Biomedical Engineering Reference
In-Depth Information
One can find that
#-C-moles of X that could be formed
#-C-moles of CO
n
CO
¼
0:036
n
X
C
mole X
YF
X
=
CO
¼
¼
1
C
mole CO
C
mole X
¼ 0:036
C
mole CO
or
Mass of X that coule be produced
Mass of CO
¼
n
X
M
X
YF
X
=
CO
¼
n
CO
M
CO
¼
0:036 ð12:011 þ 1:8 1:00794 þ 0:5 15:9994 þ 0:2 14:00674Þ
1 ð12:011 þ 15:9994Þ
kg-X
kg-CO
kg-X
kg-CO
¼ 0:03165
One can observe that the yield factor is different when different basis (C-mole or kg) is
used. For the yield factor of oxygen, we have
#-moles of O
2
that could be consumed
#-C-moles of CO
¼
n
O
2
n
CO
¼
0:0068
mole O
2
YF
O
2
=
CO
¼
1
C
mole CO
mole O
2
¼ 0:0068
C
mole CO
or
Mass of O
2
that could be consumed
Mass of CO
¼
n
O
2
M
O
2
n
CO
M
CO
YF
O
2
=
CO
¼
¼
0:068 ð2 15:9994Þ
1 ð12:011 þ 15:9994Þ
kg-O
2
kg-O
2
kg-CO
kg-CO
¼ 0:007768
3.8. REACTION RATES NEAR EQUILIBRIUM
Figure 3.2
shows the Gibbs free energy variation during a chemical reaction. Nonequilib-
rium thermodynamics stipulates that the flux of change is governed by the change of Gibbs
free energy, i.e. Eqn
(3.52)
for a reaction,
k
e
DG
f
=RT
e
DG
b
=RT
r
¼
(3.52)
where
D
G's change with the contents of the reaction mixture, temperature, and other
conditions.
More theoretically founded, in thermodynamics, we learned how to describe the compo-
sition of molecules in chemical equilibrium. For the generalized single reaction
X
N
S
n
j
A
j
¼ 0
(3.14)
j
¼1
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