Another postulate of the kinetic molecular theory is that gas particles are always in motion, like the other states of matter. But they are different in that they undergo random translational movement.
In solids, the particles mainly experience vibrational motion and in liquids they mainly vibrate and rotate, with some translational motion. Gas particles move rapidly in straight lines, unless acted upon by another particle or the walls of a container. This continuous contact with the container leads to our understanding of gas pressure, the number of collisions over a certain amount of area.As per the KMT, an ideal gas should travel rapidly in a random, yet constant speed.
In reality, gas particles do follow the assumption lead by the KMT. In extreme cases, when factors like temperature and pressure change, gases deviate from their ideal behaviour. The basis of the previous postulate, leads us to the next postulate that states that the speed of the gas particles varies accordingly to temperature. In a gas the particles are in ever changing kinetic energy, but when the speed is averaged, it becomes proportional to absolute temperature.
As the absolute temperature of a gas increases, the particles inside the gas experience more thermal energy. This leads to more kinetic energy, causing the particles to move faster and further apart. When the absolute temperature is reduced, the thermal energy is also reduced, leading to lower kinetic energy. The particles begin to move slower, minimizing the distance between them, resulting in them getting closer together.
As the temperature approaches absolute zero (-273 ? ‘oC), the particles slow down, eventually coming to complete stop.Gases, out of all the states of matter behave very uniquely. One of this behaviour is the ability to fill a container equally and completely. Gases can accomplish this task because of their constant motion, their elastic collision and the fact that there are no forces acting between the particles.
The main reason the gases fill their allotted containers is because of their collision between the particles, which occurs quickly. These collisions occur quite promptly after entering a container due to the fact that the particles are in rapid motion.The fact that the collision are elastic, means that the kinetic energy between particles are not lost (ideal gases), increasing the efficiency of the distribution. Also due the neutral polarity of the particles, the circulation of particles is not hindered.
This expandability property of gases is closely tied with its diffusion of particles. Diffusion is labelled as the movement of particles from areas of high concentration to areas of low concentration. The diffusion of gas particles is very similar to the expandability since in both they end with the particles spread evenly throughout the container.This means that the diffusion process is also caused by the gases constant rapid velocity, their perfectly elastic collisions and their neutrally charged particles.
An example of diffusion would be when someone wearing a strong perfume walked into a classroom. At first the perfume smell would only surround the person wearing it, but as time continues the smell diffuses throughout the classroom. Eventually the smell is evenly distributed around the classroom.