Question

X5.6 Show that the entropy increase due to the mixing of two different ideal gases is $\Delta S_{mixing} = -R[x \ln x + (1 - x) \ln(1 - x)]$ where x is the fraction of one kind of molecule. Assume the total number of molecules is Avogadro's number. You may assume that gases A and B are initially on two sides of a partition, each occupying a volume proportional to its number of particles. Determine the entropy increase when the partition is removed.

          X5.6 Show that the entropy increase due to the mixing of two different ideal gases is
$\Delta S_{mixing} = -R[x \ln x + (1 - x) \ln(1 - x)]$
where x is the fraction of one kind of molecule. Assume the total number of molecules is
Avogadro's number. You may assume that gases A and B are initially on two sides of a
partition, each occupying a volume proportional to its number of particles. Determine the
entropy increase when the partition is removed.

$X5.6 Show that the entropy increase due to the mixing of two different ideal gases is Δ Smixing = -R[x ln x + (1 - x) ln(1 - x)] where x is the fraction of one kind of molecule. Assume the total number of molecules is Avogadro's number. You may assume that gases A and B are initially on two sides of a partition, each occupying a volume proportional to its number of particles. Determine the entropy increase when the partition is removed.$

Added by Victor C.

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