A 6.00 L tank at 8.37 Cis filled with 11.3 g of boron trifluoride gas and 6.92 g of chlorine pentafiluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits. mole fraction: boron trifluoride partial pressure: 292 ata mole fraction: 0.241 chlorine pentafiuoride partial pressure: 0930 alm
A 6.00 L tank at 8.37 Cis filled with 11.3 g of boron trifluoride gas and 6.92 g of chlorine pentafiluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits. mole fraction: boron trifluoride partial pressure: 292 ata mole fraction: 0.241 chlorine pentafiuoride partial pressure: 0930 alm
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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![A 6.00 L tank at 8.37 C is filled with 11.3 g of boron trifluoride gas and 6,92 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 in the tank. Be sure your answers have the correct number of significant digits.
mole fraction:
boron trifluoride
partial pressure:
2.92 atm
mole fraction:
0.241
chlorine pentafluoride
partial presaure
0.930 alm](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F939c0031-fd61-489f-968a-312e01684f97%2F698069b2-b2fa-4b58-a9e2-2fbba06cdaaa%2Ff0bqbp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A 6.00 L tank at 8.37 C is filled with 11.3 g of boron trifluoride gas and 6,92 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 in the tank. Be sure your answers have the correct number of significant digits.
mole fraction:
boron trifluoride
partial pressure:
2.92 atm
mole fraction:
0.241
chlorine pentafluoride
partial presaure
0.930 alm
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