AP Chemistry Kinetics
Terms
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 Rate law, general equation...

Rate = k([A]^x)([B]^y)([C]^z)
A,B, and C are REACTANTS  Reaction rate .....with increasing concentration of reactants because....

Increases
if there are more reactant molecules moving around in a given volume, then more collisions will occur  Reaction rate...... with increasing temperature because...

Increases
increase in temp means molecules move faster and greater avg kinetic energy.  Intermediates
 appear in mechanism but cancels out of the balanced equation
 Rate determining step is...
 the slowest step
 K(eq) =?
 K(f)/K(r)

first order:
x axis...
y axis...
slope... 
x axis...time
y axis...ln[A]
slope...k  zero order half life?
 = [A]0/2k

zero order:
x axis...
y axis...
slope... 
x axis...time
y axis...[A]t
slope...k  first order half life?
 = .693/k

Second order:
x axis...
y axis...
slope... 
x axis...time
y axis...1/[A]o
slope...k  half life of second order?
 = 1/(k[A]o)
 Arrhenius Equation
 k = Ae^(Ea/RT)
 from the arrhenius equation, or from the graph

lnk = (Ea/R)(1/T) + lnA
where, on the graph, it is lnk versus 1/T (xaxis) with a slope of Ea/R  Collision Theory

Sufficient kenetic/activation energy
and...proper orientation