Examples of phase diagram in the following topics:
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- A phase diagram is a graph which shows under what conditions of temperature and pressure distinct phases of matter occur.
- The simplest phase diagrams are of pure substances.
- The major features of a phase diagram are phase boundaries and the triple point.
- The phase diagram for water is useful for learning how to analyze these diagrams.
- In this phase diagram, which is typical of most substances, the solid lines represent the phase boundaries.
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- Phase diagrams illustrate the effects selected variables of a system have on the state of matter.
- Phase diagrams illustrate the effects selected variables of a system have on the state of matter.
- 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.
- With a knowledge of the major components of phase diagrams and the features of phase plots, a phase diagram can be used to understand how altering thermodynamic parameters influences the states/phases of matter a sample of a substance is in.
- A typical phase diagram illustrating the major components of a phase diagram as well as the critical point.
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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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- A phase of a thermodynamic system and the states of matter have uniform physical properties.
- There are well-defined regions on these graphs that correspond to various phases of matter, so PT graphs are called phase diagrams .
- Using the graph, if you know the pressure and temperature you can determine the phase of water.
- The solid lines—boundaries between phases—indicate temperatures and pressures at which the phases coexist (that is, they exist together in ratios, depending on pressure and temperature).
- In this typical phase diagram of water, the green lines mark the freezing point, and the blue line marks the boiling point, showing how they vary with pressure.
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- 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.
- The system consists of 2 phases in equilibrium, a dense liquid and a low density gas.
- 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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- 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.
- Phase diagrams help describe how water changes states depending on the pressure and temperature.
- 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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- Due to the phase difference, it is useful to introduce phasors to describe these circuits.
- We say that the current and voltage are in phase.
- In the diagram, the arrows rotate in counter-clockwise direction at a frequency $\nu$.
- Its amplitude is the modulus of the vector, and its argument is the total phase \omega t+\theta.
- The phase constant \theta represents the angle that the vector forms with the real axis at t = 0.
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- Here, $\phi$ is called the phase angle.
- As seen in previous Atoms, voltage and current are out of phase in an RLC circuit.
- There is a phase angle ϕ between the source voltage V and the current I, given as
- Phasor diagram for an RLC series circuit.
- \phi is the phase angle, equal to the phase difference between the voltage and current.
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- This MO diagram depicts the molecule H2, with the contributing AOs on the outside sandwiching the MO.
- The third diagram hypothesizes the molecule dihelium (He2).
- However, removing an electron from the antibonding level produces the molecule He2+, which is stable in the gas phase with a bond order of 0.5.
- The last diagram presents the molecule dilithium (Li2).
- The molecule Li2 is a stable molecule in the gas phase, with a bond order of one.
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- Bonding and antibonding orbitals are illustrated in MO diagrams, and are useful for predicting the strength and existence of chemical bonds.
- Two atomic orbitals can overlap in two ways, depending on their phase relationship.
- An orbital's phase is a direct consequence of electrons' wave-like properties.
- If the phase changes, the bond becomes a pi bond (π-bond).
- The next step in constructing an MO diagram is filling the newly formed molecular orbitals with electrons.