7.00 L tank at 4.79 °C is filled with 7.87 g of boron trifluoride gas and 12.6 g of sulfur hexafluoride gas. You can assume both gases behave as ideal ases under these conditions. alculate the mole fraction and partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits. boron trifluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: 0 || atm atm X ? 00 do A

A 9.00 L tank at 4.62 °C is filled with 14.5 g of sulfur hexafluoride gas and 16.1 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. Be sure your answers have the correct number of significant digits. sulfur hexafluoride dinitrogen difluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 atm atm atm x10 olo 18 Ar

A 8.00 L tank at 28.6 °C is filled with 11.1 g of sulfur hexafluoride gas and 6.50 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. Be sure your answers have the correct number of significant digits. sulfur hexafluoride carbon monoxide mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm atm atm x10 X Ś

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

A 6.00 L tank at 0.46 °C is filled with 7.03 g of dinitrogen difluoride gas and 3.38 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. do mole fraction: dinitrogen difluoride partial pressure: ||atm mole fraction: sulfur tetrafluoride partial pressure: O atm Total pressure in tank: O atm Explanati Check O2021 McGraw-Hill Education. All Rights Reserved. Terms of Use I PrivacyI Accessibility > Activity Details MacBook Air esc 888 DII DD F2 F3 4) F7 F8 F3 F10 11 %23 2$ % & 3 4. 5 6. 7. 8 6. dele O

A 9.00 L tank at 1.27 °C is filled with 15.1 g of sulfur tetrafluoride gas and 3.08 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. sulfur tetrafluoride carbon monoxide mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 atm atm atm Ix10 X

A 10.0 L tank at 19.1 °C is filled with 6.04 g of dinitrogen difluoride gas and 7.73 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. mole fraction: dinitrogen difluoride partial pressure: atm mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: | atm

A 10.0 L tank at 1.29 °C is filled with 3.89 g of carbon monoxide gas and 4.35 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. carbon monoxide dinitrogen monoxide mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: atm a atm Da atm ☐ x10 X

A 9.00 L tank at 5.86 °C is filled with 2.76 g of chlorine pentafluoride gas and 12.0 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. Be sure your answers have the correct number of significant digits. chlorine pentafluoride dinitrogen monoxide mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: ■ atm atm atm 0 *0 X

A 9.00 L tank at 7.61 °C is filled with 9.76 g of sulfur hexafluoride gas and 6.26 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. sulfur hexafluoride chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 1 atm atm atm