AVS 60th International Symposium and Exhibition | |
Surface Science | Friday Sessions |
Session SS-FrM |
Session: | Oxides and Semiconductors: Structure and Reactivity |
Presenter: | D.R. Mullins, Oak Ridge National Laboratory |
Authors: | P.M. Albrecht, Oak Ridge National Laboratory D.R. Mullins, Oak Ridge National Laboratory |
Correspondent: | Click to Email |
Carbonate, [CO3]2- is a stable intermediate in the water-gas shift reaction (CO + H2O --> H2 + CO2) over inverse CeOX/Au(111) catalysts, relevant to efficient H2 production [1]. In addition, carbonate has recently been proposed as the high-temperature (600-700 K) intermediate in the dehydrogenation of methanol [2], and possibly in the complex reaction of acetaldehyde, on CeO2(100).
Here, we probe the formation and reaction of the carbonate species on CeOX(100) as a function of temperature and Ce oxidation state by adsorbing CO2 at 180 K. There is a marked variation in the stability of the carbonate species with the crystallographic orientation of the ceria thin film. Temperature-programmed desorption (TPD) identifies CO2 as the sole product, with desorption states at 230 K, 410 K, 510 K, and 655 K in the case of stoichiometric CeO2(100). On CeO2(111), carbonate desorbs entirely as CO2 by 300 K [1, 3].
On CeO2(100), soft X-ray photoelectron spectroscopy (sXPS) confirms the persistence of carbonate up to 600 K. Near-edge X-ray absorption fine structure (NEXAFS) at the C k-edge shows a strong angular dependence that becomes more pronounced at higher temperature (lower coverage). The excitation of the pi* resonance at grazing incidence indicates that the carbonate is lying flat on CeO2(100).
For partially reduced CeO1.67(100), we observe: (1) A substantial decrease in low-temperature (< 250 K) desorption, (2) The appearance of an intense CO2 desorption peak at higher temperature (765 K), and (3) The absence of well-defined peaks in the CO2 desorption between 300 K and 600 K.
The integrated intensity of the [CO3]2- peak in the C 1s spectrum following CO2 adsorption on CeO1.67(100) at 180 K is a factor of two greater than that for fully oxidized CeO2(100). On the reduced surface there is also no loss of this initial intensity upon heating to 300 K. At 700 K the carbonate coverage on the reduced surface is one-third of its starting value, whereas on the oxidized surface complete desorption (as CO2) has occurred. Furthermore, resonant photoemission spectroscopy (RPES) indicates negligible re-oxidation of the CeO1.67(100) surface. In contrast, an RPES study of CO2 on reduced CeOX(111) demonstrated partial re-oxidation at temperatures as low as 300 K [4].
Research sponsored by the Division of Chemical Sciences, Geosciences, and Biosciences, Office of Basic Energy Sciences, US Department of Energy.
[1] S. D. Senanayake et al., J. Catal. 271, 392 (2010).
[2] P. M. Albrecht and D. R. Mullins, Langmuir 29, 4559 (2013).
[3] S. D. Senanayake and D. R. Mullins, J. Phys. Chem. C 112, 9744 (2008).
[4] T. Staudt et al., J. Catal. 275, 181 (2010).