Kinetic Theory

Microscopic kinetic theory of the behavior of gas and the result of intermolecular interactions in macroscopic relations such as the law of ideal gas

In molecular gas studies, the statistical method is a good condition example, providing accurate and reliable results for macro performance of microscopic phenomena. For example, calculate the ideal gas law pressure, volume, temperature very accurately. The average energy related to molecular motion is based on the Boltzmann distribution, and the Boltzmann distribution is a statistical distribution function. However, it is possible to accurately measure the temperature of gas and energy

Under the kinetic theory assumption of gas Newton's law can be applied to determine the average force over the vessel wall. This process is based on the premise that collision with the wall is totally elastic

This development represents a high average number. It is important to note that the average force of the formula N molecules uses the mean square of the velocity, which is significantly different squared of the average velocity.

Under the assumption of the dynamical theory, it is identified that there is an average force of the vessel wall

Given the pressure, the wall forced to depend only on the average velocity component towards the wall. However, the whole can be flat, which can represent a moving average, and is assumed to be a random molecular movement

Molecular dynamics theory can be used to interpret the results obtained in Graham gas diffusion and bleeding studies. The key to this interpretation is that the average kinetic energy is assumed to be proportional to something else rather than temperature and system particles, the last hypothetical theory theory. In other words, if the average kinetic energy of the particle increase only in case, the system temperature will increase

(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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Molecular dynamics theory surprise is that it can be used to derive the ideal gas law. This derivation of the microscopic advocate's movement molecular theory with the ideal gas law is a very obvious macro behavior linked. Deriving beyond the scope of this note, you need to be able to teach the teacher if you are interested

Considering their molecular composition and movement kinetic theory provides a deep understanding of the macroscopic nature of the gas. Starting from the definition of momentum and kinetic energy, the conservation of momentum is used, and the macroscopic properties and microscopic characteristics of the system coupled cubic shape to the temperature and pressure of kinetic energy of each molecule is also good. The theory provides an average value of these two characteristics. The theory also explains how to respond to changes in natural gas systems. For example, if there is gas it (theoretically) still completely, its internal energy (temperature) is large, heated from absolute zero. Heating gas, its temperature rises, particle acceleration. It is due to the high temperature associated with collision per unit time of the container, associated high particle velocity. Collision pressure per unit time increases in proportion to the number