A 7.00L tank at 13.1°C is filled with 4.86g of chlorine pentafluoride gas and 10.0g 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

A 9.00 L tank at 26.5 °C is filled with 3.97 g of carbon monoxide gas and 7.00 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. carbon monoxide sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank 0 atm 0 0. alm atm 0.P X

A 6.00 L tank at 23.5 °C is filled with 3.75 g of sulfur hexafluoride gas and 4.79 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. Be sure your answers have the correct number of significant digits. 圖 mole fraction: Ox10 sulfur hexafluoride alo partial pressure: atm Ar mole fraction: boron trifluoride partial pressure: atm Total pressure in tank: atm O

A 7.00 L tank at 1.92 °C is filled with 4.71 g of sulfur hexafluoride gas and 8.17 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: db sulfur hexafluoride partial pressure: atm Ar mole fraction: dinitrogen difluoride atm partial pressure: atm Total pressure in tank:

A 5.00L tank at 26.5°C is filled with 3.64g of sulfur tetrafluoride gas and 12.6g 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.   sulfur tetrafluoride mole fraction:     partial pressure: atm sulfur hexafluoride mole fraction:     partial pressure: atm Total pressure in tank: atm

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A 9.00 L tank at 18.1 °C is filled with 3.17 g of dinitrogen monoxide gas and 8.90 g of carbon monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. gas dinitrogen monoxide carbon monoxide mole fraction

A 5.00 L tank at 7.96 °C is filled with 10.8 g of chlorine pentafluoride gas and 4.88 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. ol. mole fraction: x10 chlorine pentafluoride Ar ? partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm

A 5.00L tank at 0.1°C is filled with 19.4g of dinitrogen monoxide gas and 5.47g of boron trifluoride 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 monoxide   boron trifluoride

A 8.00L tank at 24.1°C is filled with 8.62g of boron trifluoride gas and 7.37g of sulfur tetrafluoride 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 boron trifluoride   sulfur tetrafluoride