Chapter 8: Gases

Kinetic Molecular Theory of Gases

A model for the behavior of a gas that helps us understand gas behavior.

Pressure (P)

The force exerted by a gas against the walls of the container.

Volume (V)

The space occupied by a gas.

Temperature (T)

The determining factor of the kinetic energy and rate of motion of gas particles.

Amount (n)

The quantity of gas present in a container.

Boyle’s Law

The pressure increases if volume decreases; pressure decreases if volume increases.

Charles’s Law

As temperature of a gas increases, its volume increases; if its temperature decreases, volume decreases.

direct

A _____ relationship is one in which the related properties increase or decrease together.

Gay-Lussac’s Law

As temperature of a gas increases, its pressure increases; if its temperature decreases, pressure decreases.

The Combined Gas Law

All of the pressure–volume–temperature relationships for gases combined into a single relationship.

Avogadro’s Law

If the moles of gas are increased, the volume must increase; if the moles of gas are decreased, the volume must decrease.

0 °C (273 K)

Standard temperature

1 atm (760 mmHg)

Standard pressure

Partial Pressure

It is the pressure it would exert if it were the only gas in the container.

Dalton’s Law

States that the total pressure of a gas mixture is the sum of the partial pressures of the gases in the mixture.

Boyle’s Law Formula

Charles’s Law Formula

Gay-Lussac’s Law Formula

Combined Gas Law

Avogadro’s Law Formula

Partial Pressure Formula