Homework Help is Here – Start Your Trial Now!
Science
Chemistry
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
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...
See similar textbooks
icon
Related questions
Question
100%

will thumbs up thanks

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.

 

steps

Step by step

Solved in 4 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Mole Concept
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS