Z. Liu et al.
Journal of Solid State Chemistry 292 (2020) 121712
types of organic acids (acetic acid, propionic acid, n-butyric acid, and
oleic acid), and found that CeO2 synthesized with acetic acid displayed
hierarchical porosity and optimal toluene combustion active. Ren [32]
et al. used tartaric acid as the complexing agent and introduced a small
amount of nitric acid to adjust the gelation rate of LaMnO3 colloid, to
successfully construct LaMnO3 with 3DOM structure, showing good ac-
tivity in the catalytic oxidation of ethyl acetate. Besides, citric acid has
been widely used as a complexing agent to prepare metal oxides and
applied to the catalytic combustion of VOCs [19,24,33]. For example,
Zhang [34] et al. successfully prepared nanocrystalline CuMn2O4 oxide
with an abundant porous structure using citric acid, which exhibited
excellent catalytic performance in the catalytic oxidation of benzene.
However, due to the similar structure of many small molecule carboxylic
acids with citric acid, the effects of different carboxylic acids on the
composition, structure, morphology, and catalytic performance of metal
oxide catalysts are rarely mentioned. To our knowledge, the effect of
small molecular carboxylic acid on the catalytic performance of Co3O4 in
the catalytic combustion of short-chain alkanes has not been reported.
In this work, three different small molecular carboxylic acids, citric
acid (CA), oxalic acid (OA), and tartaric acid (TA), were used to assist the
synthesis of nanocrystalline Co3O4. The effects of carboxylic acids on the
physicochemical properties of nanocrystalline Co3O4 were studied by FT-
IR, XRD, BET, XPS, TEM/HRTEM, H2-TPR and O2-TPD, and their cata-
lytic performance in catalytic combustion of propane (a typical short-
chain alkane) was evaluated. The purpose of this work is to study the
effect of different small molecular carboxylic acid on the catalytic activity
of Co3O4 for propane combustion and systematically discuss the
structure-activity relationship between Co3O4 and propane conversion.
temperature-programmed unit and a thermal conductivity detector
(TCD). In the experiment, 15 mg of the catalyst was put into the constant
temperature section of the U-shaped quartz tube and pretreated at 300 ꢁC
for 1 h under high purity N2. After cooling to room temperature, the gas
was switched to a 5% H2–95% N2 mixture at a flow rate of 25 ml/min.
̊
The TCD signal was recorded at 10 C/min from room temperature to 600
ꢁC after the baseline was stable. The H2 consumption of all catalysts was
calibrated by the H2-TPR treatment of CuO powder. The oxygen tem-
perature program desorption (O2-TPD) device is the same as H2-TPR. In
each test, 100 mg of the catalyst was placed in a U-shaped quartz tube
and pretreated in high purity O2 at 300 ꢁC for 1 h. After cooling to room
temperature, the gas was switched to high purity He at a flow rate of 30
ml/min. The TCD signal was recorded at 10 ꢁC/min from room tem-
perature to 600 ꢁC after the baseline was stable. During the H2-TPR and
O2-TPD tests, the two ends of the U-shaped tube are connected to a dryer
equipped with a color-changing silica gel to eliminate the effect of water
vapor.
2.3. Catalytic tests
The catalytic combustion reaction of propane was carried out on a
CGK-5A fixed bed reactor with an inner diameter of 8 mm. The propane
concentration before and after the reaction was analyzed online using an
SC-8000 gas chromatograph equipped with a flame ionization detector
(FID), while the CO and CO2 concentrations from reaction tail gas were
measured using an SC-3000 gas chromatograph equipped with a thermal
capture detector (TCD). The composition of the raw gas was 0.3 vol %
propane balanced by air. The flow rate and catalyst loadings were 100
mL/min and 200 mg, respectively, corresponding to a gas hourly space
velocity (GHSV) of 30000 mlꢂgꢀ1ꢂhꢀ1. The conversion of propane is
2. Experimental
2.1. Catalyst preparation
YðC3H8Þ ¼ ð1 ꢀ ðC3H8Þout = ðC3H8ÞinÞ ꢃ 100%
(1)
The preparation process of the Co3O4 catalyst was similar to the
literature [24]. In a typical synthesis process, 0.0274 mol of CA, OA, and
TA were added to 25 ml of 1 mol/L Co(NO3)2ꢂ6H2O aqueous solution
under stirring, respectively. The obtained solution was continuously
stirred and evaporated at 80 ꢁC for 90 min and dried at 120 ꢁC for 6 h to
obtain the corresponding precursor. Then the precursor was calcined in
an air atmosphere at 300 ꢁC for 1 h at a heating rate of 2 ꢁC/min to
decompose the organic framework [35]. Finally, the corresponding cat-
alysts were obtained by heating to 400 ꢁC at the same heating rate for 2 h
and labeled as Co-CA, Co-OA, and Co-TA, respectively.
Where Y(C3H8) is the conversion of propane, (C3H8)in and (C3H8)out
represents the volume concentration of propane before and after the
reaction, respectively.
2.4. Reaction kinetics testing
Kinetic experiments are similar to reported in the literature [36].
Before the experiment, the effect of internal and external diffusion was
excluded. The conversion of propane is controlled below 15%, and the
reaction rate (r, mol/(s⋅g)) can be expressed by equation (2):
2.2. Catalyst characterization
r ¼ NðC3H8Þ ꢃ YðC3H8Þ=WðCatÞ
(2)
Fourier-transform infrared (FT-IR) spectrum was identified from 400
to 4000 cmꢀ1 on a Nicolet 6700 FT-IR spectrometer (ThermoFisher,
USA). The N2 adsorption-desorption analyses were measured on a NOVA
2200E nitrogen adsorption instrument (Quantachrome, USA) at ꢀ196 ꢁC.
Before testing, the catalysts were degassed under vacuum at 300 ꢁC for 3
h. The specific surface areas and pore size distributions were determined
by the Brunauer-Emmett-Teller (BET) and Barrett–Joyner–Halenda
(BJH) method, respectively. X-ray diffraction (XRD) was determined by a
Where N(C3H8) is the flow rate of propane (mol/s) and W(Cat) is the
mass of the catalyst (g). The process of propane oxidation is irreversible,
and the effects of reaction products H2O and CO2 on the reaction rate can
be ignored. Thus, the reaction rate equation can also be expressed by the
r ¼ Aexpð ꢀ Ea = RTÞPa POb
(3)
C3H8
2
diffractometer (Shimadzu, Japan) with Cu K
α radiation (λ ¼ 0.1541 nm)
Where T (K) is the reaction temperature, R is the ideal gas constant
(8.314 J/(mol⋅K)), Ea (kJ/mol) is the apparent activation energy, and A
is the pre-exponential factor. During the test, when the propane con-
version rate is less than 15%, the composition of the raw gas is approx-
imately constant. The relationship between ln r and RT can be obtained
operated at 40 kV and 30 mA. The scan rate and step sizes were 4 ꢁC/min
and 0.02ꢁ, respectively. The transmission electron microscope (TEM/
HRTEM) was completed by the Tecnai G2 F20 electron microscope (FEI,
USA) at an acceleration voltage of 200 kV. X-ray photoelectron spec-
troscopy (XPS) was performed by the XSAM800 spectrometer (Kratos,
USA) using Al K
calibrated based on the C 1s spectrum (284.8 eV). The hydrogen
temperature-programmed reduction (H2-TPR) device consists of
α radiation (1253.6 eV). The electron binding energy was
lnr ¼ ꢀ Ea=RT þ C
(4)
a
2