Hydrogen Production by Partial Oxidation Reforming of Methane over Ni Catalysts Supported on High and Low Surface Area Alumina and Zirconia

: The catalytic activity of the partial oxidation reforming reaction for hydrogen production over 10% Ni supported on high and low surface area alumina and zirconia was investigated. The reforming reactions, under atmospheric pressure, were performed with a feed molar ratio of CH 4 / O 2 = 2.0. The reaction temperature was set to 450–650 ◦ C. The catalytic activity, stability, and carbon formation were determined via TGA, TPO, Raman, and H 2 yield. The catalysts were calcined at 600 and 800 ◦ C. The catalysts were prepared via the wet-impregnation method. Various characterizations were conducted using BET, XRD, TPR, TGA, TPD, TPO, and Raman. The highest methane conversion (90%) and hydrogen yield (72%) were obtained at a 650 ◦ C reaction temperature using Ni-Al-H-600, which also showed the highest stability for the ranges of the reaction temperatures investigated. Indeed, the time-on-stream for 7 h of the Ni-Al-H-600 catalyst displayed high activity and a stable profile when the reaction temperature was set to 650 ◦ C.


Introduction
Today's global energy is chiefly concentrated on power production via fossil fuels. To reduce greenhouse gas emissions, major efforts have been carried out to increase the use of renewable energy. However, the difference between renewable energy supply and energy demands necessitates further utilization of fossil fuels to supply excess energy. Fossil petroleum, commonly called natural gas, is currently employed to provide the major portion of energy requirements.
The conversion of natural gas into valuable chemical products has been the goal of several studies for some decades [1][2][3][4][5]. The most common processes employed to achieve such products include the transformation of methane into syngas [6,7]. Methane, an ozone depleting gas, is the main component present in natural gas. Clean energy application technologies have received much consideration in recent years because of their low emissions and high efficiencies [8][9][10]. The use of hydrogen as fuel for fuel cells has become the target of many investigators, as hydrogen is highly efficient, nonpolluting, and sustainable [11,12]. Owing to the great demand for H 2 and CO, for the petrochemical industry (through the Fischer-Tropsch process to generate methanol and ammonia), hydrocarbon production, and petroleum refining processes (hydrotreating and hydrocracking), their production by the reforming of natural gas has increased significantly.
Although the main way to obtain syngas from methane on an industrial scale is from steam reforming, as presented in Equation (1), feasible alternative methods, e.g., CO 2 reforming shown in Equation (2) and the partial oxidation of methane (POM) as in Equation (3), have been investigated [13][14][15].
Both CO 2 reforming and steam reforming processes are highly endothermic and need huge energy inputs. On the other hand, the POM route has the advantage of being an exothermic process, which has a lower energy cost. POM also provides a ratio of H 2 /CO = 2, which permits a straightforward syngas application for methanol or Fischer-Tropsch processes [4,14,16]. Though costly metals, like Rh, Ru, and Pt, have been employed successfully for the reactions (1)(2)(3) in terms of activity and selectivity [17][18][19], the high price and limited availability of the noble metals confine their applications. Instead, nickel and other transition metal-based catalysts have been stated to be active for these reactions (1)(2)(3). Nickel is preferred due to its availability, low cost, and high initial catalytic activity. Thereafter, extensive research has been performed on nickel supported over various oxides, for instance Al 2 O 3 [20,21].
The prevalence of deactivation and sintering of active metals necessitates the development of Ni-based catalysts with improved activity and stability.
The partial oxidation method has the benefit of giving high conversion of methane with superb selectivity for hydrogen using relatively high space velocities [22]. Although rapid reaction kinetics and satisfactory thermodynamics are available in the literature, partial oxidation has not been commercialized yet due to challenges that include small reduction in CO selectivity caused by over oxidation that results in a local temperature rise at the catalyst surface leading to catalyst deactivation owing to its sintering and carbon formation [23]. A literature survey indicates that substantial research efforts have been dedicated to developing appropriate catalysts via numerous supports and different catalyst pretreatment methods that will increase the H 2 and CO yields. The choice of a support plays an important role in the ultimate stability of the catalysts. Dissanayake et al. investigated the partial oxidation of CH 4 using 25% Ni supported on alumina [24]. The result showed that complete conversion could be obtained if the reaction temperature was above 700 • C. The results also revealed that the catalyst bed may be subdivided into three zones with different catalytic activity aspects. Zhang et al. studied the partial oxidation of CH 4 using textural promoted alumina supported on Ni (Ni/CeO 2 -ZrO 2 /γ-Al 2 O 3 ) [25]. The results indicated the effects of different preparation processes. On the other hand, Sajjadi and Haghighi examined Ni/Al 2 O 3 by means of different preparation techniques, namely sol-gel, impregnation, and hybrid sol-gel plasma [26]. They found that each preparation technique possessed advantageous properties over the others, such as good dispersion, stability, coke resistance, etc.
Usually, Al 2 O 3 is utilized as a support for Ni-based catalysts during reforming reactions. However, several problems are related with Al 2 O 3 support; for instance, carbon deposition readily increases the catalyst deactivation, damaging of the active phase, and formation of inactive spinel phases, such as nickel aluminate (NiAl 2 O 4 ) [27]. ZrO 2 is used to improve CO 2 adsorption and carbon gasification [8]. Dong et al. performed the relative investigation of partial oxidation of CH 4 over Ni/ZrO 2 , Ni/CeO 2 , and Ni/Ce-ZrO 2 catalysts [28]. They found that over Ni/ZrO 2 , CH 4 and O 2 were activated on the surface of metallic Ni, and then adsorbed carbon reacted with adsorbed O 2 to generate CO, which designed the leading path for the partial oxidation of CH 4 .
Ouaguenouni et al. investigated the preparation and catalytic activity of nickel-manganese oxide catalysts in the reaction of partial oxidation of methane [29]. In their results they found that the formation of different spinels depends on the calcination temperature. The spinel NiMn 2 O 4 was observed to be active in the POM reaction. The catalysts calcined at 900 • C develop NiMn 2 O 4 and give a higher CH 4 conversion, resulting from good Ni dispersion. Alternatively, Moral et al. studied the POM using Co as the active metal supported on a mixture of MgO and Al 2 O 3 [30]. The authors performed the reaction at 800 • C and studied the effects of Co and MgO loadings and the calcination temperatures. Their catalysts gave CH 4 conversions of 91% using a calcination temperature of 500 • C and 20 wt.% Co and 63% MgO loadings. Kaddeche et al. examined the partial oxidation of methane on co-precipitated Ni-Mg/Al catalysts modified with copper or iron [4]. They investigated the effect of catalyst composition and pretreatment conditions of these catalysts at a 750 • C reaction temperature. The catalysts displayed very high activity and selectivity that are dependent on the conditions of preparation of the catalysts. Their results showed increased activity and selectivity with decreasing calcination temperature and increasing Ni and Al contents in the catalysts' composition. A study on Ca-decorated Al 2 O 3 -supported Ni and NiB catalysts, showed that the calcination temperature could significantly affect the catalyst activity [31]. A higher reduction temperature was required to ensure the complete reduction of NiO on the catalysts calcined at higher temperatures; CH 4 conversion and syngas selectivity decreased when catalysts were calcined at 800 • C.
Thus, in light of the above, it is vital to evaluate the performance of Ni catalysts with regard to supports such as alumina and zirconia by using different calcination temperatures and various operating conditions including reaction temperature and time-on-stream. Attention has been focused on the influence of catalyst performance on reactants (CH 4 and O 2 ) conversion and H 2 yield products in the partial oxidation reforming process. Characterizations of the spent and fresh catalysts were also performed to understand the catalytic behavior, i.e., activity and stability.

Catalyst Preparation
The preparation of the desired catalysts was performed using the wet impregnation method. In the preparation of 10% nickel supported on Al 2 O 3 and zirconia catalyst, 0.9 g of the support (α-Al 2 O 3 , γ-Al 2 O 3 , α-ZrO 2 , or γ-ZrO 2 ) were impregnated with a solution having 0.495 g of (Ni(NO 3 ) 2 .6H 2 O) in 0.03 L of deionized H 2 O. The catalyst was subjected to drying at 120 • C and calcination either at 600 or 800 • C for two hours. The catalyst was activated inside the reactor at 800 • C by passing hydrogen at a rate of 40 mL/min for 2 h followed by 20 min of N 2 at a rate of 30 mL/min. The synthesized catalysts and their corresponding designations are given in Table 1.

Catalytic Reaction
The partial oxidation reaction of methane was done at atmospheric pressure in a 0.91 cm diameter and 0.30 m long stainless steel-tube fixed-bed micro reactor (the reactor is from PID Eng. & Tech Micro activity Reference Company) using 0.1 g of the catalyst. The reaction temperature was measured by a thermocouple placed in the center of the catalyst bed. The volume ratio of the feed gases (methane/oxygen/nitrogen) was 6:3:4. The total flow rate of the feed was 32.5 mL/min (i.e., 325 mL/min/gcat). The investigation was performed at reaction temperatures of 450, 500, 550, 600, and 650 • C. The effluents were analyzed using an online gas chromatograph (GC-2014 SHIMADZU) equipped with a thermal conductivity detector. The conversions of CH 4 and H 2 yield were all determined. The methane conversion and hydrogen yield were computed as:

Catalyst Characterization
Both fresh and spent catalysts were characterized by several techniques.

N 2 Physisorption
N 2 adsorption/desorption isotherms were used to find the textural characteristics of the catalysts, calculated at −197 • C with a Micromeritics Tristar II 3020 porosity and surface area analyzer. In each test, 200-300 mg of catalyst was taken. The samples were degassed at 300 • C for 3 h to remove undesired adsorbed gases, organics, and water vapor. The BET technique was employed to determine the surface areas.

XRD
X-ray diffraction (XRD) measurements for fresh catalysts were carried out. The XRD was performed using Rigaku (Miniflex), with Kα-Cu radiation at 40 kV and 40 mA. A 2θ range of 10-85 • and a scanning step of 0.02 • were used.

TPR
The activation behavior of the catalysts was investigated via an AutoChem-II Micromeritics device. For each analysis, 0.07 g of the sample were pre-treated with Ar (30 mL/ min). The samples were cooled to ambient temperature before starting the analyses. Then, the sample temperature was raised from 25 to 1000 • C in an automatic furnace at 1 atm. During temperature ramping, a H 2 /Ar mixture with a volume ratio 10:90 and a flow rate of 40 mL/min was applied, while the heating rate was kept constant at 10 K/min. The outlet gases were monitored by a thermal conductivity detector (TCD) to analyze the H 2 consumption with respect to temperature.

TGA
The extent of the total deposited C on the used catalysts was determined using Shimadzu thermo-gravimetric analysis (TGA) in air. From the used catalysts, 0.10-0.15 g were heated at the rate of 20 • C/min from 25 to 1000 • C while recording the mass loss.

CO 2 -TPD
The Micromeritics Autochem II apparatus was used to perform the CO 2 temperature-programmed desorption (TPD). First, 5 mg of catalyst were reduced at 600 • C for 60 min under an He flow (30 mL/min) and then cooled to 50 • C. The CO 2 flow was continued for 1 h, and the sample was then flushed with He to remove any physisorbed CO 2 . The peaks of desorption were recorded while temperature was changed by 10 • C/min. The CO 2 concentration in the effluent stream was computed using a thermal conductivity detector, and the areas under the peaks provided the amount of desorbed CO 2 during TPD.

TPO
Temperature program oxidation was performed in an oxidative atmosphere to determine the type of carbon deposited on the surface of the catalyst via Micromeritics AutoChem II. The analysis was executed up to 800 • C under 40 mL/min of 10% O 2 /He. The used catalyst was pre-treated in the presence of Ar at 150 • C for 30 min and afterward cooled to room temperature.

Raman Spectroscopy
Raman spectra were carried out via an NMR-4500 Laser Raman Spectrometer. A wave length with excitation beam of 532 nm was used. An objective lens with 20× magnification was used to measure the spectra. A six mW beam power and an exposure time of 0.05 h were used. The Raman shift of the spectra was computed in the range 1000-3000 cm −1 . The profiles were handled by Spectra Manager Ver.2 software.

Results and Discussion
As a control experiment, we tested an empty reactor without catalysts under the same feed ratio and various temperatures (500-650 • C). The CH 4 conversions registered during the test were 0.0% in the 500-650 • C range. Therefore, the control experiment denoted negligible interaction of the reactor tube to the catalytic activity. Figure 1 exhibits the catalyst N 2 adsorption/desorption isotherms, calcined at 600 • C. The catalyst N 2 isotherms fall under the type-IV classification. The isotherm is characterized by materials that are mesoporous (2-50 nm), in accordance with the International Union of Pure and Applied Chemistry (IUPAC) classification. The Ni-Al-H-600 sample has an H 2 -type hysteresis loop, indicating an ink bottle type pore (mouth is narrower and back broader) whereas the Ni-Al-L-600 sample has an H3-type hysteresis, confirming non-limited adsorption. Ni-Zr-H-600 and Ni-Zr-L-600 samples have H1 hysteresis loops indicating narrower pore size distribution. It is an indication of changes in the pore patterns with different supports. Interestingly, when the calcination temperature in Figure 2 increases up to 800 • C, the pore pattern of Ni-Al-H-800 changes from H 2 to H1, indicating a change of pore pattern from ink bottle to cylindrical. The same pore pattern change from H3 to H1 is seen in of Ni-Al-L-800. Ni-Zr-H-800 and Ni-Zr-L-800 samples have the same patterns as those of the low temperature (600 • C) calcined samples. The distinctive physical structure of surface area, pore volume, and pore size are shown in Table 1. The addition of 10% nickel decreases the surface area and displays a relatively substantial effect on the specific surface area of the Ni-Zr-H-600 and Ni-Zr-H-800 catalysts. Increasing calcination temperature from 600 to 800 • C decreases the surface area and pore volume and increases the pore diameter; thus resulting in a sequence of catalysts bearing diverse inventories of hydroxyl groups. The average pore diameter of all catalysts is around 12-35 nm, which is in accord with the mesoporous characteristics of the samples.  Figure 3 shows the XRD spectra of catalysts pre-reduced at 600 • C for 1 h, then calcined at 600 and 800 • C. In the present study, the mesoporous alumina and zirconia were prepared by an impregnation method. Figure 3A represents the XRD pattern of Ni-Zr-L-600 and Ni-Zr-L-800. This figure shows the diffraction peaks at 2θ values of 24.7, 29.5, 32.5, 34.0, 41.0, and 50.5, which can be ascribed to the planes of (022), (111), (040), (041), (113), and (114) of L-ZrO 2 (ICSD 01-081-0610). The two catalysts have similar spectra, but the higher calcined catalyst presents somewhat higher intensities, which means crystallinity is improved. The XRD patterns of Ni-Zr-H-600 and Ni-Zr-H-800 ( Figure 3B Figure 3 shows the XRD spectra of catalysts pre-reduced at 600 °C for 1 h, then calcined at 600 and 800 °C. In the present study, the mesoporous alumina and zirconia were prepared by an impregnation method. Figure  In these catalysts, the patterns are the same, but the Ni-Al-H-800 has higher intensity, which induced further reduction of the surface area and higher pore diameter due to the higher calcination temperature. It can be inferred from the XRD results that with increasing calcination temperature, the high surface area zirconia sample achieves a high degree of crystallinity whereas the low surface area zirconia sample achieves a high intensity of the major plane. In terms of the high surface area alumina support, all peaks achieve higher intensities at higher calcination temperatures. Figure 4 illustrates the TPR of all catalysts. The TPR results of Ni-Zr-L-600, Ni-Zr-L-800, Ni-Al-H-800, and Ni-Al-L-800 catalysts show that the peaks lie in wide ranges of temperature, which represent the characteristic reduction of stoichiometric nickel oxide [31]. Figure 4A the Zr supported catalysts present two peaks. For instance, Ni-Zr-H-800 has peaks (maxima) at 295 • C and 460 • C, Ni-Zr-L-800 has peaks (maxima) at 314 • C and 462 • C, Ni-Zr-H-600 has peaks (maxima) at 300 • C and 486 • C and Ni-Zr-L-600 has peaks (maxima) at 482 • C and 640 • C. Low temperature (<500 • C) H 2 -TPR peaks are for reduction of free NiO and it is found that Ni-Zr-L-800 and Ni-Zr-H-800 catalysts calcined at high temperatures have higher amounts of free NiO compared to the low calcined temperature samples. Intermediate temperature (<700 • C) peaks indicate moderate interaction of NiO with the support. In the Zr supported catalysts, the lower calcination temperature promotes higher interaction with the support. Figure 4B of Al supported catalysts presents single peaks, which appear at moderate or high ranges of temperature, except in the Ni-Al-L-600 catalyst, which has a prominent peak (maxima) at 360 • C. Generally, the alumina supported catalysts provide higher metal support interaction. It can be said that low temperature calcined alumina supported samples have reduction peaks in the relatively lower temperature regions than do the high temperature calcined samples. Ni-Al-L-600 has reduction peaks of free NiO whereas Ni-Al-L-800 has a reduction peak of NiO tightly interacted with its support. In these catalysts, the patterns are the same, but the Ni-Al-H-800 has higher intensity, which induced further reduction of the surface area and higher pore diameter due to the higher calcination temperature. It can be inferred from the XRD results that with increasing calcination temperature, the high surface area zirconia sample achieves a high degree of crystallinity whereas the low surface area zirconia sample achieves a high intensity of the major plane. In terms of the high surface area alumina support, all peaks achieve higher intensities at higher calcination temperatures.   Figure 4 illustrates the TPR of all catalysts. The TPR results of Ni-Zr-L-600, Ni-Zr-L-800, Ni-Al-H-800, and Ni-Al-L-800 catalysts show that the peaks lie in wide ranges of temperature, which represent the characteristic reduction of stoichiometric nickel oxide [31]. Figure 4A the Zr supported catalysts present two peaks. For instance, Ni-Zr-H-800 has peaks (maxima) at 295 °C and 460 °C, Ni-Zr-L-800 has peaks (maxima) at 314 °C and 462 °C, Ni-Zr-H-600 has peaks (maxima) at 300 °C and 486 °C and Ni-Zr-L-600 has peaks (maxima) at 482 °C and 640 °C. Low temperature (<500 °C) H2-TPR peaks are for reduction of free NiO and it is found that Ni-Zr-L-800 and Ni-Zr-H-800 catalysts calcined at high temperatures have higher amounts of free NiO compared to the low calcined temperature samples. Intermediate temperature (<700 °C) peaks indicate moderate interaction of NiO with the support. In the Zr supported catalysts, the lower calcination temperature promotes higher interaction with the support. Figure 4B of Al supported catalysts presents single peaks, which appear In this study, CO 2 -TPD was used to examine the basicity of the catalysts, as shown in Figure 5. The low surface area ZrO 2 support ( Figure 5A) provides three peaks at calcination temperatures of 600 and 800 • C. Two peaks in the low temperature region, an intense peak at 100 • C and a low intensity broad peak at 260-300 • C, and a small peak in the high temperature region at 560-600 • C. On the other hand, the profile of the high surface area ZrO 2 ( Figure 5A) shows three peaks for both calcination temperatures (600 and 800 • C). Two peaks in the low temperature region at 100 • C, with low and high intensity peaks for 600 and 800 • C calcination temperatures, respectively, and a distorted peak at 300-320 • C. There is a high intensity and broad peak at about 600 • C. It is fundamentally considered that the peaks at lower temperature regions can be ascribed to the weak basic sites resulting from the physical adsorption of CO 2 [32]. The peak at the high temperature associates to the strong basic sites and is accredited to the chemisorption of CO 2 . As a result of the number of basic sites, the peaks have different sizes [33]. High temperature calcined samples have wide distribution of basic sites whereas the low temperature calcined samples have a concentration of the majority weak basic sites. Figure 5B, displays the CO 2 -TPD of the catalysts supported by the alumina. The profile shows four peaks for both calcinations. For the low surface area catalysts, Ni-Al-L-800 and Ni-Al-L-600, the peak sizes are very small, indicating low concentrations of basic sites. The peaks for the high surface area catalysts, Ni-Al-H-600 and Ni-Al-H-800, generated prominent, high intensity peaks, denoting significant contents of basics sites. The peaks that appeared at lower than 150 • C are ascribed to weak basic sites, while the peaks at 250-400 • C are associated with medium basic sites, and the peaks at 650-800 • C are credited to strong basic sites. It is commonly agreed that basic sites on the catalyst surface can enhance the adsorption and the dissociation of CO 2 , which decreases the formation of carbon deposition to a large magnitude on active metal surface and, hence, efficiently hinders the deactivation of the catalysts. The CO 2 -TPD results justify and support the supremacy of Ni-Al-H-600. at moderate or high ranges of temperature, except in the Ni-Al-L-600 catalyst, which has a prominent peak (maxima) at 360 °C. Generally, the alumina supported catalysts provide higher metal support interaction. It can be said that low temperature calcined alumina supported samples have reduction peaks in the relatively lower temperature regions than do the high temperature calcined samples. Ni-Al-L-600 has reduction peaks of free NiO whereas Ni-Al-L-800 has a reduction peak of NiO tightly interacted with its support.   Figures 6-9 show the catalytic activity of 10% Ni catalysts supported on high and low surface area alumina and zirconia separately and calcined either at 600 or 800 °C. All the figures indicate CH4 conversion and hydrogen yield profiles that increase with the increase of the reaction temperature. This is in conformity with the fact that the reaction is exothermic (heat is generated) and, therefore,  Figures 6-9 show the catalytic activity of 10% Ni catalysts supported on high and low surface area alumina and zirconia separately and calcined either at 600 or 800 • C. All the figures indicate CH 4 conversion and hydrogen yield profiles that increase with the increase of the reaction temperature. This is in conformity with the fact that the reaction is exothermic (heat is generated) and, therefore, according to Le Chatelier's principle, increasing the temperature increases the products [34]. Figure 6 shows the CH 4 conversions for catalysts calcined at 600 • C. The Ni-Al-H-600 catalyst illustrates better methane conversion than the other catalysts; the conversion reached 90% at 650 • C. The performance Ni-Al-L-600 is lower than that of the corresponding Ni-Al-H-600 by 10%-34%, depending on the reaction temperature. On the other hand, the Ni-Zr-L-600 provides better conversion than that of Ni-Zr-H-600 or Ni-Al-L-600 for all reaction temperatures. Figure 7 exhibits CH 4 conversions for catalysts calcined at 800 • C. In this case the Ni-Al-H-800 catalyst offers better conversion than the other catalysts with 87% CH 4 conversion. The performance of Ni-Al-L-800 is less than the corresponding Ni-Al-H-800 by 5%-19%, depending on the reaction temperature. Alternatively, Ni-Zr-L-800 provides a slightly higher conversion than that of Ni-Zr-H-600 for most of the reaction temperatures. From Figures 6  and 7 it can be deduced that the calcination at 600 • C gives a better conversion than that at 800 • C. The high surface alumina support performs better than the low surface alumina whereas the opposite is true for the zirconia supports. Figure 8 shows the % hydrogen yield of catalysts calcined at 600 • C. Ni-Al-H-600 has the highest yield of 72%, while Ni-Zr-L-600 generates the lowest yield of 46% at 650 • C. The hydrogen yield for the Ni-Zr-H-600 catalyst is greater than that of Ni-Al-L-600. The yield profile of different catalysts is not in-line with that of the conversion. This is attributed to the drop in the selectivity of the catalysts calcined at 600 • C. Figure 9 displays the % hydrogen yield when the calcination was done at 800 • C. It indicates that Ni-Al-H-800 assumes the highest yield of 66%, while Ni-Zr-L-800 produces the lowest yield of 55% at 650 • C. The yield for the Ni-Al-L-800 catalyst is lower than that of Ni-Zr-H-800 except when the reaction temperature exceeds 620 • C. It can be concluded, from the perspective of hydrogen yield, that the higher surface area alumina calcined at 800 • C (Ni-Al-H-800) is preferable for the current process in the reaction temperature range of this study. Table 2 shows the comparison of catalytic performance of the present work and those in the literature; the table indicates the suitability of the adopted technique in this work. according to Le Chatelier's principle, increasing the temperature increases the products [34]. Figure  6 shows the CH4 conversions for catalysts calcined at 600 °C. The Ni-Al-H-600 catalyst illustrates better methane conversion than the other catalysts; the conversion reached 90% at 650 °C. The performance Ni-Al-L-600 is lower than that of the corresponding Ni-Al-H-600 by 10%-34%, depending on the reaction temperature. On the other hand, the Ni-Zr-L-600 provides better conversion than that of Ni-Zr-H-600 or Ni-Al-L-600 for all reaction temperatures. Figure 7 exhibits CH4 conversions for catalysts calcined at 800 °C. In this case the Ni-Al-H-800 catalyst offers better conversion than the other catalysts with 87% CH4 conversion. The performance of Ni-Al-L-800 is less than the corresponding Ni-Al-H-800 by 5%-19%, depending on the reaction temperature. Alternatively, Ni-Zr-L-800 provides a slightly higher conversion than that of Ni-Zr-H-600 for most of the reaction temperatures. From Figures 6 and 7 it can be deduced that the calcination at 600 °C gives a better conversion than that at 800 °C. The high surface alumina support performs better than the low surface alumina whereas the opposite is true for the zirconia supports. Figure 8 shows the % hydrogen yield of catalysts calcined at 600 °C. Ni-Al-H-600 has the highest yield of 72%, while Ni-Zr-L-600 generates the lowest yield of 46% at 650 °C. The hydrogen yield for the Ni-Zr-H-600 catalyst is greater than that of Ni-Al-L-600. The yield profile of different catalysts is not in-line with that of the conversion. This is attributed to the drop in the selectivity of the catalysts calcined at 600 °C. Figure 9 displays the % hydrogen yield when the calcination was done at 800 °C. It indicates that Ni-Al-H-800 assumes the highest yield of 66%, while Ni-Zr-L-800 produces the lowest yield of 55% at 650 °C. The yield for the Ni-Al-L-800 catalyst is lower than that of Ni-Zr-H-800 except when the reaction temperature exceeds 620 °C. It can be concluded, from the perspective of hydrogen yield, that the higher surface area alumina calcined at 800 °C (Ni-Al-H-800) is preferable for the current process in the reaction temperature range of this study. Table 2 shows the comparison of catalytic performance of the present work and those in the literature; the table indicates the suitability of the adopted technique in this work.      Figure 10A shows the weight loss of the used catalysts, calcined at 600 • C, and operated for 5 h. The profile shows the nonexistence of desorption of strongly adsorbed water and oxidation of volatile organic compounds since no weight loss below 650 • C was detected. The weight loss observed over 650 • C was alike for all catalysts and attributed to the oxidation of graphitic carbon species [38,39]. For the Ni-Al-L-600 and Ni-Al-H-600 catalysts, the weight loss was about 8.6% and 6.0%, respectively, justifying the different conversions obtained with these two catalysts. While for the Ni-Zr-L-600 and Ni-Zr-H-600 catalysts, the weight loss was about 2.3% and 5.5%, respectively. Figure 10B shows the weight loss of the used catalysts, calcined at 800 • C, and operated for 5 h. The weight losses are quite low: Ni-Al-H-800, Ni-Al-L-800, Ni-Zr-L-800, and Ni-Zr-H-800 give weight losses of approximately 7.0%, 0.9%, 5.2%, and 1.0%, respectively.    Figure 11A shows methane conversion against time-on-stream for different reaction temperatures. The best CH 4 conversion of 90% and the highest stability is attained using a 650 • C reaction temperature, while 52% CH 4 conversion is recorded for a 500 • C reaction temperature. The conversion enhances with the increase of the reaction temperature, since rates of reaction increase with increase of temperature. The 650 • C gives not only excellent activity but also excellent stability. Therefore, the time-on-stream analysis indicates that the 650 • C reaction temperature results in the best performance of the of Ni-Al-H-600 catalyst. Figure 11B shows hydrogen yield against time-on-stream for different reaction temperatures. The highest H 2 yield of 72% and the best stability is obtained at a 650 • C reaction temperature, while the lowest H 2 yield of 28% is registered for 500 • C. highest stability is attained using a 650 °C reaction temperature, while 52% CH4 conversion is recorded for a 500 °C reaction temperature. The conversion enhances with the increase of the reaction temperature, since rates of reaction increase with increase of temperature. The 650 °C gives not only excellent activity but also excellent stability. Therefore, the time-on-stream analysis indicates that the 650 °C reaction temperature results in the best performance of the of Ni-Al-H-600 catalyst. Figure 11B shows hydrogen yield against time-on-stream for different reaction temperatures. The highest H2 yield of 72% and the best stability is obtained at a 650 °C reaction temperature, while the lowest H2 yield of 28% is registered for 500 °C.   Figure 12 shows the TPO profiles of the spent Ni-Al-H-600 catalyst operated for 5 h at different reaction temperatures. The figure shows peaks of CO 2 desorption at lower temperatures for all reaction temperatures corresponding to atomic and amorphous carbonaceous species. At the high reaction temperatures of 600 and 650 • C, there is an additional peak corresponding to graphitic carbonaceous species. The negative peaks around at around 250-300 • C are ascribed to the oxidation of the metallic nickel and its intensity is diminished with the increase of reaction temperature. Therefore for the same catalyst, increasing the reaction temperature above 550 • C induces the formation of graphitic carbon, whereas the different oxidation regions result from the different locations of the carbon on the surface of the catalyst. Carbon deposition is an essential feature of reforming reactions. The different carbon structures are customarily assessed by Raman analysis. Figure 13 depicts the Raman spectra of spent Ni-Al-H-600 catalysts acquired for 7 h using reaction temperatures of 500, 550, 600, and 650 • C. Two comparable intensity peaks appeared at 1475 cm −1 and 1535 cm −1 , corresponding to the D band, assigned to sp3 hybridized amorphous carbon, and G band, specified by the presence of graphitized carbon, respectively. The D band and G band are typical bands of regular-structured carbon that form on the surface of Ni-Al-H-600 during the partial reforming reaction. The results of Raman analysis confirm the formation of different types of carbon, particularly for high reaction temperatures, as is illustrated in the TPO analysis. Figure 14 illustrates the TGA analysis of the Ni-Al-H-600 catalyst operated at different reaction temperatures that lasted for 5 h. The result shows 4% weight loss of the mass due to gasification of the gas formed on the catalyst when the reaction temperature was 500 • C, while 8% weight loss was determined using a reaction temperature of 650 • C. As the reaction temperature was increased, the production of carbon grew slightly as a result of increased decomposition of CH 4 . Figure 12 shows the TPO profiles of the spent Ni-Al-H-600 catalyst operated for 5 h at different reaction temperatures. The figure shows peaks of CO2 desorption at lower temperatures for all reaction temperatures corresponding to atomic and amorphous carbonaceous species. At the high reaction temperatures of 600 and 650 °C, there is an additional peak corresponding to graphitic carbonaceous species. The negative peaks around at around 250-300 °C are ascribed to the oxidation of the metallic nickel and its intensity is diminished with the increase of reaction temperature. Therefore for the same catalyst, increasing the reaction temperature above 550 °C induces the formation of graphitic carbon, whereas the different oxidation regions result from the different locations of the carbon on the surface of the catalyst. Carbon deposition is an essential feature of reforming reactions. The different carbon structures are customarily assessed by Raman analysis. Figure 13 depicts the Raman spectra of spent Ni-Al-H-600 catalysts acquired for 7 h using reaction temperatures of 500, 550, 600, and 650 °C. Two comparable intensity peaks appeared at 1475 cm −1 and 1535 cm − 1, corresponding to the D band, assigned to sp3 hybridized amorphous carbon, and G band, specified by the presence of graphitized carbon, respectively. The D band and G band are typical bands of regular-structured carbon that form on the surface of Ni-Al-H-600 during the partial reforming reaction. The results of Raman analysis confirm the formation of different types of carbon, particularly for high reaction temperatures, as is illustrated in the TPO analysis. Figure 14 illustrates the TGA analysis of the Ni-Al-H-600 catalyst operated at different reaction temperatures that lasted for 5 h. The result shows 4% weight loss of the mass due to gasification of the gas formed on the catalyst when the reaction temperature was 500 °C, while 8% weight loss was determined using a reaction temperature of 650 °C. As the reaction temperature was increased, the production of carbon grew slightly as a result of increased decomposition of CH4.

Conclusions
Different calcined 10% Ni catalysts supported on both high and low Al2O3 and on both high and low ZO2 were tested for partial oxidation reforming of methane. The catalysts were calcined at 600

Conclusions
Different calcined 10% Ni catalysts supported on both high and low Al2O3 and on both high and low ZO2 were tested for partial oxidation reforming of methane. The catalysts were calcined at 600

Conclusions
Different calcined 10% Ni catalysts supported on both high and low Al 2 O 3 and on both high and low ZO 2 were tested for partial oxidation reforming of methane. The catalysts were calcined at 600 and 800 • C. The highest CH 4 conversion of 90% and H 2 yield of 72% were obtained using Ni-Al-H-600.
The Ni-Al-H-600 catalyst retained the maximum surface area and the biggest pore volume. The study of the TGA indicated low amounts of carbon deposition except for the Ni-Al-L-600 catalyst. The TPO and Raman analyses of the catalysts denoted the presence of different types of carbon. The best activity and stability of performance of the Ni-Al-H-600 catalyst over different reaction temperatures (500-650 • C) was attained when the reaction was conducted at 650 • C for the period of 7 h.