Solve Chemistry Gas Problem: Pressure in System When Stopcocks Open

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SUMMARY

The discussion focuses on calculating the total pressure in a gas system with three bulbs containing CO2, H2, and Ar when stopcocks are opened. The pressures and volumes provided are CO2 at 2.13 atm (1.5 L), H2 at 0.861 atm (1.0 L), and Ar at 1.15 atm (2.0 L). The initial calculation using Dalton's Law of Partial Pressures (P1 + P2 + P3 = Ptotal) resulted in an incorrect total pressure of 1.414 atm, indicating a misunderstanding of the relationship between pressure and volume in the system.

PREREQUISITES
  • Understanding of Dalton's Law of Partial Pressures
  • Knowledge of gas laws, specifically the ideal gas law
  • Familiarity with concepts of pressure and volume in gas systems
  • Basic algebra for manipulating equations
NEXT STEPS
  • Review Dalton's Law of Partial Pressures and its applications
  • Study the ideal gas law and its implications for pressure and volume
  • Learn about the relationship between pressure, volume, and temperature in gas mixtures
  • Explore examples of gas calculations involving multiple components
USEFUL FOR

Chemistry students, educators, and anyone involved in gas law calculations or thermodynamics will benefit from this discussion.

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Homework Statement




The apparatus shown consists of three bulbs connected by stopcocks. What is the pressure inside the system when the stopcocks are opened? Assume that the lines connnecting the bulbs have zero volume and that the termperature remains constant.

FG09_18-14UN.JPG


CO_2 - Pressure : 2.13 atm , Volume = 1.5 L
H_2 : Pressure = 0.861 atm, Volume = 1.00 L
Ar : Pressure = 1.15 atm , volume = 2.00 L

Homework Equations



The equation i used was Daltons partial gas equation

P1 + p2 + p3 = ptotal

The Attempt at a Solution



so i just did 2.13 + 0.861 + 1.15

But the answer is 1.414 atm.

i dont' know what to do
 
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that would be too easy of course

hint: P1V1 = P2V2

what is V2 or V(total)?
 

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