A 9.00 L tank at 12.6 °C is filled with 7.50 g of carbon dioxide gas and 13.2 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: carbon dioxide partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm

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A 9.00 L tank at 12.6 °C is filled with 7.50 g of carbon dioxide gas and 13.2 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:
x10
carbon dioxide
partial pressure:
|| atm
?
mole fraction:
dinitrogen difluoride
partial pressure:
atm
Total pressure in tank:
|| atm
Transcribed Image Text:A 9.00 L tank at 12.6 °C is filled with 7.50 g of carbon dioxide gas and 13.2 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: x10 carbon dioxide partial pressure: || atm ? mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: || atm
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