Kinetic Molecular Theory (KMT) explains the behavior of gas molecules, revealing how their motion and energy levels dictate physical properties like pressure and volume. It includes core postulates, such as the constant motion of particles and the absence of intermolecular forces. Graham's Law, which relates to the effusion and diffusion rates of gases, is also discussed, alongside the Maxwell-Boltzmann distribution of molecular speeds. These concepts are vital for practical applications in science and engineering.
Show More
The five postulates of Kinetic Molecular Theory explain the behavior of gases by describing their molecular motion and interactions
Ideal Gas Law
The Ideal Gas Law, derived from Kinetic Molecular Theory, relates the pressure, volume, temperature, and number of moles of a gas
Graham's Law
Graham's Law, based on Kinetic Molecular Theory, explains the rate of diffusion and effusion of gases based on their molar mass
The Maxwell-Boltzmann Distribution graphically represents the range of velocities among gas particles at a specific temperature, influenced by factors such as temperature and molar mass
Kinetic Molecular Theory explains the expansion of gases to fill any container due to the ceaseless, haphazard motion of gas particles
The exertion of pressure on container walls by gas particles colliding is a result of their constant random motion, as described by Kinetic Molecular Theory
Kinetic Molecular Theory explains how changes in temperature and volume affect gas properties, such as pressure and expansion, through the motion and collisions of gas particles
00
KMT Assumption: Particle Motion
KMT assumes gas particles are in constant, random motion, explaining gas expansion and pressure.
01
KMT on Particle Collisions
KMT posits particles move linearly until collisions occur, leading to uniform gas distribution.
02
KMT on Particle Size and Spacing
KMT suggests particles are small and widely spaced relative to their size, minimizing interactions.
