A 9.00 L tank at 11.1 °C is filled with 14.5 g of dinitrogen difluoride gas and 13.4 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. mole fraction: dinitrogen difluoride partial pressure: atm mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: atm
A 9.00 L tank at 11.1 °C is filled with 14.5 g of dinitrogen difluoride gas and 13.4 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. mole fraction: dinitrogen difluoride partial pressure: atm mole fraction: chlorine pentafluoride partial pressure: atm Total pressure in tank: atm
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![A 9.00 L tank at 11.1 °C is filled with 14.5 g of dinitrogen difluoride gas and 13.4 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.
mole fraction:
|x10
dinitrogen difluoride
partial pressure:
||atm
?
mole fraction:
chlorine pentafluoride
partial pressure:
atm
Total pressure in tank:
atm](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F03fa78cd-6ce9-4582-bb7c-dbeac4c245c8%2F782365e0-49b2-42d0-9c3c-2ecee313e976%2Fk9wx83j_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A 9.00 L tank at 11.1 °C is filled with 14.5 g of dinitrogen difluoride gas and 13.4 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.
mole fraction:
|x10
dinitrogen difluoride
partial pressure:
||atm
?
mole fraction:
chlorine pentafluoride
partial pressure:
atm
Total pressure in tank:
atm
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