🔹 Meaning
The kinetic theory of gases states that gases are made up of tiny particles (molecules or atoms) which are in constant random motion. The behavior of gases is explained based on the motion and collisions of these particles.
🔹 Main Ideas of the Theory
Gas particles are very small.
They are far apart from one another.
They move freely and rapidly in all directions They collide with one another and with the walls of their container.
🔹 Assumptions (Postulates) of the Kinetic Theory of Gases
Gases molecules move randomly in straight lines colliding with one another r and with the walls of the container
Collisions between gas molecules and the walls of the container are perfectly elastic (no energy is lost)
The volume of the gas molecules is negligible compared to the volume of the container.
There are no forces of attraction between gas molecules.
The average kinetic energy of gas molecules is directly proportional to the absolute temperature.
Gas pressure is caused by the continuous collision of gas molecules with the walls of the container.
🔹 Explanation of Gas Properties Using Kinetic Theory
1. Pressure
Gas pressure is due to the collisions of gas molecules with the walls of the container.
2. Volume
Gases occupy the entire volume of their container because the molecules move freely.
3. Temperature
When temperature increases, gas molecules gain kinetic energy and move faster.
4. Diffusion
Gases mix easily because their particles move freely and randomly.
🔹 Limitations of the Kinetic Theory
It assumes gas molecules have no volume.
It ignores forces of attraction between molecules.
It does not apply well to real gases at high pressure or low temperature.
🧠 Important Tip
Increase in temperature leads to increase in the kinetic energy of gas molecules.
The study of the relationship between the variables above as regards the behaviour of gases studied by scientists like Boyle's, Charles, Avogadro's, Gay Lussacs, Grahams and Dalton. Each relationship is discussed in separate posts
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