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  2. Kinetic theory of gases - Wikipedia

    en.wikipedia.org/wiki/Kinetic_theory_of_gases

    The kinetic theory of gases is a simple classical model of the thermodynamic behavior of gases. Its introduction allowed many principal concepts of thermodynamics to be established. Its introduction allowed many principal concepts of thermodynamics to be established.

  3. Drude model - Wikipedia

    en.wikipedia.org/wiki/Drude_model

    The model, which is an application of kinetic theory, assumes that the microscopic behaviour of electrons in a solid may be treated classically and behaves much like a pinball machine, with a sea of constantly jittering electrons bouncing and re-bouncing off heavier, relatively immobile positive ions.

  4. Molecular chaos - Wikipedia

    en.wikipedia.org/wiki/Molecular_chaos

    James Clerk Maxwell introduced this approximation in 1867 [3] although its origins can be traced back to his first work on the kinetic theory in 1860. [4] [5] The assumption of molecular chaos is the key ingredient that allows proceeding from the BBGKY hierarchy to Boltzmann's equation, by reducing the 2-particle distribution function showing ...

  5. Kinetic theory - Wikipedia

    en.wikipedia.org/wiki/Kinetic_theory

    Kinetic theory may refer to: Kinetic theory of matter: A general account of the properties of matter, including solids liquids and gases, based around the idea that heat or temperature is a manifestation of atoms and molecules in constant agitation. Kinetic theory of gases, an account of gas properties in terms of motion and interaction of ...

  6. Van der Waals equation - Wikipedia

    en.wikipedia.org/wiki/Van_der_Waals_equation

    This article inspired further work based on the twin ideas that substances are composed of indivisible particles, and that heat is a consequence of the particle motion; movement that evolves in accordance with Newton's laws. The work, known as the kinetic theory of gases, was done principally by Clausius, James Clerk Maxwell, and Ludwig Boltzmann.

  7. Boltzmann equation - Wikipedia

    en.wikipedia.org/wiki/Boltzmann_equation

    The general equation can then be written as [6] = + + (),. where the "force" term corresponds to the forces exerted on the particles by an external influence (not by the particles themselves), the "diff" term represents the diffusion of particles, and "coll" is the collision term – accounting for the forces acting between particles in collisions.

  8. Langmuir adsorption model - Wikipedia

    en.wikipedia.org/wiki/Langmuir_adsorption_model

    The kinetic derivation applies to gas-phase adsorption. However, it has been mistakenly applied to solutions. The multiple-adsorbate case is covered in the competitive adsorption sub-section. The model assumes adsorption and desorption as being elementary processes, where the rate of adsorption r ad and the rate of desorption r d are given by

  9. Newton's laws of motion - Wikipedia

    en.wikipedia.org/wiki/Newton's_laws_of_motion

    In statistical physics, the kinetic theory of gases applies Newton's laws of motion to large numbers (typically on the order of the Avogadro number) of particles. Kinetic theory can explain, for example, the pressure that a gas exerts upon the container holding it as the aggregate of many impacts of atoms, each imparting a tiny amount of momentum.