Perovskite compound, a catalyst comprising the same, and an electrochemical device comprising the same

Abstract

The perovskite compound according to the invention has a cubic perovskite structure, has high catalytic activity in oxygen reduction and evolution reactions, and has excellent durability, and thus, can be used as a catalyst of electrochemical devices, particularly as a fuel cell catalyst.

Claims

1. A perovskite compound represented by the following Chemical Formula 1:
(A.sub.aA′.sub.1-a).sub.α(B.sub.bB′.sub.1-b)βO.sub.3-δ  [Chemical Formula 1] in Chemical Formula 1, A is Ba, A′ is one or more selected from the group consisting of lanthanoid elements, Ag, Ca, and Sr, B is Co, B′ is one or more selected from the group consisting of Ta, Nb, V, Sc, Y, Mo, W, Zr, Hf, and Ce, a is a real number greater than 0.9 and 1 or less, b is a real number greater than 0.5 and less than 0.9, α and β real numbers of 0.9 to 1.1.

2. The compound according to claim 1, wherein a is 1.

3. The compound according to claim 1, wherein B′ is Ta.

4. The compound according to claim 1, wherein b is a real number of 0.6 to 0.8.

5. The compound according to claim 1, wherein each of α and β is 1.

6. The compound according to claim 1, wherein the Chemical Formula 1 is represented by the following Chemical Formula 2:
BaCo.sub.0.8Ta.sub.0.2O.sub.3-δ  [Chemical Formula 2]

7. The compound according to claim 1, wherein the perovskite compound represented by the Chemical Formula 1 has a cubic structure.

8. A fuel cell catalyst comprising the compound according to claim 1.

Description

BRIEF DESCRIPTION OF THE DRAWING

[0034] FIG. 1(a) and FIG. 1(b) show the X-ray diffraction analysis result of the materials synthesized in Examples 1 to 3 and Comparative Examples 1 and 2. FIG. 1(a) refers to the materials synthesized in Examples 1 to 3 and Comparative Example 2, and FIG. 1(b) refers to the material synthesized in Comparative Example 1.

[0035] FIG. 2 shows the oxygen temperature programmed desorption (O.sub.2-TPD) analysis result of the materials of Example 1 and Comparative Example 1.

[0036] FIG. 3 shows the analysis result of the half cell of Experimental Example 2 through Electrochemical Impedance Spectroscopy.

[0037] FIG. 4 shows the measurement result of the performance of the solid oxide fuel cell of Experimental Example 3.

[0038] FIG. 5(a) and FIG. 5(b) show the measurement result of the performances of the protonic ceramic fuel cell (FIG. 5(a)) and water electrolysis cell (FIG. 5(b)) of Experimental Example 4.

[0039] FIG. 6 is a graph showing current according to operation time while reversibly operating the protonic ceramic electrochemical device of Experimental Example 4.

DETAILED DESCRIPTION OF THE EMBODIMENTS

[0040] Hereinafter, the invention will be explained in detail through Examples and Experimental Examples. These Examples and Experimental Examples are presented only to explain the invention more specifically, and the scope of the invention is not limited thereby.

Example 1

[0041] BaCo.sub.0.8Ta.sub.0.2O.sub.3-δ perovskite was synthesized by a solid-state method. Specifically, the metal precursors of BaCO.sub.3, Co.sub.3O.sub.4, Ta.sub.2O.sub.5 were ball milled at a stoichiometric ratio together with ethanol for 24 hours using zirconia ball, dried at 90° C. for 24 hours, and then, calcined at 1150° C. for 10 hours to synthesize BaCo.sub.0.8Ta.sub.0.2O.sub.3-δ perovskite. The powders prepared were repeatedly subjected to the process of ball milling-drying-calcination to form cubic perovskite of higher purity.

Example 2

[0042] BaCo.sub.0.7Ta.sub.0.3O.sub.3-δ perovskite was synthesized by a solid-state method. Specifically, the metal precursors of BaCO.sub.3, Co.sub.3O.sub.4, Ta.sub.2O.sub.5 were ball milled at a stoichiometric ratio together with ethanol for 24 hours using zirconia ball, dried at 90° C. for 24 hours, and then, calcined at 1150° C. for 10 hours to synthesize BaCo.sub.0.7Ta.sub.0.3O.sub.3-δ perovskite. The powders prepared were repeatedly subjected to the process of ball milling-drying-calcination to form cubic perovskite of higher purity.

Example 3

[0043] BaCo.sub.0.6Ta.sub.0.4O.sub.3-δ perovskite was synthesized by a solid-state method. Specifically, the metal precursors of BaCO.sub.3, Co.sub.3O.sub.4, Ta.sub.2O.sub.5 were ball milled at a stoichiometric ratio together with ethanol for 24 hours using zirconia ball, dried at 90° C. for 24 hours, and then, calcined at 1150° C. for 10 hours to synthesize BaCo.sub.0.6Ta.sub.0.4O.sub.3-δ perovskite. The powders prepared were repeatedly subjected to the process of ball milling-drying-calcination to form cubic perovskite of higher purity.

Comparative Example 1

[0044] BaCoO.sub.3-δ was synthesized by a solid-state method. Specifically, the metal precursors of BaCO.sub.3, Co.sub.304 were ball milled together with ethanol for 24 hours using zirconia ball, dried at 90° C. for 24 hours, and then, calcined at 1150° C. for 10 hours to synthesize BaCoO.sub.3-δ.

Comparative Example 2

[0045] BaCo.sub.0.9Ta.sub.0.1O.sub.3-δ perovskite was synthesized by a solid-state method. Specifically, the metal precursors of BaCO.sub.3, Co.sub.3O.sub.4, Ta.sub.2O.sub.5 were ball milled at a stoichiometric ratio together with ethanol for 24 hours using zirconia ball, dried at 90° C. for 24 hours, and then, calcined at 1150° C. for 10 hours to synthesize BaCo.sub.0.9Ta.sub.0.1O.sub.3-δ perovskite. The powders prepared were repeatedly subjected to the process of ball milling-drying-calcination to form cubic perovskite of higher purity.

Experimental Example 1

[0046] The X-Ray diffraction analysis results of the materials synthesized in Examples 1 to 3 and Comparative Examples 1 and 2 were shown in FIG. 1(a) and FIG. 1(b). FIG. 1(a) refers to the materials synthesized in Examples 1 to 3 and Comparative Example 2, and FIG. 1(b) refers to the material synthesized in Comparative Example 1

[0047] As shown in FIG. 1(a) and FIG. 1(b), the material of Comparative Example 1 wherein a Ta precursor was not doped, exhibits a hexagonal phase, while the materials of Example 1 to 3 and Comparative Example 2 wherein Ta was doped, exhibit cubic perovskite structures.

[0048] Further, oxygen temperature programmed desorption (O.sub.2-TPD) of the materials of Example 1 and Comparative Example 1 were analyzed, and the results were shown in FIG. 2.

[0049] As shown in FIG. 2, it was confirmed that in the cubic perovskite of Example 1, oxygen desorption occurs from 290° C., and thus, it has high oxygen mobility and the resulting good oxygen catalyst properties. To the contrary, it was confirmed that in the hexagonal phase material of Comparative Example 1, oxygen desorption does not occur until 800° C., and thus, it has low oxygen mobility.

Experimental Example 2

[0050] For evaluation of oxygen reduction property, a half cell was manufactured as follows.

[0051] Specifically, 0.35 g of Sm.sub.0.2Ce.sub.0.8O.sub.2-δ powder (SDC; fuelcellmaterials company) were molded in the form of pellet, and sintered at 1400° C. for 5 hours. 8 g of an Ink vehicle(fuelcellmaterials company) and 8 g of the BaCo.sub.0.5Ta.sub.0.2O.sub.3-δ powder prepared in Example 1 were put in a Nalgene bottle and mixed, and then, zirconia ball was introduced therein to conduct ball-milling for 24 hours, thus preparing a paste, and the paste was applied on both sides of the SDC pellet by screen printing, and heat treated at 900° C. for 2 hours to prepare a half cell.

[0052] For comparison, each half cell was prepared by the same method as above, except that each 8 g of the powders prepared in Example 2 and 3, and Comparative Example 1 and 2 were used instead of 8 g of BaCo.sub.0.8Ta.sub.0.2O.sub.3-δ powder, when preparing a paste.

[0053] The performances of each half cell prepared were analyzed through Electrochemical Impedance Spectroscopy, and the results were shown in FIG. 3.

[0054] As shown in FIG. 3, it was confirmed that the electrode made of the cubic perovskite of Example 1 has much smaller electrode resistance (R.sub.p), and lower activation energy, compared to the electrode made of the hexagonal material of Comparative Example 1. For example, at 450° C., the BaCo.sub.0.8Ta.sub.0.2O.sub.3-δ electrode has resistance of 0.29 Ωcm.sup.2, while the BaCoO.sub.3-δ electrode has resistance of 21 Ωcm.sup.2, and thus there was about 100 times difference in electrode performance.

[0055] Particularly, the amount of Ta doping also had a significant influence on the oxygen reduction reaction, and the case wherein Ta was 20% doped at B-site as in Example 1 exhibited the best performance. It was judged that in case Ta is doped in an amount greater than 20%, due to the property of Ta having an oxidation number of 5+, oxygen vacancy inside perovskite decreases, and thus, catalyst properties are lowered to some degree.

Experimental Example 3

[0056] A button-type unit device of a solid oxide fuel cell (SOFC) having oxygen ion conductor as electrolyte was manufactured as follows.

[0057] 60 wt % NiO powder and 40 wt % Gd.sub.0.1Ce.sub.0.9O.sub.2-δ powder (fuelcellmaterials company) as oxygen conductor were put in a bottle and mixed, and then, zirconia ball was introduced to conduct ball-milling for 24 hours, thus preparing mixed powders. The mixed powders were molded with a 1.3 cm×1.3 cm tetragonal mold, and then, heat treated at 950° C. for 1 hour to form a fuel-electrode support. 1 g of Gd.sub.0.2Ce.sub.0.8O.sub.2-δ powder, 2 g of triethanolamine, and 10 g of ethanol were mixed to prepare an electrolyte solution, and the electrolyte solution was coated on the fuel-electrode support by drop coating, and then, heat treated at 1450° C. for 5 hours to prepare a dense electrolyte. The BaCo.sub.0.8Ta.sub.0.2O.sub.3-δ paste prepared in Experimental Example 2 was applied on the above prepared electrolyte by screen printing, and heat treated at 900° C. for 2 hours to prepare a unit device.

[0058] The operation of the electrochemical device was progressed as follows.

[0059] The manufactured unit device was placed in a reactor, and sealed with a sealant such that that gas between the fuel-electrode and air-electrode are not mixed. For the gas phase conditions applied to the SOFC unit device, air was introduced in the air-electrode, and 3% humidified hydrogen was supplied to the fuel-electrode. The performance of the fuel cell was measured at 400° C. to 550° C., and the results were shown in FIG. 4.

[0060] As shown in FIG. 4, the maximum power density was about 1.03 W cm.sup.−2 at 550° C., thus exhibiting higher performance compared to the existing SOFC. It is judged that BaCoO.sub.3-δ was successfully stabilized to cubic perovskite by Ta, and thereby, movement of oxygen molecules became smooth, and thus, electrochemical properties were improved.

Experimental Example 4

[0061] A button-type unit device of reversible protonic ceramic electrochemical cell (PCEC) having proton conductor as an electrolyte was manufactured as follows.

[0062] Specifically, 65 wt % NiO powder and 35 wt % BaZr.sub.0.1Ce.sub.0.7Y.sub.0.1Yb.sub.0.1O.sub.3-δ powder (kceracell Co. Ltd.) as oxygen conductor were put in a Nalgene bottle and mixed, and then, zirconia ball was introduced to conduct ball-milling for 24 hours, thus preparing mixed powders. The mixed powders were molded with a 1.3 cm×1.3 cm tetragonal mold, and then, heat treated at 950° C. for 1 hour to form a fuel-electrode support. 1 g of BaZr.sub.0.1Ce.sub.0.7Y.sub.0.1Yb.sub.0.1O.sub.3-δ powder, 2 g of triethanolamine, and 10 g of ethanol were mixed to prepare an electrolyte solution, and the electrolyte solution was coated on the fuel-electrode support by drop coating, and then, heat treated at 1450° C. for 5 hours to prepare a dense electrolyte. The BaCo.sub.0.8Ta.sub.0.2O.sub.3-δ paste prepared in Experimental Example 2 was applied on the above prepared electrolyte by screen printing, and heat treated at 900° C. for 2 hours to prepare a unit device.

[0063] The operation of the electrochemical device was progressed as follows.

[0064] The manufactured unit device was placed in a reactor, and sealed with a sealant such that that gas between the fuel-electrode and air-electrode are not mixed. For the gas phase conditions applied to the PCFC unit device, 3% humidified air was introduced in the air-electrode, and 3% humidified hydrogen was supplied to the fuel-electrode. The performance of the fuel cell was measured at 450° C. to 650° C., and the results were shown in FIG. 5(a) and FIG. 5(b).

[0065] As shown in FIG. 5(a), at fuel cell mode, the maximum powder density was about 0.86 W cm.sup.−2 at 650° C., thus exhibiting higher performance compared to the existing PCFC. Further, as shown in FIG. 5(b), at water electrolysis mode, current density was 1.48 A cm.sup.−2 at 1.3V, thus exhibiting higher performance compared to the existing water electrolysis cell.

[0066] Compared to the previously used SrCoO.sub.3-δ electrode, the cubic perovskite of Example 1 has the A-site substituted by Ba, and has higher basicity, and thus, it is easy to form proton in grids, thus enabling triple ion transfer (H.sup.+, O.sup.2−, e.sup.−).

[0067] The proton conductive electrochemical device may be reversibly operated at fuel cell mode or water electrolysis mode through the following Reaction Formula.

[0068] Fuel Cell Mode (Oxygen Reduction Reaction) [0069] fuel-electrode: H.sub.2.fwdarw.2H.sup.++2e.sup.− [0070] air-electrode: 2H.sup.++½O.sub.2+2e.sup.−.fwdarw.H.sub.2O

[0071] Water Electrolysis Mode (Oxygen Evolution Reaction) [0072] fuel-electrode: 2H.sup.++2e.sup.−.fwdarw.H.sub.2 [0073] air-electrode: H.sub.2O.fwdarw.2H.sup.++½O.sub.2+2e.sup.−

[0074] Further, FIG. 6 is a graph showing current according to operation time while reversibly operating the proton conductive electrochemical device.

[0075] Specifically, the electrochemical device was operated at fuel cell mode at 0.7 V for 2 hours, and operated at water electrolysis mode at 1.3 V for 2 hours. This was set as one cycle, and total 10 cycles were operated for 40 hours. During the operation, air-electrode was continuously humidified, and in general, the humidified environment promoted segregation of the existing Sr-based electrode and more rapidly deteriorated the performance, and had a negative fluence on long-term stability of an electrochemical device. However, it was confirmed that the perovskite material of Example 1 has high stability such hat there is little degradation for 40 hours, and exhibits very stable behavior.