A 8.00 L tank at 3.04 °C is filled with 7.02 g of sulfur tetrafluoride gas and 5.96 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. Round each of your answers to 3 significant digits. mole fraction: sulfur tetrafluoride partial pressure: atm mole fraction: dinitrogen monoxide partial pressure: atm Total pressure in tank: atm O
A 8.00 L tank at 3.04 °C is filled with 7.02 g of sulfur tetrafluoride gas and 5.96 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. Round each of your answers to 3 significant digits. mole fraction: sulfur tetrafluoride partial pressure: atm mole fraction: dinitrogen monoxide partial pressure: atm Total pressure in tank: atm O
Chemistry by OpenStax (2015-05-04)
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter9: Gases
Section: Chapter Questions
Problem 101E: Under which of the following sets of conditions does a real gas behave most like an ideal gas, and...
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![A 8.00 L tank at 3.04 °C is filled with 7.02 g of sulfur tetrafluoride gas and 5.96 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. Round each of your answers to 3 significant digits.
mole fraction:
sulfur tetrafluoride
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%2F5542d9f0-74a7-4904-a970-ce3707be8ad6%2F959a0cb9-4a02-4651-b153-b6d14c038e3a%2Fdd6v6nj_processed.png&w=3840&q=75)
Transcribed Image Text:A 8.00 L tank at 3.04 °C is filled with 7.02 g of sulfur tetrafluoride gas and 5.96 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. Round each of your answers to 3 significant digits.
mole fraction:
sulfur tetrafluoride
partial pressure:
atm
mole fraction:
dinitrogen monoxide
partial pressure:
atm
Total pressure in tank:
atm
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