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A gas mixture contains 3.64 g of hydrogen, 48 g oxygen, 11.75 g helium, and an unknown amount of nitrogen in a 20794 in container at 116.54°F at 54328 Pa. Calculate the mass in grams of the nitrogen gas in the container. Atomic Mass: H: 1.008 g/mol 0: 15.999 g/mol He: 4.003 g/mol N: 14.007 g/mol

A gas mixture contains 3.64 g of hydrogen, 48 g oxygen, 11.75 g helium, and an unknown amount of nitrogen in a 20794 in container at 116.54°F at 54328 Pa. Calculate the mass in grams of the nitrogen gas in the container. Atomic Mass: H: 1.008 g/mol 0: 15.999 g/mol He: 4.003 g/mol N: 14.007 g/mol

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter6: The Gaseous State
Section: Chapter Questions
Problem 6.47QE
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Solve using dimensional analysis. Show the complete solution. Do not round off nonfinal answers.
A gas mixture contains 3.64 g of hydrogen, 48 g oxygen, 11.75 g helium, and an unknown amount of nitrogen in a 20794 in3 container at 116.54°F at 54328 Pa. Calculate the mass in grams of the nitrogen gas in the container. Atomic Mass: H: 1.008 g/mol 0: 15.999 g/mol He: 4.003 g/mol N: 14.007 g/mol
Transcribed Image Text:A gas mixture contains 3.64 g of hydrogen, 48 g oxygen, 11.75 g helium, and an unknown amount of nitrogen in a 20794 in3 container at 116.54°F at 54328 Pa. Calculate the mass in grams of the nitrogen gas in the container. Atomic Mass: H: 1.008 g/mol 0: 15.999 g/mol He: 4.003 g/mol N: 14.007 g/mol
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