A 5.00 L tank at 29.4 °C is filled with 19.9 g of sulfur tetrafluoride gas and 4.02 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 sulfur tetrafluoride chlorine pentafluoride

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 7.00 L tank at 29.4 °C is filled with 2.63 g of sulfur hexafluoride gas and 12.9 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 sulfur hexafluoride boron trifluoride mole fraction 0 0 X 00- Ar

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

Calculating partial pressure in a gas mixture A 8.00 L tank at 9.28 °C is filled with 6.17 g of boron trifluoride gas and 3.74 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: 11 ☐ x10 boron trifluoride partial pressure: ☐ a atm X S mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: ☐ atm

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

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 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