A 7.00 L tank at 25.9 °C is filled with 7.99 g of sulfur hexafluoride gas and 4.45 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. sulfur hexafluoride dinitrogen monoxide mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm 0 atm atm

Part A: A 10.0L tank at 7.31°C is filled with 8.04g of dinitrogen difluoride gas and 4.11g 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 significant digits. dinitrogen difluoride mole fraction:     partial pressure:    atm carbon monoxide mole fraction:     partial pressure:    atm Total pressure in tank: atm         Part B: Four samples of the same unknown gas G are listed in the table below. Rank these samples in increasing order of ideality. That is, select 1 next to the sample of G that will behave least like an ideal gas, and select 4 next to the sample of G that will behave most like an ideal gas. sample pressure atm volume L temperature   °C How ideal the sample is:       A 15.0 6.0 −25.0 ▼(Choose one) B 10.0…

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Calculating partial presso A 10.0 L tank at 7.7 °C is filled with 5.76 g of dinitrogen monoxide gas and 15.2 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. Be sure your answers have the correct number of significant digits. dinitrogen monoxide sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm 0 atm Dat atm M x10 X Ś 000 Ar F 8-