WordNet

a visible suspension in the air of particles of some substance (同)vapour
rise as vapor
cook something by letting steam pass over it; "just steam the vegetables"
water at boiling temperature diffused in the atmosphere
clean by means of steaming; "steam-clean the upholstered sofa" (同)steam clean
emit steam; "The rain forest was literally steaming"
get very angry; "her indifference to his amorous advances really steamed the young man"
a stoppage in a pipeline caused by gas bubbles (especially a stoppage that develops in hot weather in an internal-combustion engine when fuel in the gas line boils and forms bubbles that block the flow of gasoline to the carburetor) (同)vapour lock
lamp in which an electric current passed through a tube of sodium vapor makes a yellow light; used is street lighting (同)sodium-vapour lamp
resembling or characteristic of vapor; "vaporous clouds" (同)vapourific, vaporish, vapourish, vaporous, vapourous
the density of a gas relative to the density of hydrogen (同)vapour density

PrepTutorEJDIC

『蒸気』,湯気,水蒸気 / 蒸気の力 / 《話》力,精,力,元気 / …‘を'蒸気にさらす,蒸す / 『[水]蒸気を出す』,湯気をたてる《+『away』》 / 《副詞[句]を伴って》蒸気で動く / 《話》怒る,いきまく
=vapor

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出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2015/10/21 22:39:49」(JST)

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Water condenses into visible droplets (aerosol) after evaporating from a cup of hot tea

In physics a vapor (American English spelling) or vapour (British) is a substance in the gas phase at a temperature lower than its critical point,^[1] which means that the vapor can be condensed to a liquid by increasing its pressure without reducing the temperature. Vapor is a different substance than aerosol.^[2] Aerosol is a suspension of tiny particles of liquid, solid or both within a gas.^[2]

For example, water has a critical temperature of 374 °C (647 K), which is the highest temperature at which liquid water can exist. In the atmosphere at ordinary temperatures, therefore, gaseous water (known as water vapor) will condense to liquid if its partial pressure is increased sufficiently.

A vapor may co-exist with a liquid (or solid). When this is true, the two phases will be in equilibrium, and the gas partial pressure will equal the equilibrium vapor pressure of the liquid (or solid).^[1]

Properties

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.

Vapor pressure

Liquid–vapor equilibrium

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]

Examples

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.^{[citation needed]} 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.

Measuring vapor

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.

References

^ ^a ^b ^c R. H. Petrucci, W. S. Harwood, and F. G. Herring, General Chemistry, Prentice-Hall, 8th ed. 2002, p. 483–86.
^ ^a ^b Cheng, T. (2014). "Chemical evaluation of electronic cigarettes". Tobacco Control 23 (Supplement 2): ii11–ii17. doi:10.1136/tobaccocontrol-2013-051482. ISSN 0964-4563. PMC 3995255. PMID 24732157.
^ Thomas Engel and Philip Reid, Physical Chemistry, Pearson Benjamin-Cummings, 2006, p.194

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