Chapter 10 and 11 Vocab
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55 terms
Terms | Definitions |
|---|---|
 kinetic-molecular theory | a theory that explains that the bahavior of physical systems depends on the combined actions of the molecules constituting the system |
| ideal gas | an imaginary gas whose particles are infinitely small and do not interact with each other |
| elastic collision | a collision between ideally elastic bodies in which the final and initial kinetic energies are the same |
| diffusion | the movement of particles from regions of higher density to regions of lower density |
| effusion | the passage of a gas under pressure through a tiny opening |
| real gas | a gas that does not behave completely like a hypothetical ideal gas because of the interactions between the gas molecules |
| fluid | a nonsolid state of matter in which the atoms or molecules are free to move past each other, as in a gas or liquid |
| surface tension | the force that acts on the surface of a liquid and that tends to minimize the area of the surface |
| capillary action | the attraction of the surface of a liquid to the surface of the solid, which causes the liquid to rise and fall |
| vaporization | the process by which a liquid or a solid changes to a gas |
| evaporation | the change of a substance from a liquid to a gas |
| freezing | the change of state in which a liquid becomes a solid as energy as heat is removed |
| crystalline solids | a solid that consists of crystals |
| crystal | a solid whose atoms, ions, or molecules are arranged in a definite pattern |
| amorphous solids | a solid in which the particles are not arranged with periodicity or order |
| melting | the change of state in which a solid becomes a liquid by adding energy as heat or changing pressure |
| melting point | the temperature and pressure at which a solid becomes a liquid |
| supercooled liquids | a liquid that is cooled below its normal freezing point without solidifying |
| crystal structure | the arrangement of atoms, ions, or molecules in a regular way to form a crystal |
| unit cell | the smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice |
| phase | in chemistry, one of the four states or condictions in which a substance can exist: solid, liquid, gas, or plasma; a part of matter that is uniform |
| condensation | the change of state from a gas to a liquid |
| equilibrium | in chemistry, the state in which a chemical reaction and the reverse chemical reaction occur at the same rate such that the concentrations of reactants and products do not change |
| equilibrium vapor pressure | the vapor pressure of a system at equilibrium |
| volatile liquids | a liquid that evaporates readily or at a low temperature |
| boiling | the conversion of a liquid to a capor wirhin the liquid as well as at the surface of the liquid at a specific temperature and pressure; occurs when the vapor pressure of the liquid equals the atmospheric pressure |
| boiling point | the temperature and pressure at which a liquid and a gas are in eqiulibrium |
| molar enthalpy of vaporization | the amount of energy as heat required to evaporate 1 mol of a liquid at constant pressure and temperature |
| freezing point | the temperature at which a solid and a liquid are in equilibrium at 1 atm pressure; the temperature at which a liquid substance freezes |
| molar enthalpy of fusion | the amount of energy as heat required to change 1 mol of a substance from solid to liquid at constant temperature and pressure |
| sublimation | the process in which a solid changes directly into a gas ( the term is sometimes also used for the reverse process) |
| deposition | the change of a state from a gas directly to a solid |
| phase diagram | a graph of the relationship between the physical state of a substance and the temperature and pressure of the substance |
| triple point | the temperature and pressure conditions at which the solid liquid, and gaseous phases of a substance coexist at equilibrium |
| critical point | the temperature and pressure at which the gas and liquid states of a substance become identical and form one phase |
| critical temperature | the temperature above which a substance cannot exist in the liquid state |
| critical pressure | the lowest pressure at which a substance can exist as a liquid at the critical temperature |
| pressure | the amount of force exerted oer unit area of a surface |
| newton | the SI unit for force; th force that will increase the speed of a 1 kg mass by 1 m/s each second that the force is applied (abbreviation, N) |
| barometer | an instrument that measures atmospheric pressure |
| millimeters of mercury | a unit of pressure |
| atmosphere of pressure | the pressure of Earth's atmosphere at sea level; exactly equivilent to 760 mm Hg |
| pascal | the SI unit of pressure; equal to the force of 1 N exerted over an area of 1 m^2 (abbreviation, Pa) |
| partial pressure | the pressure of each gas in a mixture |
| Dalton's law of partial pressures | the law that states that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases |
| Boyle's law | the law that states for a fixed amount of a gas at a constant temperature, the volume of the gas increaes as the pressure of the gas decreases and the volume of the gas decreases as the pressure of the gas increases |
| absolute zero | the temperature at which all molecular motion stops |
| Charle's law | `the law that states that for a fixed amount of gas at a constant pressure, the volume of the gas increaes as the temperature of the gas increaes and the volume of the gas decreases as the temperature of the gas decreases |
| Gay-Lussac's law | the law that states that the volume occupied by a gas at a constant pressure is directly proportional to the absolue temperature |
| combined gas law | the ralationship between the pressure, volume, and temperature of a fixed amount of gas |
| Gay-Lussac's law of combining volumes of gases | the law that states that volumes of gases involved in a chemical change can be represented by a ratio of small whole numbers |
| Avogadro's law | the law that states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules |
| ideal gas law | the law that states the mathematical relationship of pressure (p), volume (v), temperature (t), the gas constant (R), and the number of moles of a gas (n); PV=nRT |
| ideal gas constant | the proportionality constant that appear in the equation of state for 1 mol of an ideal gas |
| Graham's law of effusion | the law that states that the rate of effusion of a gas is inversely proportional to the square root of the gas's density |
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