21°C is filled with 9.54g of dinitrogen difluoride gas and 13.5g of chlorine pentafluoride 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. dinitrogen difluoride mole fraction: partial pressure: atm chlorine pentafluoride mole fraction: partial pressure: atm Total pressure in tank: atm
10.0L tank at 1.21°C is filled with 9.54g of dinitrogen difluoride gas and 13.5g of chlorine pentafluoride 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. dinitrogen difluoride mole fraction: partial pressure: atm chlorine pentafluoride mole fraction: partial pressure: atm Total pressure in tank: atm
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter1: Gases And The Zeroth Law Of Thermodynamics
Section: Chapter Questions
Problem 1.21E: Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He...
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A
tank at
is filled with
of dinitrogen difluoride gas and
of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions.
10.0L
1.21°C
9.54g
13.5g
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.
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|
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