A 8.00 L tank at 2.81 °C is filled with 9.62 g of sulfur hexafluoride gas and 9.34 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 hexafluoride partial pressure: ? atm mole fraction: dinitrogen monoxide partial pressure: atm Total pressure in tank: atm
A 8.00 L tank at 2.81 °C is filled with 9.62 g of sulfur hexafluoride gas and 9.34 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 hexafluoride 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 5.61PAE: 61 As one step in its purification, nickel metal reacts with carbon monoxide to form a compound...
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![A 8.00 L tank at 2.81 °C is filled with 9.62 g of sulfur hexafluoride gas and 9.34 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:
x10
sulfur hexafluoride
partial pressure:
atm
mole fraction:
dinitrogen monoxide
partial pressure:
atm
Total pressure in tank:
atm](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4afcf4e4-9c59-4025-b729-963d9ceb8a18%2F44790360-13b7-4740-ab95-3396fca09e9b%2F3g1riy_processed.png&w=3840&q=75)
Transcribed Image Text:A 8.00 L tank at 2.81 °C is filled with 9.62 g of sulfur hexafluoride gas and 9.34 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:
x10
sulfur hexafluoride
partial pressure:
atm
mole fraction:
dinitrogen monoxide
partial pressure:
atm
Total pressure in tank:
atm
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