Partial pressure and total pressure

A clear explanation of the basic knowledge necessary to understand distillation, distillation towers, and distillation equipment!

Kansai Chemical will explain "partial pressure and total pressure." When it comes to pressure in distillation operations, it usually refers to the pressure limited on the gas side. Air is primarily composed of nitrogen and oxygen, with nitrogen making up about 80% and oxygen about 20% by volume. (The molar ratio is the same.) Now, let's consider a balloon inflated with air. Inside the balloon, nitrogen and oxygen molecules are moving vigorously. They are colliding violently and uniformly (according to Pascal's principle) against the inner walls of the balloon multiple times. The pressure inside the balloon can be said to be the result of these collision forces. One mole is a collection of 6.022×10^23 molecules, and for all gases, at 0°C and 1 atm, it occupies 22.4 L. This means that the force exerted by a single molecule on the wall during a collision is equal for both nitrogen and oxygen. While we have imagined a lot about gases, an important law regarding the handling of gases in distillation is Dalton's law of partial pressures: "Total pressure P (kPa) = Sum of partial pressures Σpi (kPa)." *For more details, please refer to the PDF document or feel free to contact us.

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