Chemistry Reference
In-Depth Information
Fig. 1.3
Evaluation of con-
version from DSC curve
Similarly, if the concentration of a reactant is available, it can easily be converted
to the conversion. For example, if the value of
C
varies throughout the reaction from
the initial value
C
0
to zero, the conversion is:
CC
C
0
α=
.
(1.6)
0
Isolating
C
from Eq. 1.6 and substituting the resulting expression into Eq. 1.3 leads
to:
d
d
α
n
(1.7)
= ′
kT
()(
1
−
α
) ,
t
where
k'
(
T
) =
C
0
n
− 1
k
(
T
). Equation 1.7 is the basic equation of homogeneous ki-
netics. Comparing it against Eq. 1.1 suggests that homogeneous kinetics can be
described by a simple reaction model:
(1.8)
n
f
() (
α
=−
1
α
) .
that is called a reaction-order model.
Fitting the rate to the reaction models may provide some clues about the reaction
mechanism. Fitting homogeneous kinetics data to a reaction-order model (Eq. 1.8)
and determining that
n
equals 1 or 2 suggests that the reaction is, respectively,
monomolecular or bimolecular. In heterogeneous kinetics, the situation is not nearly
as simple. There are dozens of heterogeneous reaction models that have been de-
rived under various mechanistic assumptions [
9
,
13
]. Such multitude of the models
arises from the need to describe the multitude of ways by which the spatially local-
ized reaction zone propagates throughout the reactants. The mathematical equations
and names of some models are collected in Table
1.1
. Figure
1.4
displays the model
dependencies of
f
(
ʱ
) on
ʱ
.
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