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# Chem 113- Unit 1

four controllable factors for reaction rate concentration, physical state, temperature, catalyst
initial rate rate (t=0) = Δ[A]/Δt
zero order rate=k
first order rate=k[A]
second order rate=[A]^2
overall reaction order the sum of all reaction orders
first order integrated rate law ln[A]t=-kt+ln[A]0
second order integrated rate law 1/[A]t=kt+1/[A]0
zero order integrated rate law [A]t= -kt +[A]0
Arrhenius equation K=Ae^(-Ea/RT)
Arrhenius equation (for T1/T2) ln (k2/k1)= (-Ea/R)(1/T2-1/T1)
ΔH (rxn)= Ea(fwd)-Ea(rev)
if temp is held constant... higher Ea= lower f
if Ea is held constant... higher temp= higher f
transition state symbolized by the activation state-> could go back to reactants or to products
reaction intermediates created and used up in elementary steps
unimolecular (elementary step) first order, rate=k[A]
bimolecular (elementary step) 2nd order, rake=k[A]^2
termolecular (elementary step) ***not likely to occur 3rd order, rate=k[A]^3
rate determining step (RDS) highest energy step; slowest step
Created by: melaniebeale