21 research outputs found
Press notice. EC agricultural price indices. Trends in EC agricultural price indices (output and input): 1st quarter 1985. 1985.3
The
high precious metal loading and high overpotential of the oxygen
evolution reaction (OER) prevents the widespread utilization of polymer
electrolyte membrane (PEM) water electrolyzers. Herein we explore
the OER activity and stability in acidic electrolyte of a combined
IrO<sub><i>x</i></sub>/RuO<sub>2</sub> system consisting
of RuO<sub>2</sub> thin films with submonolayer (1, 2, and 4 Ă
)
amounts of IrO<sub><i>x</i></sub> deposited on top. Operando
extended X-ray absorption fine structure (EXAFS) on the Ir L-3 edge
revealed a rutile type IrO<sub>2</sub> structure with some Ir sites
occupied by Ru, IrO<sub><i>x</i></sub> being at the surface
of the RuO<sub>2</sub> thin film. We monitor corrosion on IrO<sub><i>x</i></sub>/RuO<sub>2</sub> thin films by combining
electrochemical quartz crystal microbalance (EQCM) with inductively
coupled mass spectrometry (ICP-MS). We elucidate the importance of
submonolayer surface IrO<sub><i>x</i></sub> in minimizing
Ru dissolution. Our work shows that we can tune the surface properties
of active OER catalysts, such as RuO<sub>2</sub>, aiming to achieve
higher electrocatalytic stability in PEM electrolyzers
Limitations of Electrochemical Nitrogen Oxidation toward Nitrate
The electrocatalytic N2 oxidation reaction
(NOR) using
renewable electricity is a promising alternative to the industrial
synthesis of nitrate from NH3 oxidation. However, breaking
the triple bond in the nitrogen molecule is one of the most essential
challenges in chemistry. In this work, we use density functional theory
simulations to investigate the plausible reaction mechanisms of electrocatalytic
NOR and its competition with oxygen evolution reaction (OER) at the
atomic scale. We focus on the electrochemical conversion of inert
N2 to active *NO during NOR. We propose formation of *N2O from *N2 and *O as the rate-determining step
(RDS). Following the RDS, a microkinetic model is utilized to study
the rate of NOR on metal oxides. Our results demonstrate that a lower
activation energy is obtained when a catalyst binds *O weakly. We
show that the reaction is extremely challenging but also that design
strategies have been suggested to promote electrochemical NOR
Intermetallic Alloys as CO Electroreduction Catalystsî¸Role of Isolated Active Sites
One of the main challenges associated
with the electrochemical
CO or CO<sub>2</sub> reduction is poor selectivity toward energetically
rich products. In order to promote selectivity toward hydrocarbons
and alcohols, most notably, the hydrogen evolution reaction (HER)
should be suppressed. To achieve this goal, we studied intermetallic
compounds consisting of transition metal (TM) elements that can reduce
CO (Ru, Co, Rh, Ir, Ni, Pd, Pt, and Cu) separated by TM and post transition
metal elements (Ag, Au, Cd, Zn, Hg, In, Sn, Pb, Sb, and Bi) that are
very poor HER catalysts. In total, 34 different stable binary bulk
alloys forming from these elements have been investigated using density
functional theory calculations. The electronic and geometric properties
of the catalyst surface can be tuned by varying the size of the active
centers and the elements forming them. We have identified six different
potentially selective intermetallic surfaces on which CO can be reduced
to methanol at potentials comparable to or even slightly positive
than those for CO/CO<sub>2</sub> reduction to methane on Cu. Common
features shared by most of the selective alloys are single TM sites.
The role of single sites is to block parasitic HER and thereby promote
CO reduction
A Linear Response DFT+<i>U</i> Study of Trends in the Oxygen Evolution Activity of Transition Metal Rutile Dioxides
There are known errors in oxidation
energies of transition metal
oxides caused by an improper treatment of their d-electrons. The Hubbard <i>U</i> is the computationally cheapest addition one can use to
capture correct reaction energies, but the specific Hubbard <i>U</i> oftentimes must be empirically determined only when suitable
experimental data exist. We evaluated the effect of adding a calculated,
linear response <i>U</i> on the predicted adsorption energies,
scaling relationships, and activity trends with respect to the oxygen
evolution reaction for a set of transition metal dioxides. We find
that applying a <i>U</i> greater than zero always causes
adsorption energies to be more endothermic. Furthermore, the addition
of the Hubbard <i>U</i> greater than zero does not break
scaling relationships established without the Hubbard <i>U</i>. The addition of the calculated linear response <i>U</i> value produces shifts of different systems along the activity volcano
that results in improved activity trends when compared with experimental
results
Supporting data for: A linear response, DFT+U study of trends in the oxygen evolution activity of transition metal rutile dioxides
<p>This directory contains all of the finished calculations required for fully analysis of the paper "A linear response, DFT+U study of trends in the oxygen evolution activity of transition metal rutile dioxides" by Zhongnan Xu, Jan Rossmeisl, and John R Kitchin. To use this repository, download the supporting information file and run the scripts present in either 'supporting-information.pdf' or 'supporting-information.org'.</p>
<p>The is the release of the supporting data before the first submission to the first journal.</p
Bridging the Catalyst Reactivity Gap between Au and Cu for the Reverse WaterâGas Shift Reaction
The reverse waterâgas shift reaction (rWGSR) is
highly relevant
for CO2 utilization in sustainable fuel and chemical production.
Both Au and Cu are interesting for rWGSR catalysis, but it turns out
that the reactivities of Au and Cu are very different. In this study,
we consider alloys made from Au, Ag, Cu, Pt, and Pd to identify surfaces
with reactivities for CO2 dissociation between Cu(111)
and Au(111). Additionally, interesting alloy surfaces should have
activation energies for CO2 dissociation that are only
a little higher than the endothermic reaction energy. We find that
certain Cu-based alloys with Ag and Au meet these criteria, whereas
alloys containing Pt or Pd do not. The low additional cost in activation
energy occurs when the transition-state and final-state configurations
are made to look very similar due to the placement of the different
metal elements on the surface. Finally, we construct a kinetic model
that compares the rate of the rWGSR to the estimated rate of unwanted
side reactions (i.e., methane formation or coking) on AgâCu
alloy surfaces with varying compositions and random placement of the
Ag and Cu atoms. The thermodynamics favor methane formation over rWGSR,
but the model suggests that AgâCu alloy surfaces are highly
selective for the rWGSR
Unifying the 2e<sup>â</sup> and 4e<sup>â</sup> Reduction of Oxygen on Metal Surfaces
Understanding trends in selectivity is of paramount importance
for multi-electron electrochemical reactions. The goal of this work
is to address the issue of 2e<sup>â</sup> versus 4e<sup>â</sup> reduction of oxygen on metal surfaces. Using a detailed thermodynamic
analysis based on density functional theory calculations, we show
that to a first approximation an activity descriptor, Î<i>G</i><sub>OH*</sub>, the free energy of adsorbed OH*, can be
used to describe trends for the 2e<sup>â</sup> and 4e<sup>â</sup> reduction of oxygen. While the weak binding of OOH* on Au(111) makes
it an unsuitable catalyst for the 4e<sup>â</sup> reduction,
this weak binding is optimal for the 2e<sup>â</sup> reduction
to H<sub>2</sub>O<sub>2</sub>. We find quite a remarkable agreement
between the predictions of the model and experimental results spanning
nearly 30 years
Naravne oblike gibanja kot sredstvo razvoja moÄi v mali odbojki (10-12 let)
RuO<sub>2</sub> has been reported
to reduce CO<sub>2</sub> electrochemically
to methanol at low overpotential. Herein, we have used density functional
theory (DFT) to gain insight into the mechanism for CO<sub>2</sub> reduction on RuO<sub>2</sub>(110). We have investigated the thermodynamic
stability of various surface terminations in the electrochemical environment
and found CO covered surfaces to be particularly stable, although
their formation might be kinetically limited under mildly reducing
conditions. We have identified the lowest free energy pathways for
CO<sub>2</sub> reduction to formic acid (HCOOH), methanol (CH<sub>3</sub>OH), and methane (CH<sub>4</sub>) on partially reduced RuO<sub>2</sub>(110) covered with 0.25 and 0.5 ML of CO*. We have found that
CO<sub>2</sub> is reduced to formic acid, which is further reduced
to methanol and methane. At 0.25 ML of CO*, the reduction of formate
(OCHO*) to formic acid is the thermodynamically most difficult step
and becomes exergonic at potentials below â0.43 V vs the reversible
hydrogen electrode (RHE). On the other hand, at 0.5 ML of CO*, the
reduction of formic acid to H<sub>2</sub>COOH* is the thermodynamically
most difficult step and becomes exergonic at potentials below â0.25
V vs RHE. We have found that CO<sub>2</sub> reduction activity on
RuO<sub>2</sub> changes with CO coverage, which suggests that CO coverage
can be used as a tool to tune the CO<sub>2</sub> reduction activity.
We have shown the mechanism for CO<sub>2</sub> reduction on RuO<sub>2</sub> to be different from that on Cu. On Cu, hydrocarbons are
formed at high Faradaic efficiency through reduction of CO* at âź1
V overpotential, while on RuO<sub>2</sub>, methanol and formate are
formed through reduction of formic acid at lower overpotentials. Using
our understanding of the CO<sub>2</sub> reduction mechanism on RuO<sub>2</sub>, we suggest reduction of formic acid on RuO<sub>2</sub>,
which should lead to methanol and methane production at relatively
low overpotentials
The Influence of Inert Ions on the Reactivity of Manganese Oxides
Inert
ion doping is a possible method to modify electrical conductivity
and catalytic activity of transition-metal oxide electrocatalysts.
Despite the importance of dopants, little is known about the underlying
mechanisms for the change of the system properties. We have performed
density functional theory calculations to investigate the influence
of different valent ions on the O<sub>2</sub> evolution reaction activity
of β-MnO<sub>2</sub> and Mn<sub>2</sub>O<sub>3</sub>. While
Mn<sub>2</sub>O<sub>3</sub> is unaffected by dopants, β-MnO<sub>2</sub> is strongly affected by ions placed in a subsurface position.
Doping does not affect the ion charge at the active site, but instead
it effects the bond character. This is concluded through an analysis
of the density overlap regions indicator and the density of states
showing that the partially covalent nature of the bonds in β-MnO<sub>2</sub> is responsible for the changes in the adsorbate binding energies.
This mechanism is not active in the mostly ionic Mn<sub>2</sub>O<sub>3</sub>. These results highlight the need to explicitly consider
the detailed bonding situation and to go beyond simple charge transfer
considerations when describing doping of transition metal oxide catalysts
Insight into Selectivity Differences of Glycerol Electro-Oxidation on Pt(111) and Ag(111)
Electro-oxidation is a way to utilize
glycerol, a byproduct
of
biodiesel production, to produce fuels and feedstock chemicals for
the chemical industry. A significant challenge is to get products
with high selectivity, so it is desirable to understand the glycerol
oxidation mechanisms in further detail. Using density functional theory
calculations, we investigated possible glycerol oxidation intermediates
on Pt(111) and Ag(111). We find that the different adsorption preferences
of the intermediates on Pt (adsorption via carbon atoms) and Ag (adsorption
via oxygen atoms) lead to different preferred reaction pathways, resulting
in different products. The reaction pathways on both surfaces involve
glyceraldehyde as a key intermediate; however, upon further oxidation,
Pt(111) preferentially produces glyceric acid (CH2OHâCHOHâCOOH),
while on Ag(111) CâC bonds are broken, which leads to the production
of glycolaldehyde and formic acid (CH2OHâCHO and
HCOOH). These predictions agree well with the experimental outcome
of the electro-oxidation of glycerol on Pt and Ag surfaces. Our study
therefore provides useful insights for optimizing the selectivity
of glycerol oxidation and improving the utilization of glycerol