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  2. Phases of ice - Wikipedia

    en.wikipedia.org/wiki/Phases_of_ice

    Unlike most other solids, ice is difficult to superheat. In an experiment, ice at −3 °C was superheated to about 17 °C for about 250 picoseconds. [18] Pressure dependence of ice melting. The latent heat of melting is 5987 J/mol, and its latent heat of sublimation is 50 911 J/mol.

  3. List of boiling and freezing information of solvents - Wikipedia

    en.wikipedia.org/wiki/List_of_boiling_and...

    Boiling point (°C) K b (°C⋅kg/mol) Freezing point (°C) K f (°C⋅kg/mol) Data source; Aniline: 184.3 3.69 –5.96 –5.87 K b & K f [1] Lauric acid: 298.9 44 –3.9

  4. Stefan problem - Wikipedia

    en.wikipedia.org/wiki/Stefan_problem

    This is accomplished by solving heat equations in both regions, subject to given boundary and initial conditions. At the interface between the phases (in the classical problem) the temperature is set to the phase change temperature. To close the mathematical system a further equation, the Stefan condition, is required. This is an energy balance ...

  5. Phase transition - Wikipedia

    en.wikipedia.org/wiki/Phase_transition

    Below the boiling point, the liquid is the more stable state of the two, whereas above the boiling point the gaseous form is the more stable. Common transitions between the solid, liquid, and gaseous phases of a single component, due to the effects of temperature and/or pressure are identified in the following table:

  6. Superheating - Wikipedia

    en.wikipedia.org/wiki/Superheating

    In thermodynamics, superheating (sometimes referred to as boiling retardation, or boiling delay) is the phenomenon in which a liquid is heated to a temperature higher than its boiling point, without boiling. This is a so-called metastable state or metastate, where boiling might occur at any time, induced by external or internal effects.

  7. Sublimation (phase transition) - Wikipedia

    en.wikipedia.org/wiki/Sublimation_(phase_transition)

    Dry ice subliming in air. Solid carbon dioxide sublimes rapidly along the solid-gas boundary (sublimation point) below the triple point (e.g., at the temperature of −78.5 °C, at atmospheric pressure), whereas its melting into liquid CO 2 can occur along the solid-liquid boundary (melting point) at pressures and temperatures above the triple ...

  8. Molecular solid - Wikipedia

    en.wikipedia.org/wiki/Molecular_solid

    The characteristic melting point of metals and ionic solids is ~ 1000 °C and greater, while molecular solids typically melt closer to 300 °C (see table), thus many corresponding substances are either liquid (ice) or gaseous (oxygen) at room temperature.

  9. Triple point - Wikipedia

    en.wikipedia.org/wiki/Triple_point

    A typical phase diagram.The solid green line applies to most substances; the dashed green line gives the anomalous behavior of water. In thermodynamics, the triple point of a substance is the temperature and pressure at which the three phases (gas, liquid, and solid) of that substance coexist in thermodynamic equilibrium. [1]