Environmental Engineering Reference
In-Depth Information
can adsorb at very low partial pressures. At present, two types of
processes are proposed:
•
Adsorption into highly alkaline solutions (see
Box 11.3.3
) [11.10]
•
Adsorption onto solids [11.11,11.12]
The design of fl ue gas capture processes requires capture of 90% of
the inlet CO
2
; Direct Air Capture processes, however, are not subject to
Box
11.3.
3
Carbon capture with sodium hydroxide
In Chapter 5, we saw that adding a base to water will signifi cantly enhance the CO
2
solubility in the mixture because of the reaction of CO
2
with the hydroxide:
CO
2
+
NaOH
↔
Na
2
CO
3
+
H
2
O
This is a very exothermic reaction that is effi cient in capturing very small concentra-
tions of CO
2
. The idea is to use this process to capture CO
2
directly from the air.
Similar to capturing CO
2
from fl ue gasses using absorption, we need to regenerate
the solvent and compress the CO
2
for, say, geological sequestration.
The regeneration of sodium carbonate into sodium hydroxide is called caus-
ticization and is a well-known industrial process. The process involves three steps.
First, Na
2
CO
3
is reacted with lime, Ca(OH)
2
, to form NaOH and lime mud (CaCO
3
):
Na
2
CO
3
+
Ca(OH)
2
↔
2NaOH
+
CaCO
3
∆
H
100°C
=
−
5.3 kJ/mol CO
2
The calcium carbonate precipitates in this reaction and is subsequently calcined
(heated with air) to recover the CO
2
:
CaCO
3
↔
CaO(s)
+
CO
2
∆
H
900°C
=
179 kJ/mol CO
2
The CaO is converted back to Ca(OH)
2
through quicklime hydration:
CaO(s)
+
H
2
O
↔
Ca(OH)
2
,
∆
H
100°C
=
−65 kJ/mol CO
2
The enthalpy of absorption of CO
2
from air into sodium hydroxide solution for a 1 M
solution at standard conditions is -109.4 kJ/mol CO
2
. Hence, the minimum energy
to recover the CO
2
is also 109.4 kJ/mol CO
2
. We see that the calcination step
already takes 179 kJ/mol CO
2
, which indicates that the required energy for conven-
tional causticization is far beyond the thermodynamic minimum. Therefore, this
process consumes a large amount of energy.
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