Chem-101 Chapter 11: Gases

Flashcards for reviewing key concepts from Chapter 11: Gases in a Chem-101 course.

What are the properties of gases?

Gases are compressible, assume the shape and volume of their container, and have low densities compared to liquids and solids.

What is the Kinetic Molecular Theory?

It describes the behavior of gas particles, stating they are small with large distances between them, act independently due to negligible intermolecular forces, move constantly in straight lines, and have average kinetic energy proportional to temperature.

Define Boyle's Law.

At constant temperature, the pressure of a gas is inversely proportional to its volume (P1V1 = P2V2).

What is the ideal gas law?

The ideal gas law is PV = nRT, where P is pressure, V is volume, n is number of moles, R is the ideal gas constant, and T is temperature.

What is Avogadro’s Law?

At constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of gas (V1/n1 = V2/n2).

What are units for pressure?

Common units for pressure include atmosphere (atm), pascal (Pa), pounds per square inch (psi), and millimeter of mercury (mm Hg).

What is Charles’s Law?

At constant pressure, the volume of a gas is directly proportional to its absolute temperature (V1/T1 = V2/T2).

What relationship does Gay-Lussac’s Law describe?

Gay-Lussac’s Law describes the direct proportionality between the pressure and temperature of a gas at constant volume (P1/T1 = P2/T2).

What is Dalton's Law of Partial Pressures?

The total pressure exerted by a mixture of gases equals the sum of the partial pressures of each gas in the mixture (Ptot = Pa + Pb + Pc + …).

What is STP?

Standard Temperature and Pressure (STP) is 0°C (273.15 K) and 1 atm, where 1 mole of an ideal gas occupies 22.4 L.