On desolvation vacuum distillation
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There’s a question that I really can’t figure out; I’m reaching out to all of you for help, hoping you can offer some guidance. Through vacuum distillation, the gases produced consist of dry air, water vapor, and propanone. At this point, the system pressure is 17 kPa absolute, and the temperature is 15 degrees. Given that the saturated vapor pressure of water vapor at this temperature is 1.7 kPa, and that of propanone is 19.7 kPa, how can we calculate the partial pressure of dry air at this time?
Is there no one? Is really no one there? Could you give me some advice?
I completely forgot about this calculation; I think it was just a matter of applying the formula directly, right? And do you know what significance the partial pressure of dry air has for production? I sincerely seek advice.
The total system pressure is 17 kPa. Given the amount of water vapor or propane, the partial pressures of water vapor and propane can be calculated using Dalton’s law of partial pressures. The partial pressure of dry air is then obtained by subtracting the partial pressures of these two gases from the total pressure.
Okay, okay, thank you so much! Can we add each other as friends?