Studied by 8 people
chemical kinetics
the area of chemistry that models reaction rates and why they diff
reaction rate
change in concentration/ change in time= rate
rate=
K[A]^n
rate
(mol/L(sec)
k
reaction constant
A
concentration of reaction
n
order of reactant, has to be determined experimentally
0 order
change is concertation, doesn’t affect reaction rate
1st order
prop change, double concertation, rate doubles
2nd order
exponential, double concentration, rate 4x
differential rate laws
concentration and rate data
integrated rate law
concentration and time data
integrated first order rate law
Ln[A]=-kt+Ln[A]o
integrated second order rate law
1/[A]=kt+1/[A]o
reaction mechanisms
series of proposal steps
integrated zero order rate law
-kt+[A]o
intermediates
substances produced in 1 step and consumed in another
elementary steps
a step in a reaction mechanism
molecularity
# of a species much react to cause a reaction
rate determining step
slowest step, write rate law based on the slowest step
collision model (critical for success)
activation energy, orientation
activation energy (Ea)
min amount of energy required in a collision for a reaction to occur
relationship of Ea
higher Ea means the reaction will go slower, few collisions will have the energy needed to overcome Ea
slowest has the highest Ea
catalyst
speeds up a reaction without being consumed
effects of catalyst
creates a new pathway
lowers activation energy
this results in a greater # of effective collisions
heterogeneous catalysts
pressed in a different phase
homogeneous catalysts
exists in the same phase- usually a solid
Note 
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