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Research on the oxidation mechanism of C2H4 in automotive exhaust over MgO-supported Ag-Cu bimetallic synergistic catalysts
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Wei ZHANG, Genrui ZHAO, Zehong LI, Guisheng CHEN, Zhaohui CHEN*
Journal of Fuel Chemistry and Technology | 2026, 54(4) : 20250243-660 - 20250243-667
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Journal of Fuel Chemistry and Technology | 2026, 54(4): 20250243-660-20250243-667
• RESEARCH PAPER •
Research on the oxidation mechanism of C2H4 in automotive exhaust over MgO-supported Ag-Cu bimetallic synergistic catalysts
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Wei ZHANG, Genrui ZHAO, Zehong LI, Guisheng CHEN, Zhaohui CHEN*
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  • Yunnan Provincial Key Laboratory of Internal Combustion Engines, Kunming University of Science and Technology, Kunming 650500, China
Published: 2026-04-10 doi: 10.1016/S1872-5813(26)60640-8
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Ethylene (C2H4) in vehicle exhaust is a highly reactive volatile organic compound (VOC). Its photo-oxidative reaction with NOx contributes to the formation of O3 and secondary organic aerosols (SOA), the latter being a key precursor of PM2.5. In this study, a novel MgO-supported Ag-Cu bimetallic catalyst was designed and investigated using density functional theory (DFT). The effects of Ag and Cu loading on the geometric structure, stability, and reactant adsorption characteristics of the catalyst were analyzed, and the catalytic oxidation pathways of C2H4 over AgCu-MgO was elucidated. The results indicate that loading Ag significantly enhances the adsorption of C2H4. The incorporation of Cu into Ag-MgO to form a AgCu-MgO bimetallic catalyst (dual atom catalyst, DACS) further improves the oxidative activity toward C2H4. Based on the binding energies of the Ag and Cu bimetallic sites and the adsorption energies of C2H4 and O2, three representative configurations were selected for detailed reaction pathway analysis. Among them, Configuration 6 of AgCu-MgO exhibited the highest catalytic oxidation performance. This study provides new atomic-scale insights for the rational design of efficient catalysts targeting olefinic pollutants in automotive emissions and offers valuable guidance for advancing exhaust after-treatment technologies.

MgO  /  Ag-Cu  /  C2H4  /  catalytic oxidation  /  automotive exhaust
张韦, 赵根锐, 李泽宏, 陈贵升, 陈朝辉. MgO负载Ag-Cu双金属协同对汽车尾气中乙烯的氧化机制研究. 燃料化学学报（中英文）, 2026 , 54 (4) : 20250243-660 -20250243-667 . DOI: 10.1016/S1872-5813(26)60640-8
Wei ZHANG, Genrui ZHAO, Zehong LI, Guisheng CHEN, Zhaohui CHEN. Research on the oxidation mechanism of C2H4 in automotive exhaust over MgO-supported Ag-Cu bimetallic synergistic catalysts[J]. Journal of Fuel Chemistry and Technology, 2026 , 54 (4) : 20250243-660 -20250243-667 . DOI: 10.1016/S1872-5813(26)60640-8
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Vehicle exhaust emissions comprise not only conventional pollutants such as CO, HC, NOₓ, and particulate matter (PM)[1−3]，but also unconventional species such as C2H4 (ethylene)[4−5]. As a highly reactive volatile organic compound (VOC), C2H4 can undergo photochemical reactions with NOₓ under sunlight to generate O3 and secondary organic aerosols (SOA), the latter being a key precursor to PM2.5. PM poses serious threats to both human health and atmospheric environmental quality[6−7]. Therefore, the catalytic removal of olefinic pollutants such as C2H4 from vehicle emissions is essential for meeting increasingly stringent environmental regulations. Currently, noble metal-based oxidation catalysts—such as diesel oxidation catalysts (DOC) and catalyzed diesel particulate filters (CDPF)—exhibit some capability for C2H4 removal[8], yet their efficiency remains limited to approximately 65%[9]. Noble metals, due to their unsaturated d-electron orbitals, possess strong adsorption affinity for reactants and exhibit excellent catalytic performance[10]. Platinum group metals (PGMs) such as Pt and Pd are particularly effective, as they facilitate the simultaneous adsorption and activation of C2H4 and O2 on their surfaces. Huang et al.[11] reported that Pt-Pd/CeO2 catalysts show outstanding low-temperature oxidation activity toward HC and CO in diesel exhaust. Huang et al.[12] found that Pt/β-zeolite catalysts can achieve up to 90% oxidation efficiency for olefins such as propylene. However, the widespread application of PGMs is constrained by their high cost, scarcity, and susceptibility to sintering and deactivation under high exhaust temperatures[13−14].
In contrast, Ag is abundant, relatively cost-effective, and demonstrates excellent selective adsorption and oxidation capacity towards C2H4, making it a promising alternative for designing efficient and economically viable catalysts. Liang et al.[15] demonstrated that Ag loading significantly enhances the degradation efficiency of C2H4 under light irradiation. Lee et al.[16] revealed that Ag supported on ZSM-5 zeolite improves the adsorption capacity for C2H4. Yan et al.[17] found that Ag-modified aromatic microporous polyimide (MPI) exhibits enhanced selectivity for C2H4 adsorption. Giorgio et al.[18] also reported that supporting Ag on porous carbon improves the selective adsorption for olefinic species. Furthermore, studies on bimetallic systems have revealed synergistic effects. Pu et al.[19]investigated Ag-loaded Al2O3 modified with various transition metals and concluded that co-loading Ag and Cu results in better selectivity and oxidation performance for C2H4 than Ag alone. Greiner et al.[20] similarly confirmed that Ag-Cu bimetallic catalysts exhibit higher C2H4 oxidation selectivity compared to monometallic Ag. While Ag provides strong selectivity and catalytic oxidation capability for C2H4, Cu enhances the adsorption of O2. Therefore, Ag-Cu bimetallic systems are promising for synergistically improving both the selectivity and oxidation activity toward C2H4.
Layered double hydroxides (LDHs) are a class of two-dimensional layered clays with a positively charged octahedral structure similar to hydrotalcite. Among them, MgAl-LDHs have attracted widespread attention due to their low synthesis cost and readily available raw materials[21−23]. Upon high-temperature calcination, MgAl-LDHs are transformed into layered double oxides (MgAl-LDOs) with large specific surface area, high dispersion of active components, and tunable chemical properties. X-ray diffraction (XRD) analysis confirms that the dominant crystalline phase in MgAl-LDO after calcination is MgO[24−25]. Therefore, in this study, MgO was selected as a simplified structural model of MgAl-LDO to serve as the support of Ag and Cu in the catalytic oxidation of C2H4.
To mitigate the adverse effects of C2H4 emissions from automobiles on human health and the environment, this study proposes a novel AgCu-MgO catalyst for the catalytic oxidation of C2H4. Firstly, density functional theory (DFT) calculations were employed to investigate the effects of Ag and Cu loading on the geometric structure, electronic properties, stability, and adsorption characteristics of MgO. Subsequently, the detailed catalytic oxidation pathways for C2H4 over the Ag- and Cu-modified MgO catalysts were explored. Based on binding energy and adsorption energy analysis, three representative configurations were selected for further evaluation of their reaction pathways. Among them, the optimal catalytic structure was identified. This work provides valuable theoretical insights and design principles for developing efficient catalysts to control olefinic pollutants from automotive exhaust.
1　Computational methods and models
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DFT calculations were carried out using the Vienna Ab Initio Simulation Package (VASP)[26−27]. To accurately describe the interactions between electrons in the catalyst and adsorbates, as well as between electrons and atomic nuclei, the Perdew-Burke-Ernzerhof (PBE) exchange-correlation functional[28] and the projector augmented wave (PAW) method[29] were employed. A plane-wave cutoff energy of 520 eV was used. Structural relaxations were performed using the conjugate gradient algorithm. The convergence criteria for electronic iterations were set to 1×10−5 eV for energy and 0.02 eV/Å for force. Long-range van der Waals interactions, crucial for adsorption and catalytic processes, were corrected using the DFT-D3 dispersion scheme[30]. The Hubbard U parameter (U-J) was set to 4 eV based on Perdew et al.[31]. A 3×3 MgO supercell model with a four-layer slab structure was adopted, with the bottom two layers fixed during optimization. A vacuum region of 15 Å was added along the Z-direction to eliminate spurious interactions between adjacent periodic slabs. To improve convergence near the Fermi level, a Gaussian smearing width of 0.05 eV was applied.
The MgO unit cell was optimized using a 6×6×6 Monkhorst-Pack k-point mesh. Due to the relatively large size of the supercell, the surface calculations were performed using a 2×2×1 Γ-centered k-point mesh. To accurately identify transition states for elementary reactions, the climbing image nudged elastic band (CI-NEB) method[32] was first employed with a force convergence criterion of 1 eV/Å, allowing for rapid convergence. The resulting transition state structures were subsequently optimized using the improved dimer method (IDM)[33] until the forces was reduced below 0.05 eV/Å, ensuring precise transition state geometries. Each identified transition state was confirmed by vibrational frequency analysis to possess exactly one imaginary frequency. Gibbs free energies of reactions were calculated using the Vaspkit toolkit[34], with a reference temperature of 298.15 K. In addition, Bader charge analysis[35] was conducted to quantify charge transfer during reactions. All structural models and isosurfaces were visualized using the VESTA software package[36].
The binding energy ($ {E}_{{\mathrm{b}}} $) of metal atoms anchored on the MgO surface was calculated as:
$ {E}_{{\mathrm{b}}}={E}_{{\mathrm{cat}}}-{E}_{{\mathrm{m}}}-{E}_{{\mathrm{sub}}} $
where $ {E}_{{\mathrm{m}}} $ and $ {E}_{{\mathrm{sub}}} $ represent the energies of the isolated metal atom and the pristine MgO substrate, respectively. A more negative binding energy indicates stronger interaction between the metal atom and the MgO surface.
The adsorption energy ($ {E}_{{\mathrm{ads}}} $) of a gas molecule on the catalyst surface was calculated as:
$ {E}_{{\mathrm{ads}}}={E}_{{\mathrm{tot}}}-{E}_{{\mathrm{cat}}}-{E}_{{\mathrm{adsb}}} $
where $ {E}_{{\mathrm{tot}}} $ and $ {E}_{{\mathrm{adsb}}} $ represent the total energy of the adsorption system and the energy of the isolated gas molecule, respectively. A more negative value indicates stronger adsorption.
The activation energy ($ {E}_{{\mathrm{b}}} $) and reaction energy ($ \Delta E $) for an elementary step were defined as:
$ {E}_{{\mathrm{b}}}={E}_{{\mathrm{TS}}}-{E}_{{\mathrm{IS}}} $
$ \Delta E={E}_{{\mathrm{IM}}}-{E}_{{\mathrm{IS}}} $
where $ {E}_{{\mathrm{IM}}} $, $ {E}_{{\mathrm{TS}}} $ and $ {E}_{{\mathrm{IS}}} $ represent the energies of the intermediate state, transition state, and initial state along the reaction pathway, respectively.
The temperature-dependent Gibbs free energy change for a reaction step was obtained via:
$ G\left(T\right)=E+{\mathrm{ZPE}}+\Delta {G}_{0\rightarrow T} $
where G(T) represents the Gibbs free energy at a given temperature T; E represents the reaction energy associated with reactant and product molecules adsorbed on the catalyst surface at each step of the reaction; ZPE represents the zero-point energy (ZPE) correction; and $ \Delta {G}_{0\rightarrow T} $ represents the internal Gibbs free energy difference (ΔG) at T = 298.15 K.
2　Results and discussion
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2.1　Effects of single-atom Ag or Cu loading on the adsorption of C2H4 and O2
In this study, structural optimization was performed on MgO with space group Fm$ \overline{\text{3}} $m(225). The calculated lattice constants are presented in Table 1. The calculated structural parameters are in good agreement with the experimental data in Tang et al.[37], and also consistent with first-principles DFT results in Filot et al.[38−39]. The MgO(100) surface exhibited the lowest surface energy (1.30 J/m2), which aligns well with both experimental values[40−41] and theoretical calculations[42]. Consequently, a 3×3 MgO(100) surface model was selected all for subsequent computations (Figure 1(a) and 1(b)). The lattice constant was calculated using the following equation:
$ \sigma =\frac{1}{A}\left(\frac{1}{2}\left({E}_{{\mathrm{surf}}}-{N}_{{\mathrm{atoms}}}\cdot {E}_{{\mathrm{bulk}}}\right)+{E}_{{\mathrm{surf}}}{}^{{\mathrm{rel}}}\right) $
where $ {E}_{{\mathrm{surf}}} $ represents the energy of the unrelaxed surface (eV); $ {N}_{{\mathrm{atoms}}} $ represents the total number of atoms in the slab model; $ A $ represents the surface area of the slab (Å2); $ {E}_{{\mathrm{bulk}}} $ represents the energy per atom in the bulk model $ {N}_{{\mathrm{atoms}}} $(eV); and $ {E}_{{\mathrm{surf}}}{}^{{\mathrm{rel}}} $ represents the quantity after surface relaxation. A lower surface energy value indicates greater structural stability of the surface.
Loading transition metals can significantly alter the activity, selectivity, and stability of MgO-based catalysts. In this study, Ag and Cu were introduced by substituting a central Mg atom in the surface layer, with the optimized structures shown in Figure 1(c) and 1(d). The binding energies corresponding to Ag-loaded and Cu-loaded configurations were calculated using Eqs (2) and (3), with structural optimizations in Figure 1(a) and 1(b). Four adsorption sites were considered for each metal: the central substitution site (X site), the nearest neighboring Mg site, the nearest O site, and the bridge site between metal and O atoms. For both Ag-MgO and Cu-MgO structures, the calculated binding energies were all negative, indicating that the single-atom loading of Ag or Cu leads to thermodynamically stable catalyst structures. Among these sites, the one yielding the most negative adsorption energy for C2H4 and O2 was identified as the preferred site. In all cases, both C2H4 and O2 molecules tend to adsorb directly above the loaded metal atoms. The corresponding adsorption energies are summarized in Tables 2 and 3.
For the Ag-loaded MgO(100) model, the adsorption energies at the X site and bridge site were relatively large, with a maximum adsorption energy of −1.46 eV at the bridge site. Compared to the Mg and O sites, C2H4 molecules preferentially adsorb near the Ag atom. In contrast, O2 adsorption on Ag-MgO was much weaker (max −0.45 eV). For Cu-MgO, the bridge site also exhibited the strongest adsorption for C2H4, with a maximum adsorption energy of −0.87 eV. However, this adsorption strength was still weaker than the Ag-MgO system. For O2 adsorption on Cu-MgO, the bridge site again showed the highest affinity, with a maximum adsorption energy of −0.76 eV. These results suggest that Ag loading significantly enhances C2H4 adsorption but has a limited effect on O2, whereas Cu loading moderately improves C2H4 adsorption and substantially promotes O2 adsorption. This complementary behavior suggests that co-loading Ag and Cu could synergistically enhance the adsorption of both C2H4 and O2.
2.2　Effect of dual-atom Ag and Cu loading on adsorption of C2H4 and O2
Co-loading Ag and Cu atoms onto the MgO(100) surface creates dual-atom catalyst (DAC) configurations, where mutual metal-metal interactions must be considered. In this study, 17 AgCu-MgO configurations were constructed (Figure 2). In one set, one of the metal atoms (Ag or Cu) was fixed at an Mg site while the other was placed at a neighboring O site based on spatial proximity. By exchanging the positions of Ag and Cu between the Mg and O sites, 10 configurations were obtained. In another set, by placing both metal atoms at two Mg sites and varying their relative positions, 7 more configurations were generated. All DAC structures were geometrically optimized, and their binding energies were calculated using Eq. (1). The results (Table 4) show that the binding energies of 17 configurations are all negative, confirming their thermodynamic stability.
When both Ag and Cu occupy Mg sites, their binding energies are markedly more negative than those with metals on separate Mg and O sites. This indicates that AgCu-MgO structures with dual-metal atoms anchored at adjacent Mg sites are more thermodynamically stable. Given that Ag exhibited a stronger affinity for C2H4 and Cu showed better adsorption of O2, C2H4 preferentially adsorbed near Ag sites, while O2 favored Cu sites. Structural optimizations were carried out for all configurations, and the corresponding adsorption energies are shown in Figure 3. Compared to the single-atom-loaded MgO structures, most AgCu-MgO DAC configurations exhibited stronger adsorption capacity for both C2H4 and O2. Among them, Configurations 1 and 6 (both with dual Mg-site metals) showed the strongest adsorption for C2H4, with adsorption energies of −1.47 and −1.45 eV, respectively. For O2, Configuration 3, a single-Mg-site structure with Cu located at an O site, exhibited the highest adsorption energy of −1.27 eV. These results suggest that placing Cu at an O site significantly enhances O2 adsorption, while the location of Ag (whether at Mg or O site) has a less pronounced effect on C2H4 adsorption. To further investigate the effect of atomic positions on catalytic performance, detailed reaction pathway analyses are required. Based on the highest C2H4 adsorption energies in the dual-Mg-site configurations (Configurations 1 and 6) and the strongest O2 adsorption in the single-Mg-site configuration (Configuration 3), these three configurations—all featuring a short Ag-Cu atomic distance—were selected for subsequent mechanistic studies C2H4 oxidation.
2.3　Oxidation pathway analysis of selected AgCu-MgO configurations toward C2H4
The oxidation pathways of C2H4 on Configurations 1, 3 and 6 were analyzed in detail. Due to its high molecular symmetry, the four hydrogen atoms in C2H4 molecule are equivalent in both spatial configuration and chemical reactivity. As a result, each hydrogen exhibits similar behavior in dehydrogenation reactions, limiting C2H4 to only two reactive sites for initial oxidation. Following the abstraction of one hydrogen atom, C2H4 forms a highly reactive vinyl radical (C2H3·), which undergoes a barrierless addition reaction with O2 to form a peroxy radical intermediate (C2H3O2·). This addition step is considered as a key intermediate process in the catalytic oxidation of C2H4[5]. Additionally, O2 can directly add across the C=C double bond. Electrostatic potential (ESP) analysis indicates that this site exhibits strong electrophilic character, facilitating the formation of a dioxetane-like intermediate (C2H4O2). Both reaction sites were considered in this study. For each of the three selected configurations, three possible oxidation pathways were proposed based on these initial activation modes, resulting in a total of nine reaction pathways. Figure 4 presents the top and side views of the molecular structures for key states in these pathways.
Pathway 1 for Configurations 1, 3 and 6 is depicted in the Gibbs free energy diagram in Figure 5. In Configuration 1, C2H4 first adsorbs near the Ag atom, forming the intermediate CS3. Subsequently, O2 adsorbs on the Mg region of the surface, initiating a Langmuir-Hinshelwood (L-H) type oxidation. In this pathway, co-adsorbed O2 reacts with the adsorbed C2H4 to form the C2H3O2 intermediate. This intermediate then undergoes lateral rotation, with one O atom bonding to the Cu site near the vinyl group and the other to the Ag site, resulting in the formation of CS4. The ΔG for the CS3 + O2 → CS4 step in Configuration 1 is relatively small, only 0.09 eV. For Configuration 6, the ΔG for the same step is 0.26 eV, while in Configuration 3, the CS3 → CS4 transition exhibits a negative ΔG of −0.61 eV. This enhanced thermodynamic favorability in Configuration 3 is attributed to the positioning of Cu at an O site, which enhances electron donation and strengthens O2 adsorption.
For all three configurations (1, 3 and 6), the transformation of CS4 to CS5 is exothermic. This step involves the formation of a three-membered ring peroxide intermediate (CS5). The energy release is substantial for Configurations 1 (ΔG = –3.52 eV) and 3 (ΔG = –3.73 eV), but minimal for Configuration 6 (ΔG = –0.05 eV).
In Configuration 1, the CS5 → CS6 transformation is the rate-determining step for Pathway 1, with a high energy barrier of 4.33 eV. In contrast, for Configuration 6, this step has a lower barrier, making the later CS6 → CS7 step (ΔG = 0.94 eV) rate-limiting. This latter step involves the cleavage of the C=C bond in C2H4, yielding *HCO and CH2O intermediates.
Figure 6 depicts the Gibbs free energy profile for Pathway 2 of C2H4 oxidation on Configurations 1, 3 and 6. For Configuration 1, the CS5 → CS8 step is the rate-determining step, with a ΔG of 2.17 eV, which is significantly lower than the 3.52 eV barrier observed for the CS5 → CS6 step in Pathway 1. This suggests that Configuration 1 more readily proceeds through Pathway 2 to form *HCO and CH2O intermediates. For Configuration 3, both the CS5 → CS8 and CS8 → CS9 steps present high barriers (2.20 and 3.49 eV, respectively), rendering Pathway 2 less likely. For Configuration 6, the rate-determining step for Pathway 2 is CS8 → CS9, which exhibits a ΔG of 2.96 eV—significantly higher than the 0.94 eV barrier of the CS6 → CS7 step in Pathway 1. Therefore, for Configuration 6, Pathway 1 is the preferred route.
Figure 7 illustrates Pathway 3 for the formation of *CH3 and CO2 from C2H4 on Configurations 1, 3 and 6. In this pathway, the key intermediate CS5 undergoes O–O bond cleavage followed by oxygen migration, ultimately breaking the C=C bond, resulting in the formation of *CH3 and CO2. For Configurations 1 and 3, the CS5 → CS10 step is rate-determining, with ΔG values of 2.08 and 2.21 eV, respectively. For Configuration 6, the rate-limiting step occurs earlier (CS3 → CS4) with a much lower ΔG of 0.32 eV.
These results suggest that the AgCu-MgO catalyst facilitates *CH3 formation during C2H4 oxidation, with Configuration 6 demonstrating the most favorable catalytic performance among the three. The *CH3 radical is relatively stable, and further cleavage of its C–H bond requires a considerably higher activation energy. In this study, the Ag-Cu dual sites are highly effective in activating O2 and initiating its reaction with C2H4. However, the reactivity and quantity of surface O species (e.g., O or OH) generated under these conditions may be insufficient for the efficient low-temperature cleavage of the stronger C–H bonds in *CH3.
3　Conclusions
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To investigate the influence of Ag and Cu loading on the C2H4 oxidation performance of MgO-based catalysts, this study performed a systematic DFT investigation of MgO, Ag-MgO, Cu-MgO and 17 different DAC configurations with Ag and Cu co-loaded at various sites on MgO(100) surface. The reaction mechanisms of C2H4 oxidation over the selected AgCu-MgO configurations were explored through DFT calculations. The main conclusions are summarized as follows:
Loading Ag onto the MgO(100) surface significantly enhances C2H4 adsorption, resulting in a maximum adsorption energy of −1.46 eV. However, its capacity for O2 adsorption is considerably weak (−0.45 eV). Conversely, Cu-loaded MgO exhibits a moderate affinity for C2H4 (−0.87 eV at the bridge site) but a higher adsorption energy for O2 (−0.76 eV), outperforming Ag-MgO system in O2 adsorption.
Among the 17 modeled AgCu-MgO DAC configurations, structures where both Ag and Cu atoms are co-adsorbed at Mg sites are thermodynamically more stable (binding energies below −10 eV) than those with the metals at Mg and O sites. In particular, DAC configurations with Ag and Cu atoms in close proximity generally exhibit enhanced co-adsorption capabilities for both C2H4 and O2. Notably, positioning Cu at an O site significantly increases O2 adsorption energy.
On the AgCu-MgO surface, C2H4 oxidation preferentially proceeds through C=C bond cleavage, leading to the formation of *CH3 and CO2. For all three selected configurations (1, 3, and 6), the free energy barriers associated with the rate-limiting steps in the *HCO and CH2O formation pathway are consistently higher than those for the *CH3 and CO2 pathway. Among them, Configuration 6 exhibits the lowest energy barrier (0.32 eV) for its rate-limiting step in Pathway 3, indicating it as the most promoting structure for catalyzing C2H4 oxidation toward *CH3 and CO2 formation.
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Year 2026 volume 54 Issue 4
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doi: 10.1016/S1872-5813(26)60640-8
  • Receive Date：2025-09-19
  • Online Date：2026-09-23
  • Published：2026-04-10
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  • Received：2025-09-19
  • Revised：2025-10-29
  • Accepted：2025-11-20
Affiliations
    Yunnan Provincial Key Laboratory of Internal Combustion Engines, Kunming University of Science and Technology, Kunming 650500, China

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表12种不同金属材料的力学参数
科
Family		 属数
Number of
genus		 种数
Number of
species		 占总种数比例
Percentage of
total species (%)		 属
Genus		 种数
Number of
species		 占总种数比例
Percentage of total
species (%)
鹅膏菌科Amanitaceae 2 11 5.26 鹅膏菌属 Amanita 10 4.78
小菇科 Mycenaceae 2 12 5.74 丝盖伞属 Inocybe 5 2.39
多孔菌科 Polyporaceae 8 14 6.70 蜡蘑属 Laccaria 5 2.39
红菇科 Russulaceae 3 23 11.00 小皮伞属 Marasmius 6 2.87
小菇属 Mycena 11 5.26
光柄菇属 Pluteus 5 2.39
红菇属 Russula 17 8.13
栓菌属 Trametes 5 2.39
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