Examples of phase boundary in the following topics:
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- The major features of a phase diagram are phase boundaries and the triple point.
- Phase boundaries, or lines of equilibrium, are boundaries that indicate the conditions under which two phases of matter can coexist at equilibrium.
- Along the blue phase boundary, water exists as both a vapor and a liquid.
- Along the dotted green phase boundary, we see the anomalous behavior of water: it exists as a solid at low-enough temperatures and high-enough pressures.
- In this phase diagram, which is typical of most substances, the solid lines represent the phase boundaries.
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- The lines that separate these single phase regions are known as phase boundaries.
- Along the phase boundaries, the matter being evaluated exists simultaneously in equilibrium between the two states that border the phase boundary.
- When evaluating the phase diagram, it is worth noting that the solid-liquid phase boundary in the phase diagram of most substances has a positive slope.
- However, the solid-liquid phase boundary for water is anomalous, in that it has a negative slope.
- The dotted green line refers to the solid-liquid phase boundary for water.
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- In addition, there is no surface tension in a supercritical fluid, as there is no liquid to gas phase boundary.
- In the pressure-temperature phase diagram of CO2, the boiling separates the gas and liquid region and ends in the critical point, where the liquid and gas phases disappear to become a single supercritical phase.
- At the critical point, (304.1 K and 7.38 MPa) there is no difference in density, and the two phases become one fluid phase.
- The dry ice melts under high pressure, and forms a liquid and gas phase.
- When the vessel is heated, the CO2 becomes supercritical -- meaning the liquid and gas phases merge together into a new phase that has properties of a gas, but the density of a liquid.
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- Complete solid solution alloys give single solid phase microstructure.
- Partial solutions give two or more phases that may or may not be homogeneous in distribution, depending on thermal history.
- Complete solid solution alloys give single solid phase microstructure.
- Partial solutions give two or more phases that may or may not be homogeneous in distribution, depending on thermal history.
- Alloys can be further classified as homogeneous (consisting of a single phase), heterogeneous (consisting of two or more phases), or intermetallic (where there is no distinct boundary between phases).
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- Liquids and solids share a common attribute: a clear and discernible phase boundary that gives the sample a simple but definite shape.
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- Its liquid phase, the most common phase of water on Earth, is the form that is generally meant by the word "water."
- When water achieves a specific critical temperature and a specific critical pressure (647 K and 22.064 MPa), the liquid and gas phases merge into one homogeneous fluid phase that shares properties of both gas and liquid.
- Well-defined boundaries between solid and liquid, solid and gas, and liquid and gas.
- During the phase transition between two phases (i.e, along these boundaries), the phases are in equilibrium with each other.
- The three phases of water – liquid, solid, and vapor – are shown in temperature-pressure space.
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- Vaporization of a sample of liquid is a phase transition from the liquid phase to the gas phase.
- Vaporization of a sample of liquid is a phase transition from the liquid phase to the gas phase.
- Gradually, Pw will rise as molecules escape from the liquid phase and enter the vapor phase.
- At the same time, some of the vapor molecules will condense back into the liquid phase (step 2).
- A bubble is a hole in a liquid; molecules at the liquid boundary are curved inward, so they experience stronger nearest-neighbor attractions.
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- Freezing is a phase transition in which a liquid turns into a solid when its temperature is lowered to its freezing point.
- Freezing, or solidification, is a phase transition in which a liquid turns into a solid when its temperature is lowered to or below its freezing point.
- This is a first-order thermodynamic phase transition, which means that as long as solid and liquid coexist, the equilibrium temperature of the system remains constant and equal to the melting point.
- The creation of a nucleus implies the formation of an interface at the boundaries of the new phase.
- Some energy is expended to form this interface, based on the surface energy of each phase.
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- Sublimation is the phase transition from the solid to the gaseous phase, without passing through an intermediate liquid phase.
- Sublimation is the process of transformation directly from the solid phase to the gaseous phase, without passing through an intermediate liquid phase.
- It is an endothermic phase transition that occurs at temperatures and pressures below a substance's triple point (the temperature and pressure at which all three phases coexist) in its phase diagram.
- But at temperatures below that of the triple point, a decrease in pressure will result in a phase transition directly from the solid to the gaseous.
- At temperatures and pressures below those of the triple point, a phase change between the solid and gas phases can take place.
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- One orbital, based on in-phase mixing of the orbitals, will be lower in energy and termed bonding.
- Two atomic orbitals can overlap in two ways depending on their phase relationship.
- The phase of an orbital is a direct consequence of the wave-like properties of electrons.
- If the phase changes, the bond becomes a pi bond (π-bond).
- The in-phase combination of the s orbitals from the two hydrogen atoms provides a bonding orbital that is filled, whereas the out-of-phase combination provides an anti-bonding orbital that remains unfilled.