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Review

From Waste to Hydrogen: Utilizing Waste as Feedstock or Catalysts for Hydrogen Generation

Faculty of Chemistry and Chemical Engineering, University of Maribor, 2000 Maribor, Slovenia
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Authors to whom correspondence should be addressed.
Clean Technol. 2025, 7(3), 76; https://doi.org/10.3390/cleantechnol7030076
Submission received: 18 July 2025 / Revised: 16 August 2025 / Accepted: 25 August 2025 / Published: 1 September 2025

Abstract

With the world facing the twin pressures of a warming climate and an ever-increasing amount of waste, it is becoming increasingly clear that we need to rethink the way we generate energy and use materials. Despite growing awareness, our energy systems are still largely dependent on fossil fuels and characterized by a linear ‘take-make-dispose’ model. This leaves us vulnerable to supply disruptions, rising greenhouse gas emissions, and the depletion of critical raw materials. Hydrogen is emerging as a potential carbon-free energy vector that can overcome both challenges if it is produced sustainably from renewable sources. This study reviews hydrogen production from a circular economy perspective, considering industrial, agricultural, and municipal solid waste as a resource rather than a burden. The focus is on the reuse of waste as a catalyst or catalyst support for hydrogen production. Firstly, the role of hydrogen as a new energy carrier is explored along with possible routes of waste valorization in the process of hydrogen production. This is followed by an analysis of where and how catalysts from waste can be utilized within various hydrogen production processes, namely those based on using fossil fuels as a source, biomass as a source, and electrocatalytic applications.

1. Introduction

Currently, the world is increasingly concerned about matters such as greenhouse gas (GHG) emissions, changes in climate, energy security, and availability [1]. The continuous growth and rapid urbanization of the world’s population and economy have led to an ever-increasing demand for energy [2]. Fossil fuels are the most widely used energy source [3] and account for 80% of global energy demand in 2023 [4]. It is estimated that fossil fuels will remain the dominant source until 2050 [3]. The global energy share in 2023 is shown in Figure 1. As can be seen, the majority of energy is generated by fossil fuels such as oil (30%), coal (27%), and natural gas (23%). The share of renewable energies is 12% [4].
The reliance on fossil fuels in producing energy or chemicals results in the emission of GHGs like CO2, nitrogen oxides, volatile organic compounds, and solid particles, which in turn drive global climate change [5]. One of the most controversial issues in the energy sector today is the amount of CO2 emissions released into the atmosphere from the use of fossil fuels [6], which necessitates a transition to cleaner alternatives [2]. In 2023, CO2 emissions reached a new record high of 37.4 Gt [7], with coal (45%), oil (33%), and natural gas (22%) being the main contributors [4]. Consequently, global decarbonization in the transport, industry, and power generation sectors is crucial to mitigate anthropogenic climate change [2]. The world is expected to gradually switch to renewable or alternative energies to reduce GHG emissions. The leading renewable energy sources to replace fossil fuels are solar, wind, hydro, geothermal, and biomass [8]. Power generation using wind and solar sources is marked by considerable intermittency [9]. This greatly affects the current power generation and transmission grid, which was not initially developed to manage variable energy inputs. To combat this problem, research is currently underway to find a suitable technology to store energy from intermittent sources [1]. One of the possible solutions is the storage of energy in the form of chemical carriers, of which hydrogen (H2) is particularly attractive for large-scale grid storage [10]. In addition, H2 can be used as an alternative fuel to fossil-based fuels because, unlike fossil-based fuels that release CO2, it only releases water [11]. In this context, there has been a growing interest by scientists and industry in versatile production routes. Renewable energy sources for H2 production are available in abundance [2]. According to the forecast of the International Renewable Energy Agency (IRENA), H2 will be one of the few energy carriers that will play a decisive role in reducing CO2 emissions [6].
Such a transition requires a large number of critical and precious metals that are essential for the development, deployment, and operation of modern energy technologies, but are at risk of supply disruption due to geological scarcity, geopolitical issues, or limited production capacity [12]. These elements are labeled as energy critical elements (ECE). ECEs consist of rare earth elements (REEs), platinum group metals (PGMs), elements specifically related to photovoltaic systems (Photovoltaic ECE), and other ECEs, as presented in Figure 2 [13]. As a result, global demand for ECEs is expected to rise sharply in the coming decades [14]. This raises the question of the availability of resources for the large-scale implementation of these technologies [12].
These materials will be essential in the coming decades for the transition from today’s carbon-based energy system to a zero-emission, decarbonized system that draws on many elements from the periodic table. Their indispensability arises from the unique properties of ECEs, which often make them irreplaceable in critical applications [15]. Each group of ECEs has its own importance in the transition from fossil fuels. PGMs are mostly used in electrocatalytic applications for fuel cells or electrodes in electrolysis, while Pt and Ru are also used as catalysts in multiple chemical reactions for cleaner fuels [13]. Rare earth elements (REEs) play a vital role in industry and are essential for the advancement of modern defense systems, green technologies, and electronic devices. Their importance is illustrated by REE-based alloys and permanent magnets, which are fundamental components in renewable energy technologies such as electric vehicles, energy-efficient lighting, and wind turbines. [16]. Photovoltaic ECEs are tied closely to semiconductor technology and are also indispensable in solar cell technology [17]. Other ECEs have a variety of uses. Li is essential in battery technology, which is necessary in the transition from fossil fuels [14]. Co is also important in battery technology, along with being utilized as a catalyst [17]. Ag is an important conductor, Re is used in superalloys for ultra-efficient gas-turbine blades, and, lastly, He is used for superconducting magnets. Out of the ECEs, Pt and Li are the most crucial elements for a transition into H2 technology [13].
Due to their importance for the transition to a sustainable technology system, many of these elements are classified as critical raw materials (CRM) in the EU [17]. The ECEs based on the CRM list for 2020 are shown in Figure 3.
The current and traditional linear model of material and energy flow of the modern economic system—extract–produce–use–discard—is not sustainable [19]. Inefficient recycling leads to significant amounts of CRMs being discarded in landfills, demonstrating resource misuse. Globally, lithium consumption is anticipated to rise by 18 times and platinum by 30 times from 2020 to 2030 [15]. Initially, the use of these materials can be reduced by improving the design of the products that contain them, making them more robust and durable [20]. Another method is to design products in such a way that they have higher material efficiency, and CRMs are used more wisely to reduce overall demand. This can be achieved, for example, by reducing the precious metal load of the catalysts. An example of doing so is in electrolysis, where single-atom catalysts, nanoparticles, or extended surface structures could be used to reduce the amount of Ir and Pt required [15]. Finally, CRMs can be replaced by materials that are abundant on Earth [20]. For instance, MoS2 is considered a possible and cost-effective replacement for Pt in the catalysis of H2 production from water [21]. Finally, more effective collection and recycling strategies are needed [20].
With the quality and quantity of finite resources progressively falling [22], along with an ever-increasing production of municipal solid waste (MSW) [23], a circular economy (CE) is an inevitable path to address the mentioned trends. It provides the economic system with an alternative flow model, one that is cyclical [19]. This concept describes an economic framework built on business models that eliminate the idea of ‘end-of-life’ by emphasizing material reduction, reuse, recycling, and recovery within production, distribution, and consumption. It operates on three scales: micro (products, enterprises, consumers), meso (eco-industrial parks), and macro (urban, regional, national, and global), targeting sustainable development that ensures environmental integrity, economic well-being, and social justice for current and future generations [24]. The CE model seeks to redefine progress, focusing on constructive society-wide advantages. It entails gradually decoupling economic activity from consuming finite resources and designing waste out of the system. Underpinned by a transition to renewable energy sources, the circular model builds economic, natural, and social capital [25]. Its main objective is to restore and regenerate material cycles, i.e., to maintain the value of materials at each point in a product’s life [26].
At the current rate of waste generation, global MSW generation is expected to increase by 70% compared to 2016 to 2.59 Bt in 2030 and 3.4 Bt in 2050 [27]. This worrying trend calls for innovative solutions for waste management in the context of a CE [28]. In terms of its physical form, waste can be divided into solid, liquid, and gaseous waste. According to the United Nations Environment Program (UNEP), solid waste contributes to about 5% of greenhouse gas emissions, especially CO2 and CH4 [29]. Currently, the majority of MSW is generated in industrialized countries. The energy contained in the MSW can be recovered through so-called waste-to-energy (W-t-E) technologies, which can produce usable energy in the form of electricity, heat, and fuels [27]. The utilization of waste as an energy source or by-product could help to reduce waste disposal problems in the future [30]. There are two main recovery or conversion processes for W-t-E technologies (i.e., biochemical and thermochemical), which depend on the composition and moisture content of the waste [31]. Thermochemical methods for waste transformation usually include biomass gasification [32], pyrolysis [33], and hydrothermal liquefaction [34]. However, biochemical methods of waste transformation consist of dark fermentation [35], photo fermentation [36], and microbial electrolysis cell [37]. The type of waste used as feedstock and the specific W-t-E process applied determine the form of energy produced. Typically, waste with high moisture levels—such as industrial wastewater, animal manure, or sewage sludge—is treated through anaerobic digestion to generate biogas. In contrast, solid waste streams, including MSW and lignocellulosic residues, are mainly utilized to produce thermal energy or converted into intermediate products like syngas and H2 [30]. With solid waste containing about 40–60% organic matter, it represents a valuable resource for energy recovery via appropriate W-t-E technologies. Despite the progress and maturity of these technologies, challenges persist due to waste heterogeneity, the complexity of treatment systems, and the issue of air pollutant emissions [38]. Another possibility of waste utilization is to convert waste into catalysts. A plethora of wastes have shown catalytic activity, from waste generated by large-scale industrial processes to wastes derived from biological sources (biomass) [39]. The waste-derived catalyst could be used in the production of biodiesel, bioethanol, syngas, bio-oil, H2, and energy [40]. The possible routes of waste utilization towards H2 are shown in Figure 4.
Extensive research has already explored H2 production methods from diverse resources [1,2,3], including fossil fuels [6], biomass [23,27,28], and water electrolysis [41,42]. However, to date, there has been no consolidated review that specifically addresses the role of waste-derived catalysts in various H2 production processes. This review aims to fill this research gap by systematically evaluating the application of waste catalysts across various H2 production methods. The article structure is as follows: firstly, H2 is outlined as an energy carrier and its importance in the industrial sector, along with the most common production methods. The review then continues onto waste valorization for H2 production. Three possible routes are explored as depicted in Figure 4. The routes explored are thermochemical and biochemical conversion methods, followed by the utilization of waste as a catalyst for H2 production, as the main topic of this review. Waste-derived catalysts are organized into chapters by their difference in feedstocks utilized: (i) fossil fuel-based processes; (ii) biomass-based processes; and (iii) electrochemical H2 production. In each chapter, we first provide a brief introduction and overview of the relevant technologies. Then, the benchmark waste-derived catalysts against commercial or non-waste catalyst counterparts using process-appropriate metrics are discussed. The review concludes with future prospects and research directions for deploying waste-derived catalysts for H2 production.

2. Hydrogen as an Energy Carrier

H2 is the most abundant element in the universe. Due to its reactivity, it only occurs on Earth in compounds such as water and organic materials [2]. The physical and molecular properties of H2 differ considerably from those of conventional fossil fuels [43]. When used in a fuel cell, H2 can convert chemical energy directly into electricity, bypassing the inefficiencies of conventional combustion processes [44]. The heating value of H2 is higher than that of traditional hydrocarbon-based fuels. However, due to its lower density, it requires a larger storage capacity or high compression for equivalent energy storage [2]. A comparison of important parameters for fuels between H2, hydrocarbon-based fuels, and alternative fuels such as ammonia and methanol is shown in Table 1.
Everything indicates that the H2 industry is set for significant development in the coming decades. However, there are many uncertainties and risks associated with the use of H2 as part of future decarbonization strategies [6]. One such risk is the explosive nature of H2. Since H2 is an odorless, colorless, and flammable gas, there is a risk of an undetected leak that could lead to an explosion in an enclosed space [2]. The transportation and storage of H2 could also pose a problem [6]. The biggest challenge for the transportation and storage of H2 is its low volume density and the possibility of H2-induced rupture in pipelines and storage facilities [49]. H2 can be stored as a gas under high pressure [50], as a cryogenic liquid [51], as metal hydrides [52], and in the form of other chemicals such as ammonia [53] and carbon-based fuels [54]. A promising option for H2 transportation is via the existing natural gas pipeline infrastructure, which also has the added benefit of reducing CO2 emissions [8].
H2 is also an important raw material for various industries [29]. It is used for hydrotreating, hydrocracking, and hydro conversion of crude oil and as a direct participant in the production cycles of synthetic and rocket fuel [6]. The chemical industry is highly dependent on H2 [10]. It is used in the metallurgical sector [55] and in the production of methanol [56] and plays a crucial role in the fertilizer industry in the production of ammonia using the Haber–Bosch process [57]. Global H2 production for 2023 reached 97 Mt, with use mainly concentrated in industry and the refinery sector. The industrial sector accounted for 54 Mt (56%) of total demand. Within this sector, ammonia production consumed around 60%, while methanol production and the production of directly reduced iron steelmaking consumed 30 and 10% respectively. The refinery sector consumed 43 Mt (44%) of H2, mainly for desulphurization and oil refining. A small amount of H2 was also used in the transport sector (0.06 Mt) and in electricity generation [58]. In the energy sector, H2 is suitable for both stationary and mobile applications. H2 can also be used to generate electricity by burning individual fuels and co-combustion (mixing) with other fuels and fuel cells [29].
H2 can be produced from various resources, including both renewable and non-renewable ones [6]. The most important resources for H2 production are currently fossil fuels [59], which account for 96% of all H2 produced [60]. Natural gas is the most commonly used source of H2, accounting for 47% of global production. The other two most commonly used fossil fuels are coal (27%) and oil (22%). The remaining 4% of H2 production is provided by water electrolysis [58]. The most common and widely used methods for H2 production are steam methane reforming (SMR) and autothermal reforming (ATR) of methane. Other production methods from fossil fuels are partial oxidation of methane (POM), dry methane reforming (DMR), coal gasification (CG), and pyrolysis (cracking) of methane and oil [8]. Consequently, the co-production of CO2 is unavoidable, and about 830 Mt of CO2 per year is produced by these methods [59]. Alternatively, H2 can be produced by water electrolysis, thermal, and biochemical conversion of biomass [60].

3. Waste Valorization in the Process of Hydrogen Production

There is a wide range of waste that is suitable for H2 production [5]. Pre-treatment steps like drying and impurity removal are crucial for enhancing energy density and regulating the physical and chemical characteristics of waste prior to further processing [60]. First, the biomass is converted into an intermediate H2 substrate, and then H2 production is achieved by catalytic conversion of the substrates [59]. The methods for converting waste into H2 are usually divided into thermochemical and biochemical methods [29]. These methods differ in terms of energy requirements, operating conditions, use of raw materials, efficiency, reaction time, and final yield [60]. H2 production from biomass and residual waste is technically and economically feasible, given the existing technical and economic conditions in many industrialized countries [5]. The utilization of biomass encounters problems such as seasonal availability and varying composition from one source to another. Although biomass composition may vary, it is composed of three components: hemicellulose, cellulose, and lignin. The proportions of these components set conversion behavior and product yields during processing [61]. The biggest contributor of H2 among the components is lignin, while from cellulose and hemicellulose, more CH4 and CO are derived [62]. As mentioned in the introduction, waste can also be utilized in the form of catalysts for the production of H2. This chapter provides a short overview of said pathways of waste utilization in said concept of H2 production.

3.1. Thermochemical Methods

Thermochemical processes are among the more effective methods for producing H2-rich gases from biomass [5]. They have the potential to decompose industrial and agricultural waste [63]. They are essential for a sustainable, integrated MSW management system [60] and are considered low-carbon methods of H2 production [6]. A distinct advantage of thermochemical processes is their ability to process a wider range of feedstocks [29]. Thermochemical processes are faster than biochemical processes, have higher stoichiometric H2 yields, higher conversion efficiencies, and shorter reaction times [60]. When subjected to gasification or pyrolysis, the thermochemical conversion of dried biomass resembles that of fossil fuels. These processes yield CO and CH4, which can be further transformed to enhance H2 production through steam reforming and water–gas shift reactions [5]. The quality of the H2 depends on the composition of the feedstock, the water content, the temperature, the heating rate, the type of gasifier, and the oxidation of the pyrolysis products [63]. Thermochemical processes offer clear benefits for waste management, achieving a 70–80% reduction in mass and an 80–90% decrease in volume, thereby conserving landfill capacity [60].

3.2. Biochemical Methods

Biochemical processes use microorganisms to decompose waste products containing organic material, biomass, or wastewater as substrates to produce H2 [60]. Due to the simple operating conditions, uniform H2 yield, and low energy consumption, this is an environmentally friendly method for producing H2 from various organic wastes [64]. The main mechanism in the biochemical production of H2 is the microbiological conversion of organic substrates and water into H2-containing gas by the action of the enzyme hydrogenase or nitrogenase [6]. Numerous bacteria colonies or consortia are capable of degrading various organic substances to produce H2 as their metabolic product [31]. Most biochemical processes are less energy-intensive than thermochemical processes, as they take place at ambient temperatures and pressures, but have a low H2 yield and low reaction rates [60]. Biological methods offer a way to produce H2 through fermentation, microbial electrolysis [29], and hybrid systems [60]. Based on the light requirement during the fermentation process, the process can be divided into dark fermentation (light-independent) and photo fermentation (light-dependent) [29]. Fermentative methods of H2 production are considered particularly advantageous as they can acclimatize to various organic substrates [31].

3.3. Waste as a Catalyst

The field of catalysis has recently experienced renewed interest in the development of catalytic materials derived from abundant and low-cost elements. Although catalysts are required in small quantities, they can still pose a significant expense. By generating catalysts from waste materials alongside the target product, the overall system becomes more cost-effective and environmentally sustainable [65], particularly in those instances where the waste finds no additional use. Recently, an increased interest has been in the utilization of waste material as a resource for the application and preparation of heterogeneous catalysts. Waste-derived catalysts fall into three main categories. The first involves the direct use of waste as a catalyst or support without any pre-treatment. The second category includes waste that undergoes pre-treatment, such as calcination or chemical activation, before being used. The third approach utilizes waste as a chemical source, extracting specific components for the synthesis of catalysts [66].
Industrial and agricultural residues are increasingly being re-imagined as low-cost catalysts rather than landfill liabilities. A prime example is bauxite residue, or red mud (RM), which is generated during the Bayer process [67], at an estimated 150 Mt per year and typically stored in lagoons [66]. It is an alkaline waste material rich in ferric oxide (Fe2O3), aluminum oxide (Al2O3), titanium oxide (TiO2), silica (SiO2), calcium oxide (CaO), and sodium oxide (Na2O). Among these, the high Fe2O3 content makes RM particularly suitable for catalytic applications, as iron-based catalysts are commonly used in industrial chemical reactions. Additionally, it possesses a relatively large surface area, thermal stability, and resistance to sintering, which prevents degradation at high temperatures [67]. Another potential waste that could be used for catalysts is steel slag (SS), a by-product of the steel industry, which has shown significant potential as a catalytic material due to its rich composition of metal oxides such as CaO, magnesium oxide (MgO), SiO2, iron oxides (Fe2O3, FeO), and Al2O3. Through various modification processes, it can be transformed into an efficient catalyst for applications such as catalytic pyrolysis and electrocatalysis [68]. Another industrial waste fit to be used as a catalyst is fly ash (FA) as well as bottom ash [66]. FA, a residue of combustion, is composed of fine particles whose makeup reflects both the inorganic constituents of the burned fuel and the technology used in the process [39]. It is predominantly a SiO2-Al2O3 material that also contains other components such as Fe2O3, CaO, and MgO [66]. Due to its alumina and silica content, numerous studies have examined the use of coal FA as a support [39].
Biomass sources can also be utilized for catalyst synthesis. Eggshell waste is being widely recognized as a valuable resource for catalytic applications, particularly in energy-related processes such as H2 production, syngas generation, and biodiesel synthesis. Eggshells are composed of approximately 96% calcium carbonate (CaCO3), 1% magnesium carbonate (MgCO3), 1% calcium phosphate (Ca3(PO4)2), and a small fraction of organic material and water. When subjected to calcination at temperatures between 800 °C and 1000 °C, CaCO3 decomposes into CaO, which exhibits strong basicity, high surface area, and excellent reactivity [69]. Various types of biomass can also be transformed into nanocomposites that can be used for H2 production due to their unique physicochemical properties, sustainability, and cost-effectiveness [70]. These catalysts are produced through processes such as pyrolysis, electrochemical treatments, and hydrothermal carbonization. Their ability to be modified with metals or heteroatoms further enhances their performance [71], enabling their use in energy conversion and storage technologies such as water electrolyzers and fuel cells [72]. They can be utilized for H2 production via electrochemical water splitting and thermochemical processes [73]. These materials make excellent candidates for electrocatalytic applications, particularly in hydrogen evolution reactions (HER) [74]. A visual representation of which waste can be utilized for which process for H2 production is shown in Figure 5.

4. Waste-Derived Catalysts for Fossil Fuel Processes

Regarding waste-derived catalysts for H2 production via fossil-based fuels, two distinct feedstocks were utilized: methane and coal. With methane as the feedstock, several different methods were employed: dry reforming, steam reforming, pyrolysis, and partial oxidation. When using coal, steam gasification was the preferred method.

4.1. Waste-Derived Catalysts in Dry Methane Reforming

DMR is a hot research topic as it is a possible pathway for producing clean H2 via the conversion of GHG [75]. DMR is a chemical conversion process via which CO2 and CH4 are simultaneously converted, using Ni-doped active materials to generate syngas [76], usually at temperatures above 600 °C [77]. The DMR reaction is shown in Equation (1) [78]:
C H 4 + C O 2 2 H 2 + 2 C O ; H ° r = 247   k J / m o l
As a slow process, the DMR reaction requires significant energy input to dissociate the stable CO2 and CH4 molecules, thereby achieving equilibrium and producing syngas [78]. Although noble metals achieve high catalytic activity, their use is limited due to high cost. Non-noble metals like Co and Ni offer a cheaper alternative while also achieving good catalytic performance [77].
DMR has been extensively studied using waste-derived catalysts. For example, Kanamori et al. [79] used Ni-containing battery waste to produce NiO, CeO2, and LaCoO3 catalysts. Out of the catalysts, the NiO catalyst achieved the highest CH4 conversion of 100% and maintained stable performance for 9 days, achieving a H2/CO ratio of slightly above 1, outperforming the CeO2 and LaCoO3 catalysts, which achieved a CH4 conversion of 45–80% and 28–62%, respectively. Huang et al. [80] also reported that adding basic oxides to waste catalysts improves performance: they modified FA with MgO and Ni. The catalyst with 20% loading achieved the highest methane conversion of 75–80%, reaching a H2:CO ratio slightly below 1. Likewise, Gao et al. [81] used coal fly ash (CFA) as Ni support. The Ni-CFA catalyst achieved a 96% CH4 and 97.2% CO2 conversion at 850 °C. The catalyst also maintained stability with minimal carbon formation for 12 h, while achieving a H2:CO ratio of slightly below 1. Chen et al. [82] demonstrated that photovoltaic waste (SiCl4) could be converted to SiO2 as a support for Ni. The Ni/SiO2 waste-derived catalyst achieved a CH4 conversion of 92.3% at 850 °C; in addition, the high conversion also maintained stability for 40 h on stream and a H2:CO ratio of 0.95. It also outperformed the Ni catalyst on commercial SiO2. In another study, Dega et al. [83] investigated autothermal dry reforming using a Ni-based spinel catalyst derived from SS. The slag was transformed into a multi-oxide Ni-Mg-Fe-Al spinel. The catalyst achieved a 95% CH4 conversion while also achieving a H2:CO ratio of 1.62. The catalyst also showed no coke formation over 48 h on stream. The process parameters and performance metrics of waste-derived catalysts for the DMR reaction are shown in Table 2, along with a non-waste Ni-based catalyst developed by Manabayeva et al. [84] as a benchmark.
As a benchmark, the non-waste catalyst reported by Manabayeva et al. [84] achieved a 94% CH4 conversion at 850 °C with a H2:CO ratio of 1.2. Compared to the benchmark, several waste-derived catalysts achieved similar, if not better, performance. The NiO catalyst developed by Kanamori et al. [79] achieved a 100% conversion at a lower temperature of 780 °C. The 10% Ni-CFA catalyst developed by Gao et al. [81] and the 13%Ni-SS catalyst developed by Chen et al. [82] also outperformed the non-waste catalysts in terms of CH4 conversion at the same temperature, achieving 96% and 96% CH4 conversion, respectively. The waste-derived catalysts mostly achieved a H2:CO ratio of around 1, which is common for the process of DMR. The exception is the 13%Ni-SS catalyst developed by Chen et al. [82], which achieved a H2:CO ratio of 1.62, which can be explained by the increase in the feed ratio of CH4:CO.

4.2. Waste-Derived Catalysts in Other Processes Utilizing Methane

SMR is the most widely used hydrocarbon-based reforming process [5]. It is the most common method used for H2 production [3], accounting for more than half of the world’s production [85]. Its attractiveness is attributed to its large-scale capabilities and relatively inexpensive production costs [86]. The reaction is highly endothermic, and a large amount of heat is required [85]; hence, the reactor operates at a temperature of 700–1000 °C [87]. The SMR reaction is shown in Equation (2) [88]:
C H 4 + H 2 O C O + 3 H 2 ; H ° r = 206   k J / m o l
Group 8 metals, typically Ni, serve as the active catalysts for the SMR owing to their high availability and low cost [85]. Among them, Ni/Al2O3 is the most widely employed [89]. An important parameter of the SMR reaction is the S/M (steam to methane) ratio, which positively influences the activity and selectivity of the process [85]. Usually, a ratio of 2.5–3 is employed [88]. In the process of SMR, multiple waste-derived catalysts have been explored. For instance, Ayesha et al. [90] synthesized a hydrotalcite-like Mg-Ni-Al catalyst promoted with CaO from waste eggshells (WE). The optimized 10% CaO catalyst exhibited a 77% CH4 conversion at 650 °C. The catalyst also had the added benefit of reducing carbon emissions, while stability tests over three cycles confirmed negligible carbon deposition and strong regenerability. In another study, Minhas et al. [91] investigated hemp-derived activated carbon (AC) as a catalyst support for Ni- and Co-based catalysts. The catalysts were loaded with 5% Ni, Co, and NiCo. At 750 °C the Co-based catalyst achieved the highest CH4 conversion (97.2%), outperforming the Ni-based (90.3%) and NiCo-based (92.5%) catalysts. The Co-based catalyst also showed superior stability over 44 h, maintaining an average of 93.2% CH4 conversion. As the benchmark, the non-waste-derived NiO/γ-Al2O3 catalysts developed by De Freitas Silva et al. [92], which achieved a 78% CH4 conversion at 700 °C, along with a H2:CO ratio of 6.8, was chosen. The catalyst by Ayesha et al. [90] achieved a similar CH4 conversion at lower temperatures, while the Co-AC catalysts developed by Minhas et al. [91] achieved a much higher CH4 conversion of 97.7%, albeit at a higher temperature. When comparing the H2:CO ratio achieved the non-waste catalyst achieved the highest ratio of 6.8, which is most likely due to the higher S/M ratio of the feed.
Partial oxidation serves as an alternative to steam reforming [93]. This process can operate with various feedstocks ranging from CH4 to heavy fuel oil and coal [5]. Due to the mild exothermicity of the partial oxidation, this reaction can be conducted autothermally [93], and usually in the temperature range of 800–900 °C [94]. POM can be described by Equation (3) [95]:
C H 4 + 0.5 O 2 C O + 2 H 2 ; H ° r = 36   k J / m o l
To achieve a significant degree of methane conversion (more than 90%), a mixture of methane and air undergoes a heat treatment in the presence of supported metal catalysts made of transition metals (Co, Ni) [6], or noble metals (Pt, Rh, Ir, Pd) [93]. Hasanat et al. [96] studied POM using a biomass FA-supported catalyst. The study conducted research on the catalytic ability of biomass FA, as a stand-alone catalyst, as well as different dopings of Ni/La2O3. The best performing catalyst (5% Ni/La2O3) achieved a CH4 conversion of 87%, while maintaining stability for over 30 h. On the other hand, the stand-alone biomass FA achieved a methane conversion of 55%. For the benchmark catalyst, the non-waste-derived Ni/Al2O3 developed by Vermeiren et al. [97] was used. The benchmark catalysts achieved a CH4 conversion of 95.7% and a H2:CO ratio of 2 at 780 °C. When comparing the waste-derived catalyst to the benchmark one, it can be seen that the waste-derived catalyst developed by Hasanat et al. [96] fell short in terms of CH4 conversion but achieved the same H2:CO ratio at a higher temperature.
An additional route is pyrolysis, a process of thermal breakdown without O2 that converts various light hydrocarbons into H2 and solid carbon [98]. The main advantage of this process is the generation of H2 without a CO2 by-product [99]. The reaction of methane pyrolysis (MP) is shown in Equation (4) [100]:
C H 4 C + H 2 ; H ° r = 74.9   k J / m o l
Solid carbon is the by-product of the methane pyrolysis (MP) reaction and is easy to store [101], and can be used as a raw material in various valuable materials (rubbers, tires, pigments, etc.) [102]. To achieve a high H2 yield, pyrolysis requires a temperature above 1000 °C. This temperature can be lowered with the addition of a catalyst [101]. For MP, catalysts are generally classified into two groups: metal-based and carbon-based [103]. While the former enables lower-temperature operation but deactivates rapidly, the latter maintains activity for extended periods, albeit at elevated temperatures [98]. Transition metals like Ni, Fe, and Co have been widely studied as active species for MP due to their high activity and moderate operating temperature [104]. Raza et al. [105] investigated the catalytic pyrolysis of methane using biomass FA as a catalyst support. In the study, the performance of only biomass FA, as well as different Co and Co/CeO2 dopings, was studied. The best performing catalyst was the 10% Co/CeO2-doped biomass FA, achieving a conversion of 76%. While biomass FA as a stand-alone catalyst achieved only 36% CH4 conversion. The benchmark catalyst for the MP process used was a FeCo/CeZrO2 non-waste catalyst developed by Ramasubramanian et al. [106]; the catalyst achieved a CH4 conversion of 90%. When compared to the benchmark, the waste-derived catalysts by Raza et al. [105] achieved a lower CH4 conversion at a higher temperature.
The parameters for SMR, MP, and POM technologies via waste-derived catalysts, along with the parameters for the benchmark catalysts, are presented in Table 3.

4.3. Waste-Derived Catalysts in Coal Gasification

The composition of coal includes various phases such as volatile matter, char, ash, and moisture [107]. In CG, coal undergoes thermochemical transformation to yield gaseous products, including CO and H2 [5], also defined as an incomplete combustion of coal [108]. It includes the processing of raw materials with air and steam in several stages at high temperatures [109]. Fan et al. conducted two complementary studies on using WE-derived CaO as a catalyst or catalyst support for H2 production via CG using a fixed-bed reactor setting in both. In the first study [110], the CaO from WE was used as a stand-alone catalyst, also acting as a CO2 sorbent. The addition of CaO (20%) at 900 °C almost doubled the H2 yield to 1.24 mol H2/mol C from 0.69 mol H2/mol C from gasification without a catalyst. The process achieved a H2:CO ratio of 3.65. In the second study [111], Fan et al. prepared a composite catalyst, combining CaO with K2CO3. The optimal mixture of 15% K2CO3 + 5% CaO gave the highest H2 yield of 1.34 mol H2/mol C at 800 °C, improving the yield given by only CaO as a catalyst, while also achieving a higher H2:CO ratio of 4.19 at lower temperatures. Zhao et al. [112] also explored the usage of a CaO-rich catalyst for coal gasification. They used construction demolition waste as a source of Ca. The demolition waste-based catalyst achieved a H2 yield of 1.64 mol H2/mol C at 9% loading and a reaction temperature of 900 °C, while also achieving a H2:CO ratio of 4.25. As the benchmark, the non-waste-derived K2CO3 + CaO catalysts developed by Zhou et al. [113] were chosen. The parameters and performance indicators of the benchmark and waste-derived catalysts are shown in Table 4.
The benchmark catalysts developed by Zhou et al. [113] achieved a H2 yield of 1.53-1.58 mol H2/mol C at 700 °C. The WE-based catalysts developed by Fan et al. [111,112] achieved a lower hydrogen yield than the benchmark catalyst while also requiring higher temperatures. The CaO catalyst from demolition waste-developed by Zhao et al. [112] achieved a higher H2 yield compared to the benchmark catalyst, but required a higher temperature of 900 °C to achieve that. In terms of H2:CO ratios, the catalyst by Zhao et al. [112] achieved the highest ratio of 4.25, followed closely by the CaO + K2CO3 catalyst developed by Fan et al. [111], which achieved a ratio of 4.19.

5. Waste-Derived Catalysts for Biomass-Based Processes

For H2 production from biomass-based sources using waste-derived catalysts, several different methods were employed: pyrolysis, a combination of pyrolysis and reforming, reforming of pyrolysis volatiles, and gasification. Across these biomass-based processes, the literature reports H2 yield in a variety of different units. To allow for a direct comparison between studies, all reported yields have been converted to a common basis of mL/g. The converted values are presented in the tables in parentheses alongside the originally reported units. These conversions assume standard temperature and pressure.

5.1. Waste-Derived Catalysts in Biomass Pyrolysis

Pyrolysis is a thermochemical technique that converts carbon-rich materials into value-added products such as bio-oil, biochar, and syngas under oxygen-free conditions. The absence of oxygen reduces the formation of dioxides, while catalysts derived from inorganic salts—such as chlorides, carbonates, and chromates—can accelerate the process [60]. To increase H2 yield, catalytic pyrolysis is proposed using metal (e.g., Ni or alkali metals) or non-metal-based catalysts (e.g., AC) [5].
In the process of biomass pyrolysis, several waste-derived catalysts have been tested. Wang et al. [114] used a dental ceramic wasted to synthesize Na2ZrO3 as a combined catalyst and CO2 sorbent. The catalyst was tested on the pyrolysis of different biomasses (municipal sludge, spirulina algae, and methylcellulose). The highest H2 yield of 205 mL H2/gbiomass was achieved with the pyrolysis of spirulina algae at 900 °C. The pyrolysis of methylcellulose achieved a yield of 197 mL/gbiomass and waste sludge achieved a yield of 142 mL/gbiomass. In terms of H2:CO ratios, spirulina algae pyrolysis achieved the highest one of 1.6, followed by municipal sludge (1.4) and methylcellulose (1). The catalyst also achieved excellent cyclic stability for over 30 cycles. In another study, Lan et al. [115] employed FA as a support for NiO in catalytic pyrolysis of rice straw. At 600 °C and an optimum loading of 20% NiO-FA, the H2 concentration in the synthesis gas increased from 7 vol% (without catalyst) to 41 vol% with the catalyst. The addition of the catalyst also raised the H2:CO ratio from 0.8 to 1.2. Zhang et al. [116] investigated two industrial wastes—spent fluid catalytic cracking catalyst (sFCC) and blast furnace ash (BFA)—as additives for the pyrolysis of sawdust. Adding 10 wt% of either waste shifted the product slate towards gases. At 700 °C, total gas yield reached 52.6% with BFA and 48.8 with sFCC, as compared to 45.2% without a catalyst. The H2 also increased to 43 mL H2/gbiomass with BFA and 40 mL H2/gbiomass with sFCC, showing a big increase in comparison to the non-catalytic process, which produced a H2 yield of 25 mL/gbiomass. The non-catalytic process yielded an extremely low H2:CO ratio of 0.05, which later increased to 0.2 with the addition of either of the catalysts. Lastly, Zhou et al. [117] used RM as a catalyst for the pyrolysis of corn stover. Using 10–40 wt% RM in the feed, the H2 yield steadily rose to 108 mL/gbiomass with 40 wt% of RM, as compared to 60 mL/gbiomass without RM present. The gas yield also increased to 643 mL/gbiomass from 412 mL/gbiomass. For the benchmark catalyst, the NiMo/Al2O3 catalyst developed by Qinglan et al. [118] was used. The benchmark catalyst achieved a 33.6 g H2/kgbiomass yield at 450 °C while also achieving a H2:CO ratio of 1.44. The key operating conditions and performance metrics of the studies on biomass pyrolysis using waste-derived catalysts and the benchmark catalyst are shown in Table 5.
Relative to the non-waste benchmark catalyst developed by Qinglan et al. [118], which produced 374 mL H2/gbiomass, the waste-derived catalysts fall short, even though most of them were tested at a higher temperature. Out of the waste-derived catalysts, the best performing one according to H2 yield was the Na2ZrO3 catalyst from dental waste-developed by Wang et al. [114], which achieved a yield of 205 mL H2/gbiomass. The other waste-derived catalysts achieved a much lower H2 yield, below 108 mL H2/gbiomass. When comparing the H2:CO ratios, the dental waste catalyst [114] achieved the highest ratio of 1.6, followed by the non-waste NiMo-based catalyst [118], which achieved a ratio of 1.44.

5.2. Waste-Derived Catalysts in Reforming of Pyrolysis Volatiles

The process of reforming pyrolysis volatiles for H2 production involves two main steps: biomass pyrolysis followed by catalytic steam reforming of the resulting vapors [119]. Reforming typically takes place in a fluidized bed reactor at temperatures between 600–800 °C. During the steam reforming stage, pyrolysis volatiles pass through the catalytic bed, where they react with steam at the catalyst’s active sites to produce a H2-rich gas [120]. Catalysts play a crucial role in this process, with metal-based catalysts, particularly Ni-based commercial catalysts, being most commonly used [121].
Al-Rahbi and Williams [122] examined Ni-doped waste ashes as reforming catalysts of pyrolysis vapors from the pyrolysis of wood biomass. They prepared three catalysts by doping Ni (10%) onto CFA, refuse-derived fuel (RDF), and waste tire ash (WTA). All the catalysts improved gas and H2 yield compared to non-catalytic operation, which produced 3.39 mmol H2/gbiomass along with a gas yield of 39.9%. Out of the three catalysts tested, the WTA catalyst was the most effective, increasing H2 yield to 10.55 mmol/gbiomass along with gas yield to 59.3%, outperforming both CFA (7.3 mmol H2/gbiomass and 54.9% gas yield) and RDF (9.66 mmol H2/gbiomass and 58% gas yield) catalysts. All three catalysts improved the base H2:CO ratio of 0.46 to 0.7 in the case of the Ni-CFA catalyst, and a ratio of 1 in the case of the WTA and RDF catalysts. Li and Williams [123] also used WTA and RDF for the reforming of pyrolysis volatiles, but in the case of volatiles from the pyrolysis of waste plastic. They used only WTA and RDF without Ni-doping. Both wastes increased the H2 yield from the non-catalytic process, which produced 72 mmol H2/gplastic. The WTA catalyst increased the H2 yield to 83.2 mmol/gplastic, while achieving a H2:CO ratio of 1.4, and RDF increased the yield to 81 mmol/gplastic, while achieving a ratio of 1.5. Furthermore, Ryczkowski et al. [124] employed a two-stage fixed-bed setup. The first step involved the pyrolysis of either pine pulp or cellulose. After that, the vapors passed through a Ni/La-derived catalyst on an FA-derived zeolite. The Ni/La catalyst achieved a H2 yield of 15.0 mmol H2/gcellulose and 10.8 mmol H2/gpine pulp, significantly outperforming the non-catalytic process, which produced only 1.3 mmol H2/gcellulose and 0.8 mmol H2/gpine pulp. Total gas production was also enhanced, increasing from 220 cm3 without a catalyst to 398 cm3 with Ni/La-A for cellulose conversion, and from 194 cm3 to 356 cm3 for pine pulp. The addition of the catalyst also increased the H2:CO ratios in the process for both biomasses, achieving a ratio of 1.24 for pine pulp (0.10 in the non-catalytic process) and 1.43 for cellulose (0.21 in the non-catalytic process). Wu et al. [125] also explored the reforming of pyrolysis volatiles from pine sawdust. They found that Ni-Fe alloy on SS can reform pine sawdust volatiles, increasing total gas output to 1.138 Nm3/kg from 0.987 Nm3/kg. The H2 yield of the process also increased to 386.52 mL/gbiomass from 321 mL/gbiomass. Guo et al. [126,127] also conducted research on the usage of steel industry wastes for reforming biomass tar. In one article [126], they explored the effect of using SS to enhance syngas and H2 production via catalytic reforming of pine sawdust pyrolysis tar. The experiments were conducted with and without the presence of steam. In the process of dry reforming, the syngas yield was 350 mL/gbiomass, with H2 production reaching 48.6 mL/gbiomass, achieving a H2:CO ratio of 0.24. With the addition of steam, the syngas yield increased to 493.5 mL/gbiomass, and H2 production to 91.3 mL/gbiomass, the H2:CO ratio also increased to 0.34. In a subsequent study, Guo et al. [127] investigated the effect of Ni-loading (5–10 wt%) onto the SS. The best results were obtained with a 10% Ni loading, the syngas yield achieved was 463 mL/gbiomass compared to 320 mL/gbiomass in the non-catalytic process. H2 production was also significantly increasing from 55 mL/gbiomass in the non-catalytic process to 86 mL/gbiomass with the 10 wt% Ni-SS catalyst. The addition of Ni onto the SS also improved the H2:CO ratio to 0.39. For the benchmark catalyst, the commercial Ni/Al2O3 catalyst used by Arregi et al. [121] was used. The catalyst achieved a high H2 yield of 117 g/kgbiomass, at a pyrolysis temperature of 500 °C, followed by a reforming temperature of 600 °C. The key operating conditions and performance metrics of the studies on reforming of pyrolysis volatiles using waste-derived catalysts and the benchmark catalyst are shown in Table 6.
In terms of the process of combining pyrolysis and further reforming of pyrolysis volatiles with biomass as its feedstock, the benchmark catalyst used by Arregi et al. [121] achieved the highest H2 yield of 1300 mL/gbiomass. Out of the waste-derived catalysts, the Ni-SS catalyst developed by Wu et al. [125] achieved the highest H2 yield of 386.5 mL/gbiomass, followed by the 20%Ni/La-FA developed by Ryczkowski et al. [124] catalysts, which achieved a H2 yield of 336.21 mL/gbiomass. This same catalyst also achieved the highest H2:CO ratio of 1.43. The WTA-based catalyst developed by Li and Williams [123], which used HDPE instead of biomass as a feedstock, achieved a very high H2 yield of 1865.89 mL/gplastic. This H2 yield seems unusually high when compared to other studies described. However, Li and Williams attribute their high H2 is due to the high reforming temperature, which improved the conversion of hydrocarbons and steam into H2 via steam reforming and water–gas shift reactions.

5.3. Waste-Derived Catalysts in Biomass Gasification

Biomass gasification is regarded as one of the most practical, sustainable, and potentially carbon-neutral alternatives to generate H2 [2]. Lignocellulosic biomass such as oil palm, bamboo, sugar palm, and wood are common feedstocks for gasification. Additionally, food scraps and MSW can serve as alternative feedstocks, while plastic waste, in particular, has recently gained significant attention. Combining plastics with biomass can further enhance gasification efficiency [128]. In biomass gasification, biomass undergoes partial oxidation to yield a gas mixture containing H2, CO, CH4, and CO2 [129]. Oxidizing agents such as air, oxygen, or steam are necessary for gasification [130]. Depending on the gasification agent used, there exists a difference in cost, gasification temperature, and product gas composition [131]. Catalysts commonly used in biomass gasification include alkaline earth metals (mineral oxides or carbonates made from calcium or magnesium), metal oxide-based catalysts (zeolites, silicates), and natural minerals (dolomite, olivine, limestone) [128].
Raheem et al. [132] used eggshell-derived CaO for the gasification of microalgae biomass. Two microalgae species, Spirulina platensis and Chlorella vulgaris, were used as feedstock, with CaO loadings in the range of 0–50 wt%. The base H2 yield (0% CaO) was 120 mL/gbiomass and 161 mL/gbiomass for Spirulina platensis and Chlorella vulgaris, respectively. With a 50 wt% CaO addition, the H2 yield increased to 252 mL/gbiomass with Spirulina platensis, and to 344 mL/gbiomass with Chlorella vulgaris. Along with the increase in H2 yield, an increase in the H2:CO ratio also followed. The gasification of Spirulina platensis achieved a ratio of 1.21, while the gasification of Chlorella vulgaris achieved a ratio of 2.28. Another study by Chen et al. [133] explored SS as a support for Ni as a catalyst in sewage sludge steam gasification. The addition of 20% Ni-doped SS increased gas and H2 yield, from the base values of 0.56 Nm3 syngas/kgbiomass and 9.8 mol H2/kgbiomass to 0.78 Nm3 syngas/kgbiomass and 15.72 mol H2/kgbiomass, respectively. The increase in H2 yield also resulted in the increase in the H2:CO ratio from 1.75 to 2.05 with the addition of the Ni-SS catalyst. Dong et al. [134] investigated the use of RM as a catalyst support for Ni in the process of bamboo sawdust steam gasification. The addition of RM and 10% Ni-RM increased the syngas yield to 170.9 and 210.3 mmol/gbiomass, respectively, from the non-catalytic yield of 165.1 mmol/gbiomass of syngas. The RM catalyst achieved a H2 yield of 108 mmol/gbiomass and a H2:CO ratio of 6.3l; the addition of 20% Ni increased the H2 yield to 135 mmol/gbiomass and the ratio to 7.82. Vamvuka et al. [135] also explored the use of RM as a catalyst in the process of steam gasification. They combined RM with building demolition concrete for a dual-function system in the form of a catalyst and CO2 sorbent. They tested the catalytic activity of said catalyst with two different biomass feedstocks (acacia pruning and helianthus residues). In the case of acacia pruning gasification, they achieved a H2 yield of 1.5 m3/kgbiomass alongside a H2:CO ratio of 13.9 with a catalyst of 30% RM loading. In the case of helianthus residues, they achieved a higher H2 yield of 2.35 m3/kgbiomass alongside a H2:CO ratio of 9.5 with a catalyst of 20% RM loading. Irfan et al. [136] investigated the effect of waste marble powder (WMP) in the steam gasification of MSW. The highest syngas yield of 1.23 Nm3/kgbiomass (0.55 Nm3 H2/kgbiomass) was achieved with 50 wt% of WMP, where the amount of H2 in the gas rose to 44.6% as compared to 32.4% in the process with zero WMP. Although the amount of H2 rose, the H2:CO ratio change was minimal from the non-catalytic process of 2.19 to 2.3 with the addition of WMP. Meanwhile, Amin et al. [137] investigated air gasification of MSW using WMP as a calcium-based catalyst. Various ratios of WMP/MSW (0–0.20) were tested. Optimal H2 yield and gas quality were achieved at a ratio of 0.15, resulting in a gas yield of 1.46 Nm3/kgbiomass and a H2 yield of 0.12 Nm3/kgbiomass. The H2:CO ratio remained comparable at all the WMP/MSW ratios (0.63–0.67). Laghari et al. [138] researched the use of a CaO-based catalyst sourced from WE in the process of air gasification of MSW. Different catalyst loadings were tested (10–40 wt%) at a temperature of 950 °C, with the best catalytic performance achieved at 40 wt% of CaO, reaching a H2 yield of 19.37 mol/kgbiomass and a H2:CO ratio of 2.5. The optimal process parameters were later determined to be 34% CaO loading at 795 °C to achieve a H2 yield of 22.74 mol/kgbiomass and a H2:CO ratio of 2.83. As the benchmark catalyst, the Ni/CeO2/Al2O3 catalyst developed by Peng et al. [139] was used. This catalyst achieved a H2 yield of 0.706 Nm3/kgbiomass at 823 °C, whilst achieving a H2:CO ratio of 1.84 in the process of steam gasification. The key operating conditions and performance metrics of the studies on biomass gasification using waste-derived and benchmark catalysts are shown in Table 7.
Compared to the benchmark catalyst studied by Peng et al. [139], which achieved a H2 yield of 706 mL/gbiomass, most of the other waste-derived catalysts achieved a lower yield. The exceptions are the 10% Ni-RM catalyst developed by Dong et al. [134], which achieved a H2 yield of 3025.7 mL/gbiomass and the RM catalyst developed by Vamvuka et al. [135], which achieved a H2 yield of 1500–2350 mL/gbiomass, depending on the feedstock. Both these waste-derived catalysts vastly outperformed the benchmark catalyst, which could be explained by the presence of a higher amount of steam in the process, which in turn increased the production of H2, which can also be seen when comparing the H2:CO ratios, as they are much higher in the processes of these waste-derived catalysts. Besides these two catalysts, the next best performing waste-derived catalyst in terms of H2 yield was the WMP-based catalyst developed by Irfan et al. [136], which achieved a H2 yield of 550 mL/gbiomass.

6. Waste-Derived Catalysts for Electrochemical-Based Processes

In electrocatalytic water splitting, catalysts are essential for reducing the kinetic barrier. Electrocatalyst performance is typically evaluated by parameters such as Tafel slope, overpotential, and exchange current density [140]. The hydrogen evolution reaction (HER) is the initial step of water electrolysis for producing H2. Efficient H2 generation requires catalysts that minimize the overpotential. The HER pathway depends on the solution’s acidity or basicity because the underlying mechanism changes with pH. In acidic media, protons (H+) from the electrolyte adsorb on the catalyst surface and are then reduced to form H2. In alkaline media, hydroxide ions (OH-) from the electrolyte discharge at the surface and are subsequently reduced, yielding water and H2 [141]. To surpass kinetic barriers, water electrolysis must operate above its thermodynamic potential of 1.23 V, where the additional voltage applied is known as the overpotential (η) [140]. Catalyst activities are typically compared using three specific η values (η1, η10, η100), which correspond to current densities of 1, 10, and 100 mA/cm2 each [142]. The current density of 10 mA/cm2 is usually employed when comparing HER electrocatalysts in mediums of different pH [142]. A catalyst’s inherent feature that is closely linked to the rate of HER is the Tafel slope [141]. Tafel slopes are widely applied to evaluate both the kinetics and mechanisms of electrocatalytic reactions. By definition, the slope represents the millivolts needed to increase current by one order of magnitude and is expressed in mV/dec. A lower Tafel slope signifies a more active catalyst, since less overpotential is required to achieve higher current densities [143]. Electrocatalyst stability is a key factor in determining its potential for commercialization, typically evaluated by maintaining activity over long-term operation [142]. Stability is an important factor for the practical use of HER catalysts. It is usually evaluated in two ways: (1) by many cycles of cyclic voltammetry (CV) or linear sweep voltammetry (LSV) and (2) by galvanostatic (or potentiostatic) testing during prolonged electrolysis. In the voltammetric approach, the CV or LSV is performed around the onset potential, and the overvoltage is compared before and after a certain number of cycles (e.g., 10,000); small shifts in overvoltage indicate good stability. In galvanostatic (or potentiostatic) measurements, the potential is monitored over time while the current (or potential) is held constant to track any drift. Other important performance metrics are the turnover rate and Faradaic efficiency [141].
This chapter will be divided into subchapters based on the type of electrocatalyst: (i) pure carbon electrocatalysts; (ii) self-doped carbon electrocatalysts; (iii) metal-doped carbon electrocatalysts; and (iv) multiple-doped carbon electrocatalysts. Lastly, a subchapter comparing the best-performing electrocatalysts from each subcategory with commercial Pt/C and Ir/C electrocatalysts will be included.

6.1. Pure Carbon Electrocatalysts

With the case of pure carbon materials derived from biomass, Sekar et al. [144] obtained corrugated graphene nanosheets from rice husks that exhibited a low overpotential of 9 mV at 10 mA/cm2 and a Tafel slope of 31 mV/dec, all while maintaining stable performance for 10 h. Prabu et al. [145] prepared porous carbon nanosheets from palm spathe and pollen waste. The carbon achieved an overpotential of 330 mV at 10 mA/cm2 with a Tafel slope of 63 mV/dec, whilst showing negligible degradation over 10 h of operation. Similarly, Pandey and Jeong [146] produced activated porous carbon from coffee waste, which had an overpotential of 210 mV at 10 mA/cm2 and 120 mV/dec Tafel slope. It sustained HER continuously for 24 h. Thirumal et al. [147] reported an AC from tamarind shells with an overpotential of 221 mV at 10 mA/cm2 and a Tafel slope of 204 mV/dec, with moderate stability, with 51.7% of current retained after 2 h of operation. In another example, Fu et al. [148] obtained porous carbon nanosheets from walnut shells, reaching an overpotential of 170 mV at 10 mA/cm2 and a 69.8 mV/dec Tafel slope, while maintaining stable H2 generation over 15 h. The comparison of parameters of pure carbon-based electrocatalysts is shown in Table 8.
Table 8 shows that without any doping or added catalytic sites, carbon materials can drive HER but typically at the cost of higher overpotentials (often in the 170–330 mV range for biomass carbons [128,129,130,131]). The electrocatalyst designed by Sekar et al. [144] achieves a very low overpotential of 9 mV and the lowest Tafel slope of 31 mV. The pure carbon catalysts showed decent stability under operating conditions, maintaining stable performance for over 10 h. The only outlier was the tamarind shell carbon, developed by Thirumal et al. [147], which maintained only 52% of the current after 2 h of operation.

6.2. Self-Doped Carbon Electrocatalysts

Biomass often contains heteroatoms (like N, S, P) that can be incorporated into the carbon matrix during pyrolysis to create catalytically active sites. One such example was by Saravanan et al. [149], who developed N-doped carbon nanosheets from peanut shells, which showed an onset overpotential of 80 mV and a Tafel slope of 75.7 mV/dec, remaining active over 10 h of HER testing. Zhu et al. [150] derived microporous N-doped carbon frameworks from pine needles, achieving an overpotential of 62 mV at 10 mA/cm2 with a Tafel slope of 45.9 mV/dec. The carbon frameworks showed excellent durability with a slight activity drop after 1000 cycles and 100 h. Meanwhile, Sekar et al. [151] used human hair to obtain graphitized carbon nanobundles self-doped with N (and minor S). These nanobundles required a low 16 mV of overpotential at 10 mA/cm2 with a Tafel slope of 51 mV/dec. Lastly, Zhou et al. [152] converted peanut root nodules into S, N-co-doped porous carbon, reaching 116 mV at 10 mA/cm2 and a Tafel slope of 67.8 mV/dec, with stable production over 12 h and over 1000 cycles. The comparison of parameters of self-doped carbon-based electrocatalysts is shown in Table 9.
Nitrogen doping is particularly effective, as N atoms (with their lone pair electrons) can tune the electron density of adjacent carbon, creating active sites that facilitate proton adsorption and conversion to H2. Sekar et al. [151] achieved the best results, delivering an extremely low overpotential of 16 mV at 10 mA/cm2 with a 51 mV/dec Tafel slope. In general, the self-doped carbons outperform pure carbons: doping typically lowers the overpotential into the double-digit millivolt range and yields smaller Tafel slopes (often 40–80 mV/dec) due to faster kinetics.

6.3. Metal-Doped Carbon Electrocatalysts

Incorporating metal species onto carbon can improve HER performance by providing additional active sites akin to noble metal catalysts. Nikitin et al. [153] synthesized a SiC/C–carbon composite with 5 wt% Pt that achieved overpotentials as low as 22–24 mV at 10 mA/cm2 and a Tafel slope in the range of 34.60 mV/dec. The Pt-SiC catalyst maintained stability for over 1500 cycles. Yang et al. [154] loaded CoO nanoparticles onto porous carbon from watermelon peels. The CoO-doped porous carbon achieved an overpotential of 111 mV at 10 mA/cm2 with a Tafel slope of 93.9 mV/dec and a stable performance for over 20 h. Min et al. [155] also embedded Co nanoparticles into a pomelo-peel-derived carbon membrane, achieving an overpotential of 154 mV at 10 mA/cm2 and a Tafel slope of 106.4 mV/dec. The material endured 12 h and over 2000 CV cycles with minimal degradation. Lu et al. [156] developed a NiO/C nanocomposite from eggshell membranes. The nanocomposite had a relatively high overpotential of 565 mV at 10 mA/cm2 despite a moderate Tafel slope of 77.8 mV/dec. The material had minor changes in HER activity after 500 CV cycles. Chai et al. [157] deposited Ni nanoparticles on carbon derived from leaves, achieving a low overpotential of 32 mV at 10 mA/cm2, albeit with a large Tafel slope of 125.6 mV/dec. The Ni-doped carbon achieved robust stability, maintaining HER activity over 48 h and 2000 cycles. Zhou et al. [158] also explored doping Ni onto carbon. In his case, he synthesized Ni-doped graphitic carbon from rose petals that achieved an overpotential of 220 mV at 10 mA/cm2 and a 64 mV/dec Tafel slope. The catalysts remained stable for over 24 h of operation. Meanwhile, Fakayode et al. [159] added Mo2C onto porous carbon from watermelon rind, resulting in an electrocatalyst that maintained durability for over 300 h. The catalyst achieved an overpotential of 133 mV at 10 mA/cm2 with a Tafel slope of 25 mV/dec. Humagain et al. [160] also used the approach of adding Mo2C onto carbon but instead used birch-derived biochar to create porous-Mo2C. The porous-Mo2C achieved a remarkable overpotential of 35 mV at 10 mA/cm2 and a low Tafel slope of 25 mV/dec, whilst maintaining almost 100% activity for over 100 h. Mir et al. [161] also explored the use of Mo2C, making a carbon-supported Mo2C from waste plastic, which achieved an overpotential of 179 at 10 mA/cm2 and a Tafel slope of 80 mV/dec. The molybdenum carbide catalyst remained stable for 2000 cycles and 10 h. On the other hand, Sekar et al. [162] introduced WO3 nanoflakes into neem-leaf carbon, achieving an overpotential of 360 mV at 10 mA/cm2 and a low Tafel slope of 14 mV/dec. The nanoflakes-doped carbon maintained stable operation for 12 h. The comparison of parameters of metal-doped carbon-based electrocatalysts is shown in Table 10.
Multiple metal dopants were tested on a carbon platform in terms of electrocatalytic activity, showing varied results. The best performing catalysts were the 5% Pt-doped catalysts, developed by Nikitin et al. [153], and the Mo2C electrocatalyst by Humagain et al. [160]. They achieved an overpotential and Tafel slope below 35 mV. A similarly low overpotential was also achieved by a Ni-doped carbon electrocatalyst developed by Chai et al. [157], but the catalyst had a large Tafel slope of 125.6 mV/dec. On the other hand, the electrocatalysts, developed by Fakayode et al. [159] and Sekar et al. [162], achieved low Tafel slopes of 25 mV/dec and 14 mV/dec, respectively, but suffered from high overpotentials. When trying to compare similar metal dopants on carbon, it is hard to find a common demotion in regard to the activity of the electrocatalyst, which could be a consequence of different preparation methods.

6.4. Multiple-Doped Carbon Electrocatalysts

Another approach used by researchers was to combine multiple dopants or phases to boost HER activity. For instance, Mulyadi et al. [163] engineered N, S, and P-doped carbon nanofibers from softwood pulp. Achieving an overpotential of 331 mV at 10 mA/cm2. The Tafel slope was 99 mV/dec, and the catalyst showed slight degradation over time. Deng et al. [164] utilized animal bone waste to create N, P, and Ca-doped biochar, achieving an overpotential of 162 mV at 10 mA/cm2 with a Tafel slope of 80 mV/dec. The animal bone-derived carbon showed slight deviation after 2000 cycles. To further better HER activity, besides adding multiple heteroatoms, metal species can be added along with them. Yang et al. [165] synthesized an electrocatalyst using edible amaranth-derived carbon, doped in situ with Fe and N. The catalyst demonstrated a HER overpotential of 92 mV at 10 mA/cm2 and a Tafel slope of 95.8 mV/dec. The catalyst also maintained a stable current output over 10 h. On the other hand, Wang et al. [166] explored a bimetallic electrocatalyst. They introduced Ni-Fe co-doping along with N, P, and S heteroatoms on nanocarbon from alfalfa biomass. The resulting electrocatalyst achieved an overpotential of 250 mV at 10 mA/cm2 and a Tafel slope of 84 mV/dec. While also showing stable performance after 1000 cycles and 50 h of operation. Abdolahi et al. [167] loaded Ni-Co oxide onto S, N-doped carbon from chicken feathers, achieving an overpotential of 87 mV at 10 mA/cm2 and a Tafel slope of 50 mV/dec. The catalyst maintained stable operation after 20 h. Jiang et al. [168] transformed waste tires into a Zn, S, N-doped graphitic carbon, which exhibited an overpotential of 50 mV at 10 mA/cm2 and a Tafel slope of 78 mV/dec, while maintaining stability for over 110 h. Sun et al. [169] reported a Co, N-doped carbon from office paper, which showed excellent stability over 3000 cycles and 14 h, while achieving an overpotential of 226 mV/dec at 10 mA/cm2 and a Tafel slope of 91 mV/dec. Lastly, Zhao et al. [170] demonstrated a hybrid catalyst from cotton textiles, synthesizing a CoNiO2/N, P-doped carbon substrate. The catalyst showed an overpotential of 247.6 mV at 10 mA/cm2 and a Tafel slope of 120.8 mV/dec, while maintaining stability for over 50 h. The comparison of parameters of hybrid-doped carbon-based electrocatalysts is shown in Table 11.
The best performers in this group (e.g., Fe, N–C [165], Ni–Co–oxide/N, S–C [167], Zn, S, N–C [168]) achieved overpotentials well below 100 mV, some even near 50 mV, with Tafel slopes in the range of ~50–80 mV/dec. These metrics are comparable to, and in some cases better than, the simpler metal-doped carbons, indicating a successful synergy. Although the above-mentioned electrocatalysts achieved good performance, some hybrid doped electrocatalysts achieved a performance worse than that of pure carbon electrocatalysts when considering overpotential. In terms of Tafel slope, the performance of hybrid doped electrocatalysts was better than pure carbon-based ones.

6.5. Comparison of Commercial and the Best Performing Carbon Electrocatalysts

In this subchapter, the performance parameters of commercial and waste-derived carbon-based electrocatalysts will be compared. As the benchmark, the commercial Pt/C and Ir/C catalysts were used. The performance parameters for the commercial Pt/C catalyst were taken from the study of Zheng et al. [171], in which the overpotential of the catalysts was defined as 29 mV at 10 mA/cm2 and the Tafel slope was 46 mV/dec. The catalyst maintained stability for 10 h. For the Ir/C commercial catalyst, the data were taken from the study by Peng et al. [172], where it was reported that the commercial Ir/C catalyst achieved an overpotential of 28 mV at 10 mA/cm2 and a Tafel slope of 55 mV/dec, while maintaining stability for 8 h. The parameters of the commercial and the best-performing waste-derived electrocatalyst are shown in Table 12.
From the data presented in Table 12, it can be seen that waste-derived electrocatalysts have a comparable performance to the commercial Pt/C and Ir/C electrocatalysts used. In terms of overpotential, several catalysts have outperformed the benchmark ones, with the pure-carbon rice husk-based electrocatalyst developed by Sekar et al. [144] achieving the lowest overpotential of 6 mV at 10 mA/cm2, closely followed by the self-doped human hair-based electrocatalyst designed by Sekar et al. [151], which achieved 16 mV at 10 mA/cm2. In terms of Tafel slope, the best performing electrocatalyst was the metal-doped birch wood-based one designed by Humagain et al. [160], achieving a Tafel slope of 25 mV/dec.

7. Future Prospects

Although this review shows significant progress, further efforts are needed to fully explore the potential of catalysts from waste materials for H2 production. Key directions for future research and development include the following:
In-depth benchmarking: although the efficiency in catalytic parameters was compared between the commercial (non-waste) and waste-derived catalyst, further studies and research are needed for a more detailed comparison of catalyst performance. Besides the parameters for catalytic conversion, such as yield and conversion, studies on long-term performance metrics, such as catalyst stability and deactivation rates over time. Determining whether waste-derived catalysts can maintain their performance over time (comparable to existing industrial catalysts) is critical to confirming their commercial viability. Stability is a critical factor for use in practice. Besides the performance metrics, the effect of impurities in waste-derived catalysts should be extensively screened to provide a more in-depth understanding of their effects on performance variability, environmental, and safety risks.
Techno-economic and environmental assessment: Secondly, a rigorous techno-economic analysis and life cycle assessment (LCA) of waste-to-hydrogen technologies is needed. Initial results suggest that the use of waste materials can reduce the cost of catalysts and the overall cost of H2 production, but a detailed financial assessment is needed to quantify the capital and operating costs on a large scale. This should take into account the costs of waste collection, processing, and treatment, as well as the savings from reduced feedstock consumption. In parallel, an LCA should be carried out to assess the net environmental impact, taking into account factors such as the energy required for waste processing, GHG throughout the supply chain, and the handling of spent catalysts at the end of their useful life.
Resource availability and location analysis: Thirdly, a spatial analysis of the availability of waste and biomass resources should be conducted to determine the strategic location of H2 production plants. The distribution of suitable waste feedstock is uneven. By mapping the sources of waste materials using geographic information systems, optimal locations for processing facilities can be identified, ideally near abundant waste streams to minimize transportation costs. By planning facilities close to feedstock sources, supply chain logistics will be improved and the overall efficiency and carbon footprint of H2 production can be reduced.
By pursuing these future directions—from performance validation and economic analysis to strategic resource planning—the remaining challenges can be addressed, and the viability of waste-to-hydrogen technologies can be improved upon. Such efforts will be instrumental in bridging the gap between laboratory innovations and real-world applications, ultimately advancing the twin goals of clean energy production and sustainable waste management.

8. Conclusions

H2 can be used in a variety of ways, from alternative energy storage to fuel, and is an important feedstock in the chemical industry for the production of ammonia and methanol, as well as in reforming processes. Its use as an energy storage vector and fuel makes it a potential solution for decarbonizing the energy sector, along with other renewable energy alternatives. Currently, however, H2 is mainly produced from fossil fuels, so a transition to renewable feedstocks such as biomass or water is a perspective alternative. Another aspect of the transition is the need for specific CRMs, some of which are geologically scarce, unevenly distributed, and prone to geopolitical instability, leading to significant supply issues. The current linear model exacerbates this problem through the inefficient use of these elements, resulting in significant quantities of these elements ending up in landfills.
In this context, waste recycling has been presented as a promising solution to reduce the dependence on virgin CRMs. The review focuses on the investigation of waste utilization for catalyst synthesis. Different catalytic routes have been explored, showing how industrial waste (e.g., red mud, steel slag, fly ash) and agricultural waste (e.g., eggshells, biomass waste) can serve as effective catalysts or catalyst support for H2 production. The catalytic properties of these catalysts have been observed in various H2 production processes, including fossil fuel-based processes, biomass conversion, and water electrolysis. For fossil fuel-based processes, waste-derived catalysts were effectively used in steam methane reforming, dry methane reforming, methane pyrolysis, partial oxidation of methane, and coal gasification. In the case of coal gasification, waste eggshells were researched. Many different wastes have been used in methane conversion processes, but they have the common characteristic of being doped with metals such as nickel and cobalt. Waste has also been successfully used as a catalyst in biomass conversion processes such as gasification and pyrolysis of biomass and the reforming of pyrolysis volatiles. In these thermochemical methods, industrial waste was mostly used as a catalyst or catalyst support, with the most common wastes being red mud, fly ash, and steel slag. In the context of electrochemical water splitting, a clear trend emerged where mainly carbon-rich biomass waste was used to synthesize electrocatalysts. These carbon-based materials have been used in various forms, including undoped carbons, self-doped carbons (e.g., N-, S-, P-doped), metal-doped carbons (e.g., Co, Ni, Mo), and hybrid-doped carbons, which contain both metallic and non-metallic dopants. By converting waste into valuable catalytic resources, this approach not only alleviates the problems of waste management but also has the potential to reduce production costs and improve sustainability.
Future research directions should focus on overcoming the remaining technical and economic challenges associated with waste-derived catalysts, such as long-term performance and stability of the catalyst, techno-economic analyses, and life cycle assessments of waste-derived catalysts. Additionally, regional mapping and analysis of waste availability should be conducted to identify strategically optimal locations for future H2 production centers.

Author Contributions

Conceptualization, D.T.H. and D.U.; methodology, D.T.H.; validation, D.T.H., D.U., and A.N.; formal analysis, D.T.H.; investigation, D.T.H.; resources, D.T.H.; data curation, A.N.; writing—original draft preparation, D.T.H.; writing—review and editing, D.U. and A.N.; visualization, A.N.; supervision, D.U.; project administration, D.U. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the Slovenian Research and Innovation Agency (program P2-0414 and P2-0046, PhD research fellowship No. 1000-24-0552 and project J2-60044).

Data Availability Statement

The original contributions presented in this study are included in the article material. Further inquiries can be directed to the corresponding authors.

Conflicts of Interest

The authors declare no conflicts of interest.

Abbreviations

The following abbreviations are used in this manuscript:
ACActivated carbon
BFABlast furnace ash
CECircular economy
CFACoal fly ash
CGCoal gasification
CRMCritical raw materials
DMRDry methane reforming
FAFly ash
GHGGreenhouse gas
HERHydrogen evolution reaction
IRENAInternational Renewable Energy Agency
LCALife cycle assessment
MPMethane pyrolysis
MSWMunicipal solid waste
PGMPlatinum group metals
POMPartial oxidation of methane
RDFRefuse-derived fuel
REERare earth elements
RMRed mud
sFCC Spent fluid catalytic cracking catalyst
SMRSteam methane reforming
SSSteel slag
UNEPUnited Nations Environment Programme
WEWaste eggshells
WMPWaste marble powder
WTAWaste tire ash
W-t-EWaste to energy

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Figure 1. Global energy share in 2023 [4].
Figure 1. Global energy share in 2023 [4].
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Figure 2. Critical elements for the transition from fossil fuels (adapted from [13]).
Figure 2. Critical elements for the transition from fossil fuels (adapted from [13]).
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Figure 3. ECE chart based on the 2020 EU CRM list (adapted from [18]).
Figure 3. ECE chart based on the 2020 EU CRM list (adapted from [18]).
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Figure 4. Routes of waste to hydrogen.
Figure 4. Routes of waste to hydrogen.
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Figure 5. Types of wastes as catalysts for different reactions.
Figure 5. Types of wastes as catalysts for different reactions.
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Table 1. Hydrogen properties compared to other fuels [8,9,43,45,46,47,48].
Table 1. Hydrogen properties compared to other fuels [8,9,43,45,46,47,48].
ParameterHydrogenMethanolAmmoniaGasolineMethaneDiesel
Higher heating value (MJ/kg)14222.722.548.295544.8
Lower heating value (MJ/kg)119.918.018.843.95042.5
Density at STP (kg/m3)0.0897900.730730–7800.720830.0
Auto-ignition temperature (K)853733931623813523
Flammability limits in air (%)4–766.7–3615–281–7.65.3–150.6–5.5
Flame temperature (K)248021431850258021872600
Table 2. Comparisons of parameters of waste-derived catalysts in the process of DMR.
Table 2. Comparisons of parameters of waste-derived catalysts in the process of DMR.
CatalystPreparation MethodProcess ParametersSubstrate ConversionH2:CO RatioReference
Non-waste
12% Ni-Al2O3
Wet impregnation
Calcination
850 °C
CH4:CO2 = 1
10 h
94%1.2[84]
NiOAcid/Base treatment
Precipitation
Calcination
780 °C
CH4:CO2 = 1
24 h
100%Slightly over 1[79]
20% Ni/MgO-FAAlkali treatment
Sol-gel synthesis
750 °C
CH4:CO2 = 1
9 h
75–80%Slightly below 1[80]
10% Ni-CFAAlkali/acid treatment
Wet impregnation
Calcination
850 °C
CH4:CO2 = 1
1 h
96%Slightly below 1[81]
10% Ni-SiO2Wet impregnation
Calcination
800 °C
CH4:CO2 = 1
1 h
92.3%0.95[82]
13% Ni-SS oxideNi doping
Calcination
850 °C
CH4:CO2 = 3
24 h
95%1.62[83]
Table 3. Comparisons of parameters of waste-derived catalysts for processes of methane conversion.
Table 3. Comparisons of parameters of waste-derived catalysts for processes of methane conversion.
ProcessCatalystPreparation
Method
Process
Parameters
Substrate
Conversion
H2:CO RatioReference
SMRNon-waste
NiO/γ-Al2O3
Wet impregnation Calcination700 °C
S/C = 4
78%6.8[92]
Sorption-enhanced SMR10% CaO-Mg/Ni/AlCo-precipitation
Wet impregnation
Calcination
650 °C
S/C = 2
77%/[90]
SMR5% Co-ACWet impregnation
Calcination
750 °C
S/C = 2
97.7%2.7[91]
POMNon-waste
5% Ni/Al2O3
Wet impregnation
Calcination
780 °C
CH4:O2 = 2
95.7%2[97]
POM5% Ni/La2O3-FAWet impregnation
Calcination
850 °C
CH4:O2 = 2
85%2[96]
MPNon-waste FeCo/CeZrO2Wet impregnation
Calcination
700 °C90%/[106]
MP10% Co/CeO2-FAHydrothermal processes
Wet impregnation
Calcination
850 °C76%/[105]
Table 4. Comparisons of parameters of waste-derived catalysts for processes of coal gasification.
Table 4. Comparisons of parameters of waste-derived catalysts for processes of coal gasification.
CatalystPreparation MethodProcess ParametersHydrogen YieldH2:CO RatioReference
Non-waste K2CO3 + CaOMechanical mixing700 °C≈1.53–1.58 mol H2/mol CNot reported[113]
20% WE CaOCalcination900 °C1.24 mol H2/mol C3.65[110]
5% WE CaO + 15% K2CO3Calcination800 °C1.34 mol H2/mol C4.19[111]
CaO-rich catalyst from demolition wasteCalcination900 °C1.64 mol H2/mol C4.25[112]
Table 5. Comparisons of parameters of waste-derived catalysts for processes of biomass pyrolysis.
Table 5. Comparisons of parameters of waste-derived catalysts for processes of biomass pyrolysis.
CatalystPreparation MethodSubstrateProcess ParametersHydrogen YieldH2:CO RatioReference
Non-waste NiMo/Al2O3/Pine chips450 °C
40 min
33.6 g/kgbiomass
(374 mL/gbiomss)
1.44[118]
Na2ZrO3CalcinationSpirulina algae900 °C
40 °C/min
205 mL/gbiomass1.6[114]
20% NiO-FAHomogeneous precipitation
Calcination
Rice straw600 °C
20 min
41 vol%1.2[115]
10% BFACalcinationSawdust700 °C
20 min
43 mL/gbiomass0.2[116]
10% sFCCCalcinationSawdust700 °C
20 min
40 mL/gbiomass0.2[116]
40% RMDirect useCorn stover800 °C
1 h
107.7 mL/gbiomass0.63[117]
Table 6. Comparisons of parameters of waste-derived catalysts for processes of reforming of pyrolysis volatiles.
Table 6. Comparisons of parameters of waste-derived catalysts for processes of reforming of pyrolysis volatiles.
CatalystPreparation MethodSubstrateProcess ParametersHydrogen YieldH2:CO RatioReference
Non-waste Ni/Al2O3/Pine wood sawdustPyrolysis: 500 °C
Reforming: 600 °C
117 g/kgbiomass
(1300 mL/gbiomass)
/[121]
10% Ni-WTAAshing
Ni impregnation
Waste wood pelletsPyrolysis: 600 °C
Reforming: 800 °C
10.5 mmol/gbiomass
(235.35 mL/gbiomass)
1[122]
WTAOxidationHigh Density PolyethylenePyrolysis: 600 °C
Reforming:1000 °C
83.2 mmol/gplastic
(1865.89 mL/gbiomass)
1.4[123]
20% Ni/La-FAImpregnation
Calcination
CellulosePyrolysis: 500 °C
Reforming: 700 °C
15 mmol/gbiomass
(336.21 mL/gbiomass)
1.43[124]
20% Ni/La-FAImpregnation
Calcination
Pine PulpPyrolysis: 500 °C
Reforming: 700 °C
10.8 mmol/gbiomass
(242.07 mL/gbiomass)
1.24[124]
Ni-SSImpregnation
Calcination
Pine sawdust volatilesReforming: 800 °C386.5 mL/gbiomass/[125]
SSCalcinationPine sawdust tarReforming: 800 °C91.3 mL/gbiomass0.34[126]
10% Ni-SSImpregnation
Calcination
Pine sawdust tarReforming: 800 °C86 mL/gbiomass0.39[127]
Table 7. Comparisons of parameters of waste-derived catalysts for processes of biomass gasification.
Table 7. Comparisons of parameters of waste-derived catalysts for processes of biomass gasification.
CatalystPreparation MethodSubstrateTemperatureHydrogen YieldH2:CO RatioReference
Non-waste
Ni/CeO2/Al2O3
Impregnation
Calcination
Wood residue823 °C0.706 Nm3/kgbiomass
(706 mL/gbiomass)
1.84[139]
WECalcinationSpirulina platensis800 °C252 mL/gbiomass1.21[132]
WECalcinationChlorella vulgaris800 °C344 mL/gbiomass2.28[132]
20% Ni-SSImpregnation
Calcination
Sewage sludge900 °C15.7 mmol/gbiomass
(351.1 mL/gbiomass)
2.05[133]
10% Ni-RMImpregnation
Calcination
Bamboo sawdust800 °C135 mmol/gbiomass
(3025.9 mL/gbiomass)
7.82[134]
30% RMCalcinationAcacia pruning850 °C1.5 m3/kgbiomass
(1500 mL/gbiomass)
13.9[135]
20% RMCalcinationHelianthus residues850 °C2.35 m3/kgbiomass
(2350 mL/gbiomass)
9.5[135]
50% WMPCalcinationMSW900 °C0.55 Nm3/kgbiomass
(550 mL/gbiomass)
2.3[136]
10% WMPCalcinationMSW700 °C0.12 Nm3/kgbiomass
(130 mL/gbiomass)
0.66[137]
40% CaO (WE)CalcinationMSW950 °C19.4 mmol/gbiomass
(435.83 mL/gbiomass)
2.5[138]
Table 8. Pure carbon electrocatalyst performance indicators.
Table 8. Pure carbon electrocatalyst performance indicators.
Waste MaterialCatalystOverpotential (mV at 10 mA/cm2)Tafel Slope (mV/dec)StabilityReference
Rice huskGraphene nanosheets93110 h[144]
Palm spathe
Pollen waste
Porous carbon nanosheets3306310 h[145]
Coffe wastePorous carbon21012024 h[146]
Tamarind shellsAC22120451.7% after 2 h[147]
Walnut shellsPorous carbon nanosheets17069.815 h[148]
Table 9. Self-doped carbon electrocatalyst performance indicators.
Table 9. Self-doped carbon electrocatalyst performance indicators.
Waste MaterialCatalystOverpotential (mV at 10 mA/cm2)Tafel Slope (mV/dec)StabilityReference
Peanut shellsN-doped carbon80 (onset)75.710 h[149]
Pine needlesN-doped carbon6245.9100 h
1000 cycles
[150]
Human hairN-doped nanobundles1651/[151]
Peanut root nodulesS, N-doped carbon11667.812 h
1000 cycles
[152]
Table 10. Metal-doped carbon electrocatalyst performance indicators.
Table 10. Metal-doped carbon electrocatalyst performance indicators.
Waste MaterialCatalystOverpotential (mV at 10 mA/cm2)Tafel Slope (mV/dec)StabilityReference
Rice and oat husks5% Pt-SiC22–2434–601500 cycles[153]
Watermelon peelsCoO-porous carbon11193.920 h[154]
Pomelo peelCo-carbon154106.412 h
2000 cycles
[155]
Eggshell membranesNiO-carbon56577.8500 cycles[156]
leavesNi-carbon32125.648 h
2000 cycles
[157]
Rose petalsNi-carbon2206424 h[158]
Watermelon rindMo2C-porous carbon13325300 h[159]
Birch woodMo2C-porous carbon3525100 h[160]
Waste plasticMo2C-carbon1798010 h
2000 cycles
[161]
Neem leavesWO3-carbon3601412 h[162]
Table 11. Multiple-doped carbon electrocatalyst performance indicators.
Table 11. Multiple-doped carbon electrocatalyst performance indicators.
Waste MaterialCatalystOverpotential (mV at 10 mA/cm2)Tafel Slope (mV/dec)StabilityReference
Softwood pulpN, S, P-carbon nanofibers33199/[163]
Animal bonesN, P, Ca-biochar162802000 cycles[164]
AmaranthFe3O4, N-carbon9295.810 h[165]
AlfalfaNiFe-N, P, S-nanocarbon2508450 h
1000 cycles
[166]
Chicken feathersNiCoO-S, N-porous carbon875020 h[167]
Waste tiresZn, S, N-carbon5078110 h[168]
Office paperCo, N-carbon2269114 h
3000 cycles
[169]
Cotton textilesP, CoNiO2, N-carbon247.6120.850 h[170]
Table 12. Parameters of commercial and waste-derived electrocatalysts.
Table 12. Parameters of commercial and waste-derived electrocatalysts.
Catalyst TypeCatalystOverpotential (mV at 10 mA/cm2)Tafel Slope (mV/dec)StabilityReference
CommercialPt/C294610 h[171]
/Ir/C28558 h[172]
Pure carbon Rice husk-based
Graphene nanosheets
93110 h[144]
Self-dopedPine needle-based
N-doped carbon
6245.9100 h
1000 cycles
[150]
/Human hair-based
N-doped nanobundles
1651/[151]
Metal-dopedRice and oat husk-based
5% Pt-SiC
22–2434–601500 cycles[153]
/Birch wood-based
Mo2C-porous carbon
3525100 h[160]
Multi-dopedChicken feather-based
NiCoO-S, N-porous carbon
875020 h[167]
/Waste tire-based
Zn, S, N-carbon
5078110 h[168]
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Hren, D.T.; Nemet, A.; Urbancl, D. From Waste to Hydrogen: Utilizing Waste as Feedstock or Catalysts for Hydrogen Generation. Clean Technol. 2025, 7, 76. https://doi.org/10.3390/cleantechnol7030076

AMA Style

Hren DT, Nemet A, Urbancl D. From Waste to Hydrogen: Utilizing Waste as Feedstock or Catalysts for Hydrogen Generation. Clean Technologies. 2025; 7(3):76. https://doi.org/10.3390/cleantechnol7030076

Chicago/Turabian Style

Hren, David Tian, Andreja Nemet, and Danijela Urbancl. 2025. "From Waste to Hydrogen: Utilizing Waste as Feedstock or Catalysts for Hydrogen Generation" Clean Technologies 7, no. 3: 76. https://doi.org/10.3390/cleantechnol7030076

APA Style

Hren, D. T., Nemet, A., & Urbancl, D. (2025). From Waste to Hydrogen: Utilizing Waste as Feedstock or Catalysts for Hydrogen Generation. Clean Technologies, 7(3), 76. https://doi.org/10.3390/cleantechnol7030076

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