Environmental Engineering Reference
In-Depth Information
d
C
(4-20)
Hg
kC
1
g
d
t
where
(4-21)
kkC
1
HCl
Natural logarithms were substituted on both sides, and the following formula was
derived:
d
C
(4-22)
Hg
ln
ln
k
ln
C
1
Hg
d
t
d
C
Thus, a straight line could be drawn from
to ln
C
Hg
. And
α
could
Hg
ln
d
t
thus be obtained from the slope of the line. Also,
k
1
could be obtained from the
linear intercept. In order to obtain the dependence of the reaction rate on HCl,
natural logarithms were substituted on both sides of Eq. (4-21) as follows:
(4-23)
ln
k
ln
k
ln
C
1
HCl
During the experiment, with excessive HCl concentration, it was changed to
obtain the values of
k
1
~
C
HCl
. A line could be drawn from ln
k
1
to ln
C
HCl
. Then,
β
could be obtained from the slope, and
k
could be obtained from the linear intercept.
This approach was shown in the literature.
The overall reaction rate constant could be expressed using the Arrhenius for-
mula as follows:
(4-24)
kA
exp(
ERT
/
)
a
where
E
a
is the energy activation;
A
is the preexponential factor;
R
is the gas con-
stant; and
T
is the gas temperature.
Natural logarithms were substituted on both sides and the following expression
was derived:
E
1
(4-25)
ln
k
ln
A
RT
A line could be drawn from ln
k
to 1/
T
to obtain the energy activation
E
a
and the
pre-exponential factor
A
of the adsorption reaction.
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