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 1100. torr. gas N₂ mole fraction U carbon nitrogen oxygen 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. partial pressure 0 torr torr key hydrogen x10 sulfur chlorine X

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

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 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

A 9.00 L tank at 14.3 °C is filled with 3.65 g of sulfur tetrafluoride gas and 3.18 g of carbon dioxide 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 tetrafluoride carbon dioxide mole fraction 0 X

A 9.00 L tank at 1.5 °C is filled with 3.22 g of carbon monoxide gas and 16.7 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. Be sure your answers have the correct number of significant digits. carbon monoxide chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: atm atm atm x10 × Ś 0:39 0 E

A 7.00 L tank at 25.5 °C is filled with 9.44 g of sulfur hexafluoride gas and 4.78 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: ab sulfur hexafluoride partial pressure: 5 ? atm mole fraction: sulfur tetrafluoride partial pressure: | atm n 11- 5 A... Total pressure in tank: O atm Explanation Check 2021 McGraw Hill LLC. All Rights Reserved. Terms of UseI Privacy Center Accessibility etv 25 424 14. $44 F10 80 11 F6 23 F4 esc F2 F3 1 & @ %23 $ 7 8. 2 T Y U W K

A 10.0L tank at 9.41°C is filled with 4.32g of carbon dioxide gas and 4.99g 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.   carbon dioxide mole fraction:     partial pressure: atm sulfur hexafluoride mole fraction:     partial pressure: atm Total pressure in tank: atm