Chemistry 110 - Chapter 8: Gases
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These flashcards cover vocabulary and key concepts related to gases from Chemistry 110, Chapter 8.
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19 Terms
Monatomic
Gases consisting of single atoms, e.g., noble gases like He, Ne, Ar.
Diatomic
Gases consisting of two atoms, e.g., H2, N2, O2, F2, Cl2.
Kinetic-Molecular Theory
A model that describes the behavior of gas particles as conditions change, emphasizing continuous random motion.
Pressure
A measure of gas particle collisions against the walls of a container.
Volume
The amount of space that a gas occupies, equal to the volume of its container.
Temperature
A measure of the average kinetic energy of gas molecules, measured in Kelvin.
Boyle’s Law
The volume of a gas is inversely proportional to its pressure at constant temperature.
Charles’s Law
The volume of a gas is directly proportional to its absolute temperature at constant pressure.
Gay-Lussac’s Law
The pressure of a gas is directly related to its absolute temperature when volume is constant.
Avogadro’s Law
The volume of a gas is directly proportional to the number of moles of the gas at constant temperature and pressure.
Ideal Gas Law
The equation PV = nRT, relating pressure, volume, temperature, and number of moles in a gas.
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.
Molar Mass
The mass of one mole of a substance, used to convert mass to moles for calculations.
Standard Temperature and Pressure (STP)
Standard conditions defined as 0 °C (273 K) and 1 atm.
Barometer
An instrument used to measure air pressure.
Gas Constant (R)
In the ideal gas equation, R = 0.0821 L·atm/(K·mol), representing the proportionality between PV and nRT.
Kinetic Energy
The energy an object has due to its motion, significant in understanding gas behaviors.
Compressibility
The ability of a gas to decrease in volume when subjected to pressure.
Atmospheric Pressure
The pressure exerted by the weight of air in the Earth's atmosphere.