Basit Damıtma

Vapor pressure is the pressure exerted by vapor in equilibrium with its liquid phase. Boiling occurs when the total vapor pressure of a substance equals atmospheric pressure. As temperature increases, vapor pressure rises, allowing more molecules to escape the liquid as bubbles. This relationship is fundamental to understanding when and how liquids transition to gases.

In a miscible mixture, each liquid component contributes its own partial pressure to the total vapor pressure. According to Dalton's law, the total vapor pressure equals the sum of individual partial pressures. Each component's partial pressure is calculated using Raoult's law: the pure liquid's vapor pressure multiplied by its mole fraction in the mixture.

The bubble point is the temperature at which the first vapor bubbles form when a mixture is heated. The dew point is the temperature at which the first liquid drops condense from vapor. For a pure liquid, both temperatures equal the boiling point. For a miscible mixture, both occur between the boiling points of the pure components.

During distillation, the more volatile component (lower boiling point) vaporizes first and enters the condenser, enriching early distillate fractions with it. As this component is removed, the liquid becomes richer in the less volatile component, raising the boiling temperature. Collecting distillate in small fractions reveals changing molar ratios as the mixture composition shifts throughout the process.

A boiling point diagram plots bubble and dew point temperatures against mole fractions of mixture components. The lower curve shows the liquid's boiling point at each composition; the upper curve shows the vapor temperature and distillate composition. By recording vapor temperature during distillation and referencing the diagram, you can determine the liquid and vapor compositions at any point in the separation.

The two liquids must be miscible, forming a homogeneous solution. They must have a significant boiling point difference of at least 20 degrees Celsius. This difference ensures that the more volatile component vaporizes preferentially, allowing effective separation. Without sufficient boiling point difference, the vapor composition remains too similar to the liquid, reducing separation efficiency.

The condenser is a water-cooled glass tube with inner and outer chambers. Rising vapor enters the inner chamber where cold water circulating in the outer chamber cools it, causing condensation. The condensed liquid, called the distillate, drips into a collection vessel. This cooling step is essential for converting vapor back to liquid form for collection and analysis.