Environmental Engineering Reference
In-Depth Information
y
obs
X
1
+
k
decay
θ
y
x
=
.
(6.248)
As an illustration of the above equation, we shall choose the special case when
k
decay
=
0. Other relevant parameters are chosen for a typical bacteria (
E. coli
) found
in wastewater plants:
K
s
=
15 mg/L,
μ
max
=
25 d
−
1
,
y
X
=
0.6, and [S]
in
=
15 mg/L.
Figure 6.68 displays the change in [X] and [S]
∗
as a function of the mean residence
time,
θ
, in the reactor.
It should be mentioned that the above equations only predict the steady-state behav-
ior. In actual operation, the unsteady state should be considered whenever the system
experiences changes in influent concentrations. There will then exist a lag time before
the substrate consumption and microbial growth approach a steady state. The micro-
bial growth lags by several
θ
values before it adjusts to a new [S]
in
. This is called the
hysteresis effect
.
It is also useful to consider here the competition for a substrate S between an organ-
ism that utilizes it and other competing complexation processes within the aqueous
phase. Consider Figure 6.69. While an enzymatic reaction of species S (an inorganic
metal, for example) occurs via complexation with a cellular enzyme (denoted E), a
competing ligandY in the aqueous phase may bind species S. The cellular concentra-
tion of species S is determined by a steady state between cell growth (division) and
the rate of uptake of S. If [S]
cell
denotes the cellular concentration of S (moles/cell)
and
is the specific growth rate (d
−
1
)
, then the rate of cell growth is
r
cell
= μ
[S]
cell
.
From the reaction scheme in Figure 6.69, the uptake rate of species S is given by
r
uptake
=
μ
k
E
[S]
tot
[E]
tot
, which is the rate of reaction of species S with the enzyme
ligand E. This necessarily assumes that the enzyme is in excess of the concentration
E
E
Aqueous phase
Cell
E
k
-Y
(Fast)
E
SE
S
SY
k
E
(slow)
k
Y
(Fast)
k
uptake
(Fast)
E
(Quasi-equilibrium)
E
r
=
k
E
[S][E]
E
FIGURE 6.69
Kinetics of competing biological uptake and complexation in the aqueous
phase. (Adapted from Morel, F.M.M. and Herring, J.G. 1993.
Principles and Applications of
Aquatic Chemistry
, NewYork: Wiley.)
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