A container holds a mixture of N2(g) and O2(g). The total pressure is 3.35 atm. The temperature is 25.00 oC and the volume of the container is 17.1 L. If the mass of N2 in the container is 30.9 g, what is the partial pressure of O2 (in atm) in the container?

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 6.10QE
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A container holds a mixture of N2(g) and O2(g). The total pressure is 3.35 atm. The temperature is 25.00 oC and the volume of the container is 17.1 L. If the mass of N2 in the container is 30.9 g, what is the partial pressure of O2 (in atm) in the container? 

Expert Solution
Step 1: Determine the partial pressure of the oxygen gas from the given data:

Given,

total pressure of the gas mixture = 3.35 atm

volume of the container = 17.1 L

temperature = 25.00 oC

mass of N2 gas = 30.9 g.

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