Gibbs-Thomson effect

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The Gibbs-Thomson effect (named after Josiah Willard Gibbs and William Thomson ; not to be confused with the Thomson effect ) is a consequence of the interfacial energy in physical chemistry . This means that small liquid droplets (i. E. Particles with a strong surface curvature ) has a higher effective vapor pressure having as a planar phase boundary (liquid-gas) because small droplets, the interface compared to the volume of liquid is greater.

A generalization of the Gibbs-Thomson effect allows the explanation of Ostwald ripening , in which larger particles grow and smaller ones dissolve in disperse systems of small particles by means of diffusion .

The Gibbs-Thomson equation for a particle with radius is:

With

  • p - partial pressure of the droplet-forming substance
  • p saturation - saturation pressure of the droplet-forming substance
    • - Surface energy of the drop in J / m².
    • - Volume of a molecule in the drop or volume per number of particles
    • k B - Boltzmann constant
    • T - temperature in Kelvin .

Because of the increase in the internal pressure due to the curved phase boundary (see Young-Laplace equation ), there is also a decrease in the melting temperature inside small particles . Sometimes this is also referred to as the Gibbs-Thomson effect.