Temperature

reflects the average kinetic energy of its constituent particles (atoms or molecules) relative to its center of mass.

Kelvin K

$C\degree = K+273$
0K -> Absolute Zero

Laws of gases

$$P\cdot V=nRT$$
where n, R is constant when mass is constant

Kinetic Theory of Gases

Molecules of a gas behave as identical (or all have the same mass)
Molecules of gas are hard, perfectly elastic spheres
The molecules are in continuous random motion
There are no forces of attraction or repulsion between the molecules
External forces (e.g. gravity) are ignored
Newton’s laws apply
The volume of the molecules is negligible compared to the volume of the container
The molecules collide perfectly elastically with the walls of the container exerting a pressure upon them
The time of a collision is negligible compared to the time between collisions
There are a very large number of molecules

  • Pressure in a gas is caused by the collisions of particles with the walls of the container
  • When the particles travel faster (e.g. at a higher temperature), they collide with walls more frequently
    • This means the gas exerts a greater pressure