A 10.0 L tank at 8.37 °C is filled with 6.10 g of sulfur hexafluoride gas and 12.6 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. sulfur hexafluoride chlorine pentafluoride Explanation 2110 mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: Check O 00 O atm atm atm 0 x10 X © 2022 McGraw Hill LLC. All Rights Reserved Terms of Use | Privacy Center | Accessibility

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A 10.0 L tank at 8.37 °C is filled with 6.10 g of sulfur hexafluoride gas and 12.6 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.
sulfur hexafluoride
chlorine pentafluoride
Explanation
2110 E
mole fraction:
partial pressure:
Total pressure in tank:
mole fraction:
partial pressure:
Check
0
O
atm
atm
atm
0
x10
X
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Transcribed Image Text:A 10.0 L tank at 8.37 °C is filled with 6.10 g of sulfur hexafluoride gas and 12.6 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. sulfur hexafluoride chlorine pentafluoride Explanation 2110 E mole fraction: partial pressure: Total pressure in tank: mole fraction: partial pressure: Check 0 O atm atm atm 0 x10 X Ⓒ2022 McGraw Hill LLC. All Rights Reserved Terms of Use | Privacy Center | Accessibility
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