Some N, gas is mixed with some 0, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 2.55 atm. key carbon hydrogen nitrogen sulfur охудen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas.

A 10.0 L tank at 18.9 °C is filled with 13.1 g of sulfur hexafluoride gas and 6.12 g of carbon monoxide 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 hexafluoride partial pressure: atm mole fraction: carbon monoxide partial pressure: I atm atm Total pressure in tank:

A 10.00 L tank at 12.8 °C is filled with 19.2 g of carbon dioxide gas and 15,7 g of dinitrogen monoxide 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. carbon dioxide dinitrogen monoxide mole fraction 0 0

A 9.00 L tank at 3.79 °C is filled with 8.94 g of sulfur tetrafluoride gas and 13.3 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. sulfur tetrafluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 0 atm atm atm X

A 7.00 L tank at 12.4 °C is filled with 19.4 g of sulfur tetrafluoride gas and 10.3 g of dinitrogen difluoride gas. You can assume both gases behar gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction sulfur tetrafluoride dinitrogen difluoride

A 9.00 L tank at 6.02 °C is filled with 8.81 g of sulfur hexafluoride gas and 10.5 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: sulfur hexafluoride partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm

A 5.00 L tank at 6.43 °C is filled with 3.89 g of sulfur hexafluoride gas and 10.7 g of sulfur tetrafluoride gas. You can assume both gases behave a 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 hexafluoride partial pressure: atm mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure in tank: atm

Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 0.150 kPa. gas N₂ 0₂ carbon nitrogen kPa oxygen mole fraction partial pressure kPa key Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. hydrogen x10 sulfur chlorine × Ś

A 6.00 L tank at 7.53 °C is filled with 5.91 g of sulfur hexafluoride gas and 7.97 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 hexafluoride partial pressure: ? atm mole fraction: boron trifluoride partial pressure: atm Total pressure in tank: atm