What are the 5 Kinetic Theories of Gases?

What are the three main points of the Kinetic theory of gases?

• When molecules collide, there is no loss or gain of energy
• The molecules in a gas take up little space in relation to the container they are in
• The molecules are always moving in a straight line

Assumptions of Kinetic theory of gases:

• Gas molecules are constantly moving in random directions
• Gas molecules travel in a straight line
• Gas molecules are tiny compared to the distance between them, and the volume of the molecules is negligible
• Average Kinetic energy is dependent on absolute temperature
• During the random motion of molecules, there will be elastic collisions
• The motion of gas molecules is based on Newton’s laws of motion
• The time interval of collision between any two molecules is minimal

5 Kinetic theory of gases:

• Gas is made up of numerous molecules that move at random
• Intermolecular interactions are negligible
• Collisions between molecules and between molecules and container walls are always elastomeric
• The average kinetic energy of all molecules is temperature-dependent
• Gas molecules are tiny compared to the distance between them, and the volume of the molecules is negligible

Factors affecting the behaviour of gas molecules:

• Temperature(T)
• Volume(V)
• Pressure(P)
• Number of molecules(n)

Formulas based on Kinetic theory of gases:

• Total Kinetic energy of the gas:

• RMS Speed:

• Boltzmann constant:

• Pressure of gas:

Applications:

• Boyle’s law: Pressure(P) of the gas is inversely proportional to the volume(v) at constant temperature(T) i.e.P ∝ 1v

• Charle’s law: Volume(v) is directly proportional to the temperature(T) at constant pressure(P) i.e.v ∝ T

• Gay Lussac’s Law: Pressure(P) is directly proportional to the temperature(T) at constant volume(v) i.e.P ∝ T

Conclusion