Question

can anybody describe gas laws (Boyle's law,Charle's law ,avogadro's law ,and law of partial pressure)through kinetic molecular theory

Answer 1

BOYLE'S LAW

acc to k.m.t gasses molecules are widely separated and when pressure is applied there molecules come closer by which the volume is decrease(temperature must be constant)

CHARLE'S LAW

acc to k.m.t the molecules of a gas posses kinetic energy which is directly proportional to temperature(at constant pressure) and when the temp is increased kinetic energy also increases due to which the sample of a gas expands in order to keep its pressure constant and volume increases

AVOGADROES'S LAW

acc to k.m.t when two gasses have same temperature their kinetic energy is same,so they exert same pressure because molecules collide with same forcebut pressure also depends upon the number of molecules collides with the walls of container ..
thus if the gases have same T and same P means they posses same number of molecules.

DALTON'S LAW

acc to k.m.t there is no attraction between gas molecules .hence in a mixture of gasses ,each gas behaves independantly ,molecules of each gas on colliding with the walls of container produces their own pressure hence the total pressure is the sum of partial pressur of individual gasses

Answer 2

thanks to quite an extent it solved my quires......