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A 9.00 L tank at 12. °C is filled with 13.3 g of chlorine pentafluoride gas and 6.90 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. mole fraction: D.P

A 9.00 L tank at 12. °C is filled with 13.3 g of chlorine pentafluoride gas and 6.90 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. mole fraction: D.P

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter8: Properties Of Gases
Section8.4: Gas Density, Molar Mass, And The Ideal Gas Law
Problem 8.6PSP
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A 9.00 L tank at 12. °C is filled with 13.3 g of chlorine pentafluoride gas and 6.90 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. mole fraction: D.P
Transcribed Image Text:A 9.00 L tank at 12. °C is filled with 13.3 g of chlorine pentafluoride gas and 6.90 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. mole fraction: D.P
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