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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