A 8.00 L tank at 1.46 °C is filled with 3.49 g of chlorine pentafluoride gas and 5.73 g of carbon dioxide 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: chlorine pentafluoride partial pressure: atm mole fraction: carbon dioxide partial pressure: atm Total pressure in tank: atm Explanation Check 2021 McGraw-Hill Education, All Rights Reserved. Terms of Use Privacy Accessib

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A 8.00 L tank at 1.46 °C is filled with 3.49 g of chlorine pentafluoride gas and 5.73 g of carbon dioxide 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:
do
chlorine pentafluoride
partial pressure:
O atm
mole fraction:
carbon dioxide
partial pressure:
|atm
Total pressure in tank:
atm
Explanation
Check
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Transcribed Image Text:A 8.00 L tank at 1.46 °C is filled with 3.49 g of chlorine pentafluoride gas and 5.73 g of carbon dioxide 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: do chlorine pentafluoride partial pressure: O atm mole fraction: carbon dioxide partial pressure: |atm Total pressure in tank: atm Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy Accessibility > Activity Details You have viewed this topic Last Visited Feb 28, 2021 3:29 PM 888
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