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CRChem1CH10Vocabulary (new book)

spontaneous mixing of the particles of two substances due to their random motion diffusion
process by which gas particles pass through a tiny opening effusion
collision between gas particles and container walls in which there is no net loss of kinetic energy elastic collision
substance that can flow and therefore take the shape of its container; a liquid or gas fluid
imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory ideal gas
based on the idea that the particles of matter are in constant motion kinetic-molecular theory
gas that does not behave completely according to the assumptions of the kinetic-molecular theory real gas
the attraction of the surface of a liquid to the surface of a solid capillary action
process by which particles escape from the surface of a nonboiling liquid and enter the gas state evaporation
physical change of a liquid to a solid by removal of heat freezing
force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface area to the smallest possible size surface tension
process by which a liquid or solid changes to a gas vaporization
solid in which the particles are arranged randomly amorphous
substance in which the particles are arranged in an orderly, geometric, repeating pattern crystal
total three-dimensional arrangement of particles of a crystal crystal structure
solid made up of crystals crystalline
physical change of a solid to a liquid by the addition of heat melting
temperature at which a solid becomes a liquid melting point
substances that retain certain liquid properties even at temperatures at which they appear to be solid supercooled liquids
smallest portion of a crystal lattice that slows the three-dimensional pattern of the entire lattice unit cell
the conversion of a liquid to a vapor within the liquid as well as at its surface boiling
the temperature at which the equilibrium vapor pressure of the liquid equals the atmospheric pressure boiling point
the process by which a gas changes to a liquid condensation
indicates the critical pressure and critical temperature critical point
the lowest pressure at which the substance can exist as a liquid at the critical temperature critical pressure
temperature above which the substance cannot exist in the liquid state critical temperature
change of state of a gas directly to a solid deposition
dynamic condition in which two opposing changes occur at equal rates in a closed system equilibrium
the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature equilibrium vapor pressure
temperature at which a solid and liquid are in equilibrium at 1 atm of pressure freezing point
when a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress LeChatlier's principle
amount of heat energy required to melt one mole of solid at its melting point molar enthalpy of fusion
amount of heat energy needed to vaporize one mole of liquid at its boiling point molar enthalpy of vaporization
any part of a system that has uniform composition and properties phase
graph of pressure versus temperature that shows the conditions under which the phases of a substance exist phase diagram
change of state from a solid directly to a gas sublimation
indicates the temperature and pressure conditions at which the solid, liquid, and vapor of a substance can coexist at equilibrium triple point
liquids that evaporate readily volatile
Created by: CRMissK