A 5.00 L tank at 7.96 °C is filled with 10.8 g of chlorine pentafluoride gas and 4.88 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. olo mole fraction: chlorine pentafluoride partial pressure: ? atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm

A 10.0 L tank at 3.85 °C is filled with 10.3 g of sulfur hexafluoride gas and 6.25 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. mole fraction: x10 sulfur hexafluoride partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm

Calculating partial pressure in a gas mixture esc 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 R Explanation 2 mole fraction: W partial pressure: Total pressure in tank: 2 mole fraction: partial pressure: Check #3 8.0 E 54 https://azinsight.adsrvr.org/track/clk?imp=fbec12b0-713d-4127-929d-a59782e61fbb&ag=r735012&sfe=1788cd47&sig=PCK7icABpePPZol9wVL E9gKn0Pi6FOTr7R3rMUmfWw.&crid=2zvfx50b&cf=5773664&fq=0&t=2&tds-www.chegg.com&rca $ a F4 0 R atm 0 atm atm % 5 X FS T Ś < 6 s F6 Y & 7 F7 U 00 8 DIL FB 1 ( 9 DD ) O 0/5 Danasia V O F10 . P Fad d da delet

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