Gases, Liquids, and Solids Flashcards
Definition of a Gas
Uniformly fills any container Mixes completely with any other gas Exerts pressure on its surroundings 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, but overall energy is constant
Collisions of particles with container walls cause pressure exerted by gas
Volume of individual particles is approximately zero
Particles exert no force on each other
Properties of an Ideal Gas
No volume No mass No molecular attraction High temperature Low pressure
Properties of a Real Gas
Have volume
Have mass
Have molecular attraction
How to make a real gas into an ideal gas
Increase temperature, because low temperature leads to slower particles, which means more attraction which makes it less like an ideal gas. Gas can be heated
Lower pressure, can be corrected by placing the gas in a bigger container, more volume, leads to lower pressure
Ideal/Universal Gas Law
PV=nRT P=Pressure V=Volume n=moles R=Proportionate Temperature (0.08206) T=Temperature(K)
Correcting Real Gas
[(Pobs +a((n/V)^2))]*[(V-nb)]=nRT
a=gas constant
b=gas constant
P=F/A
Pressure equals (Force divided by Area)
Relationship between temperature and number of effective collisions
The higher the temperature the more number of effective collisions due to higher probability.
Units of Pressure
kPA=kilo pascals mmHg=Milimeters of Mercury atm=atmospheric pressure torr=Same as mmHg, differnt name, based on absolute scale 1 atm =101.3 kPa 1 torr=1mmHg
Law of Partial Pressures
Pt=P1+P2…Pn
How to calculate values of partial pressure?
Use equations/fractions
Avogrado’s Hypothesis
Equal volume of gasses, at the same temperature and pressure have an equal amount of particles
STP
ST:(Standard Temperature)
SP:(Standard Pressure) 1 atm/101.3 kPa
1 mole of any gas has…
- 4L
6. 02*(10^23) particles
Same volume means…
Same amount of particles
Combined Gas Law
(P1V1)/(T1)=(P2V2)/(T2)
Boyle’s Law
PV=T
Temperature is constant
P1V1=P2V2
Inverse relationship between pressure and volume
Increase Pressure –> Decrease Volume
Decrease Pressure –> Increase volume
More accurate at low pressures, because acts more like an ideal gas
k
k is constant
Value is calculated when PV
PV=k
Charles’ Law
Linear Relationship Directly proportional Extrapolates to 0, at 0 K (V1/T1)=(V2/T2) V/T=k Increase volume --> Increase Temperature Decrease Volume --> Decrease Temperature
Definition of Diffusion
Describes the mixing of gases
The rate of diffusion is the rate of the gas mixing
Definition of Effusion
Describes the passage of gas into an evacuated chamber
Graham’s Law of Diffusion/Effusion
Rate of effusion of gas is inversely proportional tot he square root of the mass of the particles
Formula for Effusion
[(Sqrt(M2))/((Sqrt(M1))]
M1 and M2 are the rates of effusion of each gas
Substitute Molar Mass(GFM) for M1 and M2
Formula for Diffusion
[(Sqrt(M2))/((Sqrt(M1))]
M1 and M2 are the distances traveled by each gas
Substitute Molar Mass(GFM) for M1 and M2
Properties of Liquids
Stronger inter-molecular force compared to gases
Indefinite shape
Definite volume
All liquids evaporate at the surface
If temperature increases, the Kinetic Energy also increases, and the rate of evaporation also increases
Boiling Point of Liquids
When atmospheric pressure is equal to vapor pressure
Normal Boiling Point of Liquids
Boiling point of a liquid at standard pressure(1 atm/101.3 kPa)
How to find boiling points?
Look on Table H
Liquid with the weakest inter-molecular attraction of liquids is…
The one that takes the least amount of heat to boil
GFM
The Molar mass, calculated with Table S, using the masses of each element times the number of each element.
Surface Tension
The resistance of a liquid to increase its surface area
Capillary Action
The spontaneous rising of a liquid in a narrow tube
Definition of Viscosity
The resistance of a liquid to flow
Properties of Solids
Definite Shape
Definite Volume
Have the strongest inter-molecular force, out of all three phases of matter
Each molecule is in a fixed position, but they do vibrate
Have a crystalline structure with geometric patterns, when viewed under a microscope
Examples of crystalline solids
Atomic Solid
Ionic Solid
Molecular Solid
Amorphous Solids
Solids that lack ordered structure
Plastics and rubber
Super Cooled Liquids
Cooled to a rigid state, without crystallizing
Glass
