The issue of dispersion
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Under certain pressure, a gas is used to remove a portion (saturated vapor) from the liquid of different substances; do the liquid molecules exist in the gas phase in molecular form, or in some other way? And if it exists in the form of gas-phase molecules, are the liquid molecules dispersed evenly or irregularly?
Does anyone know? If you do, please let me know!
…………The conditions specified in the question aren’t clear enough, I think… If only the liquid saturation vapor pressure is taken away, then it’s a gas! As for dispersion, the dispersion of gas within another gas – I don’t think I’ve heard whether it’s uniform or irregular… Given the mobility of gas molecules, if there are no strong interactions between the molecules, I believe they should be able to distribute evenly quite quickly. Of course, that’s another matter if you ask how long it takes for the vapor from a cup of water to spread evenly throughout an 80-square-meter room. It is recommended that you specify all the conditions for what you want to process, from input to output. Gas velocity, liquid area, phase space, etc.
Oh! So in a mixture of gases, they are evenly dispersed? For example, the dispersion of water in hydrogen is the same as that of water in nitrogen?
As long as space and time permit, calculate it uniformly. Except in some special cases, the issue of uniform dispersion among gases is rarely considered, as there are few forces acting between gas molecules; the distances between them are generally beyond the range of van der Waals forces, and the molecules move very rapidly. Regarding the situation you mentioned, as long as it’s not an extremely ** extreme case (like in my previous example, where water evaporates into a large space), it can be considered evenly dispersed. If you have very strict requirements for this result, it is recommended to design an experiment, as factors such as space volume, temperature, and flow velocity will all affect dispersion.