12 terms

Chem: Chapter 7 - Gas Laws

Scientific Law
A statement that describes what scientists expect to happen every time under a particular set of conditions
Scientific Theory
A well-tested explanation for a wide range of observations and experimental results
Kinetic Molecular Theory of Ideal Gases
1 Particles are small points in "empty" space
2 No attractions between particles
3 Particles are in constant motion
4 Particles move randomly
5 Collisions between particles are elastic
Boyle's Law
For For a given mass of a gas at constant temperature, volume varies inversely with pressure. P1xV1 = P2xV2
Charles' Law
For a given mass of a gas at constant pressure, volume varies directly with KELVIN temperature.
Gay-Lussac's Law
For a given mass of a gas at constant volume, as the temperature varies directly with pressure inside the container.
Combined Gas Law
the product of the volume and pressure of an ideal gas divided by its temperature is constant
Ideal Gas Law
Gas Law equation used for stoichiometry and when conditions are not at STP. The four variables are pressure (P), volume (V), number of mole of gas (n), and temperature (T) and the "Gas Constant" (R)
Dalton's Law of Partial Pressures
The total pressure of a mixture of gases is equal to the sum of all the pressures of all of the gases in the mixture.
Partial Pressure
The pressure independently exerted by a single gas when that gas is in a mixture of two or more gases.
What is the SI unit for pressure?
Graham's Law of Effusion
the rate of effusion of a gas is inversely proportional to the square root of the mass of its particles