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In physical chemistry, supersaturation occurs with a solution when the concentration of a solute exceeds the concentration specified by the value of solubility at equilibrium. Most commonly the term is applied to a solution of a solid in a liquid , but it can also be applied to liquids and gases dissolved in a liquid.
Köhler curves showing how the critical diameter and supersaturation are dependent upon the amount of solute. It's assumed here that the solute is a perfect sphere of sodium chloride with a dry diameter Dp. Köhler theory describes the vapor pressure of aqueous aerosol particles in thermodynamic equilibrium with a humid atmosphere.
Supersaturation, where the concentration of a solute exceeds its maximum solubility at equilibrium; Undersaturation, where the concentration of a solute is less than its maximum solubility at equilibrium
The red curve is a fit of a function of the Gompertz form to these data. To the right is shown an example set of nucleation data. It is for the nucleation at constant temperature and hence supersaturation of the crystal phase in small droplets of supercooled liquid tin; this is the work of Pound and La Mer. [16]
The upper curve is the line of liquidus, and the lower curve is the line of solidus. In chemistry, materials science, and physics, the liquidus temperature specifies the temperature above which a material is completely liquid, [2] and the maximum temperature at which crystals can co-exist with the melt in thermodynamic equilibrium.
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The green curve is the total (Gibbs if this is at constant pressure) free energy as a function of radius. Shown is the free energy barrier, , and radius at the top of the barrier, . This total free energy is a sum of two terms. The first is a bulk term, which is plotted in red.