A 9.00 L tank at 28.9 °C is filled with 8.24 g of sulfur tetrafluoride gas and 5.83 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 tetrafluoride chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: atm atm atm x10

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 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 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 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

A 7.00 L tank at 5.4 °C is filled with 3.81 g of sulfur tetrafluoride gas and 11.1 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 tetrafluoride dinitrogen monoxide mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm atm atm ☐ x10 X

Please answer in 3 significant digits