Ch 6 gases, solutioms, colloids, and suspensions

solids

matter with a fixed volume and shape

liquids

matter with a fixed volume, indefinite shape. takes on the shape of the container

gases

matter with indefinite shape and volume takes on both the shape and volume of the container

heat of fusion

amount of heat required to melt a solid

heat of vaporiztion

amount of heat required to evaporate a liquid

deposition

gas to solid

sublimation

slid to gas

atmospheric pressure

pressure of column of air above and around the earth’s surface. extends 32 km above sea level

STP - standard temperature and pressure

temp= 0C

pressure = 1atm

pressure

force per unit area

pounds per square inch (psi)

pounds of pressure exerted on the walls of the gas container per square inch of wall area

millimeters of mercury (mm Hg)

pressure exerted by air on column of Hg in barometer

Torr

pressure exerted by 1mm Hg at 0C

atmosphere (atm)

pressure exerted by a 760 mm column og Hg at 0C

pascal (Pa)

pressure exerted by a film of water 0.1 mm high on the service beneath

bar

=105 Pa

almost equal to atm

barometer

device used to measure atmospheric pressure

manometer

device used to measure pressure in a closed system

vapor pressure

the maximum pressure exerted by a gas formed by evaporation of a liquid. increases with increasing temperature

boiling point of a liquid

the temperature at which the vapor pressure of the liquid equals the atmospheric pressure

autoclaveis

a device used to sterilize intruments/solutions

blood pressure

the pressure that blood exerts or the walls of blood vessels

120

systolic pressure

80

diastolic pressure

hypotension

low blood pressure

hypertension

high blood pressure

boyles law

for a gas at a fixed temperature; pressure and volume are inversely proportional

P1V1=P2V2

gay-lussac’s law

states that for a sample of gas with a constant volume; pressure and temperature are directly related

P1/T1=P2/T2

Charles law

for a sample of gas at a fixed pressure; volume and temperature are directly related

V1/T1=V2/T2

avogodros law

at a given temperature and pressure, volume and the number of moles of gas are directly related

V1/n1=V2/n2

combined gas law

the name says it all

P1V1/T1=P2V2/T2

ideal gas law

states that for any gas, pressure times volume divided by number of moles times temperature is constant

PV=nRT

partial pressure

if two ideal gases are mixed they each exert the same pressure it would if it were alone in the container

dalton’s law of partial pressure

the total pressure of a mixture of gases is the sum of the partial pressures of its components

Ptotal= PA+ PB+ PC

pure substance

one element or compound

mixture

combination of two or more pure substances

homogenous mixture

uniform distribution

solution

uniform molecular mixture

solvent

component in greater amount

solute

component in lesser amount dissolves in solvent

heterogenous mixture

mixture that is not evenly distributed

precipitate (ppt)

a solid reaction product

soluble

two substances dissolve in one another

insoluble

two substances do not dissolve in one another

henrys law

solubility of a gas in a liquid is proportional to the pressure of the gas over the liquid

concentration

the amount of solute dissolved in a solvent

parts per thousand (ppt)

1 X 103

parts per million ppm

1 X 106

parts per billion ppb

1 X 109

molarity M

moles/L

equivalent

number of moles of charges that one mole of a solution contributes to solution

dilution

addition of more solvent to reduce the concentration of solute

V1C1=V2C2

solution

small < 1nm, clear, cannot be separated by filtration or centrifugation

colloid

intermediate 1nm-1micro meter, usually cloudy, particles may be seperated by special filtration or centrifugation

suspension

large > 1micro meter, cloudy, particle setting, seperated by filtration or centrifugation