Properties of Substances and Deviations from the Ideal Gas Law

These flashcards cover key vocabulary and concepts related to properties of substances, particularly focusing on deviations from the Ideal Gas Law.

Ideal Gas Law

A theoretical gas law that describes the relationship between pressure, volume, temperature, and the number of moles of a gas.

Deviation from Ideal Gas Law

A situation where real gases do not behave according to the ideal gas law criteria due to intermolecular forces and volume.

High Pressure

Conditions under which gas particles can be significantly close to each other, causing deviations from ideal behavior.

Low Temperature

Conditions that slow down gas particles, leading to increased attractive forces between them.

Intermolecular Forces (IMF's)

Attractive forces between molecules that become significant in non-ideal gas behavior.

Boyle’s Law

A gas law that states the pressure of a gas is inversely proportional to its volume when temperature is held constant.

Real Gas

A gas that does not behave ideally and is affected by intermolecular forces and particle volume.

Pressure of Real Gases

The pressure of real gases is typically lower than that predicted by the ideal gas law due to intermolecular attractions.

Volume of Real Gases

The volume occupied by real gas particles is often greater than the volume of ideal gas particles.

Examples of Deviations

Real gases like CO2 and Ar exhibit deviations from ideal behavior under conditions of high pressure and low temperature.