Properties of Gases and Gas Laws

These flashcards cover fundamental principles, laws, and formulas related to the properties and behavior of gases, important for understanding gas laws in chemistry.

Kinetic Molecular Theory

The theory describing the behavior of gas particles, which states that they move rapidly and randomly, have negligible volume, and experience no attractive forces between them.

Pressure Formula

P = \frac{F}{A}, where P is pressure, F is force, and A is area.

Boyle's Law

For a given mass of gas at constant temperature, the product of pressure and volume is constant (P1V1 = P2V2), indicating an inverse relationship.

Charles's Law

For a fixed amount of gas at constant pressure, the volume of gas is directly proportional to its temperature in Kelvin (V1/T1 = V2/T2).

Gay-Lussac's Law

For a fixed volume and mass of gas, the pressure of the gas is directly proportional to its temperature in Kelvin (P1/T1 = P2/T2).

Avogadro's Law

Under the same conditions of temperature and pressure, equal volumes of gases contain an equal number of molecules.

Ideal Gas Law

The equation PV = nRT relates the pressure (P), volume (V), number of moles (n), and temperature (T) of a gas, with R as the ideal gas constant.

Dalton's Law of Partial Pressures

The total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas in the mixture.

Standard Temperature and Pressure (STP)

STP is defined as 1 atm pressure and a temperature of 273.15 K.

Common Pressure Conversions

1 atm = 760 mm Hg = 760 torr = 101,325 Pa = 14.70 psi.