A 9.00 L tank at 5.93 °C is filled with 7.54 g of boron trifluoride gas and 17.1 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. Round each of your answers to 3 significant digits. mole fraction: boron trifluoride partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: I atm I Don't Know Submit O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center| Accessibility O Type here to search 34°F Cloudy 9:16 F 4/7/20 DELL

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Find the mole fraction and partial pressure of each gas, and the total pressure in the tank.
A 9.00 L tank at 5.93 °C is filled with 7.54 g of boron trifluoride gas and 17.1 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. Round each of your answers to 3 significant digits.
mole fraction:
boron trifluoride
partial pressure:
atm
mole fraction:
dinitrogen difluoride
partial pressure:
|atm
Total pressure in tank:
I atm
I Don't Know
Submit
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Transcribed Image Text:A 9.00 L tank at 5.93 °C is filled with 7.54 g of boron trifluoride gas and 17.1 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. Round each of your answers to 3 significant digits. mole fraction: boron trifluoride partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: |atm Total pressure in tank: I atm I Don't Know Submit O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility O Type here to search 34°F Cloudy ^ @ O O a ) 9:16 F 37 4/7/20 DELL F1 F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 F12 PrtScr Insert Delete PgUp Pg @ # $ & Num
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