High-Selectivity Electrochemical Conversion of CO2 to Ethanol using a Copper Nanoparticle/N-Doped Graphene Electrode

Authors Dr. Yang Song, Dr. Rui Peng, Dale K. Hensley, Dr. Peter V. Bonnesen, Dr. Liangbo Liang, Dr. Zili Wu, Dr. Harry M. Meyer III, Dr. Miaofang Chi, Dr. Cheng Ma, Dr. Bobby G. Sumpter, Dr. Adam J. Rondinone First published: 28 September 2016Full publication history   Abstract   Though carbon dioxide is a waste product of combustion, it can also be a potential feedstock for the production of fine and commodity organic chemicals provided that an efficient means to convert it to useful organic synthons can be developed. Herein we report a common element, nanostructured catalyst for the direct electrochemical conversion of CO2 to ethanol with high Faradaic efficiency (63?% at ?1.2?V vs RHE) and high selectivity (84?%) that operates in water and at ambient temperature and pressure. Lacking noble metals or other rare or expensive materials, the catalyst is comprised of Cu nanoparticles on a highly textured, N-doped carbon nanospike film. Electrochemical analysis and density functional theory (DFT) calculations suggest a preliminary mechanism in which active sites on the Cu nanoparticles and the carbon nanospikes work in tandem to control the electrochemical reduction of carbon monoxide dimer to alcohol. Introduction Closing the carbon cycle by utilizing CO2 as a feedstock for currently used commodities, in order to displace a fossil feedstock, is an appropriate intermediate step towards a carbon-free future. Direct electrochemical conversion of CO2 to useful products has been under investigation for a few decades. Metal-based catalysts, such as copper,[1] platinum,[2] iron,[3] tin,[4] silver,[5] and gold,[6] along with carbons such as g-C3N4 [7] have been the primary focus for CO2 reduction, with some very high Faradaic efficiencies for methane conversion. Copper is arguably the best-known metal catalyst for electrochemical CO2 reduction,[8] capable of electrochemically converting CO2 into more than 30 different products,[9] including carbon monoxide (CO), formic acid (HCOOH), methane (CH4) and ethylene (C2H4) or ethane (C2H6), but efficiency and selectivity for any product heavier than methane are far too low for practical use.[10] Competing reactions limit the yield of any one liquid product to single-digit percentages.[8]   Polycrystalline Cu foil produces a mixture of compounds in CO2-saturated aqueous solutions that are dominated either by H2 at low overpotential, or by CO and HCOO? at high overpotential, or by hydrocarbons and multi-carbon oxygenates at the most extreme potentials.[9, 11] Theoretical studies predict that graphene-supported Cu nanoparticles would enhance catalytic activity due to the strong Cu – graphene interaction via defect sites,[12] which would stabilize the intermediates from CO2 reduction and improve selectivity towards hydrocarbon products as methane and methanol at lowered overpotential. Early studies revealed that the electrode surface was dominated by adsorbed CO during the CO2 reduction and that CO acted as intermediate in the production of hydrocarbons.[13] Cu produces hydrocarbons and multi-carbon oxygenates when supplied with CO in the absence of CO2, but very negative potentials are still required to promote CO reduction over H2 evolution. Large overpotentials preclude energetically efficient electrolysis and favor hydrocarbons over liquid oxygenates. Recently, high selectivity of CO electroreduction to oxygenates, with ethanol as the major product, was achieved by oxide-derived Cu, in which the surface intermediates were stabilized by the grain boundaries.[14]   We previously reported on a highly textured nitrogen-doped, few-layer graphene electrode that presents with a surface of intense folds and spikes, which we termed carbon nanospikes or CNS. The CNS structure is disordered due to the high nitrogen content which prevents well-ordered stacking. In the current report, a carbon nanospike (CNS) electrode with electronucleated Cu nanoparticles (Cu/CNS) is shown to have much higher selectivity for CO2 electroreduction than H2 evolution, with a subsequent high Faradaic efficiency to produce ethanol. We believe this is achieved both from the high intrinsic CO2 reduction activity of Cu and from the synergistic interaction between Cu and neighboring CNS, which controls reduction to alcohol. The major CO2 reduction product is ethanol, which corresponds to a 12 e? reduction with H2O as the H+ source, display math   display math where E0 is the equilibrium potential. By comparing Cu/CNS to control electrodes comprised of 1) Cu on glassy carbon and 2) bare CNS, we demonstrate that CO2 reduction activity is not a simple consequence of either Cu or CNS. While the reaction mechanism is not yet elucidated, we hypothesize an interaction between adjacent catalytic sites on the Cu and CNS, facilitated by the nanostructured morphology of the catalyst that prevents complete electrochemical reduction to ethylene or ethane, resulting in a high yield of ethanol. Results and discussion   The bare CNS electrode (Supporting Information Figure?S1) was characterized in our previous study as a dense nanotextured carbon film terminated by randomly oriented nanospikes approximately 50–80?nm in length, where each nanospike consists of layers of puckered carbon ending in a ?2?nm wide curled tip.[15] The film is grown by a relatively simple direct-current plasma-enhanced chemical vapor deposition reaction using acetylene and ammonia as reagents.   The CNS film grows quickly and adheres well to the highly-doped silicon wafers that were used for this study. Raman spectra indicate that CNS have a similar structure to disordered, few-layer graphene.[15] The CNS is not crystalline and does not diffract. XPS indicates a nitrogen doping density of 5.1 ± 0.2?% atomic, with proportions of pyridinic, pyrrolic (or piperidinic) and graphitic nitrogens of 26, 25 and 37?% respectively, with the balance being oxidized N. In the current experiment, nanoparticles of Cu were electronucleated from CuSO4 solution directly onto the CNS (Supporting Information, Experimental Methods), and imaged via SEM shown in Figure?1. Electronucleation does not require templating surfactants to control the nanoparticle growth, and leaves the particle surfaces clean. The texture of the CNS promotes nucleation resulting in a large number of smaller particles, in comparison to the glassy carbon control which produced larger particles under identical conditions (Supporting Information Figure?S2), with a similar amount of Cu deposited. These well-dispersed Cu particles ranged from about 30?nm to 100?nm with average size of 39.18?nm, with a density ca. 2.21 × 109 particles cm?2 (Figure?1B inset). According to the average particle size, the coverage of Cu on CNS is ca. 14.2?%. TEM measurements (Figure?2 inset) confirm particle size observed via SEM. High-resolution transmission electron microscopy on scraped samples (HR-TEM) shows the Cu/CNS interface (Figure?2 main) and illustrate a close proximity between Cu and CNS. The lattice spacing of this representative Cu nanoparticle was measured as 0.204?nm, which is consistent with Cu (111). Cu2O with lattice spacing ca. 0.235?nm were present on the Cu nanoparticles surface in this image, however due to the negative potential applied for Cu deposition, the oxide likely results from exposure to air during sample preparation and transportation between measurements.[16] The surface area of the textured surface of CNS and the glassy carbon was measured based on the double layer capacitance on both electrodes in 0.1?M KOH. Capacitance was measured by recording anodic-cathodic charging currents (in the potential region where Faradaic processes are absent; see Supporting Information Figure?S3). The active surface area of CuNPs was additionally measured by Pb underpotential deposition (Supporting Information) of a representative sample, but could not be measured for each sample without contamination. The Cu nanoparticles typically contribute approximately 8?% to the total electrode ECSA for the CNS. To measure the physical stability of the catalyst, SEM images were collected of the particles and the CNS cross sections before and after a 6-hour reduction experiment (Supporting Information Figures S4, S5).   Figure 1. Figure 1. Open in figure viewerDownload Powerpoint slide Representative SEM images of Cu/CNS electrode with (A) low and (B) high magnification. The average particle size is approximately 39?nm (C) as measured by automated particle sizing of the micrographs.. Figure 2. Figure 2. Open in figure viewerDownload Powerpoint slide HR-TEM of electrodeposited copper nanoparticles on carbon nanospike electrode. Electrodeposited particles are imbedded in N-doped carbon nanospikes providing intimate contact between copper surface and reactive sites in the carbon. CO2 electroreduction activity was first measured by linear sweep voltammetry (LSV) in the potential range of ?0.00 to ?1.30?V vs. RHE at a sweep rate of 0.05?V s?1 as shown in Figure?3. In the presence of CO2-saturated potassium bicarbonate electrolyte, using the Cu/CNS, significant anodic shifts in the onset potential are observed compared to that under an argon atmosphere; the onset of activity in CO2 saturated electrolyte is ? 0.3?V more positive than in argon purged electrolyte. Note that unlike the featureless voltammograms obtained under an argon atmosphere, a subtle current plateau is obtained at ? ?0.9?V on electrodes with Cu nanoparticle in CO2 saturated electrolyte. But in the case of pristine CNS electrode, no activity towards CO2 reduction is observed except the onset of hydrogen evolution at much more negative potential. Larger current densities were obtained in Cu/CNS than either of the controls.   Figure 3. Figure 3. Open in figure viewerDownload Powerpoint slide LSV curves in potential range of 0.00 to ?1.30?V vs. RHE at a sweep rate of 0.05?V s?1 in 0.1?M KHCO3 under (A) argon and (B) CO2 atmosphere on pristine CNS (black), Cu/glassy carbon (red) and Cu/CNS (blue) electrodes. The current density is calculated using the electrochemical surface area (ECSA) of the electrode based on the double layer capacitance on CNS and glassy carbon electrodes in 0.1?M KOH, respectively.. Chronoamperometry (CA) measurements were conducted over a potential range from ?0.7 to ?1.3?V, which included these two reduction waves (representative data in Figure?4B for Cu/CNS and Supporting Information Figure S6?A for bare CNS and Cu/glassy carbon controls). New electrodes were fabricated for each data point. The gaseous and liquid products of each CA run were analyzed by gas chromatography (GC) and NMR (of headspace and electrolyte, respectively) to calculate overall current density and Faradaic efficiency for CO2 reduction and for each product. The overall sustained current density for CO2 reduction, JCO2 redn, increased with more negative potential (Supporting Information Figure?S6B) for all three electrodes, consistent with that shown in LSV curves. The Cu/CNS electrode had a greater propensity for CO2 reduction than either the Cu/glassy carbon or bare CNS electrodes; for instance, JCO2 redn from Cu/CNS was 5-fold higher than for bare CNS and 3-fold higher than for Cu/glassy carbon, at ?1.2?V.   Figure 4. Figure 4. Open in figure viewerDownload Powerpoint slide Fractional Faradaic efficiency of electrochemical reduction products at various potentials (A). The distribution of products indicates that up to ?0.9?V, only gas phase products are produced. At more negative potentials, the rate of CO production on the copper surface is high enough to allow CO dimerization to occur, producing C2 products and subsequently ethanol. Chronoamperometry on Cu/CNS at ?1.2?V (B) indicates that the electrode is stable although the distribution of products does change with time, beginning with a higher rate of H2 production which drops after the first 5000 seconds. Additional information including relative errors is available in Supporting Information Figure?S7. The fractional Faradaic efficiency was computed by dividing the total electrons into each product (determined independently by chemical analysis) by the total electrons passed during the amperometry experiment. The fractional Faradaic efficiencies for Cu/CNS plus the controls at a range of potentials are shown in Figure?4?A, and for Cu/CNS at ?1.2?V over a 6-hour experiment in Figure?4B (Additional data including relative error for Cu/CNS are available in Supporting Information Figure?S7). Due to experimental losses between the anode and cathode, the total fractions are less than 100?%. The Cu/CNS electrode appears to be stable, as the current density and fractional Faradaic efficiencies for each product barely decreased over the 6?h experiment (Figure?4?A). No significant changes in the Cu nanoparticle size and or CNS thickness was observed from SEM (Figures S4, S5), indicating that the Cu/CNS is stable under these experimental conditions.   At ?0.9?V vs. RHE and more positive potential, only gas phase products H2, CO and CH4 were obtained from all three electrodes with CH4 as the major product Cu/CNS. In contrast, with bare CNS and Cu/glassy carbon, CO was the major product and the CO / CH4 ratio was almost independent of potential. The higher selectivity towards CH4 in Cu/CNS indicates a higher degree of surface-bound CO hydrogenation, which is a key step in the formation of CH4.[17] At ?1.0?V vs. RHE and more negative potential, the current density of CO2 reduction increased and ethanol was produced (as a liquid soluble in the aqueous electrolyte) only from Cu/CNS. In comparison, only CO and CH4 were produced from both control electrodes. At-1.3?V vs. RHE the Cu/glassy carbon also produced trace ethylene (representative GC traces, Supporting Information Figure?S8). GC and NMR analysis in search of other products more commonly produced by copper electroreduction, such as methanol or ethane only indicated (representative NMR, Supporting Information Figure?S9) occasional trace formate from Cu/CNS.   Examining the breakdown of Faradaic efficiencies for various reactions on Cu/CNS, reveals that at ?1.2?V (Figure?4?A), ethanol conversion exhibited the highest efficiency at 63?% (that is, 63?% of the electrons passing through the electrode were stored as ethanol). Also at ?1.2?V vs. RHE, the Faradaic efficiency of gas phase products methane and CO dropped to 6.8?% and 5.2?%, respectively. The Faradaic efficiency of CO2 reduction (competing against water reduction) is 75?%. This means that under the best conditions, the overall selectivity of the reduction mechanism for conversion of CO2 to ethanol is 84?%.   The partial current density and Faradaic efficiency of each product from Cu/CNS electrode at various potentials were illustrated in Figure?5. The partial current density and Faradaic efficiency for CO and methane exhibited a volcanic shape dependence to the potentials applied. The maximum total current density and Faradaic efficiency were observed at ?1.0?V vs. RHE, and decreased when ethanol generation began. The partial current density for ethanol generation increased dramatically with more negative potential until reaching ?1.2?V vs. RHE, where the maximum Faradaic efficiency for ethanol generation was also achieved. Above ?1.2?V vs. RHE, the rate of increase for ethanol current density was slower, consistent with CO2 mass transport limitations. Data were not collected above ?1.3?V vs. RHE because hydrogen bubbles that evolved from water reduction blocked the electrode. The decline of Faradaic efficiency for ethanol above ?1.2?V vs. RHE suggests that the catalyst reached the mass-transport-limited current density for CO2 reduction, and therefore hydrogen evolved via H2O reduction at unoccupied active sites.   Figure 5. Figure 5. Open in figure viewerDownload Powerpoint slide Partial current density (J, red) and Faradaic efficiency (FE, blue) of CO2 reduction products from Cu/CNS electrode at various potentials. Previous reports of CO2 electroreduction on copper have demonstrated a variety of C1 and C2 products, including CO, CH4, CH2O2, ethane, ethylene, ethanol. Heavier hydrocarbons have not been reported as majority products.[9] Concerning the reaction mechanism, initial electron transfer to adsorbed CO2 will form CO2•?ads, which can be further reduced to COads or other C1 intermediates (CHOads or CH2Oads) with additional proton-electron transfer. CO will result from desorption of COads at this stage, or alternatively, further electron transfer to these surface-adsorbed species will lead to CH4.[1b, 13b] CO2 reduction results on the two controls, bare CNS and Cu nanoparticles on glassy carbon, indicate that both Cu metal and CNS are active for electrochemical CO2 reduction. On the Cu surface, stronger adsorption of CO exists than bare CNS, which provides stable intermediates for further reduction to CH4 on Cu/glassy carbon. In contrast, CO was released rather than reduced to CH4 on bare CNS.   Tafel plots (overpotential vs. the log of partial current density) for CO and CH4 are shown in Figure?6. For all three samples the plots are linear at low overpotential range with a slope that is consistent with a rate-determining initial electron transfer to CO2 to form a surface adsorbed CO2•? intermediate (120 mV / dec), a mechanism that is commonly invoked for metal electrocatalysts.[8b] At high overpotential range, steep slopes were obtained, probably indicating control by the combined effects of gas diffusion and ionic mass transport.[18] Comparing Cu/CNS to the control electrodes, a direct and intimate contact was introduced between Cu and CNS (Figure?2). Lim et?al. predicted a strong interaction between Cu nanoparticles and carbon, and we expect that to extend to CNS as well.[12] We expect that the strong interaction provides an environment in which a mechanism involving reactive sites on both the Cu surface and on the N-doped CNS may dominate.   Figure 6. Figure 6. Open in figure viewerDownload Powerpoint slide (A) CO and (B) CH4 partial current density Tafel plots. The Cu/CNS catalyst is unusual because it primarily produces ethanol rather than methane or ethylene. Ethanol, as a C2 product, requires carbon-carbon coupling between surface-adsorbed intermediates at some point during the reduction reaction. Recent calculations on C?C coupling on Cu(211) surfaces suggest the kinetic barriers for the coupling are strongly influenced by the degree of the adsorbed CO hydrogenation.[19] These kinetic barriers tend to decrease with increasing degree of the surface bound CO hydrogenation, which can favor the C2 products from CO2 reduction.[20] A high percentage of C2 products would indicate that coupling is preferred to desorption and loss of C1 intermediates, and this preference for adsorption may be due to the nanostructured nature of the surface. Although initial CO2 reduction appears to be the rate-limiting step, the resulting intermediate must be stable enough to persist until a second intermediate is available for C2 coupling. The coupling may be between two surface-bound C1 intermediates, or between a surface-bound C1 intermediate and a nearby C1 intermediate in solution.[17, 21]   The maximum Faradaic efficiency of ethanol for Cu/CNS is reached at ?1.2?V vs. RHE. Further increase in overpotential (?1.3?V vs. RHE) increases Jethanol, but results in a lower Faradaic efficiency due to an increase in H2 production. Hence the proton and electron transfers to C1 become more favorable to produce CH4, which provides a competing pathway against C2 coupling. The details of the reaction mechanism are still to be determined at this time, however there are some lessons in the literature that may yield insights into the high selectivity of this catalyst. Ordinarily, on bulk copper the coupled C2 would continue to be reduced to ethylene or ethane so long as the product was in contact with the copper electrode.[8a, 22] In contrast, with this experiment we have not been able to detect any C2 product except ethanol using the Cu/CNS (ethylene was detected in the control sample Cu/glassy carbon), indicating that the dominant reaction mechanism precludes competitive reduction to ethylene or ethane. Kondo, et al. reported that the electronic structure near the Fermi level of graphene is modified in N-doped graphene, where localized ? electronic states are reported to form at the neighboring carbon atoms, and propagate anisotropically around the defect due to the perturbation of the ?-conjugated system.[23] Due to electron-withdrawing effects in the graphene ?-conjugated system, the carbon atoms adjacent to nitrogen are positively polarized. This polarization may provide an active site adjacent to the copper for the C2 intermediates to adsorb, which may inhibit complete electroreduction.[24] Other doped or defected graphenes are well known to be catalytically active for reactions such as dehydrogenation.[25]   First-principles density functional theory (DFT) calculations were carried out to investigate whether the nitrogen dopant or strongly curled morphology in the CNS can help to adsorb the C2 intermediates. As CNS has a similar structure to multilayer graphene, a graphene sheet is adopted to model the interaction between CNS and the C2 intermediates. The dimer of CO, OCCO, was chosen as a C2 intermediate candidate[19] for modeling of the interaction with CNS. For a pristine graphene sheet, our calculations suggest the binding energy between OCCO (through one oxygen atom) and graphene is 0.19?eV with a separation distance ?2.95?Å (Supporting Information Figure?S10?A). For N-doped graphene, the N dopant and adjacent carbon atoms become more active so that the binding energy with OCCO is increased to 0.64?eV with the separation distance shortened to ?2.70?Å (Supporting Information Figure?S10B). The tripling of the binding energy to 0.64?eV clearly indicates that the C2 intermediates, once formed, can be adsorbed by N-doped CNS fairly strongly and may not desorb easily at room temperature. Furthermore, it is important to note that CNS are puckered and curled, indicating local corrugation on the surface. It has been shown previously that local deformation or buckling could enhance the molecular adsorption on carbon nanotubes and graphene.[26] Here we also considered the buckling of pristine and N-doped graphene to investigate the local curvature effect on OCCO adsorption. Upon buckling, the binding energy between OCCO and the concave surface of pristine graphene is increased to 0.34?eV (Supporting Information Figure?S10C), while the binding energy between OCCO and the concave surface of N-doped graphene is enhanced to 0.74?eV (Supporting Information Figure?S10D). Therefore, the corrugation and curvature naturally embedded into CNS could also help to strengthen the binding between CNS and the C2 intermediates. In addition, we studied the interaction between OCCO and the copper surface, and found that a strong covalent binding is present (when the molecule approaches the Cu surface oriented with one end closer to the surface) with the separation distance reduced to ?1.98?Å and binding energy increased to ?1.21?eV (Supporting Information Figure?S11). Compared to this relatively strong covalent bond, the binding between OCCO and CNS is weaker, though strong enough to prevent easy desorption of the C2 intermediate. The calculations offer important insights into the observed selective reduction, and we expect that the oxygen atom on one end of the C2 intermediates is covalently bound on reactive copper surface for complete reduction to -CH3, while the oxygen atom on the other end of the C2 intermediates is adsorbed on less reactive CNS and thus protected from complete reduction (hence forming -CH2OH), thereby providing a pathway towards selective reduction to ethanol. The possibility that a synergistic effect between Cu and CNS is responsible for the selectivity is surprising given the large size of the Cu nanoparticles, however there is no doubt that the Cu is necessary for this reaction as bare CNS do not produce the same products. Likewise, Cu nanoparticles nucleated on glassy carbon (or any other copper reported to date) do not produce the same products without CNS. While the Cu particles are relatively large, they are on the scale of the CNS which are around 50?nm in length and tend to be imbedded within the spikes. A more detailed understanding of the reaction pathway of such selective reduction of CO2 to ethanol warrants further study. Conclusion   We report an electrocatalyst which operates at room temperature and in water for the electroreduction of dissolved CO2 with high selectivity for ethanol. The overpotential (which might be lowered with the proper electrolyte, and by separating the hydrogen production to another catalyst) probably precludes economic viability for this catalyst, but the high selectivity for a 12-electron reaction suggests that nanostructured surfaces with multiple reactive sites in close proximity can yield novel reaction mechanisms. This suggests that the synergistic effect from interactions between Cu and CNS presents a novel strategy for designing highly selective electrocatalysts. While the entire reaction mechanism has not yet been elucidated, further details would be revealed from conversion of potential intermediates (e.?g. CO, formic acid and acetaldehyde) in future work. Acknowledgements   This research was conducted at the Center for Nanophase Materials Sciences, which is a Department of Energy (DOE) Office of Science User Facility. Ancillary Supporting Information   1 1a Y. Hori, K. Kikuchi, A. Murata, S. Suzuki, Chem. Lett. 1986, 15, 897–898; CrossRef | Web of Science® Times Cited: 199 1b Y. Hori, A. Murata, R. Takahashi, J. Chem. Soc., Faraday Trans. 1 1989, 85, 2309–2326; CrossRef | CAS | Web of Science® Times Cited: 318 1c D. W. DeWulf, T. Jin, A. J. Bard, J. Electrochem. Soc. 1989, 136, 1686–1691. CrossRef | CAS | Web of Science® Times Cited: 129 2 2a Y. Tomita, S. Teruya, O. Koga, Y. Hori, J. Electrochem. Soc. 2000, 147, 4164–4167; CrossRef | CAS | Web of Science® Times Cited: 43 2b M. Z. Ertem, S. J. Konezny, C. M. Araujo, V. S. Batista, J. Phys. Chem. Lett. 2013, 4, 745–748; CrossRef | PubMed | CAS | Web of Science® Times Cited: 56 2c R. Kortlever, I. Peters, S. Koper, M. T. Koper, ACS Catal. 2015. 3 3a C. Costentin, S. Drouet, M. Robert, J.-M. Savéant, Science 2012, 338, 90–94; CrossRef | PubMed | CAS | Web of Science® Times Cited: 166 | ADS 3b C. Costentin, G. Passard, M. Robert, J.-M. Savéant, J. Am. Chem. Soc. 2014, 136, 11821–11829. CrossRef | PubMed | CAS | Web of Science® Times Cited: 31 4 Y. Wang, J. Zhou, W. X. Lv, H. L. Fang, W. Wang, Appl. Surf. Sci. 2016, 362, 394–398. CrossRef | CAS | Web of Science® | ADS 5 5a C. E. Tornow, M. R. Thorson, S. Ma, A. A. Gewirth, P. J. Kenis, J. Am. Chem. Soc. 2012, 134, 19520–19523; CrossRef | PubMed | CAS | Web of Science® Times Cited: 47 5b J. Rosen, G. S. Hutchings, Q. Lu, S. Rivera, Y. Zhou, D. G. Vlachos, F. Jiao, ACS Catal. 2015, 5, 4293–4299; CrossRef | CAS | Web of Science® Times Cited: 9 5c T. Hatsukade, K. P. Kuhl, E. R. Cave, D. N. Abram, T. F. Jaramillo, Phys. Chem. Chem. Phys. 2014, 16, 13814–13819. CrossRef | PubMed | CAS | Web of Science® Times Cited: 46 | ADS 6 6a W. Zhu, Y.-J. Zhang, H. Zhang, H. Lv, Q. Li, R. Michalsky, A. A. Peterson, S. Sun, J. Am. Chem. Soc. 2014, 136, 16132–16135; CrossRef | PubMed | CAS | Web of Science® Times Cited: 52 6b D. Kim, J. Resasco, Y. Yu, A. M. Asiri, P. Yang, Nat. Commun 2014, 5; 6c W. Zhu, R. Michalsky, O. n. Metin, H. Lv, S. Guo, C. J. Wright, X. Sun, A. A. Peterson, S. Sun, J. Am. Chem. Soc. 2013, 135, 16833–16836; CrossRef | PubMed | CAS | Web of Science® Times Cited: 115 6d G. B. Stevens, T. Reda, B. Raguse, J. Electroanal. Chem. 2002, 526, 125–133. CrossRef | CAS | Web of Science® Times Cited: 41 7 S. Ye, R. Wang, M. Z. Wu, Y. P. Yuan, Appl. Surf. Sci. 2015, 358, 15–27. CrossRef | CAS | Web of Science® Times Cited: 21 | ADS 8 8a Y. Hori, I. Takahashi, O. Koga, N. Hoshi, J. Phys. Chem. B 2002, 106, 15–17; CrossRef | CAS | Web of Science® Times Cited: 84 8b M. Gattrell, N. Gupta, A. Co, J. Electroanal. Chem. 2006, 594, 1–19. CrossRef | CAS | Web of Science® Times Cited: 330 9 K. P. Kuhl, E. R. Cave, D. N. Abram, T. F. Jaramillo, Energy Environ. Sci. 2012, 5, 7050–7059. CrossRef | CAS | Web of Science® Times Cited: 250 10 10a A. M. Appel, J. E. Bercaw, A. B. Bocarsly, H. Dobbek, D. L. DuBois, M. Dupuis, J. G. Ferry, E. Fujita, R. Hille, P. J. Kenis, Chem. Rev. 2013, 113, 6621–6658; CrossRef | PubMed | CAS | Web of Science® Times Cited: 274 10b S. Ma, P. J. Kenis, Curr. Opin. Chem. Eng. 2013, 2, 191–199. CrossRef | Web of Science® Times Cited: 69 11 K. Manthiram, B. J. Beberwyck, A. P. Alivisatos, J. Am. Chem. Soc. 2014, 136, 13319–13325. CrossRef | PubMed | CAS | Web of Science® Times Cited: 42 12 D.-H. Lim, J. H. Jo, D. Y. Shin, J. Wilcox, H. C. Ham, S. W. Nam, Nanoscale 2014, 6, 5087–5092. CrossRef | PubMed | CAS | Web of Science® Times Cited: 17 | ADS 13 13a Y. Hori, A. Murata, R. Takahashi, S. Suzuki, J. Am. Chem. Soc. 1987, 109, 5022–5023; CrossRef | CAS | Web of Science® Times Cited: 113 13b J. Kim, D. Summers, K. Frese, J. Electroanal. Chem. Interf. Electrochem. 1988, 245, 223–244. CrossRef | CAS | Web of Science® Times Cited: 94 14 C. W. Li, J. Ciston, M. W. Kanan, Nature 2014, 508, 504–507. CrossRef | PubMed | CAS | Web of Science® Times Cited: 122 | ADS 15 L. B. Sheridan, D. K. Hensley, N. V. Lavrik, S. C. Smith, V. Schwartz, C. Liang, Z. Wu, H. M. Meyer, A. J. Rondinone, J. Electrochem. Soc. 2014, 161, H558-H563. CrossRef | CAS | Web of Science® 16 M. Pourbaix, J. Electroanal. Chem. 1967, 13, 471-&. 17 A. A. Peterson, F. Abild-Pedersen, F. Studt, J. Rossmeisl, J. K. Norskov, Energy Environ. Sci. 2010, 3, 1311–1315. CrossRef | CAS | Web of Science® Times Cited: 283 18 M. L. Perry, J. Newman, E. J. Cairns, J. Electrochem. Soc. 1998, 145, 5–15. CrossRef | CAS | Web of Science® Times Cited: 222 19 J. H. Montoya, A. A. Peterson, J. K. Norskov, ChemCatChem 2013, 5, 737–742. Wiley Online Library | CAS | Web of Science® Times Cited: 47 20 R. Kas, R. Kortlever, A. Milbrat, M. T. M. Koper, G. Mul, J. Baltrusaitis, Phys. Chem. Chem. Phys. 2014, 16, 12194–12201. CrossRef | PubMed | CAS | Web of Science® Times Cited: 47 | ADS 21 F. Calle-Vallejo, M. T. M. Koper, Angew. Chem. Int. Edit. 2013, 52, 7282–7285. Wiley Online Library | CAS | Web of Science® Times Cited: 51 22 22a W. Tang, A. A. Peterson, A. S. Varela, Z. P. Jovanov, L. Bech, W. J. Durand, S. Dahl, J. K. Norskov, I. Chorkendorff, Phys. Chem. Chem. Phys. 2012, 14, 76–81; CrossRef | PubMed | CAS | Web of Science® Times Cited: 108 | ADS 22b I. Takahashi, O. Koga, N. Hoshi, Y. Hori, J. Electroanal. Chem. 2002, 533, 135–143. CrossRef | CAS | Web of Science® Times Cited: 44 23 T. Kondo, Y. Honma, J. Oh, T. Machida, J. Nakamura, Phys. Rev. B 2010, 82, 153414. CrossRef | CAS | Web of Science® Times Cited: 22 | ADS 24 24a K. Gong, F. Du, Z. Xia, M. Durstock, L. Dai, Science 2009, 323, 760–764; CrossRef | PubMed | CAS | Web of Science® Times Cited: 2287 | ADS 24b L. Zhang, J. Niu, L. Dai, Z. Xia, Langmuir 2012, 28, 7542–7550; CrossRef | PubMed | CAS | Web of Science® Times Cited: 93 24c L. Zhang, Z. Xia, J. Phys. Chem. C 2011, 115, 11170–11176. CrossRef | CAS | Web of Science® Times Cited: 403 25 25a Z. W. Tang, H. Chen, X. W. Chen, L. M. Wu, X. B. Yu, J. Am. Chem. Soc. 2012, 134, 5464–5467; CrossRef | PubMed | CAS | Web of Science® Times Cited: 53 25b V. Schwartz, W. J. Fu, Y. T. Tsai, H. M. Meyer, A. J. Rondinone, J. H. Chen, Z. L. Wu, S. H. Overbury, C. D. Liang, ChemSusChem 2013, 6, 840–846; Wiley Online Library | PubMed | CAS | Web of Science® Times Cited: 18 25c G. K. P. Dathar, Y. T. Tsai, K. Gierszal, Y. Xu, C. D. Liang, A. J. Rondinone, S. H. Overbury, V. Schwartz, ChemSusChem 2014, 7, 483–491; Wiley Online Library | PubMed | CAS | Web of Science® Times Cited: 23 25d X. J. Cui, Y. H. Li, S. Bachmann, M. Scalone, A. E. Surkus, K. Junge, C. Topf, M. Beller, J. Am. Chem. Soc. 2015, 137, 10652–10658. PubMed | Web of Science® Times Cited: 12 26 26a L. B. da Silva, S. B. Fagan, R. Mota, Nano Lett. 2004, 4, 65–67; CrossRef | CAS | Web of Science® Times Cited: 65 | ADS 26b V. Tozzini, V. Pellegrini, J. Phys. Chem. C 2011, 115, 25523–25528. CrossRef | CAS | Web of Science® Times Cited: 58

One thought on “High-Selectivity Electrochemical Conversion of CO2 to Ethanol using a Copper Nanoparticle/N-Doped Graphene Electrode

  1. Hub

    Cloudy or still days mean energy production drops at solar panels or wind farms. Scientists at Oak Ridge National Laboratory developed a new process that could change this situation. They found that tiny spikes of carbon combined with copper particles convert carbon dioxide into ethanol fuel. The catalysts take a waste product of coal used in power plants and other hydrocarbon combustion reactions, in the presence of electrical energy, and create liquid fuel. Their finding was a surprise. They had been studying only the first step of a reaction and realized the catalyst was orchestrating the entire reaction, converting dissolved carbon dioxide to ethanol with a 63 percent yield.


Leave a Reply

Your email address will not be published. Required fields are marked *