How Do Gases Reach Equilibrium in Partitioned Containers?

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SUMMARY

The discussion centers on the equilibrium of gases in a partitioned container, specifically a box divided in a 3:1 volume ratio. The larger section contains 1000 molecules of Neon (Ne), while the smaller section has 100 molecules of Helium (He). At equilibrium, the mean number of Ne molecules in the larger partition is calculated to be 750, and in the smaller partition, it is 250. For He, the mean is 25 in the larger partition and 75 in the smaller partition, confirming the distribution aligns with the volume ratio.

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Homework Statement



A box is separated by a partition which divides its volume in the ratio 3:1. The larger portion of the box contains 1000 molecules of Neon gas, the smaller one contains 100 molecules of He gas. A small hole is made in the partition, and one waits until equilibrium is obtained.

Find the mean number of molecules of each type on either side of the partition.


Homework Equations



Basic statistical and probability concept.

The Attempt at a Solution



At equilibrium, maintaining the volume ratio

the mean number of molecules of Ne in bigger partition = 750
the mean number of molecules of Ne in smaller partition = 250
the mean number of molecules of He in bigger partition = 25
the mean number of molecules of He in smaller partition = 75

That is what i ended up with. Any comments or suggestions will be greatly appreciated.


Gilchrist
 
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hi gilchrist

Ne makes sense, but I wonder why 75% of HE is in the small box, I would have thought everything would be distributed evenly at equilibirum...
 
actually, you are right ! I typed the wrong information. My bad.

Thank you :)
 

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