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- W2047089466 abstract "The Gibbs free energies of key elementary steps for the electrocatalytic oxygen reduction reaction (ORR) are calculated with B3LYP type of density functional theory: O2 + M + H++ e- (0 eV) → HOO−M (ΔG1), HOO−M + M → HO−M + O−M (ΔG2), O2 + 2M + H+ + e- (0 eV) → O−M + HO−M (ΔG3), and HO−M + O−M + 3H+ + 3e- (0 eV) → 2H2O + 2M (ΔG4), where H+ is modeled as H3+O(H2O)3 and M stands for the adsorption site of a metal catalyst modeled by a single metal atom as well as by an M3 cluster. Taking Pt as a reference, ΔG4 is plotted against ΔG1 for 17 metals from groups V to XII. It is found that no single metal has both ΔG1 and ΔG4 more negative than Pt, although some of them have either more negative ΔG1 or more negative ΔG4. This enables us to explain thermodynamically why no other single metal catalyzes the ORR as effectively as Pt does. Moreover, a thermodynamic analysis reveals that the signs of ΔΔG (the difference between ΔG of other metals and ΔG of Pt) strongly correlate with the valence electronic structure of metals, i.e., ΔΔG1 < 0 and ΔΔG4 > 0 for metals M with vacant valence d orbitals, whereas ΔΔG1 > 0 and ΔΔG4 < 0 for metals M‘ with fully occupied valence d orbitals. Thus, a simple thermodynamic rule for the design of bimetallic catalysts for the ORR is proposed: couple a metal M (ΔΔG1 < 0) with a second metal M‘ (ΔΔG4 < 0) to form an alloy catalyst MM‘3. The rationale behind this selection is based on M being more efficient for the rate-determining step, i.e., for the formation of the adsorbed species M−OOH, while M‘ can enhance the reductions of O and OH in the last three electron-transfer steps." @default.
- W2047089466 created "2016-06-24" @default.
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- W2047089466 date "2005-09-17" @default.
- W2047089466 modified "2023-09-30" @default.
- W2047089466 title "Design of Oxygen Reduction Bimetallic Catalysts: Ab-Initio-Derived Thermodynamic Guidelines" @default.
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- W2047089466 doi "https://doi.org/10.1021/jp0543779" @default.
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