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. 0 chlorine pentafluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: atm 0 atm atm X

A 10.0 L tank at 28.7 °C is filled with 4.80 g of sulfur tetrafluoride gas and 13.4 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 in the tank. Be sure your answers have the correct number of significant digits. sulfur tetrafluoride chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: 1 atm 0 atm 10 X

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

What is the % by mass of water in your hydrated copper (Il) sulphate? Mass of just anhydrous compound = mass of anhydrous compound - mass of beaker and rod 108.34g - 106.87g = 1.47g %D %3D = original compound mass - anhydrous compound mass = 3.00g - 1.47g = 1.53g Mass of just water %D

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

A 8.00 L tank at 3.9 °C is filled with 17.0 g of sulfur tetrafluoride gas and 7.06 g of boron trifluoride 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 mole fraction ? sulfur tetrafluoride boron trifluoride

A 8.00 L tank at 8.88 °C is filled with 3.30 g of carbon dioxide gas and 13.9 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. mole fraction: carbon dioxide partial pressure: atm mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: atm APR ... ... 24 DII DD 80 F11 F10 F7 F8 F9 F6 F1 F4

O A 10.0 L tank at 2.36 °C is filled with 10.5 g of sulfur tetrafluoride gas and 17.4 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. mole fraction: sulfur tetrafluoride partial pressure: atm mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: atm Explanation Check 021McCraw.lEdeation Al Dinhte Resened Torms of Uce Pri MacBook A - F6

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