6 research outputs found
Toward Intelligent CO<sub>2</sub> Capture Solvent Design through Experimental Solvent Development and Amine Synthesis
In order to improve toward efficient
large scale CO<sub>2</sub> capture applications, the largest uncertainties
with postcombustion
carbon dioxide capture (PCC) still surround the chemical reactivity
and reaction rate of the solvent, the large parasitic energy penalty
introduced during the regeneration of CO<sub>2</sub> from the solvents,
and the stability of the amine solvent to resist degradation in the
presence of trace impurities present in the flue gas. Heterocyclic
amines are a class of molecules that have inherently superior kinetic
reactivity with CO<sub>2</sub> but, importantly, have demonstrated
desirable energy performance and degradation resistance. The current
work is focused on further understanding of the chemical behavior
of diamine and triamine solvents during CO<sub>2</sub> absorption
and desorption from laboratory scale measurements. In this study we
have proposed and prepared a series of cyclic diamine and triamine
derivatives which can potentially offer reductions in solvent related
costs associated with the PCC process. Thirty amines were synthesized
and their CO<sub>2</sub> absorption and cyclic capacities determined
between 40 and 90 °C using a small reactor with analysis of the
solutions performed using quantitative <sup>13</sup>C and <sup>1</sup>H NMR spectroscopy. Cyclic capacity results indicate the majority
of the amines are capable of increases in CO<sub>2</sub> uptake and
cycle (when expressed as molar or mass ratios) compared to piperazine
(PZ, the most commonly used diamine) and monoethanolamine (MEA, the
standard amine to which all other amines are compared) over a similar
temperature swing. Eight of the amines demonstrated significant improvements
with 200% or greater improvement in cyclic capacity over PZ (expressed
as moles of CO<sub>2</sub>/mol of nitrogen), with the largest improvement
achieving a 273% increase. The intimate chemical behavior of the amines
was examined by considering the relative contributions of specific
CO<sub>2</sub> species to the cyclic capacity. Nine of the amines
investigated showed significant improvements in the amount of the
targeted bicarbonate product cycled between 40 and 90 °C compared
to PZ. Despite the unoptimized and conservative desorption conditions
utilized here, the results demonstrate that CO<sub>2</sub> can be
regenerated from cyclic amines without the requirement for excessive
regeneration temperatures as is the case for PZ (∼150 °C
to achieve optimum cyclic capacity). The results here demonstrate
the potential for improved amine solvents via amine synthesis and
future development pathways through intelligent molecular design
Evaluation and Modeling of Vapor–Liquid Equilibrium and CO<sub>2</sub> Absorption Enthalpies of Aqueous Designer Diamines for Post Combustion Capture Processes
Novel
absorbents with improved characteristics are required to
reduce the existing cost and environmental barriers to deployment
of large scale CO<sub>2</sub> capture. Recently, bespoke absorbent
molecules have been specifically designed for CO<sub>2</sub> capture
applications, and their fundamental properties and suitability for
CO<sub>2</sub> capture processes evaluated. From the study, two unique
diamine molecules, 4-(2-hydroxyethylamino)Âpiperidine (A4) and 1-(2-hydroxyethyl)-4-aminopiperidine
(C4), were selected for further evaluation including thermodynamic
characterization. The solubilities of CO<sub>2</sub> in two diamine
solutions with a mass fraction of 15% and 30% were measured at different
temperatures (313.15–393.15 K) and CO<sub>2</sub> partial pressures
(up to 400 kPa) by thermostatic vapor−liquid equilibrium (VLE)
stirred cell. The absorption enthalpies of reactions between diamines
and CO<sub>2</sub> were evaluated at different temperatures (313.15
and 333.15 K) using a CPA201 reaction calorimeter. The amine protonation
constants and associated protonation enthalpies were determined by
potentiometric titration. The interaction of CO<sub>2</sub> with the
diamine solutions was summarized and a simple mathematical model established
that could make a preliminary but good prediction of the VLE and thermodynamic
properties. Based on the analyses in this work, the two designer diamines
A4 and C4 showed superior performance compared to amines typically
used for CO<sub>2</sub> capture and further research will be completed
at larger scale
CO<sub>2</sub> Absorption into Aqueous Solutions Containing 3‑Piperidinemethanol: CO<sub>2</sub> Mass Transfer, Stopped-Flow Kinetics, <sup>1</sup>H/<sup>13</sup>C NMR, and Vapor–Liquid Equilibrium Investigations
Global
efforts to reduce carbon dioxide emissions stemming from
the combustion of fossil fuels have acknowledged and focused on the
implementation of post combustion capture (PCC) technologies utilizing
aqueous amine solvents to fulfill this role. The cyclic diamine solvent
piperazine has received significant attention for application as a
CO<sub>2</sub> capture solvent, predominantly for its rapid reactivity
with CO<sub>2</sub>. A thorough investigation of alternative but simpler
cyclic amines incorporating a single amine group into the cyclic structure
may reveal further insight into the superior kinetic performance of
piperazine and the wider applicability of such cyclic solvents for
PCC processes. One such example is the cyclic monoamine 3-piperidinemethanol
(3-PM). To facilitate the evaluation of 3-PM as a capture solvent
requires knowledge of the fundamental chemical parameters describing
the kinetic and equilibrium of the reactions occurring in solutions
containing CO<sub>2</sub> and 3-PM. Additionally, in parallel with
the preceding, experimental measurements of CO<sub>2</sub> absorption
into 3-PM solutions, including mass transfer and vapor–liquid
equilibrium measurements, can be used to validate the CO<sub>2</sub> absorption performance in 3-PM solutions and compared to that of
monoethanolamine (MEA) under similar conditions. The present study
is focused in two parts on (a) determination of fundamental kinetic
and equilibrium constants via the analysis of stopped-flow kinetic
and quantitative equilibrium measurements via <sup>1</sup>H/<sup>13</sup>C nuclear magnetic resonance (NMR) spectroscopy and (b) experimental
measurements of CO<sub>2</sub> absorption into 3-PM solutions via
wetted wall column kinetic measurements, vapor–liquid equilibrium
measurements, and corresponding physical property data including densities
and viscosities of the amine solutions over a range of concentrations
and CO<sub>2</sub> loadings. Fundamental kinetic rate constants describing
the reaction of CO<sub>2</sub> with 3-PM are significantly faster
than MEA at similar temperatures (3-PM = 32 × 10<sup>3</sup> M<sup>–1</sup> s<sup>–1</sup>, extrapolated to 40 °C
from kinetic data between 15.0 and 35.0 °C; MEA = 13 × 10<sup>3</sup> M<sup>–1</sup> s<sup>–1</sup>, 40 °C).
Conversely, the equilibrium constants describing the reaction between
bicarbonate and amine, often termed carbamate stability constants,
are significantly lower for 3-PM than MEA at similar temperatures.
Overall CO<sub>2</sub> absorption rates in 3.0 M solutions of 3-PM
and MEA, assessed in overall CO<sub>2</sub> mass transfer coefficients,
are lower in the former case over the entire range of CO<sub>2</sub> loadings from 0.0 to 0.4 mol of CO<sub>2</sub> per mol of amine.
The reduced absorption rates in the 3-PM solutions can be attributed
to higher solution viscosities and thus corresponding reductions in
CO<sub>2</sub> diffusion. CO<sub>2</sub> absorption and cyclic capacities
in 3.0 M solutions of 3-PM and MEA were found to be significantly
higher in the case of 3-PM. The larger CO<sub>2</sub> capacities are
attributed to the lower stability 3-PM carbamate and the formation
of larger amounts of bicarbonate compared to MEA. Overall, the larger
CO<sub>2</sub> absorption capacity, cyclic capacity, and rapid kinetics
with CO<sub>2</sub> position 3-PM as an attractive CO<sub>2</sub> capture
solvent
Process Modeling of an Advanced NH<sub>3</sub> Abatement and Recycling Technology in the Ammonia-Based CO<sub>2</sub> Capture Process
An
advanced NH<sub>3</sub> abatement and recycling process that
makes great use of the waste heat in flue gas was proposed to solve
the problems of ammonia slip, NH<sub>3</sub> makeup, and flue gas
cooling in the ammonia-based CO<sub>2</sub> capture process. The rigorous
rate-based model, RateFrac in Aspen Plus, was thermodynamically and
kinetically validated by experimental data from open literature and
CSIRO pilot trials at Munmorah Power Station, Australia, respectively.
After a thorough sensitivity analysis and process improvement, the
NH<sub>3</sub> recycling efficiency reached as high as 99.87%, and
the NH<sub>3</sub> exhaust concentration was only 15.4 ppmv. Most
importantly, the energy consumption of the NH<sub>3</sub> abatement
and recycling system was only 59.34 kJ/kg CO<sub>2</sub> of electricity.
The evaluation of mass balance and temperature steady shows that this
NH<sub>3</sub> recovery process was technically effective and feasible.
This process therefore is a promising prospect toward industrial application
Protonation Constants and Thermodynamic Properties of Amino Acid Salts for CO<sub>2</sub> Capture at High Temperatures
Amino acid salts
have greater potential for CO<sub>2</sub> capture
at high temperatures than typical amine-based absorbents because of
their low volatility, high absorption rate, and high oxidative stability.
The protonation constant (p<i>K</i><sub>a</sub>) of an amino
acid salt is crucial for CO<sub>2</sub> capture, as it decreases with
increasing absorption temperature. However, published p<i>K</i><sub>a</sub> values of amino acid salts have usually been determined
at ambient temperatures. In this study, the p<i>K</i><sub>a</sub> values of 11 amino acid salts were determined in the temperature
range of 298–353 K using a potentiometric titration method.
The standard-state molar enthalpies (Δ<i>H</i><sub>m</sub><sup>0</sup>) and entropies
(Δ<i>S</i><sub>m</sub><sup>0</sup>) of the protonation reactions were also determined
by the van’t Hoff equation. It was found that sarcosine can
maintain a higher p<i>K</i><sub>a</sub> than the other amino
acids studied at high temperatures. We also found that the CO<sub>2</sub> solubilities and overall mass-transfer coefficients of 5 <i>m</i>′ sarcosinate (moles of sarcosine per kilogram of
solution) at 333–353 K are higher than those of 30% MEA at
313–353 K. These results show that some possible benefits can
be produced from the use of sarcosine as a fast solvent for CO<sub>2</sub> absorption at high temperatures. However, the pronotation
reaction of sarcosine is the least exothermic among those of all amino
acids studied. This could lead to a high regeneration energy consumption
in the sarcosinate-based CO<sub>2</sub> capture process
Insights into the Chemical Mechanism for CO<sub>2</sub>(aq) and H<sup>+</sup> in Aqueous Diamine Solutions - An Experimental Stopped-Flow Kinetic and <sup>1</sup>H/<sup>13</sup>C NMR Study of Aqueous Solutions of <i>N</i>,<i>N</i>‑Dimethylethylenediamine for Postcombustion CO<sub>2</sub> Capture
In an effort to advance the understanding
of multiamine based CO<sub>2</sub> capture process absorbents, we
report here the determination
of the kinetic and equilibrium constants for a simple linear diamine <i>N,N</i>-dimethylethylenediamine (DMEDA) via stopped-flow spectrophotometric
kinetic measurements and <sup>1</sup>H/<sup>13</sup>C NMR titrations
at 25.0 °C. From the kinetic data, the formation of monocarbamic
acid (DMEDACOOH) from the reaction of DMEDA with CO<sub>2</sub>(aq)
is the dominant reaction at high pH > 9.0 (<i>k</i><sub>7</sub> = 6.99 × 10<sup>3</sup> M<sup>–1</sup>·s<sup>–1</sup>). Below this pH, the formation of protonated monocarbamic
acid (DMEDACOOH<sub>2</sub>) via the pathway involving DMEDAH<sup>+</sup> and CO<sub>2</sub>(aq) becomes active and contributes to
the kinetics despite the 107-fold decrease in the rate constant between
the two pathways. <sup>1</sup>H and <sup>13</sup>C NMR spectra as
a function of decreasing pH (increasing HCl concentration) at 25.0
°C have been evaluated here to confirm the protonation events
in DMEDA. Calculations of the respective DMEDA nitrogen partial charges
have also been undertaken to support the NMR protonation study. A
comparison of the DMEDA kinetic constants with the corresponding data
for piperazine (PZ) reveals that despite the larger basicity of DMEDA,
the enhanced and superior kinetic performance of PZ with CO<sub>2</sub>(aq) above its predicted Bronsted reactivity is not observed in DMEDA