Chemistry: The Central Science - Chapter 10 Summary

These flashcards cover key concepts and definitions related to the properties and behaviors of gases as discussed in Chapter 10.

Characteristics of Gases

Gases expand to fill their containers, are highly compressible, and have extremely low densities.

Homogeneous Mixture

A mixture in which two or more gases are uniformly distributed.

Pressure (Definition)

Pressure is the amount of force applied to an area; atmospheric pressure is the weight of air per unit of area.

Standard Atmospheric Pressure

Normal atmospheric pressure at sea level, equal to 1 atm, 760 torr, or 101.325 kPa.

Boyle's Law

The volume of a fixed quantity of gas at constant temperature is inversely proportional to the pressure.

Charles’s Law

The volume of a fixed amount of gas at constant pressure is directly proportional to its absolute temperature.

Avogadro’s Law

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

Ideal-Gas Equation

The equation PV = nRT that relates the pressure, volume, temperature, and amount of gas.

Kinetic-Molecular Theory

A theory explaining the behavior of gases, stating that gases consist of large numbers of molecules in continuous motion.

Graham's Law

A law relating the molar mass of two gases to their rates of effusion or diffusion, stating lighter gases effuse or diffuse faster.

Real Gases

Gases that deviate from the ideal gas law under high pressure and low temperature conditions, where intermolecular forces and volume of gas molecules become significant.