A gas mixture contains 84 % nitrogen and 16 % oxygen. If the total pressure is 1.11 atm, what are the partial pressures of each component? Express your answers in atmospheres to two significant figures. Enter your answers numerically separated by a comma.

Sulfur hexafluoride gas is collected at 3.0 °C in an evacuated flask with a measured volume of 30.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.270 atm . Calculate the mass and number of moles of sulfur hexafluoride gas that were collected. Round your answer to 3 significant digits. mass: mole: mol

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 800. torr. gas N₂ 0₂ carbon nitrogen oxygen 0 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. mole fraction partial pressure torr key torr hydrogen x sulfur chlorine X S OL A

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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 10.0 L tank at 14.2 °C is filled with 19.3 g of sulfur hexafluoride gas and 3.57 g of dinitrogen 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. sulfur hexafluoride dinitrogen monoxide mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 8 atm atm atm D X

According to Dalton, the pressure exerted by a gas inside a container is proportional to the number of molecules of that gas.  If 4.00 x 1023 molecules of N2 and 2.00 x 1023 molecules of O2 are mixed in a container they exert a total pressure of 1686 torr.  What portion of that pressure (in torr units) is exerted by the N2?  Report answer to four significant figures in decimal notation. _____________________ torr,   What portion of that pressure (in torr units) is exerted by the O2?  Report answer to four significant figures in decimal notation. ____________________ torr

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