catalysts
Article
The Potassium-Induced Decomposition Pathway of
HCOOH on Rh(111)
Imre Kovács 1, * , János Kiss 2 and Zoltán Kónya 2,3
1
2
3
*
Institute of Technology, University of Dunaújváros, Táncsics M. u. 1/A, 2401 Dunaújváros, Hungary
MTA-SZTE Reaction Kinetics and Surface Chemistry Research Group, University of Szeged, Rerrich Béla
Square 1, 6720 Szeged, Hungary; jkiss@chem.u-szeged.hu (J.K.); konya@chem.u-szeged.hu (Z.K.)
Department of Applied and Environmental Chemistry, University of Szeged, Interdisciplinary Excellence
Centre, Rerrich Béla Squer 1, H-6720 Szeged, Hungary
Correspondence: kovacsimidr@gmail.com
Received: 28 May 2020; Accepted: 13 June 2020; Published: 16 June 2020
Abstract: Formic acid (FA) can be considered both a CO and a H2 carrier via selective dehydration and
dehydrogenation pathways, respectively. The two processes can be influenced by the modification
of the active components of the catalysts used. In the present study the adsorption of FA and the
decomposition of the formed formate intermediate were investigated on potassium promoted Rh(111)
surfaces. The preadsorbed potassium markedly increased the uptake of FA at 300 K, and influenced
the decomposition of formate depending on the potassium coverage. The work function (∆φ) is
increased by the adsorption of FA on K/Rh(111) at 300 K suggesting a large negative charge on the
chemisorbed molecule, which could be probably due to the enhanced back-donation of electrons
from the K-promoted Rh into an empty π orbital of HCOOH. The binding energy of the formate
species is therefore increased resulting in a greater concentration of irreversibly adsorbed formate
species. Decomposition of the formate species led to the formation of H2 , CO2 , H2 O, and CO, which
desorbed at significantly higher temperatures from the K-promoted surface than from the K-free
one as it was proven by thermal desorption studies. Transformation of surface formate to carbonate
(evidenced by UPS) and its decomposition and desorption is responsible for the high temperature CO
and CO2 formation.
Keywords: formic acid decomposition; formate intermediate; potassium adatom; Rh surfaces
1. Introduction
Formic acid (FA), HCOOH, is an important chemical for the renewable energy system. FA can
be decomposed to CO and H2 O by dehydration or to H2 and CO2 by dehydrogenation. A third way
gives green syngas by competitive decomposition [1–3]:
HCOOH = CO + H2 O
(1)
HCOOH = CO2 + H2
(2)
HCOOH = CO + H2 + O
(3)
The selective decomposition path of FA offers promising channels either for high purity CO,
which is widely used in semiconductor industry [4] or for H2 in high purity, which can be applied
for fuel cell vehicles; FA is a good candidate as a H2 storage compound [5–8]. The importance
of FA for fuel cell application can be demonstrated nowadays by an increased number of patents.
In addition, the FA decomposition can provide syngas with different CO/H2 ratio for chemical synthesis
Catalysts 2020, 10, 675; doi:10.3390/catal10060675
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or applications [1]. FA can be synthetized by either the catalytic CO2 hydrogenation [9,10] or the
oxidation of biomass [11,12]. It was found that alkali cation (Na+ ) near to Rh particles promote the
conversion of CO2 towards HCOOH production via formation of formate. The formate species and
the hydride rhodium complexes are considered reaction intermediates in formic acid formation [10].
Formic acid, HCOOH, is a very useful precursor molecule in producing formate surface
intermediate because it can be dehydrogenated on metal and oxide surfaces. The knowledge of
the surface chemistry of adsorbed formate as a reaction intermediate is of great assistance in the
elaboration of the mechanism of several important catalytic reactions which contain C1 species [13]
such as water -gas shift reaction [14,15], methanol synthesis [16–20] and methanation of CO [21,22] and
CO2 [23–34]. The formate species can be detected on supported metal catalysts during these reactions
mainly with IR vibrational techniques. The IR spectra obtained after the adsorption of HCOOH were
the same on supported metal (Rh) and on the support alone. It was suggested that formate ion formed
in the above mentioned reactions, on metal sites, then it is re-located on the support, or the support
basically influence the stability of the formate species on metals. Therefore, it is desirable to investigate
its formation and stability on clean metal surfaces under UHV conditions without the disturbing
effect of the support. For this purpose, the surface study of the dissociative adsorption of FA is an
excellent topic.
It turns out from several studies that not only the support, but also the different additives have a
marked influence on the decomposition of FA and the characteristics of the surface formate on different
metal surfaces [35–42]. On rhodium surfaces, the attention is focused on the effect of electronegative
(preadsorbed oxygen) and electropositive (potassium) additives. The interaction of formic acid with
clean and oxygen-covered Rh(111) surfaces has been investigated by electron energy loss (in the
electronic range), thermal desorption and photoelectron spectroscopy [43]. The formate species on
clean Rh(111) was stable up to 200 K, but decomposed completely at 200–250 K. The major products
were: H2 and CO2 , but H2 O and CO were also formed. Preadsorbed oxygen exerted a readily
observable influence on the interaction of HCOOH with the Rh(l11) surface. It increased the extent of
dissociation of FA and extended the region of stability of surface formate by at least 80–100 K. This was
demonstrated by the higher stability of photoemission peaks of formate and by the simultaneous
production of CO2 and H2 O with Tp = 377–385 K at saturation oxygen coverage. CO production
was not observed. The effect of boron contamination on the Rh foil is different, in this case the boron
segregating from the bulk interacts with the products (H2 O, CO2 ), therefore it increases the amount of
CO and H2 [44–46].
The effect of an electropositive potassium additive on the decomposition of HCOOH on Rh(111)
was studied previously [47,48]. The photoelectron [UPS] and thermal desorption spectroscopic study
was restricted only to the low temperature region (adsorption temperature was 100 K). The preadsorbed
potassium promoted the dissociation of FA and increased the surface concentration of the most stable
formate anion. In the light of the obtained results, it is desirable to investigate the interaction between
the potassium and the formate at high temperatures, and also at different potassium and FA coverages
on Rh(111). In the present study ultraviolet photoelectron spectroscopy (UPS), work function (∆φ) and
thermal desorption spectroscopy (TDS) studies were carried out.
2. Results
2.1. Thermal Desorption Measurements
In the first series of measurements, we investigated the effects of the potassium coverage on
the desorption of HCOOH, and on the formation of the decomposition products. Molecular FA
desorption was not observed after adsorption at 300 K on clean Rh(111). CO formation was detected
with Tp = 489 K (Figure 1A). H2 appeared on TPD spectra with a weak, broad peak between 320–350 K.
CO2 and H2 O as decomposition products were not observed after adsorption at 300 K. When these
products are formed, they leave the surface immediately the clean surface. In our previous work,
Catalysts 2020, 10, 675
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where the adsorption temperature was 100 K, all CO2 and H2 O desorbed below 300 K. The transient
surface intermediate was the formate species [43].
The effect of potassium coverage (Θ
ΘK ) on the adsorption of FA at 300 K was investigated between
~0.1 and 0.36 coverages. AtΘΘK = 0.36 the potassium reaches the saturation coverage (1 ML) [49].
The presence of potassium, with different coverages, altered the bonding mode of FA and the formation
temperature of the products. Both the work function changes (∆φ)
Δϕ and the core level peak shift (XPS)
support the notation of a considerable charge transfer from K to Rh at low coverages, and a gradual
neutralization at saturation [49–54]. AtΘΘK < 0.15 the potassium is positively charged (K+ ), whileΘat
ΘK = 0.36 the potassium exhibits mainly metallic character.
A
690
B
680
593
HCOOH exp.
(L)
0.36
0.33
0.17
0.09
438
489
QMS signal M(28)
QMS signal M(28)
K coverage
587
60
36
18
3
1.5
0.25
671
0.00
Background
Figure 1. (A) Thermal desorption spectra of CO from different potassium covered Rh(111) FA exposure
was 12 L. (B) Thermal desorption spectra of CO as a function of HCOOH exposure at monolayer K
coverage (ΘK = 0.3).
Θ
Figure 1A shows the TD spectra of CO after adsorption of FA at different potassium coverages.
At Θ
ΘK = 0.09, where the potassium exhibits ionic character, a very broad feature was detected. At a
higher K concentration the potassium acquires a metallic-like character, and the CO desorption
temperature shifted to 593 and 690 K. Detailed CO desorption spectra are displayed at ΘΘK = 0.36 as a
function of FA exposures on Figure 1B. Very similar desorption features were detected after CO was
adsorbed on potassium-dosed Rh(111) [55–57]. The results indicate both strengthening of the M-C
bond and the weakening of the C-O bond in the presence of potassium, due presumably to an increased
electron occupancy of the 2π*-orbitalπof CO. Broadening and asymmetry of the vibrational peaks
suggest that the proximity of the CO molecules to the potassium adatoms influence the chemisorption
behavior, although nonlocal interactions are also indicated. Hydrogen desorbs independently of
the potassium coverage at Tp = 345 K (Figure 2A), at high exposures a tailing can be seen at the
high temperature side (~450 K). As follows from the results plotted in Figure 2B, the desorption of
H2 O occurred in new high temperature states (Tp = 440 and 500–600 K) from K covered Rh(111)
These states could be associated with the potassium stabilized water desorption and adsorbed OH
recombination especially at around monolayer potassium coverage. Strong interaction between K and
water including dissociation was established previously, and a strong thermodynamic driving force to
KOH formation (∆Hf(KOH) = −424.7 kJ/mol) was calculated
[57].
Δ
− The amount of H2 O formed during
desorption significantly increased with potassium coverages at the same FA exposure.
Catalysts 2020, 10, 675
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A
A
345 K
K
345
346 K
K
346
343 K
K
343
HCOOH exp.
exp.
HCOOH
(L)
(L)
QMS signal M(18)
QMS signal M(2)
585
585
440
440
K coverage
coverage
K
570
570
99
0.32
0.32
524
524
66
0.25
0.25
0.02
0.02
0.00
0.00
33
300
300
400
400
500
500
600 T/K
T/K 700
700
600
Θ (ΘK = 0.3).
Figure 2. (A) Thermal desorption spectra of H2 from monolayer potassium coverage,
(B) Thermal desorption spectra of H2 O from different potassium covered Rh(111).
372
372
365
365
B
B
A
A
HCOOH exp.
exp.
HCOOH
(L)
(L)
12
12
99
350
350
K coverage
coverage
K
CO 22 TDS area /a.u./
QMS signal M(44)
The CO2 TD spectra, after adsorption of FA at 300 K, are more complex, due to the desorption and
different steps of decomposition of surface complexes. Significant differences can be seen at different
potassium coverages. TDS for CO2 at ΘK = 0.1 Θ
are displayed in Figure 3A.
xx
xx
0.36
0.36
O
O
xx
1.5
1.5
O
O
0.2
0.2
++
0.1
0.1
O
O
xx
L
66 L
Background
Background
xx
xx
++
xx
O
O
xx
++
HCOOH exp.
exp. // L
L
HCOOH
++
55
10
10
15
15
ΘK = 0.1). (B) The
Figure 3. (A) Thermal desorption spectra of CO2 from low potassium coverage, (Θ
amount of desorbed CO2 as a function of potassium coverage after different HCOOH exposures at
300 K.
One dominant peak was detected; its peak temperature shifted from 350 K to 372 K with increasing
HCOOH exposure. Very probably, the potassium stabilized the formate species via an electronic
interaction [37–40], and then the stabilized formate decomposes at this temperature giving CO2 and
H2 . As the potassium coverage was increased the stabilization effect to formate also increased, very
probably surface compounds are formed. The amount of CO2 formed during desorption significantly
increased with the potassium coverage. The areas of the desorption peaks are plotted as a function of
FA exposures at different potassium coverages in Figure 3B. The effect of potassium was exhibited in
the higher desorption temperatures of decomposition products. The TD spectra obtained at ΘK = 0.2
shows an additionalΘhigh temperature desorption peak; the first two peaks developed at 672 and
Catalysts 2020, 10, 675
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705 K. When the FA exposure was increased to 6 L, a weak peak appeared at Tp = 466 K, and an
intense one developed at 581 K (Figure 4A). The TD spectra of CO2 as a function of FA exposures
Θ
the potassium has a metallic character, are
at monolayer potassium coverage (ΘK = 0.3), at which
displayed in Figure 4B. At low FA exposures, 0.3–0.6 L, two high temperature peaks with Tp = 654 K
and Tp = 675 K were developed. From 3 L exposure, the intensity of these peaks increased, and a third
peak was developed at Tp = 589 K. It is important to mention again that CO desorption happened also
at Tp = 587 K and Tp = 680 K. These coinciding temperatures in the CO and CO2 desorption strongly
suggest the same source of products. It should be emphasized that potassium stabilization also occurs
in the co-adsorbed layer, in this potassium desorption was detected at Tp = 587 K and Tp = 680 K [49].
Similar coincidence temperatures were observed after CO2 adsorption from K/Rh [49,58] and K/Pd
surfaces [59].
360
HCOOH exp.
(L)
HCOOH exp.
(L)
581
QMS signal M(44)
466
X0.5
668
705
6
X2
369
672
3
X2
664
0.3
Background
QMS signal M(44)
12
363
675
B
A
12
X2
702
528
x1
9
6
3
1.5
X2
589
0.6
0.3
Background
x1
596
706
682
x1
x1
654
700
x2
x2
x2
x2
Figure 4. (A) Thermal desorption spectra of CO2 at ΘK = 0.2. (B) CO2 desorption spectra at monolayer
Θ
K coverage, (ΘK = 0.3) as a function of HCOOH exposure.
Θ
2.2. Work Function (∆φ) and UPS Measurements
Δϕ understand the mechanism of the surface reactions in the co-adsorbed layer,
In order to help
work function and photo electron spectroscopic measurements (UPS) were carried out. The work
function changes observed following potassium deposition on a clean Rh(111) surface were reported
previously [49]. The work function of Rh decreased linearly with K exposure up to ΘK ~ 0.15,
(∆φ = −3.5 eV). Further K deposition led to a slight increase (0.5 eV) in (∆φ). The large
Θ linear decrease
Δϕ
− in the work function at low potassium coverages indicates the
Δϕformation of a species with high
dipole moment; the formation of an ionic K. Above ΘK = 0.15, a strong dipole-dipole depolarization
starts to compensate the effect of the increasing
K concentration, (formation of metallic potassium).
Θ
Independently of the potassium coverage the adsorption of FA at 300 K resulted in work function
increases (Figure 5A). The extent of increase is proportional with the K coverage. Heating of the
coadsorbed layer resulted in a complex picture (Figure 5B). A decrease in the work function corresponds
to the desorption and decomposition of adsorbed HCOOH species. Above 600 K the work function
started to increase slowly. The original value for the clean Rh surface was attained only above
900–1000 K.
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WF/ eV
WF/ eV
A
B
K coverage
0.0
+
+
+
O
+
O
O
O
+
+
+
+
0.0
K coverage
+
+
+
+
+
+
O
O
O
0.05
O
0.0
+
+
+
O
O
0.05
O
O
O
0.12
-1.0
-2.0
O
0.12
0.36
0.36
-3.0
-4.0
2.0
4.0
HCOOH exp. / L
6.0
400
600
800
Δϕ at different potassium coverage with FA exposure.
Figure 5. (A) Change of the work function, (∆φ),
(B) Change the work function during heating the adsorbed layer.
The photoemission spectra of adsorbed HCOOH were taken on a clean and K-dosed Rh(111)
surface at ΘK = 0.3. The observed photoemissions obtained after HCOOH adsorption are collected
in Table 1. Figure 6 shows the HeII UP spectra obtained on clean surface at different FA exposures.
FA adsorption
Θ at 300 K resulted in two photoemission peaks at 8.2 and 11.5 eV, which correspond to
the 5σ/1π and 4δ orbitals of CO, respectively. These orbitals can be detected also after CO adsorption
on a clean surface [55,56]. Their intensities remained constant up to 395 K, then they decreased and
disappeared
σ π
δaround 510 K. Photoemissions attributable to formate at 5.3, 8.6, 10.2 and 14.2 eV [43,60,61]
were not observed. This result supports the hypothesis that the formate is not a stable intermediate
above 300 K on a clean surface.
Table 1. Binding energies (in eV) of adsorbates observed following HCOOH on Rh(111) and K/Rh(111).
HCOOH
only at 100K
HCOO−
CO3 2−
CO
O
θK
UPS
References
0
0.1
0.33
θ
0
0.1
0.33
0.33
0
0.1
0.33
0
0.33
6.2 8.9 10.5 11.9
6.2 9.1 10.5 12.0
6.2 9.1 10.5 12.0
5.3 8.9 10.2 13.2
5.2 8.9 10.2 14.2
5.2 8.9 10.3 14.0
8.4 10.2
8.0 10.8
8.0 10.9
9.0 11.5
~6
5.2
[43]
[48]
[48]
[43,60,61]
[48]
[48], this work
[48,62] this work
[55,56]
[48]
[48,51], this work
[57]
[56,57], this work
UPS after FA adsorption at 300 K and subsequent heating are presented in Figure 7. When the
FA was introduced to the potassium-covered Rh(111) at ΘK = 0.3, which corresponds to monolayer
coverage, the ultraviolet spectrum was complex at 300 K (Figure 7). On this potassium-covered surface
peaks were found at 5.4, 8.9, 10.3, 14.2 eV, which correspond, to the 6a1 , 4b2 , 5a1 and 4a1 orbitals of
formate, respectively [43,60,61]. Above 420 K this adsorption form cannot be detected above 507 K.
The strong peaks are due to adsorbed CO found up to 705 K at 8.1 and 11.5 eV, which are characteristic
Θ
Catalysts 2020, 10, 675
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of adsorbed CO on potassium-covered Rh(111) [48,51,56]. From 507 K shoulders are visible at ~8.4
and 10.3 eV. These emissions can be attributed to surface carbonate and are detectable up to 640 K.
The weak feature could be due either to the
σ πlow concentration of this surface compound or to the
strong overlapping of the CO 5σ/1π orbital with the unresolved combination of 3e’/1a” molecular
orbitals of the CO3 species at 8.4 eV. The observed photoemission peaks conform well to those obtained
for other carbonate species (3e’.1a” unresolved and 4a’ orbitals) including K2 CO3 [48,62]. From 640 K
an additional emission showed up at ~5.0 eV which could be attributed to adsorbed oxygen bonded to
potassium (K2 O) [56,57].
510 K
455 K
N(E) / a u /
395 K
6 L HCOOH
11.5
8.2
Clean Rh(111)
EF
BINDING ENERGY / eV
Figure 6. UP spectra after adsorption of FA on clean Rh(111) at 300 K and subsequent heat treatment.
FA exposure was 12 L.
Catalysts 2020, 10, 675
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713 K
640 K
N(E) / a. U. /
4.8
551 K
10.3
11.5
7.9
507 K
420 K
359 K
14.2
10.3
17.6
8.9
5.4
6 L HCOOH
Monolayer K
BINDING ENERGY / eV
EF
Figure 7. UP spectra after adsorption of FA on potassium covered Rh(111) at monolayer K coverage,
ΘK = 0.3 at 300 K and subsequent heat treatment. FA exposure was 12 L.
Θ
3. Discussion of Surface Reaction Mechanism
The study of the decomposition of HCOOH (FA) and the surface chemistry of formate (HCOO)
is receiving increasing attention nowadays. As we demonstrated in the Introduction, the selective
decomposition path of FA offers promising channels to access high purity H2 production and FA is a
good candidate as a H2 storage compound [2–4]. The classic Sachtler–Fahrenfort volcano curve for
HCOOH decomposition by metal powder catalysts is revisited with application of a modern catalysis
approach. The Rh is positioned around the top of the volcano curve [63]. From a catalytic point of
view, FA is a very useful precursor molecule in producing formate surface intermediates formed in
several catalytic reactions. Formate could be an important intermediate in CO2 methanation [31–34,64].
Formate may also be hydrogenated to methoxy species, which produces methanol [16–20]. Both
formate [37,48,65] and methoxide [66,67] can be stabilized by alkali promotors. Rh is one of most
investigated metals for CO2 hydrogenation reactions [31,32]. In this, reaction the formate intermediate
may decompose to CO, or on the other hand, the formate may be further hydrogenated producing
CH4 . Moreover, the production of CO and the methane on supported Rh catalysts depend upon
the temperature, pressure, and presence or absence of promotor. Addition of Ba and K to the Al2 O3
support results in significant differences in the catalytic behavior [31,68]. CH4 was preferentially
formed on Ba-containing and pure Rh/Al2 O3 and only CO was observed with K-containing catalysts.
All these findings motivated us to focus experimentally on the surface chemistry of
HCOOH/formate on Rh without support. The ongoing interest in the surface chemistry of FA
Catalysts 2020, 10, 675
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has also attracted recently extensive density functional theory (DFT) calculations for HCOOH
decomposition on slabs of modified metal surfaces with different facets [69]. Different additives
(B, O, alkali metals and NH4 ) significantly alter the decomposition pathway of FA and formate on
metal surfaces [35,37–40,42,43,48,70]. Electropositive adatoms (Cs, K, NH4 ) on metals enhance the
extent of dissociation of FA [37–40,48,70]. In the present study, the adsorption and decomposition
of FA were studied on potassium-promoted Rh(111). The adsorption temperature was 300 K.
We demonstrated that this adsorption temperature caused a higher dissociation and it altered the
product (CO, CO2 , H2 and H2 O) distribution. The promotor effect was significantly higher at 300 K
adsorption then at lower temperature (100 K). The quantity of the products formed during desorption
proportionally increased with potassium coverages, the product distribution was also altered at
different potassium concentrations.
The work function (∆φ) increases during the adsorption of FA on K/Rh(111) (Figure 5).
This suggests a large negative charge on the chemisorbed molecule, which is probably due to
the enhanced back-donation of electrons from the potassium-promoted Rh into an empty π orbital of
HCOOH. We may assume that this enhanced back-donation occurs directly between the formate and
the K/Rh surface. The binding energy of the formate species is therefore increased. This would result
in a greater concentration of irreversibly adsorbed formate species, and this found in TD studies. At
low potassium coverage, where the potassium is of fully ionic character, we suggest to the following
steps of formate decomposition from the observed TD spectra:
HCOOH(a) + K(a) + = {HCOO− + K(a) + } + H+ (a)
(4)
{HCOO− + K(a) + } + H+ (a) = H2(g) + CO2 + K+ (a)
(5)
{HCOO− + K(a) + } + H+ (a) = COg + H2 O(g) + K+ (a)
(6)
At higher potassium coverages the interpretation of TD spectra is more complex due to the
various desorption states. It cannot be excluded that potassium at certain coverages may stabilize the
transiently produced CO2 in dimer form. This dimer may disproportionate to carbonate and CO or
releases CO2 with Tp = 466 K. It is clearly visible at ΘK = 0.2 (Figure 4A). At monolayer K coverages
the interaction of formate and potassium could be stronger, and potassium formate is formed. The first
step of decomposition of formate the oxalate formation route in which H2 release below 450 K. In our
UP spectra, formate can be detected up to 507 K (Figure 7). This compound decomposes above 550 K
giving CO and CO2 desorption with Tp = 589 K. At the same time H2 O evolution was also detected.
Potassium formate is stable compound [71], its decomposition is described by two parallel occurring
reactions via oxalate and carbonate formation according to the literature [71]. It is important to note
that carbonate appeared in our UP spectra around 551 K at 8.4 and 10.3 eV (Figure 7). Accepting
these observations, we conclude that the potassium formate decompose similar way on the potassium
covered Rh surfaces, too:
2HCOOK(a) = K2 C2 O4(a) + H2(g)
(7)
2HCOOK(a) = K2 CO3(a) + H2 O(g)
(8)
K2 C2 O4(a) = K2 CO3(a) + CO(g)
(9)
K2 CO3(a) = K2 O + CO2(g)
(10)
CO liberates from oxalate-carbonate transformation, the CO2 releases from carbonate
decomposition. The CO and CO2 show up in gas phase at somewhat higher temperature then
steps (6) and (7) occur, because the adsorbed potassium may further stabilize them. The highest
temperature desorption peak of CO2 (Tp = 702 K) may also corresponds to K-CO2 decomposition formed
in direct interaction of two species. This feature was found after CO2 adsorption on potassium-covered
Rh(111) and Pd(100) surfaces [42,52]. The appearance of the photoemission peak at ~5 eV around
Catalysts 2020, 10, 675
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640 K may be attributed to the formation of K2 O. The schematically illustration of decomposition of
potassium stabilized formate intermediate is displayed in Figure 8.
H
HCOOH
C
O
K
H2O
H2
CO
Rh
HCOOH
Figure 8. Schematic illustration of formate decomposition on potassium promoted Rh(111) surfaces.
4. Experimental
Experiments were performed in a stainless steel UHV chamber equipped with an electron source
for Auger electron spectroscopy (AES), a photon source (He I, He II) for UPS which was pumped
differentially, and a quadrupole mass spectrometer for thermal desorption spectroscopy (TDS). An
electrostatic hemispherical energy analyzer (LRS 10, Leybold-Hereaus, Cologne, Germany) detected
auger and photoelectrons. Changes in work function ((∆φ)
Δϕ were obtained from the He I UPS spectra.
TDS were taken in “line of sight” with a heating rate of 10 Ks−l− . The Rh crystal was cut from a single
crystal. It was a product of Materials Research Corporation (Orangeburg, Route 303, NY, USA); the
purity was 99.99%. The surface orientation was determined by LEED before the present measurements
in a separate chamber. The sample was heated resistively, and its temperature was measured by a
chromel-alumel thermocouple spot-welded to the edge of the crystal. The cleaning procedure contains
argon ion bombardment (600 eV, 1 × 10−6 mbar Ar, 3 µA for 10–30
min), and annealing at 1270 K for
−
some minutes. Contaminations including boron impurity were not detected by AES. A commercial
SAES Getter alkali metal source (Lainate, Milan, Italy) was used to deposit K. The K coverage was
determined by means of AES and TDS. The determination of K coverage is described in our previous
works [48,51].
5. Conclusions
Formic acid (FA) decomposes on clean Rh(111) at room temperature leaving only CO on the
surface. Potassium adatom basically altered the reaction pathway. Potassium stabilizes the transiently
formed formate species. At low potassium coverage (ΘK < 0.15), where the K is fully ionized, a two
Θ ˂
dimensional {HCOO− + K(a) + } surface complex is formed, which decomposes to CO2 , CO, H2 and
water. At monolayer potassium coverage (ΘK ~ 0.33), the formate stabilized by potassium transforms
Θ
into surface compounds (oxalate, carbonate) in consecutive reactions, while H2 and H2 O are released.
Finally CO and CO2 are liberated from the surface. Potassium was also stabilized by coadsorbates.
Catalysts 2020, 10, 675
11 of 14
Author Contributions: All authors contributed to write the paper. All authors have read and agreed to the
published version of the manuscript.
Funding: This research received no external funding.
Acknowledgments: The authors wish to thank Albert Oszkó for the careful revision of the manuscript. Financial
support of this work by the National Research Development and Innovation Office through grant NKFIH OTKA
K120115 (Zoltán Kónya).
Conflicts of Interest: The authors declare no conflict of interest.
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