A 9.00 L tank at 24.9 °C is filled with 10.2 g of dinitrogen difluoride gas and 16.0 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

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A 9.00 L tank at 24.9 °C is filled with 10.2 g of dinitrogen difluoride gas and 16.0 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:
do
dinitrogen difluoride
O atm
?-
partial pressure:
Ar
mole fraction:
sulfur hexafluoride
partial pressure:
O atm
Total pressure in tank:
O atm
ST
Explanation
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Transcribed Image Text:A 9.00 L tank at 24.9 °C is filled with 10.2 g of dinitrogen difluoride gas and 16.0 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: do dinitrogen difluoride O atm ?- partial pressure: Ar mole fraction: sulfur hexafluoride partial pressure: O atm Total pressure in tank: O atm ST Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy I Accessibility MacBook Air 888 DD 4) esc F6 F7 F10 F11 F3 F4 F5 FB F9 @ %23 2$ % & 1 4 5 6. 7. 8 6. %3D delete Q W R Y A S D H J K ck .... L. C9
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