OIA1011 KINETIC THEORY OF GASES

Assumptions of Kinetic Theory

1. Gas has molecule of mass (m) and diameter (d) in endless random motion.

2. Size of gas molecules are negligible.

3. Molecules do not interact (neither attract nor repulse) except during collisions.

4. Elastic collision occurs between molecules. Energy may transfer between molecules, but total energy of all molecules remains same.

Pressure from Molecular Collisions

Gas pressure arises from collisions with container walls.

Formula for Gas Pressure

The equation links pressure with molecular speed.

Root Mean Square (RMS) Speed

speed dependent on temperature.

Effect of Temperature on Speed

Doubling T increases RMS speed by sqrt{2}.

Maxwell Distribution of Speeds

Not all molecules move at the same speed; higher T broadens distribution.

Real Gas Behavior

Intermolecular forces cause deviations from ideality.

Elastic Collisions

Energy transfer occurs during collisions, total system energy conserved.

Examples of Kinetic Theory

Explains phenomena like Brownian motion.

Applications in Pharmaceuticals

Aerosol particle dispersion utilizes principles of gas motion.