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Understanding the Influence of the Alkaline Cation K+ or Na+ in
the Regeneration Efficiency of a Biogas Upgrading Unit.
Francisco M. Baena-Moreno a,b *, Mónica Rodríguez-Galán a, Fernando Vega a, T. R.
Reina b, Luis F. Vilches a, Benito Navarrete a.
a Chemical and Environmental Engineering Department, Technical School of
Engineering, University of Seville, C/ Camino de los Descubrimientos s/n, Sevilla
41092, Spain
b Department of Chemical and Process Engineering, University of Surrey, GU2 7XH
Guildford, United Kingdom
*Corresponding author.
E-mail address: [email protected] (Francisco M. Baena-Moreno)
Abstract
This paper reveals a regeneration method for a carbonate compound after carbon
dioxide (CO2) absorption in a biogas upgrading unit run with caustic mixtures, obtaining
precipitated calcium carbonate (PCC) as valuable by-product. This process arises as
an alternative to physical regeneration, which is highly energy intensive. This work
provides novel insights on the regeneration efficiency of carbonates to hydroxides while
also studying the influence of K+ or Na+ in the caustic CO2-trapping solution. The
compared parameters were the reaction time, temperature and molar ratio. Moreover,
psychochemical characterization of solids was obtained by means of Fourier-transform
infrared spectroscopy (FTIR), Raman spectroscopy, X-ray powder diffraction (XRD)
and Scanning Electron Microscopy (SEM) images. The results indicate that
regeneration efficiencies are slightly lower when potassium is used instead of sodium,
but quite acceptable for both of them. The chemical characterization experiments
showed the predominance of calcium carbonate. Overall, the results obtained in this
1
study proved that this process is feasible to upgrade biogas through PCC precipitation,
which appears to be a promising economically viable process to synergise CCS and
CCU.
Keywords
Carbon Capture and Utilization; Biogas Upgrading; Precipitated Calcium Carbonate;
Caustic Absorption; Biomethane Production;
1. Introduction
Our environment is seriously affected by climate change, carried out largely by human
action. In addition, the future shortage of conventional energy sources requires greater
use of renewable energy [1,2]. Within this context, biogas is one of the most promising
sources of renewable energy, having increased the existing number of biogas
processing plants in recent years considerably (Figure 1). Biogas is obtained through
the anaerobic digestion of biomass [3]. Regarding biogas composition, it is mainly
composed by methane (CH4) and carbon dioxide (CO2), in an approximate percentage
of 60% and 40% respectively [4–6]. After a complete upgrading for CO2 removal,
biomethane is obtained from biogas as a valuable product [7]. Biomethane uses
include heat or electricity production, natural gas substitute, compressed natural gas
and diesel replacement alongside liquid natural gas after a compression stage [8–10].
Due to this variety of applications, biogas upgrading technologies have been studied by
multiple researchers, chemical absorption being one of the most propitious due to the
high CO2 capture efficiency of this process. Solvents typically employed for this
process are monoethanolamine (MEA), piperazine (PZ), sodium hydroxide (NaOH) or
potassium hydroxide (KOH) [11–14]. Even though promising results have been found
2
by the employment of amines, nowadays there are some disadvantages discussed by
the scientific community. Some examples are the toxicity produced by the amine
degradation through the formation of nitrosamine as a potential carcinogenic
compound and the high regeneration cost in the stripping step [12,15–17]. Also the use
of caustic solvents requires an elevated energy consumption to regenerate the solvent
via temperature increase [12,17,18]. However, NaOH and KOH present advantages of
being cheaper, having a greater theoretical CO2 capture capacity and their availability
in the industry market [19].
0
4000
8000
12000
16000
20000
Number of plants
2010 2011 2012 2013 2014 2015 20160
2000
4000
6000
8000
10000
Year
Total installed capacity (MW)
Figure 1. Number of biogas processing plants and total installed capacity [8,20].
For this reason, previously an alternative path for solvent regeneration was proposed
by our group [13], which resulted to be much less energy intensive and economically
attractive due to the production of a valuable by-product. A general scheme of the
process can be seen in Figure 2. In brief, NaOH was employed as a CO2 capture agent
to form sodium carbonate (Na2CO3), according to reaction (1). In order to make the
process economically appealing, a regeneration of Na2CO3 via chemical reaction with
3
calcium hydroxide (Ca(OH)2) was chosen to generate precipitated calcium carbonate
(PCC) (reaction (2)). PCC is demanded as raw material in several applications, such as
for example in paper industry, polymers applications and as a neutralizer in healthcare
[21–23].
2NaOH ( aq )+CO2 (g )→+Na2CO3+H 2O (1)
Na2CO3 ( aq )+Ca (OH )2(s)→2NaOH ( aq )+CaCO3(s) (2)
High regeneration efficiencies as promising results for further investigations were
achieved. Since KOH was proven to have improved CO2 absorption compared to
NaOH [24,25], in this paper a characterization of regeneration efficiencies in a
precipitation reactor for this novel method is presented. Hence, in this work novelty
data regarding the comparison between both cations is presented, which have not
been found in the literature. For the collection of these inputs, the purpose of this study
was to analyze the differences between regeneration efficiencies and psychochemical
composition of both NaOH and KOH, with the intention to investigate the effect of
potassium ion in comparison with sodium. Potassium ion may have an enhancement
effect into the regeneration efficiencies, as well as in the purity of final PCC. The
chemical reaction carried out if reflected by reaction (3).
K2CO3 (aq )+Ca (OH )2(s)→2KOH (aq )+CaCO3(s) (3)
4
Figure 2. Bio-waste to PCC production and biogas upgrading process.
The key variables studied were the reaction time, the reaction temperature, and the
molar ratio between Ca(OH)2 and K2CO3 (R), since these variables were proved to
have an effect on the reaction rate [13,26,27]. Inasmuch as in the previous work [13] an
exhaustive characterization of these reaction parameters was done. However, in this
paper a selected number of tests were chosen to investigate the potassium ion effect.
2. Materials and Methods
2.1 Materials
PanReac-AppliChem supplied the reagents employed in this work (Ca(OH)2, Na2CO3,
K2CO3, CaCO3) in a pure-pharma grade (99% purity).
2.2 Regeneration experiments
5
The methodology was explained in detail in [13]. Firstly, both the carbonate aqueous
solution and hydroxide slurry were prepared. Secondly, a 600 mL beaker was chosen
as reactor to carry out the lab scale batch precipitation experiments, under the
conditions that can be found in Table 1. Once the reaction time was finished, the
solution was quickly filtered and separated for chemical analysis. The solid obtained
was dried during one day at 105°C. After this time, the samples were weighed to obtain
the PCC grams precipitated. The main result were considered on the KOH
regeneration efficiency, which is defined as follows:
KOH regeneration efficiency (%)=PCC obtained (g)×
2×PM KOH
PMCaCO3
Maximum KOH ¿regenerate(g)¿×100
The maximum KOH to be regenerated can be obtained stochiometrically from K2CO3
initial concentration. The reaction carried out at 50°C, with a molar ratio Ca/K2CO3 of
1.2 mol and a reaction time of 30 minutes was selected as a reference experiment
[13,27]. The concentration of the aqueous solution was fixed in 20g/100mL since it is
an expectable value after chemical absorption of KOH [27,28]. On the other hand the
Ca(OH)2 solution concentration was calculated stoichiometrically for each experiment
accordingly with the molar ratio.
Table 1. Matrix of experiments done in this study.
EXPERIMENT CARBONATE TO REGENERATE TIME (MIN) TEMPERATURE (ºC) MOLAR RATIO (R)1 Na2CO3 30 50 1.22 Na2CO3 15 50 1.23 Na2CO3 60 50 1.24 Na2CO3 30 30 1.25 Na2CO3 30 50 1.26 Na2CO3 30 70 1.27 Na2CO3 30 50 18 Na2CO3 30 50 1.29 Na2CO3 30 50 1.510 K2CO3 30 50 1.211 K2CO3 15 50 1.212 K2CO3 60 50 1.213 K2CO3 30 30 1.214 K2CO3 30 50 1.215 K2CO3 30 70 1.216 K2CO3 30 50 117 K2CO3 30 50 1.218 K2CO3 30 50 1.5
6
FTIR, Raman spectroscopy. XRD and SEM technique were employed for the
characterization of the solid samples. A Perkin Elmer FTIR BX spectrometer was used
to perform the attenuated total reflection Fourier transform infrared spectroscopy in the
powders (ATR-FTIR). Background subtracted spectra of the raw and the treated
samples were collected at room temperature by co-adding 32 scans at 4 cm−1
resolution in transmittance mode. Data were baseline corrected using Spectrum 5™
software. XRD analysis was completed by an X’Pert Pro PAN analytical instrument.
The 2θ angle was increased by 0.05o, with a 450 time per step over a range of 10-90o.
Diffraction patterns were then recorded at 40 mA and 45 kV, using Cu Kα radiation
(λ=0.154 nm).
Raman measurements of the powders samples were recorded using a Thermo DXR2
spectrometer equipped with a Leica DMLM microscope. A diffraction grating of 600
grooves per mm, a CCD detector, a green laser with a wavelength of 532.14 nm
(maximum power 20 mW), and a 50x objective were used. The morphology of the
samples were studied using SEM. This was carried out on a JSM6400 equipped with
an Energy Dispersive X-ray Spectroscope (EDS) analyzer (Oxford Link) and operated
at 20 KV. Reproducibility of the experiments were conducted giving as result ±2% of
error.
3. Results
Herein regeneration results are presented and discussed. Firstly, both NaOH and KOH
regeneration efficiencies are compared under the reaction conditions indicated above.
Secondly, chemical comparison between both carbonates obtained are shown by
means of Raman, FTIR and XRD measurements as well as SEM images.
3.1 Regeneration efficiencies results
7
Figures 3, 4 and 5 reveal the curves of NaOH and KOH resulting from the precipitation
experiments previously identified in section 2. The left hand side of the Figures
correspond to the net regeneration efficiency obtained with both caustic solutions, while
the right hand side indicates the regeneration efficiency differences between NaOH
and KOH.
10 15 20 25 30 35 40 45 50 55 60 65
60
65
70
75
80
85
90
95
100
Reg
ener
atio
n ef
ficie
ncy
(%)
Reaction time (min)
KOH NaOH
0.00.51.01.52.02.53.03.54.04.55.05.56.06.57.07.5
Differences
Reg
ener
atio
n ef
ficie
ncy
diffe
renc
es
Figure 3. Comparison of NaOH and KOH regeneration with time at T=50oC and R=1.2.
3.1.1 Reaction Time Variation
The evolution of regeneration efficiencies during the reaction time is shown in Figure 3.
Curiously, KOH regeneration efficiencies are to be lower than those of NaOH. This
result is in good agreement with separated previous studies [29] and may be caused by
the higher stability of K2CO3 in comparison to Na2CO3. Given these circumstances, it
may be better to employ NaOH instead of KOH. However, as discussed previously,
KOH was proven to be a better solvent for CO2 removal [12,30] and the differences in
the regeneration stage can be overcome by increasing the reaction time. At 60
8
minutes, the differences between NaOH and KOH regeneration efficiencies are much
lower than that at 15 minutes (1.27% vs 3.99%). In any case, an almost 4% of
difference in regeneration efficiency could be industrially assumed as long as the
overall economic balance results positive.
25 30 35 40 45 50 55 60 65 70 7555
60
65
70
75
80
85
90
95
100
Reg
ener
atio
n ef
ficie
ncy
(%)
Temperature (°C)
KOH NaOH
0.00.51.01.52.02.53.03.54.04.55.05.56.06.57.07.5
Differences
Reg
ener
atio
n ef
ficie
ncy
diffe
renc
es
Figure 4. Influence of temperature variation at R=1.2 and t=30min.
3.1.2 Temperature Influence
Figure 4 reflects the strong impact of temperature in the regeneration efficiencies. It
seems clear that in the low temperature range both solutions behave differently while at
the high temperature window similar behavior was identified. In particular, at 30oC a
6.88% of regeneration efficiency difference is obtained, whereas at 70oC this value
drops to 0.86%. This again can be ascribed to the greater stability of K2CO3 compared
to Na2CO3. In a hypothetical industrial application, in the case of choosing a
temperature around 50°C, a high regeneration efficiency would be achieved for both
hydroxides, without significant discrepancies between them. This is a remarkable
9
finding that deserves to be featured, since a process temperature as low as 50°C is
feasible to achieve by the employ of renewable energy, being an important advance
from an energy consumption perspective.
1.0 1.2 1.4 1.6
79
80
81
82
83
84
85
86
87
Reg
ener
atio
n ef
ficie
ncy
(%)
R
KOH NaOH
0.00.51.01.52.02.53.03.54.04.55.05.56.06.57.07.5
Differences
Reg
ener
atio
n ef
ficie
ncy
diffe
renc
esFigure 5. Regeneration experiments for R values at t=30min and 50oC.
3.1.3 Molar Ratio Influence
The impact of precipitant/reactive molar ratio is depicted in Figure 5. As shown in the
plot, both NaOH and KOH regeneration are favored when the molar ratio increases.
Nevertheless, NaOH regeneration efficiency is always higher than KOH regeneration
capacity at every studied value of R. In addition, the differences in regeneration
efficiencies remains consistently steady across the studied R range. Contrary to the
observations for the other reaction parameters, it seems that the impact of R in the
performance is rather constant and the two families of solvent do not display similar
behavior when tuning this parameter. Assuming 80% of regeneration efficiency as an
acceptable result in an industrial case, an R value of 1 would be required to meet this
10
value employing Na2CO3. However, a R=1.2 would be necessary for K2CO3, what
promotes a higher amount of free calcium ions that need to be eliminated before
recirculating the resulting aqueous KOH solution in order to prevent fouling in the
absorption tower. In other words, it can speculated that KOH is more prone to produce
solid fouling in the absorption column thus leading to higher operational cost in terms of
shut-down / clean-up /star-up cycles.
3.2 Physicochemical Comparison for both PCC Obtained
Once regeneration efficiencies differences have been compared, the purpose of this
section is to contrast both PCC obtained from K2CO3 and Na2CO3. The analyses were
carried out over the tests number 1 and 10 (T=50oC, R=1.2, t=30 min), which were
selected as standard tests in a previous study [13]. At the same time, these two
samples were compared with commercial Ca(OH)2 and CaCO3. Figure 6 shows the
representative FTIR spectra of the studied samples for sake of comparison. CaCO3 is
characteristic of monoclinic structure inside P21/c group [31,32]. As can be seen in
Figure 6, both PCC represented are quite similar to commercial CaCO3, suggesting an
almost pure calcium carbonate was obtained. A strong Characteristic peak of CaCO3
polymorphs is shown at 874 cm-1 wavenumber [33]. This peak is presented by both
PCCs, so it could be an indication of CaCO3 purity.
11
Figure 6. FTIR spectra for selected samples.
500 1000 1500
Ram
an in
tens
ity (a
.u.)
PCC from K2CO3
PCC from Na2CO3
Commercial Ca(OH)2
Raman shift (cm-1)
Commercial CaCO3
12
Figure 7. Raman spectra for PCCs obtained (t=30min, T=50°C, R=1.2) in comparison
with commercial Ca(OH)2 and CaCO3.
In order to investigate the purity of the selected samples, Raman spectra are
represented in Figure 7. In this analysis, it is easier to identify a weak peak of
remaining Ca(OH)2 at around 300 cm-1 in both PCCs spectra. This result agrees with
those discussed previously in section 3.1, where 100% of regeneration efficiency is
never achieved indicating some leftovers of Ca(OH)2 in the obtained solids. In fact, the
high intensity Raman mode of the PCCs spectra at around 1150 cm-1 again reveals the
major contribution of CaCO3 in the obtained solid. To corroborate Raman experiments
and further gather information regarding the crystalline structure of the solids, Figure 7
shows XRD patterns of the studied samples. Herein it can be Clearly observed that
some contamination of Ca(OH)2 remains in both PCCs, denoted by the diffraction peak
at 34 degrees. Nevertheless, as announced before, this phase is present in very small
concentrations in comparison with CaCO3 as intended from the low intensity peak
demonstrated by PCCs. Overall, the two XRD patterns of the obtained PCCs are quite
similar to that of the commercial CaCO3 further confirming the predominance of this
crystalline phase in the solid composition. Concretely, the XRD pattern exhibited by our
PCCs is characteristic of calcite phase. Comparing both PCCs obtained from K2CO3
and Na2CO3, the first one presents a different peak at around 32 degrees. This seems
to be a minor contribution of vaterite phase formed in good agreement with previous
reports [34]. It is relevant to mention that such a secondary phase – vaterite – is only
formed when KOH is used as a capturing solution in the tower what points out the
impact of the alkaline cation not only in the regeneration efficiency of the upgrading
process but also in the structure of the obtained solid.
13
20 25 30 35 40 45 50 55 60
PCC from K2CO3
PCC from Na2CO3
VateriteCalcite
Ca(OH)2
Commercial Ca(OH)2
Commercial CaCO3
2q (degree)
Inte
nsity
(a.u
.)
Figure 8. XRD bands for selected samples.
Finally, SEM images were taken to get further insights into the precipitated carbonates
morphology (Figure 9-10). PCC from Na2CO3, represented in Figure 9, seems to have
a polymorphous calcite structure, as previously reported in a recent study [13]. On the
other hand, PCC from K2CO3, present a morphology dominated by calcite polymorphs.
One main conclusion from the SEM images is that no significant morphology
differences exist between both products.
14
Figure 9. PCC SEM from Na2CO3.
Figure 10. PCC SEM from K2CO3.
4. Conclusions
15
The present paper shows an interesting method for biogas upgrading from an
economical point of view. With respect to other commercial methods for biogas
upgrading, this process generates bio-methane and PCC as valuable products. The
process performance results are quite promising exhibiting high regeneration
efficiencies (60-95%) for both tested carbonates. Generally and comparing with other
previous studies in which waste were chosen as precipitating agents [27,29], our
results are enhanced regarding regeneration efficiency (60-95% vs 50-60%). Thus, our
process seems to be more viable from an industrial point of view.
KOH regeneration efficiencies are always lower than those of NaOH, probably due to
the greater stability of K2CO3. However, these are subtle differences that might be
subjugated by the enhancement of operation parameters, as long as the overall
economics of the process is improved. Regarding the effects of the different
parameters studied, it seems that temperature is the most influential factor indeed, an
increase in its value from 30oC to 50oC has caused an almost 20% of improvement in
the overall regeneration performance. Nevertheless, reaction time could also play a key
role in the hypothetical case of an industrial plant to enhance the regeneration
efficiencies.
FTIR and XRD studies confirm the purity of the carbonate phase obtained in the
precipitation experiments, whereas no significant differences in the morphology were
detected by the employment of SEM. This however could open new research avenues
since other precipitating materials could be tested to get a more valuable product.
Overall, the technical feasibility of this process was demonstrated for both solvents,
indicating that further research on this process is worth considering in the context of
carbon capture/utilization.
Future works will deal with finding new precipitating materials that can produce a more
valuable final product, in order to improve the overall economy of the process.
Furthermore, preliminary studies for scaling up the lab-scale work presented in this
16
paper to a bench-scale unit will be carried out, where the economy of the process could
be examined more accurately. Potentially our work could be integrated with other
industrial processes in the future. For instance, there is a possibility to use the
carbonate solution obtained after the absorption step as draw solution in forward
osmosis and then precipitating CO2 as valuable by-product [35].
Acknowledgments and Funding
This work was supported by University of Seville through its V PPIT-U. Financial
support for this work was also provided by the EPSRC grant EP/R512904/1 as well as
the Royal Society Research Grant RSGR1180353. This work was also partially
sponsored by the CO2Chem UK through the EPSRC grant EP/P026435/1.
Furthermore this work was supported by EMASESA through NURECCO2 project and
Corporación Tecnológica de Andalucía (CTA).
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