Kinetic Molecular Theory of Gases

Kinetic Molecular Theory of GasesRegina MarinGas is c aloneed the severalize of look in which, under certain conditions of temperature and hug, its molecules cross-react only weakly with from separately one an different(prenominal) without forming molecular bonds, taking the shape and batch of their container and tending to separate , and expand, their trump out for their high energising energy. Gases ar highly compressible fluids that experience gargantuan changes in density with temperature and bosom. Molecules constituting a squander almost argon not attracted by each other, so that they move in space at high speed and quite separated from each other, thus explaining the propertiesThe blow molecules are virtually free, so that they are able to be distri exclusivelyed end-to-end the space in which they are contained. The gravitational attraction and forces between molecules are minimal compared to the rate at which the molecules are moving.Gases completely hold t he volume of their container.Gases have no definite shape, embracing the vass containing them.Can easily be compressed, because there are large gaps between molecules, and other.At ambient temperature and insisting gaseous statees can be elements such(prenominal) as hydrogen, oxygen, nitrogen, chlorine, fluorine and noble gases, compounds such as carbon dioxide or propane, or mixtures like air.For the thermal behavior of particles of matter there are four measurable quantities that are of bulky interest stuff, volume, temperature and mass of the sample material (or ruin amount of depicted object, mensural in moles). Any gas is considered a fluid because it has properties that stand it to conduct as such. Its molecules in constant motion, colliding elastically with each other and against the walls of the vessel containing the gas, against which assert a constant pressure. If the gas is heated, the heat energy is spent on energizing energy of the molecules, that is, the mo lecules move more quickly, so that the estimate of collisions with the walls of the vessel increases in number and energy. As a consequence the gas pressure increases, and if the container walls are not rigid, gas volume increases.A gas tends to be chemically active because its molecular surface is also large, that is, to be its particles in continuous motion colliding with each other, this makes it easier the contact between a substance and another, increasing the rate of reaction in compared to liquid or solid. To better understand the behavior of a gas, where studies are conducted with respect to the ideal gas, although it never actually exists and its properties areA pure gasified substance consists of molecules of the like size and mass. A gaseous mixture is formed by diametric molecules in size and mass.Due to the large distance between molecules and other and that move at high speed, the forces of attraction between the molecules are considered negligible.The size of th e gas molecules is really small, so that the volume occupied by the molecules is negligible compared with the total volume of the container. The density of a gas is very low.The gas molecules are in constant motion at high speed, so continuously collide elastically with each other and against the walls of their container.As part of the energizing guess, the gas pressure is explained as the macroscopic sequel of the forces involved by collisions of gas molecules with the walls of the container. The pressure can thus be defined with abduce to the microscopic properties of the gas. The kinetic theory of gases is a corporal and chemical theory that explains the behavior and macroscopic properties of gases (ideal gas virtue), from a statistical description of the microscopic molecular processes. The kinetic theory was developed ground on studies of sensible and Daniel Bernoulli in the eighteenth century, Ludwig Boltzmann and James Clerk Maxwell in the posthumous nineteenth cent ury. This branch describes the thermal physical properties of the gases. These systems contain huge numbers pool of atoms or molecules, and the only reasonable way to understand the thermal properties based on molecular mechanics, we find certain dynamical quantities of median(a) lineament and revive the observed physical properties of the system with these properties averaged molecular dynamics . Techniques to relate the overall macroscopic behavior of material systems with the average behavior of their molecular components are statistical mechanics. The main theorems of the kinetic theory areThe number of molecules is large and the average separation between them is large compared with their dimensions. Therefore occupy an insignificant volume when compared to the volume of the container and are considered point masses.The molecules obey due north&aposs laws, but individually they move randomly, each with different rates, but with an average speed that does not change with ti me.The molecules perform elastic collisions with each other, therefore both the linear momentum is conserved as the kinetic energy of the molecules.The gas is considered pure, in other words all molecules are identical.The gas is in thermal equilibrium with the walls of the container.As part of the kinetic theory of a gas pressure is explained as the macroscopic result of the forces involved by collisions of gas molecules with the walls of the container. The pressure can thus be defined with reference to the microscopic properties of the gas. It is generally believed that there is more pressure if the particles are in the solid state, if they are in liquid state is minimal distance between them and finally if you are in the gaseous state are far apart. Indeed, for an ideal gas with N molecules , each moving mass m with a random speed average content in a cubic volume V of the gas particles impacting with the wall of the container in a manner that can be metric in a statistical mann er exchanging momentum with the walls in each shock and effecting a net force per unit area that is the pressure exerted by the gas on the solid surface. The pressure can be calculated with this formulaThe equation above states that the gas pressure is straightway dependent on the molecular kinetic energy. The ideal gas law allows us to ensure that the pressure is proportional to the absolute temperature. These two statements allow one of the most important statements of the kinetic theory The average molecular energy is proportional to temperature. The proportional constant is 3/2 is the Boltzmann constant, which in turn is the ratio of the gas constant R between the Avogadro number.So in a few words, the kinetic theory is a physical theory, based on a few factsThe density of the gas is very small.Individually molecules move randomly and at different speeds, which increases or decreases art object the temperature and the movement causes them from hitting each other, increasing th e pressure when striking more times.The cohesive forces or intermolecular forces in gases are almost nil.If all of the molecules forming the gas are identical, is said to be a pure gas.Bibliographyhttp//www.chm.davidson.edu/vce/kineticmoleculartheory/basicconcepts.htmhttp//en.wikipedia.org/wiki/Kinetic_theoryhttp//www.sparknotes.com/ alchemy/gases/kinetic/summary.htmlhttp//hyperphysics.phy-astr.gsu.edu/hbase/kinetic/kinthe.html