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in the solid stability region (left side of the diagram), increasing the temperature of the system would bring it into the region where a liquid or a gas is the equilibrium phase (depending on the pressure). If the piston is slowly lowered, the system will trace a curve of increasing temperature and pressure within the gas region of the phase diagram. At the point where gas begins to condense to liquid, the direction of the temperature and pressure curve will abruptly change to trace along the phase line until all of the water has condensed.
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445:(is insoluble) in oil, and oil has a low solubility in water. Solubility is the maximum amount of a solute that can dissolve in a solvent before the solute ceases to dissolve and remains in a separate phase. A mixture can separate into more than two liquid phases and the concept of phase separation extends to solids, i.e., solids can form
561:. As the temperature and pressure approach the critical point, the properties of the liquid and gas become progressively more similar. At the critical point, the liquid and gas become indistinguishable. Above the critical point, there are no longer separate liquid and gas phases: there is only a generic fluid phase referred to as a
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kinetic energy to break away from the liquid phase and enter the gas phase. Likewise, every once in a while a vapor molecule collides with the liquid surface and condenses into the liquid. At equilibrium, evaporation and condensation processes exactly balance and there is no net change in the volume of either phase.
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to another) it usually either takes up or releases energy. For example, when water evaporates, the increase in kinetic energy as the evaporating molecules escape the attractive forces of the liquid is reflected in a decrease in temperature. The energy required to induce the phase transition is taken
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suggests that different phases are completely determined by these variables. Consider a test apparatus consisting of a closed and well-insulated cylinder equipped with a piston. By controlling the temperature and the pressure, the system can be brought to any point on the phase diagram. From a point
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An unusual feature of the water phase diagram is that the solid–liquid phase line (illustrated by the dotted green line) has a negative slope. For most substances, the slope is positive as exemplified by the dark green line. This unusual feature of water is related to ice having a lower density than
503:
At room temperature and pressure, the water jar reaches equilibrium when the air over the water has a humidity of about 3%. This percentage increases as the temperature goes up. At 100 °C and atmospheric pressure, equilibrium is not reached until the air is 100% water. If the liquid is heated a
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Water in a closed jar with an air space over it forms a two-phase system. Most of the water is in the liquid phase, where it is held by the mutual attraction of water molecules. Even at equilibrium molecules are constantly in motion and, once in a while, a molecule in the liquid phase gains enough
322:
is a region of material that is chemically uniform, physically distinct, and (often) mechanically separable. In a system consisting of ice and water in a glass jar, the ice cubes are one phase, the water is a second phase, and the humid air is a third phase over the ice and water. The glass of the
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Left to equilibration, many compositions will form a uniform single phase, but depending on the temperature and pressure even a single substance may separate into two or more distinct phases. Within each phase, the properties are uniform but between the two phases properties differ.
522:
A typical phase diagram for a single-component material, exhibiting solid, liquid and gaseous phases. The solid green line shows the usual shape of the liquid–solid phase line. The dotted green line shows the anomalous behavior of water when the pressure increases. The
369:. (Phase boundaries relate to changes in the organization of matter, including for example a subtle change within the solid state from one crystal structure to another, as well as state-changes such as between solid and liquid.) These two usages are not
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Between two phases in equilibrium there is a narrow region where the properties are not that of either phase. Although this region may be very thin, it can have significant and easily observable effects, such as causing a liquid to exhibit
715:(MBL) systems has provided a framework for defining phases out of equilibrium. MBL phases never reach thermal equilibrium, and can allow for new forms of order disallowed in equilibrium via a phenomenon known as
436:
Distinct phases may also exist within a given state of matter. As shown in the diagram for iron alloys, several phases exist for both the solid and liquid states. Phases may also be differentiated based on
807:
Bhanage, B.M.; et al. (1998). "Comparison of activity and selectivity of various metal-TPPTS complex catalysts in ethylene glycol — toluene biphasic Heck vinylation reactions of iodobenzene".
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361:
phases of the same state of matter (as where oil and water separate into distinct phases, both in the liquid state). It is also sometimes used to refer to the equilibrium states shown on a
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Another interesting though not unusual feature of the phase diagram is the point where the solid–liquid phase line meets the liquid–gas phase line. The intersection is referred to as the
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as in polar (hydrophilic) or non-polar (hydrophobic). A mixture of water (a polar liquid) and oil (a non-polar liquid) will spontaneously separate into two phases. Water has a very low
554:. The markings show points where two or more phases can co-exist in equilibrium. At temperatures and pressures away from the markings, there will be only one phase at equilibrium.
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The transitions between different MBL phases and between MBL and thermalizing phases are novel dynamical phase transitions whose properties are active areas of research.
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and pressure. The number and type of phases that will form is hard to predict and is usually determined by experiment. The results of such experiments can be plotted in
615:. In terms of modeling, describing, or understanding the behavior of a particular system, it may be efficacious to treat the interfacial region as a separate phase.
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A single material may have several distinct solid states capable of forming separate phases. Water is a well-known example of such a material. For example, water
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Experimentally, phase lines are relatively easy to map due to the interdependence of temperature and pressure that develops when multiple phases form.
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little over 100 °C, the transition from liquid to gas will occur not only at the surface but throughout the liquid volume: the water boils.
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In the diagram, the blue line marking the boundary between liquid and gas does not continue indefinitely, but terminates at a point called the
468:), silicones, several different metals, and also from molten phosphorus. Not all organic solvents are completely miscible, e.g. a mixture of
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from the internal thermal energy of the water, which cools the liquid to a lower temperature; hence evaporation is useful for cooling. See
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with the formal definition given above and the intended meaning must be determined in part from the context in which the term is used.
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The phase diagram shown here is for a single component system. In this simple system, phases that are possible, depend only on
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and that associated with a solid to gas transition is the
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between solid and liquid form other states of matter.
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775:Solvents and Solvent Effects in Organic Chemistry
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330:More precisely, a phase is a region of space (a
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847:Modell, Michael; Robert C. Reid (1974).
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569:(374 °C or 705 °F) and 22.064
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855:. Englewood Cliffs, NJ: Prentice-Hall.
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851:Thermodynamics and Its Applications
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735:One such system is, from the top:
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823:10.1016/S0040-4039(98)02225-4
1429:Order and disorder (physics)
901:Clement John Adkins (1983).
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1047:Bose–Einstein condensate
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693:Enthalpy of vaporization
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427:Bose–Einstein condensate
231:List of chemistry awards
30:Not to be confused with
1348:Enthalpy of sublimation
880:. Courier Corporation.
701:enthalpy of sublimation
39:Phases of Matter (film)
1363:Latent internal energy
1113:Color-glass condensate
944:, and 4-methylpyridine
773:Reichardt, C. (2006).
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531:are shown as red dots.
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876:Enrico Fermi (2012).
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596:Interfacial phenomena
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1052:Fermionic condensate
332:thermodynamic system
262:Chemistry portal
183:Analytical chemistry
160:Chemical equilibrium
44:For other uses, see
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1267:Chemical ionization
1159:Programmable matter
1149:Quantum spin liquid
1017:Supercritical fluid
810:Tetrahedron Letters
713:many-body localized
563:supercritical fluid
340:index of refraction
198:Inorganic chemistry
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1343:Enthalpy of fusion
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150:Acid–base reaction
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1409:Equation of state
1257:Flash evaporation
1209:Phase transitions
1194:String-net liquid
1087:Photonic molecule
1057:Degenerate matter
912:978-0-521-27456-2
887:978-0-486-13485-7
862:978-0-13-914861-3
817:(51): 9509–9512.
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781:. pp. 9–10.
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491:Phase equilibrium
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65:
64:
61:
58:
57:
53:
52:
47:
40:
33:
19:
1449:Superheating
1322:Vaporization
1317:Triple point
1312:Supercooling
1277:Lambda point
1227:Condensation
1144:Time crystal
1122:Other states
1062:Quantum Hall
938:cyclodextrin
931:
902:
896:
877:
871:
850:
842:
814:
808:
797:
774:
741:silicone oil
731:
710:
685:
650:Polymorphism
643:rhombohedral
622:
605:
586:
582:triple point
579:
575:
556:
545:
534:
525:triple point
502:
498:
494:
478:
455:
435:
404:
397:Iron-carbon
371:commensurate
350:
348:
329:
319:
313:
188:Biochemistry
165:Chemical law
129:
72:
1358:Latent heat
1307:Sublimation
1252:Evaporation
1187:Ferromagnet
1182:Ferrimagnet
1164:Dark matter
1096:High energy
737:mineral oil
552:temperature
537:temperature
456:As many as
1469:Categories
1373:Volatility
1336:Quantities
1297:Regelation
1272:Ionization
1247:Deposition
1199:Superglass
1169:Antimatter
1103:QCD matter
1082:Supersolid
1077:Superfluid
1040:Low energy
834:References
769:45 °C
666:fullerenes
512:See also:
443:solubility
439:solubility
431:mesophases
359:immiscible
779:Wiley-VCH
654:allotropy
613:interface
481:Emulsions
429:. Useful
349:The term
60:Chemistry
18:Gas phase
1434:Spinodal
1382:Concepts
1262:Freezing
662:graphite
548:pressure
527:and the
485:colloids
409:such as
275:Category
215:Research
177:Branches
107:timeline
94:Glossary
1394:Binodal
1282:Melting
1217:Boiling
1134:Crystal
1129:Colloid
765:mercury
761:gallium
749:aniline
658:diamond
474:toluene
336:density
314:In the
221:Chemist
103:History
89:Outline
1022:Plasma
1003:Liquid
909:
884:
859:
805:. See
785:
763:, and
670:carbon
664:, and
646:ice II
641:, the
451:alloys
423:plasma
415:liquid
273:
125:Matter
1012:Vapor
998:Solid
991:State
942:water
745:water
723:Notes
636:ice I
629:ice I
419:solid
382:argon
351:phase
320:phase
155:Redox
130:Phase
84:Index
983:list
936:– α-
932:rise
907:ISBN
882:ISBN
857:ISBN
783:ISBN
550:and
483:and
472:and
318:, a
225:list
135:Bond
1008:Gas
819:doi
625:ice
571:MPa
425:or
411:gas
327:.)
145:Ion
1471::
1010:/
940:,
815:39
813:.
777:.
759:,
755:,
751:,
747:,
743:,
739:,
703:.
672:.
660:,
573:.
543:.
421:,
417:,
413:,
342:,
338:,
985:)
981:(
971:e
964:t
957:v
915:.
890:.
865:.
825:.
821::
791:.
638:c
631:h
567:K
464:(
303:e
296:t
289:v
227:)
223:(
109:)
105:(
48:.
41:.
34:.
20:)
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