Chapters 6 and 7 – Flashcards
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| DENSITY |
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| mass of a sample of matter divided by the volume of the ame sample. |
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| SHAPE, GAS |
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| depends on the physical state of matter. ____ always fills container completely. |
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| COMPRESSIBILITY |
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| change in volume of a sample resulting from a pressure change acing on th sample |
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| THERMAL EXPANSION |
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| change in volume of a sample resulting from change in the temperature of the sample. |
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| KINETIC ENERGY |
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| energy a particle has when it is in motion. KE=1/2 mv(squared) |
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| POTENTIAL ENERGY |
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| energy a particle has as a result of attractive or repulsive forces acting on it. |
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| COHESIVE ENERGY |
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| attractive force between particles; associated with potential energy. |
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| DISRUPTIVE FORCE |
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| force resulting between particles; associated with kinetic energy. |
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| GAS LAW |
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| mathematical relationship that describes behavior of gasses as they are mixed, subjected to pressure or temperature change, or allowed to diffuse. |
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| STANDARD ATMOSPHERE |
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| pressure needed to support a 760 mm column of mercury in a barometer tube. |
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| TORR |
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| pressure needed to support a 1 mm column of mercury in a barometer tube |
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| BOYLE'S GAS LAW; INVERSE; DECREASE |
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| gas law that describes pressure and volume behavior of gasses kept at constant temperature. PV=K Presuure and volume have a/an ___________ relationship.(increase pressure and then _________ volume) |
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| ABSOLUTE ZERO |
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| temperature at which all particle motion stops; a value of 0 on Kelvin scale. |
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| CHARLE'S LAW;proportional; increases |
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| gas law that describes temperature and volume behavior of gasses kept at constant pressure. V=k'T. Temperature and volume are ____________, increasung one __________ the other as long as the PRESSURE IS CONTANT. |
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| COMBINED GAS LAW |
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| gas law that describes pressure, volume and temperature behavior of gasses. PV/T=K. Combines elements of Boyle's and Charle's Laws. |
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| AVOGADRO'S LAW |
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| equal volume of gasses measured at the same temperature nad pressure contain equal number of molecules. The MASS would not be the same since each gas has a different molecular weight. |
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| STANDARD CONDITIONS (STP) |
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| specific temperature and pressure measurements chosen by chemists for gas measurements. |
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| STP=0 degrees celcius (273 K); 1.00 atm |
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| __________ standard temperature; __________ standard pressure |
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| IDEAL GAS LAW |
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| gas law that relates the pressure, volume temperature, and number of moles in a gas sample. PV=nRT (WITH pressure, volume, number of moles in the gas sample, universal gas constant and temperature respectively). |
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| UNIVERSAL GAS CONSTANT |
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| constant that relates pressure, volume, temperature, and number of moles of gas in the ideal gas law. |
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| DALTON'S LAW |
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| the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases in the mixture. |
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| PARTIAL PRESSURE |
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| the pressure an individual gas of a mixture would exert if it were in a container alone at the same temperature as the mixture. |
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| GRAHAM'S LAW |
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| relates rates of effusion or diffussion of two gasses to the masses of the molecules of the two gasses. |
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| EFFUSION |
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| process in which a gas escapes from a container through a small hole. |
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| DIFFUSSION |
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| process that causes gases to spontaneously intermingle when they are brought together. |
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| EVAPORATION. |
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| a change from liquid to gas state at temperatures below the boiling point. |
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| EVAPORATION AND VAPORIZATION |
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| are endothermic reactions that are the result of molecules leaving the surface of the liquid. |
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| CONDENSATION |
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| is an exothermic process in which gas or vapor is changed into a liquid or solid state. |
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| EQUILIBRIUM |
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| occurs when there are equal rates of evaporation and condensation resulting in the number of molecules in the vapor state remaining constant. |
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| VAPOR PRESSURE |
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| is the pressure exerted by vapor that is in equilibrium with its liquid. |
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| BOILING POINT |
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| temperature at which the vapor pressure of a liquid is equal to the prevailing atmospheric pressure resulting in a change to a gas state. |
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| NORMAL OR STANDARD BOILING POINT; LOWER |
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| is the temperature at which the vapor pressure of a liquid is equal to 1 standard atm (760 torr). At higher elevations where atmos[heric presure is lower, the boiling point is also _______. |
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| SUBLIMATION |
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| endothermic process in which a solid is changed directly into a gas without first becoming a liquid. |
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| MELTING POINT |
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| is the temperature at which a solid changes to a liquid; the solid and liquid has the same vapor pressure. |
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| DECOMPOSITION |
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| change in chemical composition that can result from heating. Ex. Cotton and paper char (decompose) rather than melt. |
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| STATES OF MATTER AND ENERGY |
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| energy is absorbed or released when matter is changed in temperature or changed from one state to another. |
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| SPECIFIC HEAT |
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| refers to the heat energy required to produce heat energy or "heat of fusion" if the change involves a change of state of matter. |
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| SOLUTION |
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| homogenous mixture of two or more substances in which the components are present as atoms, molecules, or ions. |
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| SOLVENT |
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| substance present in a solution in the largest amount. |
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| SOLUTE |
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| one or more substances present in a solution in amounts less than that of a solvent. |
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| DISSOLVING |
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| process of solution formation when one or more solutes are dispersed in a solvent to form a homogenous mixture. |
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| SOLUBLE SUBSTANCE |
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| substance that dissolves to a significant extent in a solvent. |
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| INSOLUBLE SUBSTANCE |
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| substance does not dissolve to a significant extent in a solvent. |
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| IMMIRSCIBLE |
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| liquids that are insoluble to each other. |
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| SOLUBILITY |
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| maximum amount of solute that can be dissolved in a specific amount of solvent under specific conditions of temperature and pressure. |
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| SATURATED SOLUTION |
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| solution containing the maximum amount possible of dissolved solute in a stable situation under the prevailing conditions of temperature and pressure. |
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| SUPERSATURATED SOLUTION |
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| unstable solution that contains an amount of solute temperature and pressure. |
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| HYDRATED ION |
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| ion in a solution that is surrounded by water molecules. |
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| SOLUTION PROCESS |
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| process of solvent molecules attracting the solute particles away from the solute crystal lattice. |
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| CONCENTRATION |
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| relationship between amount of solute and specific amount of solution in which it is contained. |
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| MOLARITY |
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| solution concentraion expressed in terms o the number of moles of solute/liters of solution. M=moles of solute/liters of solution. |
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| PERCENT |
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| solution concentration expressing amount of solute in 100 parts of solution. |
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| WEIGHT/WEIGHT PERCENT |
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| concentration expressing mass of solute contained in 100 mass units of solution. |
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| WEIGHT/VOLUME PERCENT |
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| concentration expressing grams of solute contained in 100 ml of solution. |
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| ELECTROLYTE |
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| solute that when dissolved in water forms a solution that conducts electricity. |
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| NONELECTROLYTE |
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| solute that when dissolved in water forms a solution that does NOT conduct electricity. |
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| COLLIGATIVE PROPERTY |
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| solution property that depends only on the concentration of solute particles in solution. Ex. boiling point, vapor point, freezing point |
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| OSMOTIC PRESSURE |
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| hydrostatic pressure required to prevent the net flow of solvent through a semipermeable membrane membrane into a solution. |
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| OSMOSIS |
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| process in which solvent flows through a semipermeable membrane into a solution |
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| COLLOID |
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| homogenous mixture of two or more substances in which the dispersed substances are present as larger particles than are found in solutions. |
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| DISPERSING MEDIUM |
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| substance present in a colloidal dispersion in the largest amount. |
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| DISPERSED PHASE |
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| substance present in a colloidal dispersion amounts less than the amount of the dispersing medium. |
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| TYNDALL EFFECT |
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| property of colloids in which the path of a beam of light through the colloid is visible because the light is scattered. |
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| EMULSIFYING AGENT OR STABILIZING AGENT |
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| substance added to some colloidst to prevent coalescing and setting. This is usually a coating agent to keep droplets separated and suspended in liquid. |
