kinetic theory of gases

Gas can be studied by considering the small scale action of a single molecule or by considering the large scale action of the whole gas. You can directly measure or detect the large impact of gas. However, in order to study the role of a molecule, we must use a theoretical model. The model is invoked assuming that the distance between the molecules to the molecule is very small. Molecules are always random movements, often colliding with each other or colliding with walls of any container.

A single molecule has standard physical properties of mass, momentum and energy. Gas density is simply the molecular weight divided by the volume occupied by gas. Gas pressure is a measure of the linear momentum of a molecule. When a gas molecule collides with the wall of a container, the molecule gives the momentum of the wall and creates a measurable force. The force divided by the area is defined as pressure. Gas temperature is a measure of the average kinetic energy of gas. Molecules have a constant random motion, and there is energy related to movement (mass squared × speed). The higher the temperature, the bigger the movement will be.

For solids, the position of the molecule relative to each other remains nearly constant. However, in gas, molecules move with each other and interact with the surrounding environment in various ways. As mentioned above, there is always a random component in molecular motion. The entire fluid can also move with regular movement (flow). Ordered movements are superimposed or added to the normal random motion of the molecule. At the molecular level, there is no difference between random and ordered ingredients. Measure pressure generated by random component as static pressure. The pressure generated by regular movement is called dynamic pressure. Bernoulli's equation shows that the sum of static pressure and dynamic pressure is the total measurable pressure.

(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 scientists observing gas to explain its 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 collide more often with the edge of the container. If the reactions maintain a constant pressure they have to be kept farther apart and the increase in volume will compensate for the increased collision with the surface of the particle container.