Everything about Volatility Chemistry totally explained
Volatility in the context of
chemistry,
physics and
thermodynamics is a measure of the tendency of a substance to
vaporize. It has also been defined as a measure of how readily a substance vaporizes. At a given temperature, substances with higher
vapor pressures will vaporize more readily than substances with a lower vapor pressure.
Although usually applying to
liquids, volatility can apply to
solid materials such as
dry ice (solid
carbon dioxide) and
ammonium chloride, which can change directly from solid to
vapor without becoming liquid. The direct transition of a solid to a vapor is called
sublimation.
Relation between vapor pressures and normal boiling points of liquids
pressure of a vapor which is in equilibrium with its non-vapor phases (for example, liquid or solid). Most often the term is used to describe a liquid's tendency to
evaporate. It is a measure of the tendency of
molecules and
atoms to escape from a liquid or a solid. A liquid's
atmospheric pressure boiling point corresponds to the
temperature at which its vapor pressure is equal to the surrounding atmospheric pressure and it's often called the
normal boiling point.
The higher is the vapor pressure of a liquid at a given temperature, the higher is the volatility and the lower is the normal boiling point of the liquid.
The vapor pressure chart to the right has graphs of the vapor pressures versus temperatures for a variety of liquids. As can be seen in the chart, the liquids with the highest vapor pressures have the lowest normal boiling points.
For example, at any given temperature,
propane has the highest vapor pressure of any of the liquids in the chart. It also has the lowest normal boiling point(-43.7 °C), which is where the vapor pressure curve of propane (the purple line) intersects the horizontal pressure line of one atmosphere (
atm) of absolute vapor pressure.
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