Kinetic theory of gases

Gas dynamics theory, theory based on descriptions of molecules or particles that simplified gas. From there we can derive the general properties of many gases.

The aim of kinetic theory is to explain the nature of gas based on intermolecular forces. We assume that the movement of a molecule is described by the law of dynamics (quantum mechanics is necessary but usually classic Newtonian mechanics).

British scientist James Clark Maxwell and Austrian physicist Ludwig Bozman established this theory in the 19th century and became one of the most important concepts of modern science.

The simplest kinetic model is based on the following assumptions: (1) the gas consists of a number of identical molecules that move in a random direction with a distance greater than their size; (2) The molecular wall between them undergoes complete elastic collision (no energy loss), otherwise it does not interact; (3) kinetic energy transfer between molecules is heat. These simplified assumptions make gas properties within the mathematical processing range.

Such a model describes an ideal gas (qv), which is a reasonable approximation of true gas, especially at extreme dilution and high temperature limits. However, this simplified explanation is not sufficient to accurately account for the behavior of dense gas.

Based on kinetics, the pressure on the vessel wall can be attributed quantitatively to the random collision of molecules whose average energy depends on the gas temperature. Therefore gas pressure is directly related to temperature and density. Many other general characteristics of the gas can be derived, such as viscosity, heat and electrical conduction, diffusion, heat capacity and mobility. In order to account for deviations from the observed perfect gas behavior (eg condensation), these assumptions must be properly modified. Doing so gave considerable insight into the molecular dynamics and the nature of the interaction.

(Also called Movement - Molecular Theory) Gas kinetic theory explains the behavior of the assumed ideal gas. According to this theory, the gas from the fine particles is composed of random linear motion. They quickly and continuously move the collision and collide with the walls occurred. This is the first explanation theory container wall collision gas pressure rather than pressing a static force on another molecule. The theory of gas dynamics also explains how different size particles grant that different individual velocity

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In the late nineteenth century, James Clerk Maxwell and Ludwig Boltzmann were able to use the kinetic energy of gas molecules to identify the temperature of the gas in the well-known dynamic (gas) theory of gas. At least then, "total kinetic energy". Clear recognition is not to distinguish the meaning between the terms used - the problem of equality. However, identification is not done in the way assumed in the Herbst model. These talented theorists did not experiment by individualizing the temperature of the gas first and individualizing the kinetic energy of the molecule experimentally. Gas Instance Identity Relations However, this identity is very mature and is no longer considered a matter of discussion.

However, the attributes of rationalism are quite different. The only thing in the whole universe may be an illustration of "property"

By the end of the nineteenth century scientists began accepting material atomism and began to associate them with individual molecules. Molecular theory of gas dynamics comes from the observation of gas by scientists to explain their macroscopic nature. Below is the basic assumption of the theory of kinetic molecules. According to the theory of kinetic molecules, the rise in temperature increases the average kinetic energy of the molecule. As the particles move faster, they may strike the end of the container more frequently. If the reactions maintain a constant pressure they have to be kept farther apart and the increase in volume will compensate for the increase in collision with the surface of the particle container.