Kindle
Williams
,
Nathan
Corbin
,
Joy
Zeng
,
Nikifar
Lazouski
,
Deng-Tao
Yang
and
Karthish
Manthiram
*
Department of Chemical Engineering, Massachusetts Institute of Technology, Cambridge, MA 02139, USA. E-mail: karthish@mit.edu
First published on 11th March 2019
Electrochemical CO2 reduction is a promising path toward mitigating carbon emissions while also monetizing waste gas through chemicals production and storage of surplus renewable energy. However, deploying such a technology for use on industrial CO2 sources requires an understanding of the effects that gas feed impurities have upon CO2 reduction reaction (CO2RR). In this work, we elucidate the impact of molecular oxygen on the network of reactions occurring in a CO2 reduction system. Our findings indicate that for a planar, polycrystalline Au electrode in an aqueous environment, oxygen reduction current is limited by the transport characteristics specific to the cell geometry and solvent; as a result, mass transport confers a protective effect by mitigating the otherwise thermodynamically and kinetically favorable reduction of oxygen. The presence of oxygen does not appear to have a significant impact on either CO2RR or hydrogen evolution partial currents, indicating that the mechanisms of reduction reactions involving oxygen are independent of CO2RR and hydrogen evolution. Further, an electrokinetic mechanistic analysis indicates many feasible candidates for the rate-determining step of CO2RR; there is no indication that the CO2RR mechanism at PCO2 = 0.5 atm is altered by the presence of oxygen, as the Tafel slopes (59 mV dec−1) and reaction orders with respect to bicarbonate (0), CO2 (∼1.5), and protons (0 from lack of KIE) are consistent between systems with PO2 = 0 atm and those with PO2 = 0.5 atm. While this is promising for the robustness of CO2RR to oxygen impurities in gas feeds, the ultimate design tradeoff when utilizing CO2 sources containing oxygen is between the cost of separation processes and the corresponding cost of power inefficiency as a result of electrons lost to oxygen reduction. This represents a first step in understanding kinetic and transport considerations in the design of gas-impurity-tolerant CO2 reduction systems.
A major limitation of existing studies of CO2 electroreduction, however, is that almost all experiments conducted to date have utilized gas feeds of 99.9% or purer CO2. Those investigations which have focused on dilute streams of CO2 have so far mostly done so in the context of low-conversion molecular catalysts and inert gas impurities such as nitrogen (N2).5 If CO2 reduction is ever to be practically employed, it may not be feasible – logistically or economically – to expect end-users of CO2 reduction technology to supply feedstocks of high CO2 purity. Some estimates have indicated that the purification of CO2 from air (which currently contains ∼400 ppm or 0.04% CO2)6 would cost roughly $1000 per metric ton CO2 captured, while similar capture from the effluents of coal-fired power plants (containing 10–15% CO2) would cost about $25–100 per metric ton CO2.7 A more promising study on the design of a system for direct CO2 capture from air was able to decrease the cost of air capture to $94–232 per ton CO2.8 However, even this cost may prove prohibitive for the commercialization of CO2 reduction technology, as many technoeconomic analyses investigating CO2 reduction viability rely on CO2 capture costs being no more than $30–60 per ton CO2.9,10 Therefore, it would be valuable for developed CO2 reduction technologies to exhibit some degree of tolerance to gas feed impurities.
Previous studies involving non-inert impurities in CO2 reduction streams have focused on the effects of NOx, SOx, and O2 on CO2RR at Cu cathodes.11,12 In these contexts, O2 was treated either as a species with the propensity to interfere with other impurities (e.g. by oxidizing poisoning sulfide ions),11 or as a catalyst oxidant.12Ex situ catalyst characterization and changes in bulk product distribution were the primary metrics of the impurities' effects, whereas impacts on the electroreduction mechanisms occurring in the cell and the physical phenomena governing the feed impurities' behavior in these contexts were not explicitly treated. Thus, there is a need to build upon these efforts in order to ensure the catalysts being developed for CO2 reduction today will be viable for implementation in the future.
In particular, an abundant and reactive impurity in most anticipated CO2 feed streams is molecular oxygen (O2). Oxygen-tolerant catalytic networks are increasingly being studied for hydrogen evolution; methods for minimizing O2 competition include the development of bio-inspired catalytic pockets in order to exclude, photo-reduce, or otherwise steer molecular oxygen away from poisoning catalytic systems for proton reduction.13 Platinum catalysts for the hydrogen evolution reaction (HER) seem to maintain current density to HER in the presence of 0.21 atm O2;13 however, the exact means by which this is possible have not been investigated. It is equally as important, if not more so, for the impact of O2 on CO2 reduction to be studied and mitigated, since O2 may very well be a constituent of CO2 reduction gas feeds.
The goal of the present work is to demonstrate the effects of the presence of oxygen on the network of reactions occurring during electrochemical CO2 reduction on gold catalysts. Gold was chosen as a test catalyst due to its high activity toward CO2 reduction and for ease of study due to its high selectivity toward only gas-phase products (CO and H2).2,4,14–18 Cultivating an understanding of oxygen's effect on such an electrocatalytic system will pave the way for the development of systems with tolerance toward a broader variety of gas-phase impurities characteristic of many CO2 point sources, which may be required for industrially viable CO2 reduction.
As increasing amounts of oxygen were added to the gas feed, current toward ORR increased linearly while partial currents toward CO2RR and HER remained roughly constant. This implies that ORR chemistry did not affect CO2RR or HER catalysis. Further, it suggests the nature of the catalyst itself may have been unaffected by the presence of oxygen. It should be noted that there is somewhat larger uncertainty in the partial current measurements toward CO2RR and HER, consistent with previous studies using foil electrodes.20,21 This is because foil preparation by polishing introduces surface irregularities that cannot be easily replicated from run to run. However, the uncertainties expressed in the error bars of this figure are noticeably small for the ORR data points. This is indicative that the quality of the foil preparation has no effect on ORR currents, and reinforces our confidence in the data.
At less reductive potentials and lower current densities, an apparent negative trend in both CO2RR and HER current is observed (Fig. S11†). The fact that this trend is evident only at low overpotentials suggests either that oxygen interferes with these mechanisms in a distinct way at lower overpotentials, or that the effect of O2 in the system is constant, but kept small on an absolute scale, therefore only showing up at low current densities.
To investigate why these trends hold true, the factors governing each reaction – namely, the kinetic versus transport control of ORR, as well as mechanistic aspects of CO2RR and HER – were studied in the context of PCO2 = 0.5 atm.
CO2RR (E0 = −0.52 V vs. SHE):
CO2 (aq) + H2O (l) + 2e− ⇌ CO (g) + 2OH− (aq) |
HER (E0 = −0.41 V vs. SHE):
2H2O (l) + 2e− ⇌ H2 (g) + 2OH− (aq) |
4e− ORR (E0 = 0.82 V vs. SHE):
O2 (aq) + 2H2O (l) + 4e− ⇌ 4OH− (aq) |
2e− ORR (E0 = 0.28 V vs. SHE):
O2 (aq) + 2H2O (l) + 2e− ⇌ H2O2 (l) + 2OH− (aq) |
Thermodynamics would dictate that at CO2 reduction conditions that allow for the formation of CO, reducing oxygen is extremely favorable. Since the equilibrium potential for CO2 reduction is roughly −0.52 V vs. SHE in neutral media, the cathode must be held at more reductive potentials than −0.52 V vs. SHE in order to achieve significant CO2 reduction currents. It is reasonable to imagine that at greater than 1.3 V of overpotential, the rate of ORR may not be strictly dictated by kinetics. However, it was prudent to confirm this experimentally.
In this vein, cyclic voltammograms taken at PCO2 = 0.5 atm were compared with and without a half-atmosphere of oxygen (Fig. 2A). It can be observed that at around 0.25 V vs. SHE, the onset of ORR occurs. This reduction current density plateaus at −0.26 mA cm−2 around −0.2 V vs. SHE. HER and CO2RR onset, meanwhile, do not occur until the potential is swept down to almost −0.8 V vs. SHE. It is therefore concluded from this plot that ORR is transport-limited at the CO2RR potentials of interest. This explains the phenomenon wherein ORR current is not impacted by changes introduced to the catalyst surface by polishing – the current is limited by diffusion.
For a planar electrode, assuming a stagnant boundary layer model (Fig. 2B), the formation of a linear species concentration profile at the catalyst surface leads to the expression:23
![]() | (1) |
To understand more about the mass-transport boundary layer in the cell, its thickness was determined by measuring the diffusion-limited current density of the ferricyanide ion and back-calculating its mass-transport boundary layer thickness using eqn (1).25 A conversion was then applied to account for the difference in the diffusion coefficients of ferricyanide and gas-phase species such as CO2 and O2 (see ESI Section S.7.5†). For the transport of dissolved O2 gas, the calculated boundary layer thickness was 200 ± 7 μm. Using the values n = 4 (see below), DO2 = 2.10 × 10−5 cm2 s−1,26 and Cbulk,O2 = 0.65 mM at 0.5 atm,24 the resulting prediction for the ORR diffusion-limited current density is 0.26 ± 0.01 mA cm−2, in remarkable agreement with our voltammogram.
In addition, it was necessary to confirm which type of ORR was occurring under CO2 reduction conditions. Gold is a known peroxide-forming ORR catalyst,27 more typically implicated in selective H2O2 formation under acidic conditions,28,29 whereas within the bicarbonate mass transport boundary layer, conditions should be slightly basic (up to pH 9–10, depending on the current density drawn).30 Long-term experiments passing over 50C of charge were conducted in order to study the accumulation of ORR liquid-phase products; the colorimetric assay corresponding to the quantification of hydrogen peroxide in this electrolyte returned negative results, meaning that less than 10% of the oxygen being reduced is forming hydrogen peroxide (Section S.8.3†). We can therefore posit not only that ORR is transport-limited at relevant testing potentials, but also that it is primarily forming water. As water is the chief component of the electrolyte, the ORR products are not expected to interfere with any other catalytic cycles occurring in the cell.
Kinetic data were captured through Tafel analysis, bicarbonate dependence, CO2 dependence, and kinetic isotope effect (KIE) experiments. The results are displayed and discussed below (Fig. 3).
The Tafel slope of 59 mV dec−1 indicates that a chemical step past the initial electron transfer to CO2 is the rate-determining step (RDS) (see ESI Section S.11†). Subsequent experiments were designed to probe what this chemical step might be. Experiments were intended to probe purely the kinetics of the reaction and therefore were primarily conducted in the linear Tafel region – here selected as 300 mV overpotential, or −0.41 V vs. RHE in 0.1 M NaHCO3 (−0.82 V vs. SHE).
While most conceivable CO2RR mechanisms consistent with the Tafel data might have either a zeroth- or first-order dependence on bicarbonate, the slope in the bicarbonate plot suggests that CO2RR is negatively impacted by increased bicarbonate concentrations. The slope without O2 is −0.1 ± 0.2, while the slope with O2 is −0.23 ± 0.05. This trend is especially true as we approach the solubility limit of sodium bicarbonate at roughly 1.2 M (see Section S.7.2†).33 Results of the same experiment repeated with potassium bicarbonate, which is of a different purity than and nearly three times as soluble as the sodium salt, are shown in the ESI (Section S.7.2.2†). Because the potassium bicarbonate data yields a fairly clear zero-order dependence on bicarbonate, it is anticipated that the negative slope in the sodium case is the result of a secondary effect and that the reaction order in bicarbonate is 0.
It was shown that at the testing conditions, the KIE is negligible (KIE = kH/kD = 1 within error) for CO2 reduction, while for HER the value of the KIE is greater than 10. This is suggestive that while the KIE could be considerable in this experiment given the participation of a proton in the RDS, the KIE is not observed, and therefore it is unlikely that a proton transfer is involved. Notably, KIE experiments have been known to lead to false negative conclusions, but only in very specific and rare instances.34
RDS | Tafel slope form | Tafel slope at 298 K, β = 0.5 | Acidic proton order | P CO2 order | KIE? | |
---|---|---|---|---|---|---|
a Outcomes of experiments to probe the kinetics are listed next to each step in every postulated mechanism, under the circumstances that the step in question is the respective mechanism's rate-determining step (RDS). θ represents a catalytic active site on the Au electrode. β is the symmetry factor, interpreted as being 0.5. X.1 represents the first step in each of the proposed mechanisms. Bolded steps remain plausible RDS candidates after the kinetic investigation conducted here. *C.2 and F.2 are written such that any proton donor could in principle serve as the proton source, including water and bicarbonate. †G.1 is a separate mechanistic step also involved in the HER pathway. ‡Mechanism G requires the assumption that θH is dictated by equilibrium described by the Tafel step of HER. See derivation (S.11.4). ◊H.n steps could in principle be almost anything, including previously listed mechanisms. H.2 is simply the rearrangement of CO2˙− on the surface to generate an intermediate which then reacts to form products. It does not necessarily require that γ differs from θ. | ||||||
X.1 |
![]() |
2.3RT/βF | 118 | 0 | 1 | N |
A.2 |
![]() |
2.3RT/F | 59 | 1 | 1 | Y |
A.3 | θ COOH + e− ⇌ θ + CO + OH− | 2.3RT/(β + 1)F | 39 | 0 | 1 | N |
B.2 |
![]() |
2.3RT/F | 59 | 0 | 1 | Y |
B.3 | θ COOH + e− ⇌ θ + CO + OH− | 2.3RT/(β + 1)F | 39 | 0 | 1 | N |
C.2* |
![]() |
2.3RT/F | 59 | 1 | Y | |
C.3 | θ COOH + θ ⇌ θCO + θOH | 2.3RT/F | 59 | 0 | 1 | N |
C.4 | θ CO ⇌ θ + CO | 2.3RT/2F | 30 | 0 | 1 | N |
D.2 |
![]() |
2.3RT/F | 59 | 0 | 1 | N |
D.3 | θ CO ⇌ θ + CO | 2.3RT/2F | 30 | 0 | 1 | N |
E.2 |
![]() |
2.3RT/F | 59 | 0 | 2 | N |
E.3 | θ CO+ + e− ⇌ θ + CO | 2.3RT/(β + 1)F | 39 | 0 | 2 | N |
F.2* |
![]() |
2.3RT/F | 59 | 1 | Y | |
F.3 | θ COOH ⇌ θCO+ + OH− | 2.3RT/F | 59 | 0 | 1 | N |
F.4 | θ CO+ + e− ⇌ θ + CO | 2.3RT/(β + 1)F | 39 | 0 | 1 | N |
G.1† | HCO3− + θ + e− ⇌ θH + CO32− | |||||
G.2 |
![]() |
2.3RT/F | 59‡ | 0 | 1 | Y |
G.3 | θ COOH − ⇌ θ + CO + OH − | 2.3RT/F | 59 ‡ | 0 | 1 | N |
H.2 |
![]() |
2.3RT/F | 59 | 0 | 1 | N |
H.n◊ | — |
In these mechanisms, CO2RR is regarded as proceeding through inner-sphere transformations. The mechanistic step X.1, representing an adsorptive electron transfer to CO2, is regarded as the first step in each of the proposed mechanisms. While the list of mechanistic possibilities compiled here is not exhaustive, it encompasses many of the commonly reported mechanisms of CO2 reduction to CO on Au, as well as a number of speculative possibilities.31 In particular, excluded from this list are possibilities involving concerted proton-electron transfer (CPET). However, all mechanisms with CPET corresponding to initial CO2 adsorption can also be collapsed down into the starting points represented by mechanistic steps C.2 and F.2, and therefore are also encompassed by this treatment.
The more commonly accepted intermediates for CO2RR are implicated in mechanisms A and B. However, RDS candidates A.2 and B.2 are ruled out due to lack of bicarbonate dependence and KIE, respectively.
If we allow for the participation of surface sites or adsorbed species which are uncommon in the existing literature, then many RDS candidates remain (bolded options, Table 1). These include steps involving the formation of an Au–O bond, which we deem unlikely on the basis of gold's low oxophilicity; examples of this are θCOOH dissociation into adsorbed CO and OH (mechanism C, excluded on the grounds of pH dependence) and the dissociation of adsorbed CO2˙− into CO and an oxygen atom anion radical adsorbate (D.2). Mechanisms forming an Au–O bond can be avoided by instead invoking a cationic θCO+ adsorbate species, which seems only to have been described in metal complexes rather than on surfaces;35,36 this is exemplified in mechanisms which exhibit the participation of CO2 in the RDS (E.2) and the dissociation of the θCOOH intermediate into charged species (mechanism F, excluded on the grounds of pH dependence). Further, under certain mathematical assumptions and allowing for the θCOOH− anion, the desorption of CO (G.3) is an RDS that is consistent with the data. A conformation change of adsorbed CO2˙− (H.2) may also serve as the RDS.
Accumulation of surface intermediates involved in these mechanisms could be assessed by use of FT-IR in order to further narrow down the mechanistic possibilities or develop new, more plausible hypotheses. For instance, a large IR band associated with θCO may indicate that this species has accumulated on the surface and is therefore the bottleneck in CO2RR, supporting a CO desorption step as an RDS. The observation of such intermediates is currently a subject of debate.16,18
More relevant to the discussion of oxygen's effects, however, is the understanding of whether the mechanism of CO2 reduction changes under oxygenated conditions in the electrochemical cell. The findings presented above suggest that so far, we have no reason to believe the mechanism of CO2 reduction changes in the presence of oxygen. This is a promising result if we hope to develop oxygen-tolerant CO2 reduction systems in the future.
![]() | ||
Scheme 1 Interactions between CO2RR, HER, and ORR during cathodic polarization on a bulk Au surface. |
Because oxygen is less soluble than CO2 in aqueous electrolyte, transport provides a protecting effect against ORR. However, that does not mean that ORR even in this context is entirely benign. It is important to note that for practical design purposes, a high-rate CO2 reduction reactor may need to operate under configurations such as a gas diffusion electrode (GDE) or a flowing-electrolyte design, wherein the length scales over which interfacial transport occurs are much smaller, and protecting effects of solubility are lessened. In such a scenario, the mechanistic analysis conducted here may not apply; further, power inefficiencies as a result of ORR may dominate economic considerations. Even in the context of the aqueous cell with a planar electrode reported here, assuming CO2:
O2 ratios typical of flue gas streams from natural gas power plants (roughly 1.67
:
1),37 and assuming activity and selectivity to CO2 matching those reported here at −1.06 V vs. SHE, roughly 12% of applied power would be lost to ORR. In the case that this value in a practical system is smaller than the equivalent power loss required to purify a CO2 stream of oxygen, direct reduction of a mixed O2/CO2 stream may be a viable design option. The strategy to accept loss of power in a CO2 electrolyzer could be viewed as complementary to other techniques which have been suggested for thermochemically reducing dilute oxygen impurities in CO2-rich feedstocks using methane.38
Future work should be dedicated toward developing a better understanding of the RDS of CO2RR on gold, as well as conducting similar studies on more oxophilic metals. Further, for power efficiency purposes, it may prove economical to invest effort toward the design of an inherently oxygen-tolerant CO2RR system through modulating transport parameters at the electrode surface.
Footnote |
† Electronic supplementary information (ESI) available: In-depth materials & methods, discussion re: effects of O2 at lower overpotentials, transient current decay phenomena, and kinetic rate law derivations. See DOI: 10.1039/c9se00024k |
This journal is © The Royal Society of Chemistry 2019 |