11.1 kinetic molecular theory (KMT) with ideal gas approximation

26/5/25

law 1: particles in a gas will move..

in straight lines called translational motion until they collide elastically (with no energy or momentum lost) with other particles or sides of the container

law 2: temperature is a measure of..

the average kinetic energy (E_k = ½ mv²) of particles in a sample of matter

law 3: in an ideal gas, the volume of particles

is taken to be 0, they are modelled as a mathematical point.

law 4L in an ideal gas, there are..

no forces acting between particles, the kinetic energy of the particles overwhelms attraction, so attraction does not greatly affect particles

how do you increase kinetic energy?

add more kinetic energy or heat

acceleration

any change in speed, faster or slower, or any change in direction

what do the approximations of ideal gas laws break down?

these approximations will break down for real gasses at very low temperatures or at very high compression (pressure)

particles exert force on the sides of a container when they collide leading to this formula

pressure exerted by a gas = force / area

pressure = force / area

newtons (N) / m² = Pascal (Pa)