A 9.00 L tank at 4.62 °C is filled with 14.5 g of sulfur hexafluoride gas and 16.1 g of dinitrogen difluoride 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. sulfur hexafluoride dinitrogen difluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 0 atm atm atm 0x10 X 0 C
A 9.00 L tank at 4.62 °C is filled with 14.5 g of sulfur hexafluoride gas and 16.1 g of dinitrogen difluoride 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. sulfur hexafluoride dinitrogen difluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 0 atm atm atm 0x10 X 0 C
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter13: Gases
Section: Chapter Questions
Problem 106A
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![A 9.00 L tank at 4.62 °C is filled with 14.5 g of sulfur hexafluoride gas and 16.1 g of dinitrogen difluoride 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.
sulfur hexafluoride
dinitrogen difluoride
mole fraction:
partial pressure:
mole fraction:
partial pressure:
Total pressure in tank:
0
0
atm
atm
atm
x10
olo
18
Ar](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb8911fe5-ebf9-45d0-a907-59fcc6519a95%2Faba52ae7-ea69-4b65-bf34-7393dd5e7e00%2F2k0xj7h_processed.png&w=3840&q=75)
Transcribed Image Text:A 9.00 L tank at 4.62 °C is filled with 14.5 g of sulfur hexafluoride gas and 16.1 g of dinitrogen difluoride 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.
sulfur hexafluoride
dinitrogen difluoride
mole fraction:
partial pressure:
mole fraction:
partial pressure:
Total pressure in tank:
0
0
atm
atm
atm
x10
olo
18
Ar
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