Kinetic Gas theory

•State the 5 laws of Kinetic Theory of Gases

Gas particles move in continous rnadom straight line motion

Negligible intermolecular forces between gas particles

Volume of individual gas particles is negligible compared to the volume of the container

Collisions between gas particles are elastic (dont losoe energy when they collide)

Average kinetic energy of particles is proportional to its temperature

• temp increase, KE increases

•Apply the Kinetic Theory of Gases to explain the properties of gases

Gas take shape of their container because they have negligible intermolecular forces of attraction having constant random motion and elastic collisions resulting gas particles spreading out occupying the shape of the container

Gas have low density when gas spread out in a container theres space between particles resulting in low density

• Density = mass/velocity

Can be compressed because the distance between particles is very large compared to the size of the particle themsleves

• increase oressure by reducing the distance

Exert pressure When they collide with themseleves and the walls of the container they exert pressure

due to the negligible intermolecular forces between prticles and they move in contious rnadom straight-line motion

affected by:

• amount of gas

• Container volume

• Temp inside container

Readily diffuse through other gases because gas particles are in constant random motion, negligible intermolecular forces of attraction, and the volume of individual gas particles is neglibile compared to the volume of the container.