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Glossary of AP Chemistry Kinetics

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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 (x-axis) with a slope of -Ea/R
Collision Theory
Sufficient kenetic/activation energy
and...proper orientation

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