A 9.00 L tank at 9.4 °C is filled with 10.7 g of dinitrogen monoxide gas and 13.1 g of carbon dioxide 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 dioxide mole fraction X

A 8.00 L tank at 3.9 °C is filled with 17.0 g of sulfur tetrafluoride gas and 7.06 g 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 ? sulfur tetrafluoride boron trifluoride

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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

Some N, gas is mixed with some O, gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 1100. torr, key carbon hydrogen nitrogen sulfur охудen chlorine Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 4 significant digits. You may assume each gas behaves as an ideal gas. gas mole fraction partial pressure N2 torr ? O2 torr

A 8.00 L tank at 21.1 °C is filled with 11.6 g of chlorine pentafluoride gas and 12.6 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: x10 chlorine pentafluoride partial pressure: ? atm mole fraction: sulfur tetrafluoride partial pressure: atm Total pressure in tank: atm

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 0,120 kPa. key carbon hydrogen nitrogen sulfur охудеn 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. gas mole fraction partial pressure N2 | kPa O2 kPa

A  7.00L  tank at  0.68°C  is filled with  7.59g  of boron trifluoride gas and  17.5g  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. Be sure your answers have the correct number of significant digits. boron trifluoride mole fraction:   partial pressure: atm chlorine pentafluoride mole fraction:   partial pressure: atm

A 10.00 L tank at -7.6 °C is filled with 5.09 g of chlorine pentafluoride gas and 16.3 g of dinitrogen difluoride 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 chlorine pentafluoride dinitrogen difluoride mole fraction 0 10 X S

Calculate the mole fraction and partial pressure of each gas as well as the total pressure in the tank using the information below.