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60 L tank containing 2.5 mol of CH4 . Initially, when Poutside was 1 atm, there was no leakage. But the next day, when the atmospheric pressure dropped to 0.98 atm, the CH4 started to leak out. Assuming the temperature was the same on both days, how much (ideal) methane was left in the tank once the pressures equalized?

60 L tank containing 2.5 mol of CH4 . Initially, when Poutside was 1 atm, there was no leakage. But the next day, when the atmospheric pressure dropped to 0.98 atm, the CH4 started to leak out. Assuming the temperature was the same on both days, how much (ideal) methane was left in the tank once the pressures equalized?

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 6.133QE
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60 L tank containing 2.5 mol of CH4 . Initially, when Poutside was 1 atm, there was no leakage. But the next day, when the atmospheric pressure dropped to 0.98 atm, the CH4 started to leak out. Assuming the temperature was the same on both days, how much (ideal) methane was left in the tank once the pressures equalized?
Transcribed Image Text:60 L tank containing 2.5 mol of CH4 . Initially, when Poutside was 1 atm, there was no leakage. But the next day, when the atmospheric pressure dropped to 0.98 atm, the CH4 started to leak out. Assuming the temperature was the same on both days, how much (ideal) methane was left in the tank once the pressures equalized?
Expert Solution
Step 1

Given: Volume of tank = 60 L

Initial moles of CH4 = 2.5 mol.

Initial pressure of CH4 = 1.0 atm.

And final pressure of CH4 = 0.98 atm.

 

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