A 7.00 L tank at 29, °C is filled with 6.44 g of chlorine pentafluoride gas and 13.6 g of boron trifluoride 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. chlorine pentafluoride boron trifluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm 0 atm atm 0.0 X 5 dh Ar

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

Curved arrows are used to illustrate the flow of electrons. Using the provided resonance structures, draw the curved electron- pushing arrows to show the interconversion between resonance hybrid contributors. Be sure to account for all bond- breaking and bond-making steps. :S: •S: O Select to Add Arrows > KO KO

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 7.00 L tank at 27.5 °C is filled with 2.64 g of chlorine pentafluoride gas and 2.36 g of dinitrogen monoxide 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.

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 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 8.00 L tank at 24.8 °C is filled with 4.16 g of chlorine pentafluoride gas and 11.6 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. chlorine pentafluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0- 0 atm 0- atm X