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Chapters 6 and 7
Terms/ Concepts
64
Chemistry
Undergraduate 1
02/20/2007

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