May I use flash evaporation to simulate the boiling point of calcium chloride solution?
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I tried a 60% calcium chloride solution at atmospheric pressure; I’m not sure if the temperature shown in the image below is its boiling point
Young man, study hard – mixtures don’t have a boiling point
It can be considered that the temperature at which the first bubble is formed is the starting point, and as the salt concentration increases, the temperature also rises
It seems you know a lot. Then, can Aspen simulate the temperature at which a salt solution boils under different pressures?
1. Yes. 2. For your substance, the boiling point will range from over 100 degrees to the melting point of salt. 3. Who knows if Tema is accurate or not. Doing this is nothing but pointless nonsense; if one has the time, it’s better to study the physical models of electrolytes and truly understand the principles behind them.
Since no suitable instruments have been found for conducting pressure experiments at the moment, I want to first use software simulations to see at what temperature a salt solution will boil under 2–3 atmospheres of pressure; I think it will be acceptable if the error is not too large
Do it if you like to; I just don’t find it interesting anyway. Especially the parameters of the thermodynamic model for electrolytes – I don’t think they are reliable