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Sarayu Jaladanki/Period 3 (solutions (Raoult's Law says that the the…
Sarayu Jaladanki/Period 3
gases
partial pressure can be found using mole fraction
charles law: V/T = V/T
Boyles Law: PV = PV
ideal gas law: PV = nRT
ideal gas has small particle size
KE is proportional to temperature
all collisions are elastic meaning all KE is saved
avagadros: V/n = V/n
KE = mv^2
KE = square root (3RT/M)
KE at a given temperature is the same however the velocity varies because is not the same
mean free path is because gas particles do not travel in a straight line due to collisions so this tells you how long before it collides
lighter gases travel faster than heavier ones
gases are affected by pressure and temperature
molar volume is the volume when there is one mole at STP
IMF
properties of the three phases
gases are least dense, no definite volume or shape and have weak IMF bonds
solids have strong IMF, and do not move around due to defined shape and volume
liquids move around a little but do not have defined shape but have a definite volume and medium IMF bond strength
phase diagrams usually have a positive fusion curve except for water because as pressure increases it favors liquids although others normally favor the denser state which is usually solid
triple point is when all three phases are in equilibrium
supercritical fluids have properties of both liquids and gases are good solvents and happen at critical temperature and pressure
water in liquid state does not go beyond 0 unless all solid has melted
bonds
london dispersion bonds are the weakest and happen between ALL molecules due to fluctuations of electrons
dipole - dipole are permanent dipoles that create bonds between the polarity of the molecules
hydrogen bonds are a type of dipole dipole bonds and happen between H and N, O, or F and are stronger
ion dipole occur between an ion and a polar molecule and this is the strongest of all
only gases are affected by pressure and increasing pressure can lead to liquid or decreasing heat
decreasing heat leads from liquid to solid
increasing heat or decreasing pressure leads from liquid to gas
the stronger the IMF bond the higher the melting and boiling point and in general solids and liquids have higher of both
solutions
solvent dissolves the solute
heat of a solution is the heat absorbed or released for specific amounts of solute dissolved
mixing to gases has more to do with entropy than attractions since ideally there are no attractions between them
if the solvent-solute interactions are greater than the solute-solute and solvent-solvent interactions then a solution forms but sometimes can form without these conditions being met
usually breaking of solute-solute and solvent-solvent bonds is endothermic and mixing is exothermic
solvent-solvent and mixing is called heat of hydration
if heat of hydration is greater than solute enthalpy then the process is exothermic and large
if the heat of hydration is less than the solute enthalpy then the process is endothermic
"like dissolves like"
there are amorphous and crystalline solids
saturation depends on temperature and more can be dissolved when the temperature is greater for solids
as temperature increases the amount of gas dissolved decreases but as pressure increases the solubility of a gas increases
Henry's Law says that the constant times the partial pressure of a gas gives you the solubility of the gas
colligative properties are ones where it doesn't matter what the gas just the number of particles
the vapor pressure decreases, freezing point lowers, boiling point increases, and osmotic pressure increases
for electrolyte solutions there are greater changes because more particles
Raoult's Law says that the the mole fraction of solvent times the partial pressure gives the pressure of the solution and if there is a volatile solvent and solute then you add both
when both are volatile this is an ideal solution
negative deviation from Raoult's law means that solvent and solute are similar and have strong bonds
positive deviation means that solute and solvent are dissimilar with weak attractions
solids can be dissolved better by stirring, heating, and grinding and gases can be by decreasing temperature and increasing pressure