A 8.00 L tank at 7.77 °C is filled with 2.52 g of dinitrogen difluoride gas and 5.22 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. Round each of your answers to 3 significant digits. mole fraction: dinitrogen difluoride partial pressure: atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm
A 8.00 L tank at 7.77 °C is filled with 2.52 g of dinitrogen difluoride gas and 5.22 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. Round each of your answers to 3 significant digits. mole fraction: dinitrogen difluoride partial pressure: atm mole fraction: sulfur hexafluoride 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 5.92PAE
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