Kinetic Molecular Theory
Gas particles are constantly doing this
Moving
A substance that takes the shape of its container
Fluid
Change from liquid to gas
Evaporation
Force exerted over a given surface area
Pressure
Law stating volume is inversely proportional to pressure
Boyle's Law
Collisions in gases conserve kinetic energy and are called these
Elastic collision
Force pulling outer, adjacent liquid particles together
Surface tension
Change from gas directly to solid
Deposition
Another name for mmHg
torr
Law stating volume is proportional to temperature
Charles's Law
Spontaneous mixing of substances due to random motion
Diffusion
Solid with particles arranged randomly
Amorphous solid (supercooled liquid)
Energy required to vaporize one mole of liquid
Molar enthalpy of vaporization
Sum of all partial pressures in a mixture is described by this law
Dalton's Law of Partial Pressures
Law stating pressure is proportional to temperature at constant volume
Gay-Lussac's Law
Temperature measures this property of gas particles
Average kinetic energy
Smallest repeating portion of a crystal lattice
Point where all three phases coexist
Triple point
SI unit equal to N/m²
Pascal
One mole of gas at STP occupies this volume
22.4 L
Movement of a gas through a tiny opening
Effusion
Type of crystal bonded through intermolecular forces
Covalent molecular crystal
Temperature beyond which a gas and liquid cannot be distinguished
Critical point
Standard atmospheric pressure in mmHg
760 mmHg
Equation relating pressure, volume, moles, and temperature
Ideal Gas Law