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Absorption of Nitric Oxide from Flue Gas
using Ammoniacal Cobalt(II) Solutions
by Hesheng Yu
Supervisor: Dr. Zhongchao Tan
2013-03-16
APRIL Group
1
Outline
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1. Background
2. Selection of Absorbent
3. Determination of Equilibrium Constants
4. Kinetic Study
5. Effect of Oxygen and Absorbent Regeneration
6. Mass Transfer in Industrial Gas-Liquid Contactors
7. Conclusions
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1. Background
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2.49 2.40
3.33 3.65 3.80 3.96 4.14
4.53
5.19 5.29 5.64
5.96
0
1
2
3
4
5
6
7
201020092008200720062005200420032002200120001999
Nit
rog
en
Oxid
es (
Mt)
Year
NOx Emissions from Conventional Power Plants in U.S., 1999-2010
Mobile Stationary
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Nitrogen Oxides Facts
Formula Name Nitrogen
Valence
Properties
N2O nitrous oxide 1 colorless gas
water soluble
NO
N2O2
nitric oxide
dinitrogen dioxide
2 colorless gas
slightly water soluble
N2O3 dinitrogen trioxide 3 black solid
water soluble, decomposes in water
NO2
N2O4
nitrogen dioxide
dinitrogen tetroixe
4 red-brown gas
very water soluble, decomposes in
water
N2O5 dinitrogen pentoxide 5 white solid
very water soluble, decomposes in
water
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NOx Hazards & Threats:
Tropospheric Ozone Acid Rain
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NOx Control Technologies
NOx Control
Technologies
Fuel Switching
Combustion
Modification
Flue Gas
Treatment (FGT)
Reduce nitrogen content
Less Excess Air
Staged combustion
Flue gas recirculation
Low-NOx burners
Water/steam injection
Selective catalytic reduction
Selective non-catalytic reduction
Combined plasma photolysis
Adsorption
Wet scrubbing
(not very realistic)
(20-70%)
Required to meet increasingly stringent
(<15ppm) emission regulation (cost-effective)
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Absorbent for Wet Scrubbing
Absorbent
Strong Oxidant
for conversion
NO into NO2
Reagent for
formation of a
nitrosyl complex
ClO2/NaClO2
KMnO4
O3
H2O2/ with NH3
FeSO4
Fe(II)-EDTA
Ammoniacal Cobalt(II) Ions
H2O2
Advantages of Ammonical Cobalt(II) Complexes:
Fast reaction
Positive effect of oxygen on NO absorption
Easy regeneration
Potential to simultaneously remove NO and SO2
Environmentally friendly by-products – Nitrate and nitrite
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Ammonia – Cobalt(II) System
(with concentrated ammonium)
Reaction Number
𝐶𝑜(𝐻2𝑂)62++𝑁𝐻3 ⇌ 𝐶𝑜(𝑁𝐻3)(𝐻2𝑂)5
2++𝐻2𝑂 (1-1)
𝐶𝑜(𝑁𝐻3)(𝐻2𝑂)52++𝑁𝐻3 ⇌ 𝐶𝑜(𝑁𝐻3)2(𝐻2𝑂)4
2++ 𝐻2𝑂 (1-2)
𝐶𝑜(𝑁𝐻3)2(𝐻2𝑂)42++𝑁𝐻3 ⇌ 𝐶𝑜(𝑁𝐻3)3(𝐻2𝑂)3
2++𝐻2𝑂 (1-3)
𝐶𝑜(𝑁𝐻3)3(𝐻2𝑂)32++𝑁𝐻3 ⇌ 𝐶𝑜(𝑁𝐻3)4(𝐻2𝑂)2
2++𝐻2𝑂 (1-4)
𝐶𝑜(𝑁𝐻3)4(𝐻2𝑂)22++𝑁𝐻3 ⇌ 𝐶𝑜 𝑁𝐻3 5(𝐻2𝑂)
2+ +𝐻2𝑂 (1-5)
𝐶𝑜(𝑁𝐻3)5(𝐻2𝑂)2+ +𝑁𝐻3 ⇌ 𝐶𝑜(𝑁𝐻3)6
2++𝐻2𝑂 (1-6)
𝑁𝐻𝟒+ ⇌ 𝑁𝐻3 + 𝐻+ (1-7)
Reactive Complexes
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Ammonia - Cobalt (II) System for different pH values at
T=30 oC
0
10
20
30
40
50
60
70
80
90
100
3.5 4.5 5.5 6.5 7.5 8.5 9.5 10.5 11.5 12.5
Perc
en
tag
e (
%)
pH value
Co2+
[CoA]2+
[CoA2]2+
[CoA3]2+
[CoA4]2+
[CoA5]2+
[CoA6]2+
CoA6
CoA5
CoA4
Co2+
CoA
A=NH3
[NH4+] = 2mol∙L-1
pH =7.5
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2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 6]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ + 2𝑁𝐻3 (1-8)
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 5]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ (1-9)
Light Yellow Pink or Red
Reactions of NO Absorption into Penta- and Hexa-
amminecobalt(II) solutions
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2. Selection of Absorbent
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Experimental Setup for Absorbent Selection
Scrubbing bottle
Water Jacket
Column Reactor
Valve 5
Valve 3
Valve 4
Valve 2
Valve 1
Beaker
Testo 350 XL
Mixer Connector
NO O2 N2
Mass flow meters
Thermostatic Bath
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Comparison of NO Reduction between Different Absorbents
Hydrogen Peroxide
Fe(II)-EDTA
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40
50
60
70
80
90
100
0 15 30 45 60 75 90 105 120
NO
Rem
ova
l (%
)
Time (min)
19
35
50
Inlet flow rate = 500ml/min,
NO = 500 ppm, O2 = 5.0%, pH = 10.5, Cobalt (II) = 0.06 mol∙L-1
Effect of Temperature on NO Removal Efficiency
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3. Determination of Equilibrium
Constants
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Laboratory Setup for Equilibrium Study
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Picture of Main Section of Testing Rig
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Validation of Complex Reactivity – NO Absorption Curve
99.65%
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Validation of Complex Reactivity – Colour Change
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 6]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ + 2𝑁𝐻3 (3-1)
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 5]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ (3-2)
Light Yellow Pink or Red
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Brief Calculation of Equilibrium Constants
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 6]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ + 2𝑁𝐻3 (3-1)
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 5]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ (3-2)
[Co(NH3)5-6]2+
e is given by mass balance of cobalt(II)
where aw = water activity; fNH3 = the activity coefficient of the ammonia;
Gm = molar flow rate, mol∙s-1
KNO5 = the equilibrium constant of Reaction 3-1, L3∙mol-3;
KNO6 = the equilibrium constant of Reaction 3-2, L3∙mol-3;
PT = total pressure, atm;
yin, yout = NO concentration at inlet and out, ppm;
η = NO removal efficiency
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𝑙𝑛𝐾𝑁𝑂5 = 3598.5 ∙
1
𝑇+ 16.759 (R2=0.994) (3-3)
𝑙𝑛𝐾𝑁𝑂6 = 1476.4 ∙
1
𝑇+ 26.597 (R2=0.970) (3-4)
𝐾𝑁𝑂5 = 1.90 × 107exp(
3598.5
𝑇) (3-5)
𝐾𝑁𝑂6 = 3.56 × 1011exp(
1476.4
𝑇) (3-6)
Rewritten as,
where KNO5 --- the equilibrium constant of Reaction 3-1, L3∙mol-3;
KNO6 --- the equilibrium constant of Reaction 3-2, L3∙mol-3;
T --- temperature, K
Equilibrium Constants of Reactions (3-1) and (3-2)
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4. Kinetic Study
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Double-Stirred Tank Reactor
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Laboratorial Setup for Kinetic Study
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Picture of actual laboratorial setup for kinetic study
(a) flue gas simulation system (b) double stirred tank section
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𝑁𝑁𝑂 = (1
𝐻𝑘𝐺+
1
𝐷𝑁𝑂2
𝑚 + 1𝑘𝑚𝑛5 𝐵5
𝑛𝑐𝑁𝑂𝑖𝑚−1 +
2𝑝 + 1
𝑘𝑝𝑞6 𝐵6
𝑞𝑐𝑁𝑂𝑖𝑝−1
)−1𝑐𝑁𝑂𝑖 (4-3)
According to film theory and enhancement factor for parallel reactions, the rate of NO
absorption into ammoniacal cobalt(II) solutions, presented in Reactions 4-1 and 4-2, can
be described as follows:
where NNO --- NO absorption rate, mol∙m-2∙s-1; H --- Henry Law constant, L∙atm∙mol-1; kG --- gas-phase mass transfer coefficient, mol∙s-1∙m-2∙atm-1;
DNO --- molecular diffusivity of NO in liquid phase, m2∙s-1;
m, n, p, q, reaction orders with respect to reactant;
k --- reaction rate, unit is dependent upon reaction orders
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 6]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ + 2𝑁𝐻3 (4-1)
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 5]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ (4-2)
Calculation Scheme
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Determination of Reaction Order with regard to NO
m=p=1 can be given by the obvious
linear relationship between NNO and cNOi
as shown in the figure. Therefore,
substituting of m=p=1 into Eq. 4-3 gives
𝑘1𝑛5 𝐵5
𝑛 + 𝑘1𝑞6 𝐵6
𝑞=
𝑐𝑁𝑂𝑖𝑁𝑁𝑂
−1
𝐻𝑘𝐺
−2
𝐷𝑁𝑂(4−4)
𝑁𝑁𝑂 = (1
𝐻𝑘𝐺+
1
𝐷𝑁𝑂2
𝑚 + 1𝑘𝑚𝑛5 𝐵5
𝑛𝑐𝑁𝑂𝑖𝑚−1 +
2𝑝 + 1
𝑘𝑝𝑞6 𝐵6
𝑞𝑐𝑁𝑂𝑖𝑝−1
)−1𝑐𝑁𝑂𝑖 (4-3)
Y
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Determination of Reaction Orders with regard to Penta- and
Hexa-amminecobalt(II) Solutions
The value of reaction rate decreases
with temperature
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(a) (b)
Analysis of Reaction Orders with respect to Penta- and Hexa-
amminecobalt(II) Solutions
𝑐𝑁𝑂𝑖𝑁𝑁𝑂
−1
𝐻𝑘𝐺
−2
𝐷𝑁𝑂−𝑘2
6𝐵6 = 𝑘25𝐵5(4−5)
𝑐𝑁𝑂𝑖𝑁𝑁𝑂
−1
𝐻𝑘𝐺
−2
𝐷𝑁𝑂−𝑘2
5𝐵5 = 𝑘26𝐵6(4−6)
Y
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5. Effect of Oxygen and
Regeneration
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Laboratory Setup
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Effect of Oxygen on NO Absorption into Ammonical
Cobaltous Solutions
0%
5.6%
2.1%
8.7%
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Proposed Scheme for NO Absorption with Presence of Oxygen
Hentaaminecobalt(II)
Pexaaminecobalt(II)
Nitrosylpentaamminecobalt(III)
(1b)
μ-peroxo-bis[pentaamminecobalt(III)]
(2b)
O2
O2
NO
NO
Cobalt peroxynitrite
intermediate
2b
Cobalt peroxynitrito
Nitrate
and/or
Nitrite
O2
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Proposed Scheme for NO Absorption with Presence of Oxygen
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 6]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ + 2𝑁𝐻3 (5-1)
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 5]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ (5-2)
Conclusion:
For continuous feed of flue gas into ammoniacal cobalt(II) system, Reactions 5-1 and 5-
2 are in fact irreversible with the existence of oxygen. The presence of oxygen
significantly improves the NO absorption into ammoniacal cobaltous complexes. The
final NO absorption amount into the ammoniacal absorbent is entirely dependent upon
the original absorbent concentration regardless of nitric oxide and oxygen
concentration. This finding corresponds with our experimental results.
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Regeneration Tests of Different Additives at Various
Temperatures
Without KI at RT
With KI at RT
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Regeneration Tests of Different Additives at Various
Temperatures
Without KI at 52 oC
With KI at 52 oC
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Performance of Combination of AC and Na2S5O8
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Performance of Combination of AC and KI
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6. Mass Transfer in Industrial
Gas-Liquid Contactors
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Experimental Setup of the Gas-Liquid Contactor System
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Effect of Impeller Speed on Degassing Efficiency in GIAT and
CSTR
CSTR: conventional
stirred tank reactor
GIAT: gas-inducing
agitated tank
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Effect of Purge Nitrogen Flow Rate on Degassing Efficiency in
CSTR and BC
CSTR: conventional
stirred tank reactor
BC: bubble column
(Porous media)
(Multiorifice)
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Degassing Efficiency of the Semi-batch Degasser at Different
Conditions
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7. Conclusions
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Conclusions:
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 6]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ + 2𝑁𝐻3 (3-1)
2𝑁𝑂 + 2[𝐶𝑜 𝑁𝐻3 5]2+⇌ 𝐶𝑜 𝑁𝐻3 5𝑁2𝑂2 𝑁𝐻3 5𝐶𝑜
4+ (3-2)
𝑙𝑛𝐾𝑁𝑂5 = 3598.5 ∙
1
𝑇+ 16.759 (R2=0.994) (3-3)
𝑙𝑛𝐾𝑁𝑂6 = 1476.4 ∙
1
𝑇+ 26.597 (R2=0.970) (3-4)
The reaction rate constants of Reactions 3-1 and 3-2 are calculated based on the
enhancement factor derived for gas absorption accompanied by parallel chemical reactions.
Both reactions are first order with respect to NO and first order with respect to liquid
absorbent. The forward reaction rate constants of Reactions 3-1 and 3-2 are 6.43×106
and 1.00×107 L∙mol-1∙s-1, respectively at 298.15 K, and increase to 7.57×106 and
1.12×107 L∙mol-1∙s-1, respectively at 303.15 K.
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Proposed Scheme for NO Absorption with Presence of Oxygen
Hentaaminecobalt(II)
Pexaaminecobalt(II)
Nitrosylpentaamminecobalt(III)
(1b)
μ-peroxo-bis[pentaamminecobalt(III)]
(2b)
O2
O2
NO
NO
Cobalt peroxynitrite
intermediate
2b
Cobalt peroxynitrito
Nitrate
and/or
Nitrite
O2
Conclusions:
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Conclusions:
Liquid-phase mass transfer coefficient for different reactors
Conventional stirred tank reactor 𝑘𝐿𝑎𝐶 = 1.59𝑁𝐼𝑁𝑐𝑑
1.342
𝑈𝐺0.93(
𝑑𝑇𝑑𝐼)0.415
Gas-inducing agitated tank 𝑘𝐿𝑎𝐺𝐼 = 1.212𝑃𝑐𝑉𝐿
0.0816
(𝑄𝐼
𝑑𝑇2)
0.692(𝑠
𝑑𝑇)−0.390
Bubble column with efficient gas sparger 𝑘𝐿𝑎𝐵 = 1.091𝑈𝐺0.8
Bubble column with simple gas sparger 𝑘𝐿𝑎𝐵𝑑𝑇
2
𝐷𝐿= 0.6(
𝜈𝐿𝐷𝐿)0.5(
𝑔𝑑𝑇2𝜌𝐿𝜎𝐿
)0.62(𝑔𝑑𝑇
3
𝜈𝐿2 )0.31𝜀𝐺
1.1
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Acknowledgement
Dr. Zhongchao Tan
Dr. Mark J.Rood
Dr. Xianguo Li
Dr. John Z. Wen
Dr. Eric Croiset
Dr. Qunyi Zhu
Dr. Guangyuan Xie
Dr. Sudong Yin
Grace Pan
Chao Yan
Harry Lei
Ke Zhang
Zhe Li
Stephen Kuan
Raheleh
Fang Liu
2013-03-16
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ENGINEERING 50