Flashcards in Exam 2 Deck (58)
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1
see last deck for colligative properties
okayt
2
isotonic
concentration inside equals outside
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hypotonic
high concentrations of solute inside cell so water flows in
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hypertonic
concentration of solute is greater outside cell so it leaves
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suspension
particles settle out
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colloids
particles don't settle out
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surfactant
hydrophilic head with a hydrophobic tail
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monolayer
one layer of surfactant
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micelles
nonpolar tails surround with polar heads sticking out. helps dissolve stuff AKA soap
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vesicles
polar inside, non polar facing each other and then polar heads facing outside again
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cell membrane
phospholipid bilayer. polar phospholipid head with 2 lipid tails that are hydrophobic
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supersaturated solutions
more than can dissolve, very unstable
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reaction mechanisms
the pathway that the materials follow while becoming products. can be unimolec, with one reactant, bi with two tri with three
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elementary reaction
one step of a mechanism
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mechanism
has multiple elementary reactions
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intermediate
appears between steps and not in products
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reaction rate
number of molecules reacting per second.
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rate determining step
slowest elementary reaction
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rate units
molarity per second
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as you go on with reactions, rate
decreases as there are fewer reactant molecules present. fewer collisions occur. the rate per collision is constant
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High conc, hi molecules, hi collisions
hi rate
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Twice as many NO moles
number of collisions doubles compared to just NO one mol
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overall order
sum of exponents
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Rate laws mirror the reactions stoichiometry for
rate- limiting steps
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first order reaction
Ln(A0/A)= kt
ln of A vs t is straight
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second order reactiona
1/A-1/A0 = kt
graph of 1/a vs t gives a line with slope k
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zero order reactions
A= -kt+ A0
graph of A vs t gives a line
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slopes are equal to
k
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half life of first order reaction
ln2/K
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half life is independent of A0 in
first order reactions
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energy profile for unimolecular reactions
fragmentation is when the products is higher than reactants
rearrangement is when the energy rises but still releases
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energy profile for bimolecular reactions
energy rises then falls, still releases
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activated complex
AKA THE TRANSITION STATE. TOP O FTHE GRAPH
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RATE increases with
temperatrue
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Arrhenius equation
Ln (K2/K1) = - Ea/ R(1/t2 - 1/T1)
T in kelvin
R is 8.314 j since it is about activation energy!!
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catalysts
INCREASE RATES OF REACTION
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homo and hetero catalyst
same vs different phase of reactant
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in equilibrium
rates of forward and reverse reactions are equal NOT CONCENTRATIONS
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can be Keq or Kp
okay
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Keq
describes concenreatrions of reactants and products when the NET rate of reaction is zero
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Q
products over reactants. tells you which way equilibrium shifts
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when the reaction is reversed
K IS INVERSE NOT -VE
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converting between Kp and Kc
Kp= Kc (RT)^ delta N of gas
R is 0.0821
T in K
Delta n is # of moles of gas in products- number of moles of gas. can be -ve
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what is not in equilibrium
pure liquids and solids
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if K is huge
then reaction is basically completion
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if K is small
it basically doesn't occur
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increase in pressure
shifts to side with less gas moles
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K varies only with
temperature.
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what happens to k with for endothermic reaction when you add heat
K eq increases, shifts to produce less heat
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what happens to k with for exothermic reaction when you add heat
K eq decreases, shifts to side with less heat
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to prove X is negligble
put initial concentration over K and if its over 1000 , its negligble
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if K is very large
reaction goes to nearly completion so X is ALL final concentration
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strong acids
Her, HI, HCLO4, Hal, HNO3, N2SO4
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strong bases
group ! and 2 OH and CaOH, Sr OH and BaOh
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strong acids and bases K
dissociate. very large K
have Ka and Kb
make Oh or H3O
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solubility equilibrium
ksp
usually makes solid
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complexation equilibrium
Kf
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