A 8.00 L tank at 9.38 °C is filled with 10.5 g of dinitrogen difluoride gas and 4.54 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. Be sure your answers have the correct number of significant digits. dinitrogen difluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 0 0 atm atm atm X

A 8.00 L tank at 19.1 °C is filled with 11.l g of dinitrogen difluoride gas and 17.4 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction dinitrogen difluoride chlorine pentafluoride

A 6.00 L tank at 18.3 °C is filled with 4.25 g of sulfur tetrafluoride gas and 7.37 g of boron trifluoride 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: boron trifluoride partial pressure: atm Total pressure in tank: atm O

A 10.0 L tank at 28.9 °C is filled with 7.97 g of sulfur tetrafluoride gas and 15.3 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: x10 sulfur tetrafluoride partial pressure: atm mole fraction: sulfur hexafluoride partial pressure: atm Total pressure in tank: atm

A 10.0 L tank at 3.85 °C is filled with 10.3 g of sulfur hexafluoride gas and 6.25 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. mole fraction: x10 sulfur hexafluoride partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm

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A 8.00 L tank at 18. °C is filled with 6.96 g of dinitrogen difluoride gas and 11.8 g of chlorine pentafluoride 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: Ox10 dinitrogen difluoride partial pressure: ? atm mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: atm

Calculating partial presso A 10.0 L tank at 7.7 °C is filled with 5.76 g of dinitrogen monoxide gas and 15.2 g of sulfur tetrafluoride 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. dinitrogen monoxide sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm 0 atm Dat atm M x10 X Ś 000 Ar F 8-

A 10.0 L tank at 13.5 °C is filled with 15.4 g of dinitrogen difluoride gas and 4.72 g of sulfur tetrafluoride 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 tetrafluoride partial pressure: || atm Total pressure in tank: atm