What is the ending pressure of the Helium gas?

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SUMMARY

The pressure exerted by helium gas when it evaporates from liquid at 4.2 K to a supercritical state at 30 K can be calculated using the ideal gas law. Given that the density of liquid helium at its boiling point is 0.125 g/cm³ and the volume occupied is 0.01065 L, the transition to a supercritical state allows for accurate pressure calculations. This process involves understanding the properties of helium gas and applying the ideal gas law effectively.

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If I know that liquid helium at 4.2 K (boiling point) occupies 0.01065 L, then how do I calculate the pressure exerted on the walls of its containers if the helium evaporates and warms up to 30 K?
 
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At 30K, Helium is supercritical (cannot be liquid in conventional sense) and follows ideal gas law quite well. Density of liquid helium at boiling point is 0.125g/cm³. That should be all you need to know to solve this problem.
 

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