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- этимология
multi-phase - перевод на голландский
![critical point]] of carbon dioxide](https://commons.wikimedia.org/wiki/Special:FilePath/Carbon dioxide pressure-temperature phase diagram.svg?width=200 "critical point]] of carbon dioxide")
![A crescent Moon over [[Kingman, Arizona]]](https://commons.wikimedia.org/wiki/Special:FilePath/BethinAZ - 10-13.002 (by).jpg?width=200 "A crescent Moon over [[Kingman, Arizona]]")
.jpg?width=200 "200px")
![Earth's orbital plane]]) results in the revolution of the [[lunar nodes]] relative to the Earth. This causes an [[eclipse season]] approximately every six months, in which a [[solar eclipse]] can occur at the [[new moon]] phase and a [[lunar eclipse]] can occur at the [[full moon]] phase.](https://commons.wikimedia.org/wiki/Special:FilePath/Eclipse vs new or full moons, annotated.svg?width=200 "Earth's orbital plane]]) results in the revolution of the [[lunar nodes]] relative to the Earth. This causes an [[eclipse season]] approximately every six months, in which a [[solar eclipse]] can occur at the [[new moon]] phase and a [[lunar eclipse]] can occur at the [[full moon]] phase.")
![overexposed]] photograph of a crescent Moon reveals earthshine and stars.](https://commons.wikimedia.org/wiki/Special:FilePath/Lumiere cendrée (12273290216).jpg?width=200 "overexposed]] photograph of a crescent Moon reveals earthshine and stars.")
.gif?width=200 "Animation showing progression of moon phase.")
![The observed orientation of the Moon at different phases from different latitudes on Earth (the different orientation displayed between the phases at each latitude show merely the extremes of orientation due to [[libration]])](https://commons.wikimedia.org/wiki/Special:FilePath/Moon phases by latitude.svg?width=200 "The observed orientation of the Moon at different phases from different latitudes on Earth (the different orientation displayed between the phases at each latitude show merely the extremes of orientation due to [[libration]])")
![The phases of the Moon as viewed looking southward from the [[Northern Hemisphere]]. Each phase would be rotated 180° if seen looking northward from the [[Southern Hemisphere]]. The upper part of the diagram is not to scale, as the Moon, the Earth, and the Moon's orbit are all much smaller relative to the Earth's orbit than what is shown here.](https://commons.wikimedia.org/wiki/Special:FilePath/Moon phases en.jpg?width=200 "The phases of the Moon as viewed looking southward from the [[Northern Hemisphere]]. Each phase would be rotated 180° if seen looking northward from the [[Southern Hemisphere]]. The upper part of the diagram is not to scale, as the Moon, the Earth, and the Moon's orbit are all much smaller relative to the Earth's orbit than what is shown here.")
![A [[full moon]] sets behind [[San Gorgonio Mountain]] in California on a midsummer's morning.](https://commons.wikimedia.org/wiki/Special:FilePath/Moondrop.jpg?width=200 "A [[full moon]] sets behind [[San Gorgonio Mountain]] in California on a midsummer's morning.")
Определение
Википедия
In thermodynamics, the phase rule is a general principle governing "pVT" systems, whose thermodynamic states are completely described by the variables pressure (p), volume (V) and temperature (T), in thermodynamic equilibrium. If F is the number of degrees of freedom, C is the number of components and P is the number of phases, then
- : 123–125
It was derived by American physicist Josiah Willard Gibbs in his landmark paper titled On the Equilibrium of Heterogeneous Substances, published in parts between 1875 and 1878. The rule assumes the components do not react with each other.
The number of degrees of freedom is the number of independent intensive variables, i.e. the largest number of thermodynamic parameters such as temperature or pressure that can be varied simultaneously and arbitrarily without determining one another. An example of one-component system is a system involving one pure chemical, while two-component systems, such as mixtures of water and ethanol, have two chemically independent components, and so on. Typical phases are solids, liquids and gases.
