A 6.00 L tank at 11. °C is filled with 12.3 g of sulfur hexafluoride gas and 5.56 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. sulfur hexafluoride chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: atm atm atm X

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A 6.00 L tank at 11. °C is filled with 12.3 g of sulfur hexafluoride gas and 5.56 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.
sulfur hexafluoride
chlorine pentafluoride
mole fraction:
partial pressure:
mole fraction:
partial pressure:
Total pressure in tank:
0
atm
atm
atm
x10
X
S
Transcribed Image Text:A 6.00 L tank at 11. °C is filled with 12.3 g of sulfur hexafluoride gas and 5.56 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. sulfur hexafluoride chlorine pentafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 atm atm atm x10 X S
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