Chemistry Reference
In-Depth Information
(1.20)
−
1
− −
=+
1
1
,
k
k
k
ef
D
where
k
ef
,
k,
and
k
D
, respectively, are the effective, reaction, and diffusion rate con-
stants. Assuming that
k
and
k
d
obey the Arrhenius temperature dependence, we can
derive the effective activation energy of the overall process as follows
ER
k
T
d
d
ln
Ek Ek
kk
+
+
=−
=
ef
D
D
,
(1.21)
ef
−
1
D
where
E
and
E
D
are the activation energies of the reaction and diffusion. In Eq. 1.21,
E
D
can be reasonably well approximated by the activation energy of viscous flow
[
37
]. Because both
k
and
k
D
vary with temperature,
E
ef
should generally vary with
temperature taking the values between
E
and
E
D
. Figure
1.11
displays the respec-
tive temperature dependence of
E
ef
estimated under assumption that
E
D
is typically
smaller than
E
. Equation 1.21 also suggests that
E
ef
can be constant in two special
cases. First, when diffusion is much faster than the reaction (
k
D
>>
k
) the process
is said to occur in the reaction regime, and the value of
E
ef
=
E
. Second, when the
process occurs in the diffusion regime (
k
>>
k
D
) then
E
ef
=
E
D
. The effect of diffu-
sion is equally important for reactions of solids such as decomposition or oxidation
when escape of a gaseous product or delivery of gaseous reactant can be controlled
by diffusion through a solid product formed on the surface of a solid reagent [
38
].
All in all, we should recognize that strong intermolecular interactions encoun-
tered in condensed-phase media generally affect a single reaction step to such extent
that its kinetics depends on the reaction medium properties and the energy barrier
varies as these properties change with conversion and/or temperature. Furthermore,
a single reaction step can be complicated by additional steps such as diffusion.
Then the kinetics of the overall process that involves a reaction and diffusion step
becomes driven by two energy barriers. The temperature dependence of such pro-
Fig. 1.11
Temperature varia-
tion of the effective activation
energy of a process, whose
overall rate is determined by
the rate of both diffusion and
reaction (Eq. 1.20)
E
ef
= E
E = E
D
T
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