 
Summary: Basics of Chemical Kinetics  1
Rate of reaction = rate of disappearance of A =
# of moles of A reacting ("disappearing") per unit time per unit volume
rA = d[A] /dt =
[A] = concentration of A = (# moles/volume) ; 1 mole = 6.023x1023 molecules
rA = k [A] rA = k [A]2 rA = k1 [A]/(1+k2[A])
Reaction rate law is an algebraic equation involving concentrations
(not a differential equation)
For a given reaction, the rate law is determined experimentally
Measure [A] as a function of time and calculate slope (d[A]/dt) at
various time points.
oductPrA
Basics of Chemical Kinetics  2
In general : rA = k(T)ˇf ([A],[B],...)
Temperature
dependence
Concentration
dependence
Rate Constant
(Not really "constant", just
