Cliffs AP Chemistry, 3rd Edition

• Zero order: m= 0, rate is independent of the concentration of the reactant. Doubling the
  concentration of the reactant does not affect the rate.
  First order: m= 1, rate is directly proportional to the concentration of the reactant.
  Doubling the concentration of the reactant doubles the rate.
  Second order: m= 2, rate is proportional to the square of the concentration of the reactant.
  Doubling the concentration of the reactant increases the rate by a factor of 4.


• rate = ∆concentration∆time


• Arrhenius equation
  k =Ae-ERTa/
  where
  k = rate constant
  A = Arrhenius constant
  e = base of natural logarithm
  Ea= activation energy
  R = universal gas constant
  T = temperature (K)

lnk RTEaalnA lnkk ER TTTT

2

1

12

=- +=cm^12 -

logkAlog. RT

E

230

=-a

. R
slope E
230
= - a

logk.

k

R

E

TT

TT

230

a

1

2

12

21

= :

• ^

^

h

h

• ∆E = ΣEproducts−ΣEreactants

• collision theory: rate = f ⋅Z

where

Z = total number of collisions

f = fraction of total number of collisions that occur at sufficiently high energy for

reaction

Z = Z 0 [A]n[B]m

where

Z 0 = collision frequency when all reactants are at unit concentration

• ∆H = Ea−Ea'
  where
  Ea= forward reaction activation energy
  Ea' = reverse reaction activation energy

Part II: Specific Topics