Gases, Liquids, and Solids Flashcards
Definition of a gas
Uniformly fills any container Mixes completly with any other gas Exerts pressure on its surrondings Indefinite shape Indefinite volume
Kinetic Molecular Theory
All gases move in random, straight-line motion seperated by empty space
Collisions between gas particles may result in a transfer of energy, bu toverall energy remains constant
Collisions of particles with container walls cause pressure exerted by gas
Volume of individual particles is approximately zero
Particles exert no forces on each other
The amount of pressure is dependent on _____________
Amount of kinetic energy
The larger the volume becomes the more ________________ the volume of the gas becomes
Insignificant
Properties of an Ideal Gas
High temperature Low pressure No volume No masss No attractive force
Properties of a Real Gas
Have volume
Have mass
Have attraction of other particles
Ideal/Universal Gas Law
PV=nRT P=Pressure V=Volume n=moles T=Temperature R=Proportionate constant (.08206)
P=F/A
Presuure equals (Force divided by Area)
Effect temperature has on the probabilty of number of effective collisons.
The higher the temperature the higher the probability of effective collisions
GFM
Molar Mass
Molecular Mass
Formula weight
How to calculate GFM
Use periodic table to add up each element
Law of Partial Pressure
Pt=Pa+Pb
Use fractions/formula to solve for each value
Relationship between volume and number of particles
If they have the same volume (22.4), they have same number of particles and moles. 1 mole is (6.02*10^23)
Avogadro’s Hypothesis
Rqual volume of gases at the same temperature and pressure, have an equal amount of molecules
STP
Standard Temperature(ST) Standard Pressure(SP)
