KMT & Real/Ideal Gasses

Front

What is the Kinetic Molecular Theory (KMT)?

Back

The Kinetic Molecular Theory explains the behavior of gases in terms of particles in motion. It states that gas molecules are in constant, random motion and that their collisions are elastic, meaning no energy is lost.

Front

What are the characteristics of ideal gases?

Back

Ideal gases have no intermolecular forces, occupy no volume, and their collisions are perfectly elastic. They behave according to the ideal gas law (PV=nRT) under high temperature and low pressure.

Front

What happens to gas molecules at high temperatures?

Back

At high temperatures, gas molecules move faster, increasing their kinetic energy and leading to more frequent and energetic collisions.

Front

What is the relationship between pressure and volume in gases?

Back

According to Boyle's Law, at constant temperature, the pressure of a gas is inversely proportional to its volume (P1V1 = P2V2).

Front

What is the significance of elastic collisions in gases?

Back

Elastic collisions mean that when gas molecules collide, they do not lose kinetic energy. This is a key assumption in the Kinetic Molecular Theory.

Front

How do real gases differ from ideal gases?

Back

Real gases exhibit intermolecular forces and occupy space, especially under high pressure and low temperature, deviating from ideal behavior.

Front

What conditions favor ideal gas behavior?

Back

Ideal gas behavior is favored at high temperatures and low pressures, where intermolecular forces and molecular volume become negligible.

Front

What is the effect of increasing pressure on gas volume?

Back

Increasing pressure on a gas decreases its volume, as described by Boyle's Law, assuming temperature remains constant.

Front

What is the definition of absolute zero?

Back

Absolute zero is the theoretical temperature (0 Kelvin) at which all molecular motion stops, and a gas would have zero volume.

Front

What is Avogadro's Law?

Back

Avogadro's Law states that equal volumes of gases, at the same temperature and pressure, contain an equal number of molecules.