Vapor

The vapor-liquid critical point in a pressure-temperature phase diagram is at the high-temperature extreme of the liquid–gas phase boundary. (The dotted green line gives the anomalous behaviour of water.)

Vapor refers to a gas phase at a temperature where the same substance can also exist in the liquid or solid state, below the critical temperature of the substance. (For example, water has a critical temperature of 374 °C (647 K), which is the highest temperature at which liquid water can exist.) If the vapor is in contact with a liquid or solid phase, the two phases will be in a state of equilibrium. The term gas refers to a compressible fluid phase. Fixed gases are gases for which no liquid or solid can form at the temperature of the gas, such as air at typical ambient temperatures. A liquid or solid does not have to boil to release a vapor.

Vapor is responsible for the familiar processes of cloud formation and condensation. It is commonly employed to carry out the physical processes of distillation and headspace extraction from a liquid sample prior to gas chromatography.

The constituent molecules of a vapor possess vibrational, rotational, and translational motion. These motions are considered in the kinetic theory of gases.

Liquid–vapor equilibrium

If the vapor pressure exceeds the equilibrium value, it becomes supersaturated and condenses on any available nucleation sites e. g. particles of dust. This principle is used in cloud chambers, where particles of radiation are visualized because they nucleate formation of water droplets.

The vapor pressure is the equilibrium pressure from a liquid or a solid at a specific temperature. The equilibrium vapor pressure of a liquid or solid is not affected by the amount of contact with the liquid or solid interface.

The normal boiling point of a liquid is the temperature at which the vapor pressure is equal to normal atmospheric pressure.[1]

For two-phase systems (e.g., two liquid phases), the vapor pressure of the individual phases are equal. In the absence of stronger inter-species attractions between like-like or like-unlike molecules, the vapor pressure follows Raoult's law, which states that the partial pressure of each component is the product of the vapor pressure of the pure component and its mole fraction in the mixture. The total vapor pressure is the sum of the component partial pressures.[3]

Water vapor is responsible for humidity

• Perfumes contain chemicals that vaporize at different temperatures and at different rate in scent accords, known as notes.
• Atmospheric water vapor is found near the earth's surface, and may condense into small liquid droplets and form meteorological phenomena, such as fog, mist, and haar.
• Mercury-vapor lamps and sodium vapor lamps produce light from atoms in excited states.
• Flammable liquids do not burn when ignited.[4] It is the vapor cloud above the liquid that will burn if the vapor's concentration is between the lower flammable limit (LFL) and upper flammable limit (UFL), of the flammable liquid.
• E-Cigarettes allow users to inhale "e-liquid" aerosol/vapor, rather than cigarette smoke.[2]

Since it is in the gas phase, the amount of vapor present is quantified by the partial pressure of the gas. Also, vapors obey the barometric formula in a gravitational field, just as conventional atmospheric gases do.

Look up vapor or vapour in Wiktionary, the free dictionary.

• Dilution (equation)
• Evaporation – Type of vaporization of a liquid that occurs from its surface; surface phenomenon
• Henry's law – Relation of equilibrium solubility of a gas in a liquid to its partial pressure in the contacting gas phase
• Contrail, also known as Vapor trail – Long, thin artificial clouds that sometimes form behind aircraft
• Vaporizer (disambiguation)