Solve Chemistry Gas Problem: Pressure in System When Stopcocks Open

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The discussion revolves around calculating the total pressure in a system of three gas bulbs when the stopcocks are opened, using Dalton's Law of Partial Pressures. The initial pressures and volumes of CO2, H2, and Ar are provided, with the user attempting to sum the pressures directly. However, the correct approach requires considering the combined volumes of the gases, leading to a recalculation using the formula P1V1 = P2V2. The user is uncertain about the total volume of the system, which is crucial for determining the final pressure. Ultimately, understanding the relationship between pressure, volume, and the number of moles of gas is essential for solving the problem accurately.
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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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