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32 Cards in this Set
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Pressure

Defined as the force per unit area on a surface
caused by collisions 
Pascal

defined as the pressure exerted by a force of one newton acting on an area of one square meter

newton

the force that will increase the speed of a one kilogram mass by one meter per second each second it's applied

millimeter of mercury

unit of pressure
symbolized mm Hg 
barometer

device used to measure atmospheric pressure

atmosphere of pressure

(atm) defined as being exactly quivalent to 760mm Hg

ideal gas

an imaginary gas that perfectly fits all the assumptions of the kineticmolecular theory

kineticmolecular theory (4 constants)

based on the idea that pa rticles of matter are always in motion
1) gases consist of large #s of tiny particles that are far apart 2) elastic collisions 3) constant, rapid, random motion 4) no forces of attraction or repulision (weak dispersion forces) 
real gas

a gas that does not behave completely according to the assumptions of the kineticmolecular theory

fluid

gas particles glide easily past one another
liquids and gases that flow 
elastic collision

 collisions between gas particles and between particles and container walls are elastic collisions
 no net loss of kinetic energy 
effusion

a process by which gas particles under pressure pass through a tiny opening

ideal gas constant

R= 0.0821 (L X atm / mol X k)
the constant R 
diffusion

spontaneous mixing of the particles of two substances caused by their random motion

ideal gas law

PV= nRT
R= 0.0821 L atm/ mol K the mathematical relationship of P,V,T and mols 
standard molar volume of a gas

the volume ocupied by one mole of a gas at STP
found to be 22.4 L 
Avogadro's Law

states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

GuyLussac's law of combining volumes of gases

states that at cosntant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers

Graham's law of effusion

R1 radical MW2
R2= radical MW1 
Boyle's law

V1P1=V2P2
(n,T) 
Charle's law

V1T2=V2T1

vaporization

the process by which a liquid or solid changes to a gas

expansion

process of diffusion to where a gas fills its container

mm > atm

divide by 760

C > K

+ 273

standard temperature and pressure

scientists have agreed on standard conditions of 1 atm pressure and 0 degrees C
STP 
absolute zero

 273. 15 degrees C
given a value of zero on the kelvin scale 
gas laws

simple mathematical relationships between the volume, temperature, pressure, and quantity of a gas

partial pressure

preesure of each gas in a mixture

Guy Lussac's law

T12=T21

Dalton's law of partial pressures

Pt= p1 + p2 +p3

combined gas law

V1P1T2=V2P2T1
(n) 