States of Matter and Gas Laws chapter 7

These flashcards cover key concepts from the lecture on the states of matter, gas laws, and related thermodynamics.

Three States of Matter

The three states are gas, liquid, and solid, each defined by unique properties including shape, volume, and particle arrangement.

Boyle’s Law

States that the pressure of a gas is inversely proportional to its volume when temperature and the amount of gas are constant.

Charles’s Law

States that the volume of a gas is directly proportional to its Kelvin temperature at constant pressure.

Gay–Lussac’s Law

States that the pressure of a gas is directly proportional to its Kelvin temperature at constant volume.

Avogadro’s Law

States that the volume of a gas at constant temperature and pressure is directly proportional to the number of moles of gas.

Ideal Gas Law

Combines pressure (P), volume (V), number of moles (n), and temperature (T) into the equation PV = nRT.

Intermolecular Forces

Attractive forces between molecules that affect properties like boiling/melting points and state of matter.

Vapor Pressure

Pressure exerted by vapor in equilibrium with its liquid phase; increases with temperature.

Viscosity

Measure of a fluid's resistance to flow, influenced by intermolecular forces.

Specific Heat

Amount of heat energy required to raise the temperature of 1 gram of a substance by 1°C.

Boiling Point

Temperature at which a liquid's vapor pressure equals the external pressure.

Heat of Fusion

The amount of energy needed to convert a solid into a liquid at its melting point.

Heat of Vaporization

The amount of energy required to convert a liquid into a gas at its boiling point.