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34 Cards in this Set
- Front
- Back
- 3rd side (hint)
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empirical formula
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simpliest whole number ration of element in the compound
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CH2O = 30 g/mol
m.f = 180 g/mol m.f = C6H12O6 |
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molecular formula
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exact # of atoms of each element in the compound
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percent composition
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mass of x in compound/formula weight of compound x 100%
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percent yield
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actual yield/theoretical yield x 100
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rate
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decrease in the conc. of reactant / time
or increase in conc. of product / time |
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rate determining step
(rate limiting step) |
slowest step in a proposed mechanism
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Rate Law
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for rxn aA+bB->cC+dD
rate = k[A]^x[B]^y k=rate constant x and y = rate order for nearly all forward, irreversible rxn, the rate is proportional to the product of the concentrations of the reactants each raised to some power |
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zero order rxn
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has constant rate which is independent of the reactants concentration
Rate = K (M/sec) |
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first order rxn
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radioactive decay
order=1 has rate proportional to the concentration of one reactant Rate=K[A] or k[B] (1/sec) |
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second order rxn
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has rate propotional to the product of concentration of two reactant or square of the concentration of single reactant
rate=k[A]^2 or k[A][B] |
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reactant concentration
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higher the concentration of reactant, more frequently particle came together thus higher chance of reacting.
Rate law inc as reactanc conc inc (except fo zero order) |
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temperature and rxn rate
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inc temp = inc rxn rate due to collisoin theory
rate of rxn will approximately double for each 10C inc higher T lead to higher K |
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collision theory
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molecule react only if smash with at least enough for bond to be broken
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catalysts (enzyme)
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speed up the rate determining step
inc the rate of chem rxn by lowering the activation energy does not being consumed |
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Equilibrium
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foward and reverse rxn rate is same
occur in closed sys, product is not allowed to escape molar concentration of reactants and products are not equal |
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equilibrium expression
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aA+bB <=> cC+dD
Keq = [C]^c[D]^d / [A]^a[B]^b = Kf/Kr |
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Properties of Keq
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1. pure solid and pure liquid do not appear in the equillibrium constant exp
2. in gase phase rxn, the partial pressure of the gas involved can be used instead of concentration 3. gas phase and aq phase take part in Keq |
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Keq = very large
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favors product
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Keq = very small
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favor reactant
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Keq = 1
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equal amount of reactants and products
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Qc =Keq
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rxn is equilibrium
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Qc > Keq
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rxn favors reactant
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Qc < Keq
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rxn favors product
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La Chatelier's principle
conc and stress |
1.if a stress is applied to a system at equilibrium the system will shift in such a way as to relieve the applied stress
2. change in concentration inc the concentration of a species will shift equilibrium away from the species added |
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La Chatelier's principle
pressure and volume |
not applicable to solid and liquid
change in pressure cuase change in volume if pressure inc, eq will shift so that the side of the exn producing fewer mole is favored if volume inc then pressure dec then lead to the shift in the eq to where more mole is present |
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La Chatelier's principle
temp |
A <=> B + heat (exo)
in ice bath, temp dec and drive rxn to the right to the heat loss boiling water, temp inc and drive to the left due to inc conc of heat |
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Ion Product = Ksp
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all the solid are dissolved
satuarated |
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Ion Product > Ksp
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supersaturated
not everything is dissolved see left of solute that didn't get dissloved |
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Ion Product <Ksp
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unsaturated
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difference btw aq phase and liquid phase
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aq phase is water phase
liquid phase it could be any liquid like mercury |
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catalyst will () the rate determining step
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speed up
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catalyst will () the activation energey of a reaction
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lower
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law of mass action equation is same thing as
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Keq
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according to the chemical kinetic theory
reaction can occur if |
1. reactant collide with proper orientation
2. reactant possess sufficient energy of colision 3. reactants are able to form a correct transistion state. |
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