On the condensation of mixed gases
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I need help. When considering the condensation of mixed gases, the partial pressures must be taken into account, but in practice there are cases where liquid formation is possible even when the values exceed the partial pressures. Why is this? Is it related to the direction of molecular movement? Or in another direction, thank you
I can’t understand your description; add the data at the end
It is acetaldehyde in the condensed mixed gas, accounting for about 4%. From the perspective of gas partial pressure, a temperature of -80 degrees is required for it to condense; however, with a spiral-wound heat exchanger, it can be condensed at 0 degrees under normal pressure. Therefore, I am seeking help as stated in the question
Spiral-wound heat exchangers: It’s not clear what the structure of this type of heat exchanger is, nor what distinguishes it from other heat exchangers. -80°C is presumably the equilibrium temperature calculated theoretically; in practice, operations may take place at a non-equilibrium state
What does this non-equilibrium state refer to?
Under ideal conditions, the temperature inside the tube is identical at every point, from the wall to the axis, and the gas and liquid phases are in equilibrium, following the laws of saturated vapor pressure and partial pressures. In reality, during condensation, there is a temperature gradient from low to high from the tube wall toward the axis; the lower temperature at the wall facilitates condensation. This helically wound heat exchanger may be able to accelerate condensation