Imagine a closed container filled with air.

There is some liquid substance on a bottle placed on the floor of the container.

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Let's heat the liquid until it starts to evaporate. Let's say 20% of the liquid evaporates.

Disregard any effect of pressure buildup in the container which would block the evaporation.

Note: the liquid we are considering generates a vapour that is denser than air, so a "cloud" of vapour would start forming at the bottom on the container, unable to rise. (unlike water vapor for example, which would be less dense than the surrounding air and would start to rise)

enter image description here

If it's not clear enough, imagine what happens when solid carbon dioxide (dry ice) sublimates:

enter image description here

Would this patch of saturated air block the evaporation of the rest 80% of liquid?

I am thinking that the liquid would be soon in contact only with saturated air and the evaporation would stop even though there would be still plenty of unsaturated air in the upper section of the container.

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    $\begingroup$ You think right. Of course, this situation won't be stable forever; diffusion will gradually mix everything. $\endgroup$ – Ivan Neretin Apr 1 '20 at 17:43
  • $\begingroup$ Entropy of molecules won't decrease, rather will increase (cuz, gravity as well as heat both will increase entropy). Thus, there's no question of settling down of vapours, they will diffuse, however might diffuse to within small height first. Continuous heat supply will help vapours to diffuse to higher heights.. $\endgroup$ – Zenix Apr 1 '20 at 18:45
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    $\begingroup$ SF6 happily mixes with air. $\endgroup$ – Jon Custer Apr 1 '20 at 19:33