What is the total pressure and partial pressure of gases in a closed system?

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SUMMARY

The discussion centers on calculating the total pressure and partial pressures of hydrogen and helium gases in a closed system. Using the ideal gas law (PV=nRT) and Dalton's law of partial pressures, participants determined the moles of each gas and addressed the total pressure when the stopcock is opened. The total volume is the sum of the individual cylinder volumes, and the tube connecting the cylinders is neglected in these calculations.

PREREQUISITES
  • Understanding of the ideal gas law (PV=nRT)
  • Familiarity with Dalton's law of partial pressures
  • Basic knowledge of gas behavior at constant temperature
  • Ability to perform calculations involving moles and pressure
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  • Learn how to apply the ideal gas law in different scenarios
  • Study Dalton's law of partial pressures in multi-gas systems
  • Explore the effects of temperature changes on gas pressure
  • Investigate real gas behavior versus ideal gas assumptions
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Chemistry students, educators, and professionals involved in gas law applications, particularly those studying thermodynamics and gas behavior in closed systems.

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1. Assume that two cylinders at 27° C are connected by a closed stopcock(valve) system. The right-hand cylinder contains 2.4L of hydrogen at 0.600 atm; the left cylinder is larger and contains 6.8 L of helium at 1.40 atm.
a) How many moles of each gas are present?
b) What is the total pressure when the valve is open?
c) Determine the partial pressure of these two gases at 27° C when the stopcock is opened.




2. Homework Equations : PV=nRT and Dalton's partial pressure equation.



3. I got the moles of each gas for part a. For b and c, do I just add up the the individual volumes to get the total volume when the valve is opened? For some reason I'm just thinking that there is a tube connecting the two cylinders which would add additional volume. Thanks.
 
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Neglect the tube volume.
 

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