Thermal Equilibrium: Calculating Pressure of Helium Gas in 3.11L Container

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SUMMARY

The discussion focuses on calculating the pressure of helium gas in a 3.11-liter container after vaporizing from liquid form. The initial volume of liquid helium is 0.87 liters, and the laboratory temperature is set at 24.8°C. Participants confirm the use of the Ideal Gas Law (PV = nRT) for the calculation, emphasizing the need to determine the mass of helium and convert it to moles using its atomic mass. The density of liquid helium is noted as 122.1 kg/m³, which is crucial for calculating the mass.

PREREQUISITES
  • Understanding of the Ideal Gas Law (PV = nRT)
  • Knowledge of converting mass to moles using atomic mass
  • Familiarity with the properties of helium, including its density
  • Basic thermodynamics concepts related to thermal equilibrium
NEXT STEPS
  • Calculate the mass of helium using the density formula
  • Convert the mass of helium to moles using the atomic mass of helium
  • Apply the Ideal Gas Law to find the pressure of helium gas
  • Explore the effects of temperature changes on gas pressure in closed systems
USEFUL FOR

Students studying thermodynamics, chemistry enthusiasts, and anyone involved in gas law applications or laboratory experiments involving helium gas.

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Homework Statement



A sealed, evacuated 3.11 liter container initially contains 0.87 liter of liquid helium. As the contents of the container come into thermal equilibrium with the surroundings, the liquid helium vaporizes and turns into gas. If the temperature of the laboratory is 24.8°C, what is the pressure of the helium gas inside the container? (Note: The density of liquid helium is 122.1 kg/m3.)

Homework Equations



Truthfully I don't have any idea on how to set this up. Any help at all would be thankful.
Thanks

The Attempt at a Solution

 
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Figure first the mass of the helium in the container.

The total mass divided by the atomic mass will tell you how many moles of helium atoms you have inside.

At that point it's

PV = nRT isn't it?
http://en.wikipedia.org/wiki/Ideal_gas_law

You know T, you know V and you know n moles so ...
 
Yep that was it all along i was just missing a step and using the wrong constant. Thanks
 

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