What is kinetic theory?

Kinetic theory is a scientific theory of the nature of gases. The theory goes through many names, including kinetic gase theory, kinetically molecular theory, collision theory and kinetically molecular gas theory. It explains observable and measurable, also called macroscopic properties of gases in terms of their molecular composition and activity. While Isaac Newton theorized that gas pressure was caused by static resistance between molecules, kinetic theory claims that pressure is the result of collisions between molecules.

kinetic theory creates a number of prerequisites. First, the gas is made of very small particles, each with non -zero mass, constantly moving randomly. The number of molecules in the gas sample must be sufficiently large for statistical comparison.

kinetic theory assumes that gas molecules are perfectly spherical and elastic, and that their collisions with the walls of their container are also elastiIt means that they do not lead to a change in speed. The total volume of gas molecules is negligible compared to the total volume of their container, which means that there is plenty of space between molecules. In addition, the time is negligible during the collision of the gas molecule with the container wall in relation to the time between collisions with other molecules. The theory further relies on the assumption that any relativistic or quantum mechanical effects are negligible and that any effects of gas particles are negligible, with the exception of the force developed by the collisions. The temperature is the only factor affecting average kinetic energy or energy due to the movement of gas particles.

These prerequisites must be maintained in order for the equations of kinetic theories to work. The gas that fills all these assumptions is simplified theoretical -known known as the ideal gas. Real gases usually behave enough to make the ideal gases for kinetic equations, but the model is not perfectly accurate.

Kinetic theory defines pressure as a force exerted by gas molecules as they collided with the container wall. The pressure is calculated as a force on an area or p = f/a. The strength is the product of the number of gas molecules, n, the weight of each molecule, M and squares of their average speed, in 2 _{rms , all divided by three times the length of the container, 3l. Therefore, we have the following equation for strength: F = NMV 2 RMS /3L. The abbreviation, RMS, means root medium quadrate, speed diameter of all particles.}

4 Since the area multiplied by the length is equal to the volume, V, this equation can be simplified as P = NMV 2 RMS /3V. The pressure and volume product, PV equals two -thirds of the total kinetic energy or K, allowing the macroscopic properties to be derived from microscopic.

An important part of the kinetic theory is that kinetic energy differs in direct proportion to the absolute gas temperature. Kinetic energy equals the product of absolute temperature, T and BoltzmaNovy constants, K b , multiplied by 3/2; K = 3TK _{b /2. Therefore, whenever the temperature is raised, kinetic energy is increased and no other factors have a effect on kinetic energy.}