General Chemistry 102 - Gases

These flashcards cover key vocabulary and concepts related to gases in General Chemistry 102, including gas laws, properties, and related theories.

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 (in Kelvin).

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 Law

An equation of state for an ideal gas, expressed as PV = nRT, where P is pressure, V is volume, n is moles, R is the gas constant, and T is temperature in Kelvin.

Dalton's Law of Partial Pressures

The total pressure of a mixture of gases equals the sum of the pressures that each would exert if present alone.

Kinetic Molecular Theory

A model that explains the behavior of ideal gases based on the assumptions of fast-moving particles in constant motion with negligible volume and no intermolecular forces.

Standard Temperature and Pressure (STP)

Standard reference conditions defined as 0°C (273 K) and 1 atmosphere (101.3 kPa) for gas calculations.

Gas Mixture

A combination of two or more gases that do not react chemically and each behaves independently.

Absolute Temperature

Temperature measured on a scale where 0 is the absolute minimum (0 Kelvin); important for gas law calculations.

Pressure (P)

The amount of force exerted per unit area; for gases, is often measured in atmospheres (atm), torr, or pascals (Pa).

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 (in Kelvin).

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 Law

An equation of state for an ideal gas, expressed as PV = nRT, where P is pressure, V is volume, n is moles, R is the gas constant, and T is temperature in Kelvin.

Dalton's Law of Partial Pressures

The total pressure of a mixture of gases equals the sum of the pressures that each would exert if present alone.

Kinetic Molecular Theory

A model that explains the behavior of ideal gases based on the assumptions of fast-moving particles in constant motion with negligible volume and no intermolecular forces.

Standard Temperature and Pressure (STP)

Standard reference conditions defined as 0°C (273 K) and 1 atmosphere (101.3 kPa) for gas calculations.

Gas Mixture

A combination of two or more gases that do not react chemically and each behaves independently.

Absolute Temperature

Temperature measured on a scale where 0 is the absolute minimum (0 Kelvin); important for gas law calculations.

Pressure (P)

The amount of force exerted per unit area; for gases, is often measured in atmospheres (atm), torr, or pascals (Pa).

Boyle's Law Formula

P1 V1 = P2 V2

Charles's Law Formula

\frac{V1}{T1} = \frac{V2}{T2}

Gay-Lussac's Law

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

Gay-Lussac's Law Formula

\frac{P1}{T1} = \frac{P2}{T2}

Avogadro's Law Formula

\frac{V1}{n1} = \frac{V2}{n2}

Combined Gas Law Formula

\frac{P1 V1}{T1} = \frac{P2 V2}{T2}

Dalton's Law Formula

P{\text{total}} = P1 + P2 + P3 + \dots

Graham's Law of Effusion Formula

\frac{\text{Rate}1}{\text{Rate}2} = \sqrt{\frac{M2}{M1}}, where M is the molar mass.

Ideal Gas Law for Density

d = \frac{P M}{R T}, where d is density and M is molar mass.

Root Mean Square Speed (v_{\text{rms}})

v_{\text{rms}} = \sqrt{\frac{3RT}{M}}, which calculates the average speed of particles based on temperature and molar mass.