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32 Cards in this Set
 Front
 Back
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) 