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Definition
| mass of a sample of matter divided by the volume of the ame sample. |
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Definition
| depends on the physical state of matter. ____ always fills container completely. |
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Definition
| change in volume of a sample resulting from a pressure change acing on th sample |
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Definition
| change in volume of a sample resulting from change in the temperature of the sample. |
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Definition
| energy a particle has when it is in motion. KE=1/2 mv(squared) |
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Definition
| energy a particle has as a result of attractive or repulsive forces acting on it. |
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Definition
| attractive force between particles; associated with potential energy. |
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Definition
| force resulting between particles; associated with kinetic energy. |
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Definition
| 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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Definition
| pressure needed to support a 760 mm column of mercury in a barometer tube. |
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Definition
| pressure needed to support a 1 mm column of mercury in a barometer tube |
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Term
| BOYLE'S GAS LAW; INVERSE; DECREASE |
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Definition
| 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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Term
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Definition
| temperature at which all particle motion stops; a value of 0 on Kelvin scale. |
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Term
| CHARLE'S LAW;proportional; increases |
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Definition
| 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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Term
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Definition
| 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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Term
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Definition
| 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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Term
| STANDARD CONDITIONS (STP) |
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Definition
| specific temperature and pressure measurements chosen by chemists for gas measurements. |
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Term
STP=0 degrees celcius (273 K);
1.00 atm |
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Definition
__________ standard temperature;
__________ standard pressure |
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Term
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Definition
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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Term
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Definition
| constant that relates pressure, volume, temperature, and number of moles of gas in the ideal gas law. |
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Term
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Definition
| 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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Definition
| 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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Term
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Definition
| relates rates of effusion or diffussion of two gasses to the masses of the molecules of the two gasses. |
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Definition
| process in which a gas escapes from a container through a small hole. |
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Definition
| process that causes gases to spontaneously intermingle when they are brought together. |
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Term
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Definition
| a change from liquid to gas state at temperatures below the boiling point. |
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Term
| EVAPORATION AND VAPORIZATION |
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Definition
| are endothermic reactions that are the result of molecules leaving the surface of the liquid. |
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Term
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Definition
| is an exothermic process in which gas or vapor is changed into a liquid or solid state. |
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Term
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Definition
| 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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Term
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Definition
| is the pressure exerted by vapor that is in equilibrium with its liquid. |
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Term
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Definition
| 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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Term
| NORMAL OR STANDARD BOILING POINT; LOWER |
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Definition
| 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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Term
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Definition
| endothermic process in which a solid is changed directly into a gas without first becoming a liquid. |
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Term
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Definition
| is the temperature at which a solid changes to a liquid; the solid and liquid has the same vapor pressure. |
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Term
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Definition
| change in chemical composition that can result from heating. Ex. Cotton and paper char (decompose) rather than melt. |
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Term
| STATES OF MATTER AND ENERGY |
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Definition
| energy is absorbed or released when matter is changed in temperature or changed from one state to another. |
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Term
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Definition
| 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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Term
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Definition
| homogenous mixture of two or more substances in which the components are present as atoms, molecules, or ions. |
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Term
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Definition
| substance present in a solution in the largest amount. |
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Term
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Definition
| one or more substances present in a solution in amounts less than that of a solvent. |
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Term
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Definition
| process of solution formation when one or more solutes are dispersed in a solvent to form a homogenous mixture. |
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Term
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Definition
| substance that dissolves to a significant extent in a solvent. |
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Term
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Definition
| substance does not dissolve to a significant extent in a solvent. |
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Term
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Definition
| liquids that are insoluble to each other. |
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Term
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Definition
| 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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Term
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Definition
| 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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Term
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Definition
| unstable solution that contains an amount of solute temperature and pressure. |
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Term
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Definition
| ion in a solution that is surrounded by water molecules. |
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Term
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Definition
| process of solvent molecules attracting the solute particles away from the solute crystal lattice. |
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Term
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Definition
| relationship between amount of solute and specific amount of solution in which it is contained. |
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Term
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Definition
| 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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Term
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Definition
| solution concentration expressing amount of solute in 100 parts of solution. |
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Term
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Definition
| concentration expressing mass of solute contained in 100 mass units of solution. |
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Term
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Definition
| concentration expressing grams of solute contained in 100 ml of solution. |
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Definition
| solute that when dissolved in water forms a solution that conducts electricity. |
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Definition
| solute that when dissolved in water forms a solution that does NOT conduct electricity. |
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Definition
| solution property that depends only on the concentration of solute particles in solution. Ex. boiling point, vapor point, freezing point |
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Term
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Definition
| hydrostatic pressure required to prevent the net flow of solvent through a semipermeable membrane membrane into a solution. |
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Term
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Definition
| process in which solvent flows through a semipermeable membrane into a solution |
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Term
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Definition
| 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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Term
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Definition
| substance present in a colloidal dispersion in the largest amount. |
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Term
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Definition
| substance present in a colloidal dispersion amounts less than the amount of the dispersing medium. |
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Term
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Definition
| 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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Term
| EMULSIFYING AGENT OR STABILIZING AGENT |
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Definition
| substance added to some colloidst to prevent coalescing and setting. This is usually a coating agent to keep droplets separated and suspended in liquid. |
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