CATALYSTS FOR SYNGAS PRODUCTION CROSS-REFERENCE TO RELATED APPLICATION [0001] This application claims benefit of US Provisional Application No. 63/330,017 filed on April 12, 2022. US Provisional Application No.63/330,017 is incorporated herein by reference. A claim of priority is made. BACKGROUND [0002] The dry reforming of methane (DRM) is a process to convert two major greenhouse gases, carbon dioxide (CO ₂ ) and methane (CH ₄ ), into syngas. It could potentially alleviate the adverse influence of these pollutants while supplying widely consumed chemicals. The syngas produced in the reaction has a stoichiometric ratio of molecular hydrogen (H ₂ ) to carbon monoxide (CO) of 1:1, so to obtain a more favorable ratio, such as that for Fischer– Tropsch synthesis (2:1), processes such as steam reforming (3:1) or autothermal reforming (2.5:1) may be implemented. The problem is that these two processes have a very negative carbon (C) footprint, and it can be more efficient to trap C and raise theH ₂ :CO ratio by taking advantage of the reactivity of CO. Moreover, the ratio can be even lower due to the reverse water-gas shift reaction. The additional reactions involved in the process are the Boudouard reaction and CH ₄ decomposition. One of the critical elements in this reaction is the catalyst stability, which depends on various factors, including coking. SUMMARY [0003] According to one aspect, a catalyst includes a double-layer perovskite support and nanoparticles including nickel and one or more transition metals, wherein the nanoparticles are in contact with the double-layer perovskite support. [0004] According to another aspect, a method of processing a feed stock includes contacting the feed stock with a catalyst, sufficient to generate a reaction product, wherein the catalyst includes: a double-layer perovskite support and nanoparticles including nickel and one or more transition metals, wherein the nanoparticles are in contact with the double-layer perovskite support. [0005] According to another aspect, a method of making a catalyst includes contacting praseodymium salt, barium salt, manganese salt, nickel salt, and a transition metal salt with one or more complexation agents sufficient to form a solution, heating the solution sufficient to form a gel, heating the gel sufficient to separate a solid, and calcining the solid. BRIEF DESCRIPTION OF DRAWINGS [0006] This written disclosure describes illustrative embodiments that are non-limiting and non-exhaustive. Reference is made to illustrative embodiments that are depicted in the figures, in which: [0007] FIG. 1 illustrates a method 100 of processing a feed stock, according to some embodiments. [0008] FIG. 2 illustrates a method 200 of making a catalyst, according to some embodiments. [0009] FIG. 3A illustrates crystalline structures of the parent PrBaMn ₂ O _5+δ (P) and the corresponding exsolved counterparts P-Ni _0.2-x Fe _x (x = 0, 0.05, 0.1, 0.2) with different Ni/Fe loading analyzed using x-ray diffraction (XRD), according to some embodiments. [0010] FIG. 3B illustrates crystalline structures of the parent PrBaMn ₂ O _5+δ (P) and P-Ni _0.2-x Fe _x (x = 0, 0.05, 0.1, 0.2) after reduction, according to some embodiments. [0011] FIG. 3C illustrates a closeup schematic of FIG. 3B showing the crystalline structures of the parent PrBaMn ₂ O _5+δ (P) and P-Ni _0.2-x Fe _x (x = 0, 0.05, 0.1, 0.2) after reduction, according to some embodiments. [0012] FIG.3D illustrates scanning electron microscopy (SEM) of pristine P-Ni _0.15 Fe _0.05 , according to some embodiments. [0013] FIG. 3E illustrates scanning electron microscopy of exsolved (E)-Ni _0.15 Fe _0.05 , according to some embodiments. [0014] FIG. 3F illustrates transmission electron microscopy (TEM) of exsolved E- Ni _0.15 Fe _0.05 , according to some embodiments. [0015] FIG. 3G illustrates high-angle annular dark-field scanning TEM (STEM) imaging and elemental mappings computed from STEM-energy dispersive x-ray spectroscopy data for the E-Ni _0.15 Fe _0.05 catalyst after H ₂ -reduction, according to some embodiments. [0016] FIG. 4A illustrates normalized Ni K-edge x-ray absorption near-edge structure (XANES) spectra of various catalysts, according to some embodiments. [0017] FIG. 4B illustrates normalized Fe K-edge x-ray absorption near-edge structure spectra of various catalysts, according to some embodiments. [0018] FIG. 4C illustrates corresponding k3-weighted Ni K-edge extended XAFS (EXAFS) spectra in k spaces, according to some embodiments. [0019] FIG. 4D illustrates Fourier transform of k3-weighted Ni K-edge EXAFS for E- Ni _0.15 Fe _0.05 and E-Ni _0.2 , according to some embodiments. [0020] FIG. 4E illustrates Ni K-edge with linear combination fitting of E-Ni _0.15 Fe _0.05 , according to some embodiments. [0021] FIG. 4F illustrates Fe K-edge with linear combination fitting of E-Ni _0.15 Fe _0.05 , according to some embodiments. [0022] FIG.4G illustrates a wavelet transform EXAFS plot of Ni foil, according to some embodiments. [0023] FIG. 4H illustrates a wavelet transform EXAFS plot of NiO, according to some embodiments. [0024] FIG. 4I illustrates a wavelet transform EXAFS plot of E-Ni _0.15 Fe _0.05 , according to some embodiments. [0025] FIG.5 illustrates dry reforming of methane activity of various catalysts after a 12 h test, according to some embodiments. [0026] FIG. 6A illustrates dry reforming of methane performance of E-Ni _0.2 and E- Ni _0.15 Fe _0.05 for a continuous catalytic reaction, according to some embodiments. [0027] FIG. 6B illustrates dry reforming of methane performance of E-Ni _0.2 and E- Ni _0.15 Fe _0.05 for a continuous catalytic reaction, according to some embodiments. [0028] FIG. 6C illustrates thermogravimetric analysis of used E-Ni _0.2 (135 h) and E- Ni _0.15 Fe _0.05 (260 h) catalysts after different times, according to some embodiments. [0029] FIG. 6D illustrates a particle size distribution histogram for E-Ni _0.15 Fe _0.05 and I- Ni _0.2 catalysts after reduction and DRM with different times on stream, according to some embodiments. [0030] FIG.7 illustrates a comparison of the present catalysts to conventional catalysts, according to some embodiments. [0031] FIG. 8A illustrates potential energy profiles for the C atom and CH oxidation pathways on Ni (111) and Ni ₄ Fe ₁ (111) surfaces, respectively, according to some embodiments. [0032] FIG.8B illustrates geometries of transition states for CH dehydrogenation and C oxidation (C oxidation pathway), according to some embodiments. [0033] FIG.8C illustrates CH oxidation and CHO dissociation (CH oxidation pathway), according to some embodiments. DETAILED DESCRIPTION [0034] Dry reforming of methane (DRM) achieves several sustainability goals simultaneously – valorizing methane and activating CO ₂ while producing hydrogen and synthesis gas. The catalyst used in DRM has an enormous effect on the process viability by controlling activity, selectivity, and stability. Typically, conventional catalysts suffer from coking and sintering. Embodiments of the present disclosure describe novel catalysts and approaches to improve conversions, improve stability, and reducing coking in catalytic reactions. The novel catalysts of the present disclosure exhibit enhanced performance and stability due to excellent anti-sintering and coking resistance. [0035] In one example, a catalyst includes a double-layer perovskite support and nanoparticles including one or more transition metals. A perovskite may include the general formula ABX ₃ , where A and B are cations and X is an anion (such as O) that binds to both. This perovskite may have a perovskite crystal structure. In another example, a catalyst includes a double-layer perovskite support and nanoparticles including nickel and one or more transition metals. For example, a catalyst may include a binary alloy system. The nanoparticles may be anchored, attached, and/or socketed to the double-layer perovskite support. For example, nanoparticles may be anchored into the support and/or anchored to the surface of the support. Anchoring may include the support being in contact with at least 20 % of the nanoparticle outer surface. Anchoring may include the support being in contact with at least 30 % or 40 % of the nanoparticle outer surface. A catalyst may be the product of exsolving and/or reducing a single or double perovskite. For example, reducing a single-layer perovskite may increase the number of layers of the perovskite. [0036] The double-layer perovskite support may include one or more of praseodymium, barium, manganese, and oxygen. In one example, the double-layer perovskite support includes all of praseodymium, barium, manganese, and oxygen homogeneously distributed across the support. The double-layer perovskite may be formed from a single perovskite. For example, reducing a single-layer perovskite may include the transformation to a layered perovskite in the tetragonal phase. Before reduction, the perovskite may include hexagonal and cubic phases. This reduction may increase the specific surface area due to formation of nanoparticles on/in the support and defects in the support lattice. The reduced support may include all of praseodymium, barium, and manganese. [0037] The nanoparticles may include transition metals, actinoids, and lanthanoids. The nanoparticles may include nickel and one or more transition metals. Transition metals may include scandium, titanium, vanadium, chromium, manganese, iron, cobalt, nickel, copper, zinc, yttrium, zirconium, niobium, molybdenum, technetium, ruthenium, rhodium, palladium, silver, cadmium, hafnium, tantalum, tungsten, rhenium, osmium, iridium, platinum, gold, and mercury. In one example, the transition metals are selected from iron, cobalt, copper, and molybdenum. For example, the nanoparticles may include nickel and iron. [0038] The nanoparticles may include a binary Ni ₃ Fe ₁ alloy. The binary Ni ₃ Fe ₁ alloy may be the product of exsolving the metal phase. For example, the nanoparticles may include a Ni/Fe molar ratio of about 1-6:1. The nanoparticles may include a Ni/Fe molar ratio of about 2-5:1. Most of the Ni may be in the metallic state. In one example, the loading of Ni ranges from about 1 wt.% to about 8 wt.%. For example, the loading of Ni may range from about 2 wt.% to about 4 wt.%. In one example, the loading of Fe ranges from about 1 wt.% to about 4 wt.%. For example, the loading of Fe may range from about 1 wt.% to about 2 wt.%. In one example, the diameter of the nanoparticles ranges from 5 nm to 150 nm. In another example, the diameter of the nanoparticles ranges from 5 nm to 75 nm. In yet another example, the diameter of the nanoparticles ranges from 10 nm to 40 nm. For example, the average diameter of the nanoparticles may range from 20 nm to 35 nm. The nanoparticles may substantially be uniformly-sized. The nanoparticles may be any shape sufficient to be in contact with the support. In one example, the nanoparticles include a spherical shape. These nanoparticles may be homogeneously distributed across the surface of the support. [0039] The nanoparticles may include exsolved nanoparticles. Exsolved nanoparticles may include nanoparticles that have migrated from a host lattice and have agglomerated. For example, transition metal cations may partially substitute the perovskite oxide (ABO ₃ ) B-site cations, then migrate (exsolve) from the host lattice and agglomerate in the form of nanoparticles. In one example, a higher percentage of exsolved nanoparticles translates to enhanced catalytic activity. These exsolved nanoparticles may possess a unique anchor effect with the support, significantly reducing sintering. For example, the nanoparticles may be at least partially socketed within the support. In one example, the exsolved fraction of Ni nanoparticles is greater than 90 %. In another example, Ni-Fe alloy nanoparticles are located in B-sites of the support. In yet another example, iron may be at least partially reduced to the metallic phase and exsolved to the surface of the perovskite matrix, forming an alloy with Ni. [0040] Nanoparticles may be anchored into a perovskite via a facile one-step in situ reduction and may have metal-support interactions. Reduction may form a double layer perovskite from a single perovskite including a mixture of hexagonal phases and cubic phases with a smooth surface. A binary alloy nanoparticle may be anchored to the double-layer perovskite by the simultaneous in situ exsolution of the active sites with a second metal promoter. These nanoparticles may stay anchored to the perovskite throughout a chemical reaction such as DRM. Anchored nanoparticles may refer to nanoparticles in contact with a support, nanoparticles secured to a support, nanoparticles within a support, and nanoparticles with metal-support interactions. The anchor effect ensures outstanding anti-sintering ability in a catalytic reaction, and the nanoparticles may exhibit excellent coking resistance ability. [0041] In one example, the catalyst may include the following formula: PrBaMn _1.6 Ni _{0.2- x} Fe _x , wherein X ranges from 0 to 0.2. For example, X may be selected from 0, 0.05, 0.1, and 0.2. This catalyst may be formed from Pr0.5Ba _0.5 Mn0.8Ni _0.2-x Fe _x , where X is selected from 0, 0.05, 0.1, and 0.2. The series Pr _0.5 Ba _0.5 Mn _0.8 Ni _0.2-x Fe _x may be altered to PrBaMn _1.6 Ni _0.2-x Fe _x by exsolving nanoparticles and reducing the catalyst. The Ni/Fe loading may be adjusted sufficient for use in a catalytic reaction. In another example, the catalyst may include the following formula: PrBaMn _1.6 Ni _0.15 Fe _0.05 . This catalyst may be formed from Pr0.5Ba _0.5 Mn _0.8 Ni _0.2-x Fe _x , where X is selected from 0, 0.05, 0.1, and 0.2. The Ni/Fe loading may be adjusted sufficient for use in a catalytic reaction. [0042] The catalyst may be synthesized by an improved sol-gel method. The catalyst may be exsolved and reduced. Exsolving may include separating two or more components. Reducing may include heating the catalyst. Reducing may also include heating the catalyst in a gas for a time setpoint. Reducing a transition metal may transform the transition metal to the metallic state. Reducing transition metals may transform a majority of the total transition metal to the metallic phase. For example, reducing Ni may include reducing more than 70% of the total Ni to the metallic state. In another example, reducing Ni may include reducing more than 90% of the total Ni to the metallic state. Therefore, only 10% or less Ni may remain in the oxidation state. Reducing a second transition metal, such as iron, may partially reduce to the metallic phase and exsolve to the surface of the support, forming an alloy with Ni. [0043] The catalyst may be utilized for DRM, steam reforming of methane (SRM), catalytic decomposition of methane (CDM), and electrochemistry including solid oxide fuel cell (SOFC). In the application of thermal catalysis, the catalyst possesses outstanding anti- sintering and coking resistance, so that the catalyst exhibits a non-existent or slow coke formation rate and robust stability in chemical reactions. In the application of the electrochemistry, the catalyst can be used as electrode, which activates the fuel and also conducts the electrons, thus facilitating the anode reaction. For example, in SOFC fueled with hydrocarbon and their derivatives, the catalyst can be utilized as an anode that shows high C- H activation, excellent conductivity, and carbon resistant ability for long term SOFC stability. [0044] During DRM with a catalyst including a binary alloy system, the CHO* oxidation route may prevailingly dominate, promoting the oxidation of CH* instead of decomposing to C*, inhibiting the C deposition. Moreover, the weakening binding strength of the C* atom alleviates the C deposition on the binary alloy surface. The enrichment of the oxygen- containing species facilitates the oxidation of intermediate CH _x and surface C, eliminating coking on the binary alloy surface, thereby significantly boosting the stability of the nanoparticle-decorated double-layer perovskite during the DRM reaction. [0045] In one example, a metal alloy including two or more distinct transition metals may provide a synergistic effect. This synergistic effect is not shown in nanoparticles including only one metal. The electron density of the first metal may be changed, effecting the rate determining step in DRM: CH ₄ dissociation. Importantly, the metal alloy formed between a first metal and second metal can improve stability and alleviate C deposition, compared to a traditional catalyst with nanoparticles including a single metal. Further, the catalyst systems involving metal alloy nanoparticles may include a greater number of exsolved nanoparticles for enhancing catalytic activity. [0046] Importantly, compared to conventional catalysts, the present catalyst shows excellent sintering and coking resistance - two of the biggest problems with conventional catalysts. The present catalyst shows robust performance in harsh, high pressure conditions of chemical reactions. Additionally, the catalyst has long-term stability due in part to its unique nanoparticles and support. The nanoparticles contribute to the coking resistance – facilitating the long-term stability in reactions such as DRM. The catalyst may be resistant to coking and sintering even at pressure above 5 bar, such as 14 bar or greater. Further, the catalyst can be prepared by a one-step synthesis method involving exsolution. [0047] Referring to FIG.1, a method 100 of processing a feed stock is illustrated. Method 100 includes the following steps: [0048] STEP 110, CONTACT A FEED STOCK WITH A CATALYST, SUFFICIENT TO GENERATE A REACTION PRODUCT, includes contacting a feed stock with a catalyst, wherein the catalyst includes a double-layer perovskite support and nanoparticles include nickel and one or more transition metals, wherein the nanoparticles are in contact with the double-layer perovskite support. The catalyst may be a catalyst of the present disclosure. The feed stock may include one or more of carbon dioxide, methane, water, and hydrogen. For example, the feed stock may include methane and carbon dioxide. The reaction product may include one or more of hydrogen, water, and carbon monoxide. For example, the reaction product may include hydrogen and carbon monoxide. [0049] In one example, the reaction is selected from DRM, SRM, CDM, and SOFC. DRM converts methane and carbon dioxide to hydrogen and carbon monoxide (syngas). In one example, DRM may include a reactant mixture including methane, carbon dioxide, and nitrogen. For example, a reactant mixture may include about 33 % methane, about 34 % carbon dioxide, and about 33 % nitrogen. SRM converts methane and water to hydrogen and carbon monoxide (syngas). Produced syngas may be utilized for downstream processes. For example, syngas may be used in the Fischer-Tropsch synthesis process to produce valuable fuels and chemicals. Further, syngas must be compressed from 1-10 bar for utilization. Since the present catalyst is stable at high pressures, the produced syngas can be sent to downstream processes at high pressure. CDM converts methane to hydrogen and carbon. SOFC may utilize a solid oxide electrolyte to conduct oxygen ions from a cathode to an anode. [0050] The one or more transition metals may be selected from any transition metal. For example, the one or more transition metals may be selected from iron, cobalt, copper, and molybdenum. The double-layer perovskite support may include the tetragonal phase. This support may be free of any hexagonal and cubic phases. The catalyst may include the following formula: PrBaMn _1.6 Ni _2(0.2-X) FeX, wherein X ranges from 0 to 0.2. For example, X may be selected from 0, 0.05, 0.1, and 0.2. The Ni-Fe may be in the form of a binary alloy. This catalyst is sufficient to reduce coking and sintering in catalytic reactions, even at elevated pressures. [0051] In one example, the reaction may be operating at a pressure at or above atmospheric pressure, such as about 5 bar. In another example, the reaction may be operating at a pressure above 10 bar. In yet another example, the reaction may be operating at a pressure at or above 14 bar. This catalyst is sufficient to reduce coking and sintering in catalytic reactions, even at elevated temperatures and pressures. In one example, the reaction may be operating at a temperature above 400 °C, such as 500 °C or 600 °C. In another example, the reaction may be operating at a temperature above 700 °C, such as 800 °C or 850 °C. In yet another example, the reaction may be operating at a temperature above 900 °C. [0052] The reaction may have a gas hourly space velocity (GHSV) sufficient to produce syngas. In one example, the GHSV is above 10,000 mL g _cat ^-1 h ^-1 . For example, the GHSV may be about 12,000 mL g _cat ^-1 h ^-1 at 14 bar. In another example, the GHSV is above 15,000 mL g _cat - 1 h ^-1 . In yet another example, the GHSV is above 25,000 mL g _cat ^-1 h ^-1 . The catalyst may be utilized in any reaction vessel sufficient for the catalytic reactions of the present disclosure. The catalyst may be utilized in various reaction vessels such as an isothermal reactor and a thermal gradient reactor. [0053] In one example, the catalyst may be sufficient for over a 40% conversion of methane at T= 800 °C, CH ₄ /CO ₂ /N ₂ = 33/34/33, and GHSV = 30,000 mL g _cat ^-1 h ^-1 (DRM). In another example, the catalyst may be sufficient for over a 50% conversion of methane at T= 800 °C, CH ₄ /CO ₂ /N ₂ = 33/34/33, and GHSV = 30,000 mL g _cat ^-1 h ^-1 (DRM). In one example, the catalyst may be sufficient for over a 50% conversion of carbon dioxide at T= 800 °C, CH ₄ /CO ₂ /N ₂ = 33/34/33, and GHSV = 30,000 mL g _cat ^-1 h ^-1 (DRM). In another example, the catalyst may be sufficient for over a 60% conversion of carbon dioxide at T= 800 °C, CH ₄ /CO ₂ /N ₂ = 33/34/33, and GHSV = 30,000 mL g _cat ^-1 h ^-1 (DRM). The H ₂ /CO ratio during DRM at these conditions may be above 0.7 or above 0.8. In one example, the catalyst may have a methane conversion above 80% or above 90% for high pressure (14 bar) reactions with the following conditions: T = 800 °C, CH ₄ /CO ₂ /N ₂ = 20/60/20, and 12,000 mL g _cat ^-1 h ^-1 . [0054] In one example, the catalyst may be stable and free from deactivation in a catalytic reaction for more than 40 hours at a pressure at or above 14 bar. In another example, the catalyst may be stable and free from deactivation in a catalytic reaction for more than 100 hours. In yet another example, the catalyst may be stable and free from deactivation in a catalytic reaction for more than 250 hours. In contrast, conventional catalysts may deactivate by over 10% in just 12 hours. The rate of coke formation for the present catalyst may be less than 3E-5 mmol g _cat - ¹ s ^-1 during the catalytic reaction. For example, the rate of coke formation may be less than 5E- 8 mmol g _cat ^-1 s ^-1 , even during 260 hours of reaction. This rate of coke formation is unprecedented for these reactions. For example, the nanoparticles may be still partially anchored in the support without any observable carbon after 260 hours on stream. [0055] Importantly, the catalyst exhibits excellent catalytic performance at elevated temperatures and pressures. In the nanoparticle system, the CHO* oxidation route dominates which promotes oxidation of CH*. This oxidation occurs instead of the decomposition of C*, which inhibits C deposition. The enrichment of the oxygen-containing species assists in eliminating coking on the nanoparticle surface. The stability is enhanced during long reactions at high pressures, such as hydrogen production reforming reactions. Therefore, the catalyst is efficient for realistic and harsh reactions, long operating times on stream, and while using realistic amounts of catalyst. Enhancing the catalyst stability and run time reduces syngas production operating costs. [0056] Referring to FIG. 2, a method 200 of making a catalyst, such as the catalyst utilized in method 100, is illustrated. Method 200 includes the following steps: [0057] STEP 210, CONTACT PRASEODYMIUM SALT, BARIUM SALT, MANGANESE SALT, NICKEL SALT, AND A TRANSITION METAL SALT WITH ONE OR MORE COMPLEXATION AGENTS SUFFICIENT TO FORM A SOLUTION, includes contacting praseodymium salt, barium salt, manganese salt, nickel salt, and a transition metal salt such as iron. Praseodymium salt may include praseodymium nitrate hexahydrate, barium salt may include barium nitrate, manganese salt may include manganese nitrate tetrahydrate, and nickel salt may include nickel nitrate hexahydrate. Contacting may include mixing, stirring, placing in physical contact, and heating. Contacting may include simultaneously placing the salts and complexation agent in contact. Contacting may include simultaneously placing the salts in contact and subsequently adding the complexation agent. Contacting may include adding the salts to distilled water and/or adding the salts in any order sufficient to form the solution. [0058] Transition metal salts may include scandium, titanium, vanadium, chromium, manganese, iron, cobalt, copper, zinc, yttrium, zirconium, niobium, molybdenum, technetium, ruthenium, rhodium, palladium, silver, cadmium, hafnium, tantalum, tungsten, rhenium, osmium, iridium, platinum, gold, and mercury. In one example, the transition metal salt is selected from iron, cobalt, copper, and molybdenum. In one example, the transition metal salt includes iron nitrate nonahydrate. All salts may be dissolved in distilled water or a solvent. [0059] In one example, the one or more complexation agents include citric acid and/or ethylene glycol. The mole ratio of the metal ion to citric acid to ethylene glycol may be adjusted as desired. In one example, the mole ratio of metal ion to citric acid to ethylene glycol is 1:3:1.5. Additionally, a base may be added to the solution to maintain the solution at a desired pH. For example, a base such as ammonium hydroxide may be added to the solution. In one example, the desired pH of the solution is between 7 pH and 9 pH. In another example, the desired pH of the solution is about 8 pH; [0060] STEP 220, HEAT THE SOLUTION SUFFICIENT TO FORM A GEL, includes heating, and optionally stirring, the solution sufficient to form a gel or gel-like network. The solution may be an aqueous solution. The heating process may form a uniform gel. In one example, heating the solution may include heating the solution to/at a temperature ranging from 30 °C to 120 °C. In another example, heating the solution may include heating the solution to/at a temperature ranging from 50 °C to 100 °C. In yet another example, heating the solution may include heating the solution to/at a temperature ranging from 75 °C to 95 °C. For example, the solution may be heated to/at a temperature of about 85 °C. STEP 220 may be optionally performed simultaneously or after STEP 210. In one example, the gel includes a gel-like network of both a liquid phase and a solid phase. In another example, the gel may be a soft, solid or solid-like phase consisting of two or more components. In yet another example, the gel may include a cross-linked network of fluid. During STEP 210 and/or STEP 220, a colloidal suspension of nanoparticles may formed, and a network between phases may form. This network may be an interconnected network. During STEP 210 and/or STEP 220, agglomeration of particles or molecules in the solution may occur; [0061] STEP 230, HEAT THE GEL SUFFICIENT TO SEPARATE A SOLID, includes heating the gel, and/or drying, sufficient to separate a solid, such as a powder. In one example, heating the gel may include heating the gel to/at a temperature ranging from 100 °C to 500 °C. In another example, heating the gel may include heating the gel to/at a temperature ranging from 200 °C to 400 °C. In yet another example, heating the gel may include heating the gel to/at a temperature ranging from 300 °C to 400 °C. The gel may be heated to/at a temperature above 300 °C. For example, the gel may be heated to/at a temperature of about 350 °C. Heating the gel may be sufficient to decompose the gel slowly and completely. In one example, decomposition includes one or more organic components undergoing combustion. Heating the gel may be sufficient to form a solid, such as a powder. STEP 230 may include drying the gel sufficient to form a powder. STEP 230 may further include grinding a powder sufficient to form smaller size particles; [0062] STEP 240, CALCINE THE SOLID, includes calcining the solid, such as a powder, sufficient to form the catalyst. Calcining may refer to thermal treatment of the solid. The solid from the gel may be ground and calcined in air after heating the gel sufficient to separate the solid. In one example, the solid is calcined in gas atmosphere at a temperature ranging from 500 °C to 1200 °C. In another example, the solid is calcined at a temperature above 700 °C. In yet another example, the solid is calcined at a temperature ranging from 900 °C to 1000 °C. The solid may be calcined for any time sufficient for proper thermal treatment of the solid. In one example, the solid is calcined for about 1 hour to about 10 hours. In another example, the solid is calcined for about 2 hours to about 6 hours. In yet another example, the solid is calcined for about 4 hours in air. Calcining the solid may form a synthesized catalyst including the following formula: Pr _0.5 Ba _0.5 Mn _0.8 Ni _0.2-x Fe _x , where X is selected from 0, 0.05, 0.1, and 0.2. This catalyst may include a single perovskite with a mixture of hexagonal and cubic phases with a smooth surface. [0063] Method 200 may further include reducing the formed catalyst to form a double- layer perovskite with the exsolution of substantially spherical nanoparticles. Exsolution may include transition metals inserted into a B site of a parent perovskite oxide during the material synthesis progress. In reduction atmosphere, the transition metals may be exsolved from the perovskite lattice and are partially anchored in the perovskite matrix as uniformly dispersed nanoparticles. During the exsolution of the nanoparticles, the following changes may occur: (1) partial escape of the intensely bonded lattice oxygen atoms from the perovskite; (2) the reduction of metal cations located at the B site such as the exsolved process of Ni or Ni-Fe to the double-layer perovskite surface; and (3) the phase transformation of the single perovskite phase to the double layer perovskite phase. In one example, the catalyst is reduced to/at a temperature about 500 °C. In another example, the catalyst is reduced to/at a temperature ranging from 150 °C to 1000 °C. In yet another example, the catalyst is reduced to/at a temperature ranging from 600 °C to 900 °C. For example, the catalyst may be reduced at a temperature of about 800 °C. The catalyst may be reduced in a gas environment, such as an environment including one or more of hydrogen gas and argon. For example, the catalyst may be reduced in a 10 % H ₂ /Ar atmosphere. The reduction process may occur for about 1 hour to about 8 hours. For example, the reduction process may occur for about 5 hours to about 7 hours. [0064] The formed catalyst may include a binary metal alloy and a double-layer perovskite support. The transition metal cations may partially substitute the perovskite oxide B-site cations, then migrate (exsolve) from the host lattice and agglomerate in the form of nanoparticles. The double-layer perovskite support may include the tetragonal phase. This support may be free of any hexagonal and cubic phases. Further, the support may include praseodymium, barium, manganese, and oxygen homogeneously distributed across the support. The catalyst may include the following formula: PrBaMn _1.6 Ni _2(0.2-X) FeXO _5+δ , wherein X ranges from 0 to 0.2. For example, X may be selected from 0, 0.05, 0.1, and 0.2. The Ni-Fe may be in the form of a binary alloy. This catalyst is sufficient to reduce coking and sintering in catalytic reactions, even at elevated pressures. In one example, only Ni and Fe atoms are found in the emergent nanoparticles. [0065] The catalyst prior to reduction may include a perovskite structure with a mixture of hexagonal and cubic phases with no detectable impurity phases. After reduction, the catalyst may include a layered perovskite in the tetragonal phase. The catalyst may include Ni, wherein over 80 % of the Ni is reduced to the metallic state. In one example, the catalyst includes Ni, wherein about 94 % of Ni is reduced to the metallic state, and only 6.0 % of the Ni remains in the oxidation state. The catalyst may include iron, wherein over 70 % of the iron is in the oxidation state. The catalyst may include iron, wherein over 20 % of the iron is in the metallic state. For example, the catalyst may include iron, wherein about 25 % of the iron is in the metallic state and about 75 % of the iron is in the oxidation state. Therefore, the catalyst may include a Ni ₃ Fe ₁ alloy formed in the reduction process. The Ni ₃ F ₁ alloy nanoparticles may have an average diameter ranging from 15 nm to 30 nm. [0066] In conventional synthesis of catalysts, such as wet impregnation or vapor deposition, the synthesis lacks control of particle size, dispersion, morphology, and metal- support interaction. Importantly, this process of exsolution on perovskites overcomes these problems by improving the metal-support interactions and stabilizing the exsolved nanoparticles. The formed catalyst has significantly superior performance and longer stability compared to other catalysts, such as those formed with wetness impregnation. Further, the present catalyst may be formed with a single-step synthesis method. As the method of forming the catalyst requires few steps, this is a cost effective method of producing the stable catalyst. [0067] Importantly, a nickel alloy system may be utilized without substantially increasing the price of the catalyst. Additional transition metals may be utilized to provide a synergistic effect upon interaction with nickel. Overall, the strong metal-support interactions between the nanoparticles and the support provide anti-sintering and anti-coking properties to the catalyst. Further, the present catalyst exhibits robust stability with negligible C deposition. Since the catalyst is stable and efficient at realistically high pressures, the high pressure syngas produced may be sent directly to downstream processes. This reduces operating costs as the pressure differential between syngas production and downstream utilization is decreased. Example 1 [0068] Most conventional Ni supported catalysts suffer from sintering and coking. In this case, the goal is to change the electron density of the Ni atoms, affecting the typically considered rate determining step: CH ₄ dissociation. The alloy formed between the Ni and second metal can improve the stability, alleviating the C deposition (e.g., noble metals can enhance the stability of Ni-based catalysts). A promising approach to enhance the performance of Ni supported catalysts without affecting the price that much is to use a secondary metal, such as iron (Fe), cobalt (Co), copper (Cu), or molybdenum (Mo). In addition, Fe is very promising due to its low cost and synergistic effect upon intimate interaction with Ni. [0069] A series of Pr _0.5 Ba _0.5 Mn _0.8 Ni _0.2-x Fe _x (x = 0, 0.05, 0.1, 0.2) were synthesized using the improved sol-gel method. Stoichiometric Pr(NO ₃ ) ₃ ·6H ₂ O (99.9%, metal basis), Ba(NO ₃ ) ₂ (99%), Mn(NO ₃ ) ₂ ·4H ₂ O (98%), Ni(NO ₃ ) ₂ ·6H ₂ O (98.5%), and Fe(NO ₃ ) ₃ ·9H ₂ O (98%) were dissolved in distilled water. The appropriate amounts of citric acid (99.5%) and ethylene glycol were added into the solutions as complexation agents, adjusting the mole ratio of metal ion to citric acid to ethylene glycol as 1:3:1.5. The pH value of the solution was maintained at around 8 by adding ammonium hydroxide. The resulting aqueous solution was continuously stirred at 85 °C, forming a uniform gel, which was heated at 350°C to decompose slowly and completely. Then, the precursor powder was ground and calcined at 950 °C for 4 h in air. A sequence of Pr0.5Ba0.5Mn1-xNix (x = 0, 0.1, 0.3) was also prepared with the same procedure to investigate the effect of the Fe promoter. In contrast, the corresponding Ni-impregnated Pr _0.5 Ba _0.5 Mn ₂ O _5+δ catalyst was prepared via the wetness impregnation method and annealed at 950 °C for 4 h. The chemical composition of the prepared materials and their abbreviations are presented in Table 1. The nominal and actual loading of different catalysts are presented in Table 2.

Table 1. Chemical Compositions and abbreviations of samples. Table 2. Nominal and actual loading wt.% of catalysts. [0070] FIG. 3A illustrates crystalline structures of the parent PrBaMn ₂ O _5+δ (P) and the corresponding exsolved counterparts P-Ni _0.2-x Fe _x (x = 0, 0.05, 0.1, 0.2) with different Ni/Fe loading analyzed using x-ray diffraction (XRD), according to some embodiments. FIG. 3A shows the results after sintering at 950 °C for 4 h in air. The parent and exsolved materials include a perovskite structure with a mixture of hexagonal and cubic phases with no detectable impurity phases. FIG. 3B illustrates crystalline structures of the parent PrBaMn ₂ O _5+δ (P) and P-Ni _0.2-x Fe _x (x = 0, 0.05, 0.1, 0.2) after reduction, according to some embodiments. Reduction was completed at 800 °C in 10% H ₂ /Ar for 6 h. The reduction induced the transformation of the original perovskite into a layered perovskite in the tetragonal phase, which can increase the specific surface area due to the formation of metal (Ni or Ni-Fe alloy) nanoparticles on the support surface and defects in the lattice. [0071] FIG. 3C illustrates a closeup schematic of FIG. 3B showing the crystalline structures of the parent PrBaMn ₂ O _5+δ (P) and P-Ni _0.2-x Fe _x (x = 0, 0.05, 0.1, 0.2) after reduction, according to some embodiments. The exsolution of a metallic Ni phase was verified by the appearance of the crystal planes (111) with a d-spacing of 2.030 Å for P-Ni _0.2 . Concerning P- Ni _0.15 Fe _0.05 , the d-spacing of the exsolved metal phase increases to 2.037 Å, assigned to the (111) crystalline planes of the Ni-Fe alloy, deriving from Fe dissolving into the Ni lattice, revealing that the exsolved metal forms a binary Ni-Fe alloy. Upon reduction, the exsolved nanoparticles in B sites are MnO for P, metallic Ni for P-Ni _0.2 , and Ni-Fe alloy for P-Ni _0.15 Fe _0.05 and P‑Ni _0.1 Fe _0.1 , whereas no exsolved Fe phase is evident for P-Fe _0.2 . The same trend of transition metal exsolution in the layered perovskite was previously observed, indicating that Ni exsolves more efficiently to the surface than Mn and Fe. The results demonstrate that, although Fe alone hardly exsolves, it does so primarily with Ni, forming a Ni-Fe alloy nanoparticle. [0072] FIG.3D illustrates scanning electron microscopy (SEM) of pristine P-Ni _0.15 Fe _0.05 , according to some embodiments. FIG.3E illustrates scanning electron microscopy of exsolved (E)-Ni _0.15 Fe _0.05 , according to some embodiments. FIG. 3F illustrates transmission electron microscopy (TEM) of exsolved E-Ni _0.15 Fe _0.05 , according to some embodiments. The exsolution of the nanoparticles was observed from the morphology of the P-Ni _0.15 Fe _0.05 material. The pristine P-Ni _0.15 Fe _0.05 material is relatively smooth, whereas numerous nanoparticles emerged on the surface after H ₂ treatment (FIG. 3E), and the exsolved nanoparticle was partially socketed in the support (FIG.3F). [0073] FIG.3G illustrates high-angle annular dark-field scanning TEM (STEM) imaging and elemental mappings computed from STEM-energy dispersive x-ray spectroscopy data for the E-Ni _0.15 Fe _0.05 catalyst after H ₂ -reduction, according to some embodiments. FIG. 3G indicates the spherical shape of the Ni-Fe particles anchored to the surface of the double-layer perovskite. The interplanar spacing of the nanoparticles is 2.05 Å, which is consistent with the d‑spacing of the (111) plane of the Ni-Fe alloy phase. The particle size analysis of the E- Ni _0.15 Fe _0.05 catalyst indicates an average of 21 ± 5.6 nm. The EDS elemental mappings highlight that only Ni and Fe atoms were found in the emergent nanoparticles. The quantitative analysis of the EDS data operated on more than 30 nanoparticles indicated a molar Ni/Fe ratio of 3.6 ± 1.0. The chemical elements Pr, Ba, Mn, and O are homogeneously distributed across the support. Only traces of Ni atoms remained in the perovskite, whereas a substantial number of Fe atoms were still present. The same exsolution phenomenon of Ni nanoparticles was also observed for E-Ni _0.2 . [0074] FIG. 4A illustrates normalized Ni K-edge x-ray absorption near-edge structure (XANES) spectra of various catalysts, according to some embodiments. In the normalized Ni K-edge x-ray absorption near-edge structure (XANES) spectra, the Ni K-edge spectra almost fit with the Ni foil reference concerning the energy position and pattern, indicating that Ni is prevailingly reduced to Ni ⁰ in the two catalysts. In addition, the pre-edge peak slightly shifts to higher energy from E-Ni _0.2 to ENi _0.15 Fe _0.05 (enlarged region in FIG. 4A), demonstrating the minor increase in the Ni average oxidation state. [0075] FIG. 4B illustrates normalized Fe K-edge x-ray absorption near-edge structure spectra of various catalysts, according to some embodiments. Moreover, the white line (7131 eV) of the Fe K-edge XANES spectrum of the E-Ni _0.15 Fe _0.05 catalyst is more intense than that of Fe foil in FIG. 4B, indicating that part of the Fe is oxidized. The intensity of the pre-edge peak of E-Ni _0.15 Fe _0.05 is stronger than that of the Fe ₂ O ₃ reference. Thus, it is deduced that part of the Fe is reduced to metallic Fe ⁰ , whereas another part remains oxidized in the double-layer perovskite support. [0076] FIG. 4C illustrates corresponding k3-weighted Ni K-edge extended XAFS (EXAFS) spectra in k spaces, according to some embodiments. FIG. 4D illustrates Fourier transform of k3-weighted Ni K-edge EXAFS for E-Ni _0.15 Fe _0.05 and E-Ni _0.2 , according to some embodiments. The monometallic E-Ni _0.2 reveals the same oscillations as those of the Ni foil, whereas in terms of the bimetallic E-Ni _0.15 Fe _0.05 , the changes minorly shift to a smaller k-value. The EXAFS spectra of both E-Ni _0.2 and E‑Ni _0.15 Fe _0.05 have features similar to the Ni foil, with the majority of Ni-Ni coordination at ∼2.18 Å and a minority of Ni-O coordination (FIG.4D). The wavelet transform signals of the Ni-metal bond were observed around 8 Å ⁻¹ in the contour plots of the E-Ni _0.15 Fe _0.05 , E-Ni _0.2 , NiO reference, and Ni foil. In contrast, the Ni-O bond signals were absent except for the NiO standard. This result confirms that most Ni exists in the metallic state. [0077] FIG. 4E illustrates Ni K-edge with linear combination fitting of E-Ni _0.15 Fe _0.05 , according to some embodiments. The linear combination fitting method was adopted based on the identifiable features of each reference in the XANES spectra to quantify the distribution of different Ni and Fe oxidation states. The linear combination fitting analysis of the Ni K-edge XANES spectrum reveals that about 94.0% of Ni is reduced to the metallic state, which is almost double the results for conventional catalysts (58% Ni exsolved), and only 6.0% of Ni remains in the oxidation state in E-Ni _0.15 Fe _0.05 . [0078] FIG. 4F illustrates Fe K-edge with linear combination fitting of E-Ni _0.15 Fe _0.05 , according to some embodiments. The distribution of Fe in E‑Ni _0.15 Fe _0.05 is approximately 25.1% Fe ⁰ and 74.9% in the Fe oxidation state. FIG.4G illustrates a wavelet transform EXAFS plot of Ni foil, according to some embodiments. FIG. 4H illustrates a wavelet transform EXAFS plot of NiO, according to some embodiments. FIG. 4I illustrates a wavelet transform EXAFS plot of E-Ni _0.15 Fe _0.05 , according to some embodiments. FIGS.4G-4I confirm that most Ni exists in the metallic state. It is inferred that Fe was partially reduced to the metallic phase and exsolved to the surface of the perovskite matrix, forming an alloy with Ni. [0079] The catalytic activity and stability of the preceding impregnated (I-) and exsolved (E-) catalysts were further evaluated in dry reforming at 800 °C at atmospheric pressure and high pressure (14 bar), respectively. Catalytic tests were performed in a four-channel reactor The reactors are 300-mm-long quartz tubes, of which the outside and inside diameters are 3 and 2 mm, respectively. One of the reactors was adopted as the blank without a loading catalyst among the four channels. The proper amount of catalyst and reactant mixture gas flow was used to maintain the gas hourly space velocity (GHSV) per channel at 30,000 mL g _cat ^–1 h ^–1 under atmospheric pressure and 12,000 mL g _cat ^–1 h ^–1 under high pressure at 14 bar, respectively. The composition of the reactant mixture gas was CH ₄ :CO ₂ :N ₂ = 33%:34%:33%. Before the test, the catalysts were reduced in situ in a 10% H ₂ /Ar atmosphere for 6 h at 800°C. [0080] FIG.5 illustrates DRM activity of various catalysts after a 12 h test, according to some embodiments. FIG. 5 corresponds to the following reaction conditions: T = 800 °C, CH ₄ /CO ₂ /N ₂ = 33/34/33, and GHSV = 30,000 mL g _cat ^–1 h ^–1 . The initial reaction rate of both CH ₄ and CO ₂ is much higher for exsolved catalysts (E‑Ni _x , x = 0.1, 0.2, and 0.3) than for their impregnated counterparts (I-Nix). However, the deactivation is much faster in the impregnated catalysts than the exsolved counterparts at an 11.5% drop within 12 h on stream for the I-Ni _0.2 catalysts. The E-Nix catalysts remain stable for the CH ₄ and CO ₂ reaction rate throughout 40 h on stream, mirroring the same stability as the H ₂ /CO ratio. As for the effect of the Ni loading, the reaction rate decreased as the amount of Ni increases, in spite of the conversion delivered opposite trend, which is probably caused by the incomplete exsolution of the Ni active site. [0081] Based on the aforementioned results, E-Ni _0.2 is further modified with the dopant of Fe in the B site (E-Ni _0.2-x Fe _x (x = 0.05, 0.1, 0.2)). The CH ₄ reaction rate of the E-Ni _0.15 Fe _0.05 catalyst is slightly lower than that of the E-Ni _0.2 (FIG. 5). The CH ₄ reaction rate of the ENi _0.1 Fe _0.1 catalyst is not stable during 40 h on stream. Moreover, the CH ₄ reaction rate of E- Fe0.2 is null, indicating that the perovskite substrate and Fe nanoparticles are both inert in the conversions of CH ₄ and CO ₂ . The reaction rate of CO ₂ is faster than that of CH ₄ for all catalysts, independent of the metal loading and its nature. This phenomenon is highlighted in the Ni-Fe alloy catalyst because Fe is an active site for the reverse water-gas shift reaction. [0082] FIG. 6A illustrates DRM performance of E-Ni _0.2 and E-Ni _0.15 Fe _0.05 for a continuous catalytic reaction, according to some embodiments. The reaction conditions are as follows: T = 800 °C, CH ₄ /CO ₂ /N ₂ = 33/34/33, GHSV = 30,000 mL g _cat ^–1 h ^–1 . After around 135 h on stream, the stability test of E-Ni _0.2 ceases because the catalyst bed is congested with coke (the pressure drop rises and the flow rate decreases). The E-Ni _0.15 Fe _0.05 catalyst displays a stable reaction rate with no noticeable deactivation for 260 h on stream at 800°C. This result indicates that Fe plays a critical role in stabilizing the catalyst. Industrial syngas must be compressed, such as compression from 1 to 10 bars, for utilization, which costs more than 85% of the total capital investment and 60% of the operational costs. Additionally, high-pressure operation also increases the production capacity. [0083] FIG. 6B illustrates DRM performance of E-Ni _0.2 and E-Ni _0.15 Fe _0.05 for a continuous catalytic reaction at 14 bar, according to some embodiments. The reaction conditions are the following: T = 800 °C, CH ₄ /CO ₂ /N ₂ = 20/60/20, GHSV = 12,000 mL g _cat ^–1 h ^-1 . Coking is highly thermodynamically favored at high-pressure operation conditions, which is the central dilemma to address. Both E-Ni _0.15 Fe _0.05 and E-Ni _0.2 exhibit 40 h stability in reaction conditions at 14 bar. Compared to some conventional catalysts, E-Ni _0.15 Fe _0.05 exhibits similar CH ₄ conversion, lower CO ₂ conversion, and a much higher H ₂ /CO ratio, even without 10% H ₂ O feeding, indicating that E-Ni _0.15 Fe _0.05 is also a promising catalyst for the high- pressure dry reforming of CH ₄ . [0084] To elucidate the role of Fe on the carbon resistance of Ni-based catalysts under reaction conditions, thermogravimetric techniques were applied to measure the carbon deposition on the used catalyst. The CO ₂ signal was analyzed in a mass spectrometer during combustion. FIG. 6C illustrates thermogravimetric analysis of used E-Ni _0.2 (135 h) and E- Ni _0.15 Fe _0.05 (260 h) catalysts after different times, according to some embodiments. The analysis was completed at 800 °C in 10% O ₂ /Ar. As depicted in FIG.6C, the coke formation rate on the E-Ni _0.2 catalyst is 2.57 E-5 mmol g _cat alyst ⁻¹ s ⁻¹ during the 135 h on stream, whereas the coke formation rate significantly drops to 4.71 E-8 mmol g _catalyst ⁻¹ s ⁻¹ for the E-Ni _0.15 Fe _0.05 catalyst during the 260 h on stream. [0085] FIG. 6D illustrates a particle size distribution histogram for E-Ni _0.15 Fe _0.05 and I- Ni _0.2 catalysts after reduction and DRM with different times on stream, according to some embodiments. As shown, the average particle size of the exsolved catalyst increased much less than the wetness impregnation catalyst. The particle size distribution analysis revealed that the used E-Ni _0.15 Fe _0.05 catalyst possessed exsolved Ni-Fe nanoparticles with an average size of 30.1 nm after 260 h on stream, slightly larger than the nanoparticles of the E-Ni _0.15 Fe _0.05 before the reaction (21.0 nm). The exsolved nanoparticles of the used E-Ni _0.15 Fe _0.05 catalyst are still partially anchored in the support without any observable C with a morphology similar to the pristine one. However, the counterpart used I-Ni _0.2 catalyst exhibited severe sintering of Ni particles from 35.2 to 56.6 nm, only after 12 h on stream with apparent filament C on the catalyst surface. In addition, elemental mappings focused on Ni-Fe nanoparticles of E- Ni _0.15 Fe _0.05 depicted identical features before and after the reaction: a homogenous distribution of Ni and Fe through the particles without noticeable metal segregation. Hence, the exsolved E-Ni _0.15 Fe _0.05 catalyst exhibited improved sintering resistance compared with the I-Ni _0.2 catalyst, which is closely associated with their stability (FIG.6A). [0086] FIG.7 illustrates a comparison of the present catalysts to conventional catalysts, according to some embodiments. Compared with approximately 140 conventional catalysts, the proposed ENi _0.15 Fe _0.05 catalyst has the slowest coke formation rates of the relatively extensive catalyst portfolio. Many studies do not assess coke fouling on the catalysts for the following reasons: (i) insufficient time on stream, (ii) unrealistically mild reaction conditions, or (iii) inappropriate excess of catalyst and the subsequent underestimation of coke formation. Per the thermogravimetric results, contrary to the severe coking on the used E-Ni _0.2 catalyst, the Raman spectra indicated no coke accumulation on the used E-Ni _0.15 Fe _0.05 catalyst. The minor coking deposition convincingly demonstrates the coking-resistant effect of Fe, coinciding with previous reports that Fe substitution improves the C resistance of Ni-based catalysts in reaction conditions. [0087] The DFT calculations were performed to compare the adsorption energy of the key intermediates on Ni ₄ Fe ₁ (111) models to that on monometallic Ni (111) models to elucidate the improved coking resistance of the Ni-Fe bimetallic catalyst. These surfaces were identified experimentally using high-resolution TEM. The support in the E-Ni _0.2 and E-Ni _0.15 Fe _0.05 catalysts was perovskite, which is almost inert to the main reactions (in FIG. 5, E-Fe0.2 has negligible activity); thus, only the monometallic Ni and bimetallic Ni-Fe alloy were considered for the slab model. [0088] The binding energies of the critical intermediates on Ni ₄ Fe ₁ (111) were compared with those on Ni (111), as presented in Table 3. Despite the same binding energy of CH ₄ between Ni (111) and Ni ₄ Fe ₁ (111), the binding strength of C-containing intermediates, including CH3*, CH ₂ *, CH*, C*, and CO*, are all weaker on the Ni ₄ Fe ₁ (111) surface than on the Ni (111) surface, on which coke is likely prone to form due to the higher C* binding energy. In addition, due to the stronger Fe-O bond, the adsorption of the oxygen-containing species, such as O* and CHO*, on the Ni ₄ Fe ₁ (111) surface are stronger than that on the Ni (111) surface. The O* and CHO* adsorption strengths are 0.15 and 0.08 eV higher than the pure Ni (111) surface. Table 3. Comparison of energy barriers of elementary reactions involved in DRM. [0089] FIG. 8A illustrates potential energy profiles for the C atom and CH oxidation pathways on Ni (111) and Ni ₄ Fe ₁ (111) surfaces, respectively, according to some embodiments. FIG.8B illustrates geometries of transition states for CH dehydrogenation and C oxidation (C oxidation pathway), according to some embodiments. FIG. 8C illustrates CH oxidation and CHO dissociation (CH oxidation pathway), according to some embodiments. The C formation is determined by the surface C* concentration, which is considered the precursor to C formation. The surface C* primarily originates from CH* and CO* dissociating from CH ₄ and CO ₂ , respectively. The DFT calculation results indicate that the CO* dissociation is highly unfavored due to much higher energy barriers on both Ni (111) (2.97 eV) and Ni ₄ Fe ₁ (111) (2.70 eV) surfaces compared with barriers to the CH* dissociation, consequently restraining the C* formation from CO* dissociation (Table 3). The barrier energy for CH* dissociation is 1.10 eV on the Ni (111) surface and 1.03 eV on the Ni ₄ Fe ₁ (111) surface. Hence, the C* concentration depends on the formation and consumption of C* deriving from the intermediate CH*. [0090] Two pathways, (i) the C and (ii) CH oxidation pathways, should be considered to establish the energy diagram of the reactions from intermediate CH* to the final state of CO* and H* because the CH* results in the competitive formation of C* and CO*. Each pathway includes two steps: CH direct dissociation (CH* → C* + H*) and C oxidation (C*+ O* → CO*) for the C oxidation pathway, and CH oxidation (CH* + O* → CHO*) and CHO dissociation (CHO* → CO* + H*) for the CH oxidation pathway, as illustrated in FIGS. 8A- 8C. The effective barriers were calculated for the two pathways, defined as the difference between the highest-transition and lowest intermediate states in the whole reaction. The effective barriers for the C and CH oxidation pathways are 2.22 and 1.13 eV, respectively, on the Ni ₄ Fe ₁ (111) surface, indicating that the CH oxidation pathway is much more favorable than the C oxidation pathway. [0091] A similar trend is observed on the Ni (111) surface. However, the energy barrier distinction between the two oxidation pathways strikingly increases from 0.88 eV on Ni (111) to 1.09 eV on Ni ₄ Fe ₁ (111), revealing the prevailing dominance of the CHO* oxidation pathway on the Ni ₄ Fe ₁ (111) surface. This outcome significantly alleviates the C* atom coverage on Ni4Fe1 (111) surface because the formed CH* prefers to couple with oxygen to form CHO*, further converting to CO* and H*, rather than directly decomposing into C*. [0092] More CH* species accumulated on the Ni (111) surface due to the relative inferiority of the CHO* oxidation pathway compared to Ni ₄ Fe ₁ (111), part of which further decomposes to C* and H*, leading to severe coking. Moreover, adding Fe to the Ni-based catalysts facilitates CO ₂ activation (exhibiting a slightly inferior CH ₄ activation activity for Ni), releasing more O* species as an oxidant to promote C removal, to an extent. Overall, the calculations demonstrate that the prevailing dominance of the CHO* oxidation pathway and the increased available atomic O* species synergistically contribute to the outstanding coking resistance of the Ni-Fe binary alloy catalyst, which is consistent with the experimental results. [0093] Compared with the conventional impregnated catalysts, the exsolved catalysts possess unique anchor effect, which significantly prevents sintering. The exsolved fraction of Ni attained 94%. The CH ₄ reaction rate in DRM reached to 1.74 E-03 mol gNi ^–1 s ^–1 . More importantly, the E-Ni _0.15 Fe _0.05 catalyst achieved 260 h stability at 800 °C under CH ₄ /CO ₂ /N ₂ =33/34/33 with the coke formation rate of 4.71 E-8 mmol g _cat alyst ⁻¹ s ⁻¹ , which is one of the slowest coke formation rates compared with the conventional catalysts. Further, no deactivation is observed during 40 h operation at high pressure (14 bar). In the Ni ₄ Fe ₁ binary alloy system, the CHO* oxidation route prevailingly dominates, promoting the oxidation of CH* instead of decomposing to C*, inhibiting the C deposition. Moreover, the weakening binding strength of the C* atom and the enrichment of the oxygen-containing species on the binary alloy Ni ₄ Fe ₁ (111) surface alleviates the C deposition and facilitates the oxidation of intermediate CHx and surface C, respectively. [0094] Importantly, exsolved Ni nanoparticles on double-layer perovskite are resistant to sintering under harsh dry reforming conditions due to the unique anchoring and metal-support interaction. This catalyst has significantly superior performance and longer stability than the corresponding counterpart catalyst prepared via the wetness impregnation method. The addition of Fe led to the formation of Ni ₄ Fe ₁ alloy, which exsolves on the double-layer perovskite. This catalyst exhibits robust stability with negligible C deposition during the 260 h on stream. The comprehensive characterization and DFT calculations revealed that, in the Ni- Fe binary alloy system, the CHO* oxidation route prevailingly dominates, promoting the oxidation of CH* instead of decomposing to C*, inhibiting the C deposition. Moreover, the weakening binding strength of the C* atom alleviates the C deposition on the Ni ₄ Fe ₁ (111) surface. The enrichment of the oxygen-containing species facilitates the oxidation of intermediate CH _x and surface C, eliminating coking on the binary alloy Ni ₄ Fe ₁ (111) surface, thereby significantly boosting the stability of the Ni ₄ Fe ₁ nanoparticle-decorated double-layer perovskite during the prolonging reaction. Overall, the simultaneous in situ exsolution of the active sites with the second metal promoter to form binary alloy nanoparticle-anchored double- layer perovskite is a low-cost and efficient route to design a highly coking-resistant and robust catalyst for hydrogen production reforming reactions. [0095] The catalyst can be used in the technology which involves the activation of C-H bond in hydrocarbons and their derivatives such as thermal catalysis including DRM, SRM, CDM, and electrochemistry including SOFC. In the application of thermal catalysis, the catalyst possesses outstanding anti-sintering and coking resistant ability so that the catalyst exhibits quite slow coke formation rate and robust stability in the thermal catalysis reactions. In the application of the electrochemistry, the catalyst can be used as electrode which activates the fuel and also conducts the electrons, thus facilitating the anode reaction. For example, in SOFC fueled with hydrocarbon and their derivatives, the catalyst can be utilized as a promising anode which shows high C-H activation, excellent conductivity and carbon resistant ability, so that the SOFC has long stability. Example 2 [0096] A comparison was completed for the DRM performance with conventional catalysts. The results are shown in Table 4 below. Table 4. Comparison of DRM performance. Discussion of Possible Embodiments [0097] According to one aspect, a catalyst includes a double-layer perovskite support and nanoparticles including nickel and one or more transition metals, wherein the nanoparticles are in contact with the double-layer perovskite support. [0098] The catalyst of the preceding paragraph can optionally include, additionally and/or alternatively any one or more of the following features, configurations and/or additional components. [0099] The double-layer perovskite support may include praseodymium, barium, and manganese. [00100] The one or more transition metals may be selected from iron, cobalt, copper, and molybdenum. [00101] The nanoparticles may include iron and the double-layer perovskite support may be in the tetragonal phase. [00102] The nanoparticles may include a Ni ₃ Fe ₁ alloy. [00103] The diameter of the nanoparticles may range from 10 nm to 40 nm. [00104] The nanoparticles may be substantially spherical and may be anchored into the double-layer perovskite support, and wherein greater than 90% of the total Ni may be in the metallic state. [00105] The catalyst may include the following formula: PrBaMn _1.6 Ni _2(0.2-X) FeXO _5+δ , wherein X ranges from 0 to 0.2. [00106] The catalyst may include the following formula: PrBaMn _1.6 Ni _2(0.2-X) FeX, wherein X ranges from 0 to 0.2. [00107] The catalyst may include the product of one or more of exsolving the nanoparticles and reducing a single perovskite support. [00108] According to one aspect, a method of processing a feed stock includes contacting the feed stock with a catalyst, sufficient to generate a reaction product, wherein the catalyst includes: a double-layer perovskite support and nanoparticles including nickel and one or more transition metals, wherein the nanoparticles are in contact with the double-layer perovskite support. [00109] The method of the preceding paragraph can optionally include, additionally and/or alternatively any one or more of the following features, configurations and/or additional components. [00110] The feed stock may include one or more of carbon dioxide, methane, water, and hydrogen and the reaction product may include one or more of hydrogen, water, and carbon monoxide. [00111] The method may include a reaction selected from dry reforming of methane (DRM), steam reforming of methane (SRM), catalytic decomposition of methane (CDM), and electrochemistry including solid oxide fuel cell (SOFC). [00112] The one or more transition metals may be selected from iron, cobalt, copper, and molybdenum and the double-layer perovskite support may be in the tetragonal phase. [00113] The catalyst may include the following formula: PrBaMn _1.6 Ni _2(0.2-X) FeXO _5+δ , wherein X ranges from 0 to 0.2. [00114] The catalyst may include the following formula: PrBaMn _1.6 Ni _2(0.2-X) FeX, wherein X ranges from 0 to 0.2. [00115] According to one aspect, a method of making a catalyst includes contacting praseodymium salt, barium salt, manganese salt, nickel salt, and a transition metal salt with one or more complexation agents sufficient to form a solution, heating the solution sufficient to form a gel, heating the gel sufficient to separate a solid, and calcining the solid. [00116] The method of the preceding paragraph can optionally include, additionally and/or alternatively any one or more of the following features, configurations and/or additional components. [00117] The complexation agent may include one or more of citric acid and ethylene glycol. [00118] Heating the gel may include heating at a temperature greater than 300 °C and calcining includes heating the solid at a temperature greater than 700 °C. [00119] The method may include reducing the catalyst in gas at a temperature above 500 °C. [00120] The catalyst may include Ni3Fe1 alloy nanoparticles. [00121] The catalyst may include a double-layer perovskite support in the tetragonal phase. [00122] The catalyst may include the following formula: PrBaMn _1.6 Ni _2(0.2-X) Fe _X O _5+δ , wherein X ranges from 0 to 0.2. [00123] The catalyst may include the following formula: PrBaMn _1.6 Ni _2(0.2-X) Fe _X , wherein X ranges from 0 to 0.2. [00124] While the disclosure has been described with reference to an exemplary embodiment(s), it will be understood by those skilled in the art that various changes may be made, and equivalents may be substituted for elements thereof without departing from the scope of the embodiment(s). In addition, many modifications may be made to adapt a particular situation or material to the teachings of the embodiment(s) without departing from the essential scope thereof. Therefore, it is intended that the disclosure is not limited to the disclosed embodiment(s), but that the disclosure will include all embodiments falling within the scope of the appended claims. Various examples have been described. These and other examples are within the scope of the following claims.