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Article

Study on Explosion Mechanism of Dimethyl Ether/H2-Blended Gas Based on Chemical Kinetics Method

by
Yong Zhou
1,
Yang Kong
2,3,*,
Qi Zhang
2,3,4,
Qi Huang
2,3,
Zhikai Wei
2,3 and
Huaheng Lu
2,3
1
National Energy Group Wuhai Energy Co., Ltd., Wuhai 016000, China
2
College of Safety and Environmental Engineering, Shandong University of Science and Technology, Qingdao 266590, China
3
State Key Laboratory of Mining Disaster Prevention and Control Co-Founded by Shandong Province and the Ministry of Science and Technology, Shandong University of Science and Technology, Qingdao 266590, China
4
State Key Laboratory of Explosion Science and Technology, Beijing Institute of Technology, Beijing 100081, China
*
Author to whom correspondence should be addressed.
Fire 2024, 7(9), 328; https://doi.org/10.3390/fire7090328
Submission received: 1 August 2024 / Revised: 27 August 2024 / Accepted: 5 September 2024 / Published: 20 September 2024
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Abstract

:
In order to reveal the deflagration mechanism of DME/H2-blended gasses, the micro-mechanism was studied based on the constructed UC San Diego 2016 pyrolysis oxidation mechanism model. The results show that adiabatic flame temperature and laminar flame speed increase with the increase in the equivalence ratio (Φ); they first increase and then decrease with the increase in the hydrogen (H2)-blended ratio (λ), and with the increase in λ, the Φ corresponding to the peak laminar flame speed of the blended gas increases. The addition of H2 increases the consumption of O2, and H2 reacts with CO to form H2O and CO2, promoting complete combustion. When Φ = 1.0–1.2, the equilibrium mole fraction of H and OH-activated radicals reach the maximum, and with the addition of H2, the concentration of activating radicals gradually increases, while the number of promoted elementary reactions increases by two, and the number of inhibited elementary reactions does not increase. Meanwhile, the addition of H2 increases the reaction rate of most reactions on the main chemical reaction path CH3OCH3→CH3OCH2→CH2O→HCO→CO→CO2 of DME and increases the risk of the deflagration of DME/H2-blended gas.

1. Introduction

Since the 21st century, the coordinated development of economy, energy, and environment has become the key to social sustainable development, and the development of economy, science, and technology is closely related to the degree of development and utilization of energy [1,2]. However, with the depletion of fossil fuels and the worsening of environmental pollution, countries around the world have successively put forward the concept of “carbon neutrality” and set goals in stages. For example, in September 2020, China proposed a “dual-carbon” strategic goal entitled “2030 carbon peak and 2060 carbon neutral” [3]. Due to the energy shortage and improving emission regulations, people have been conducting more and more extensive and in-depth research on fuels. Dimethyl ether (DME), as the simplest aliphatic ether, can be made from natural gas, coal, petroleum coke, or biomass as raw materials. DME is considered to be one of the cleanest fuels with the most potential for development because it does not contain a C-C bond, has high oxygen content and cetane number, good combustion performance, a short stagnation period, low NOx emissions, low combustion noise, a higher latent heat of vaporization compared to diesel fuel, and it is a kind of renewable and clean energy [4,5,6]. In addition, DME has high energy density, easy liquefaction, transportation, and storage, and can produce hydrogen (H2) in the reforming reaction, so it can be used as a good safe carrier of hydrogen energy. The direct transportation of hydrogen has a very low utilization rate of hydrogen energy [7], so the Oberon Fuel Company, one of the largest fuel companies in the United States, designed and developed a hydrogenation station based on DME reforming to produce hydrogen [8].
Expanding and popularizing the scale of the hydrogen production process using DME has made it possible to use DME/H2-blended gas as a mixed fuel [9]. Meanwhile, because of the wide ignition limit and fast combustion rate of H2, adding H2 to gaseous fuels can increase the combustion rate of the mixed fuel and enhance the risk of deflagration [10,11,12]. Therefore, the study of the micro-deflagration mechanism of DME/H2-blended gas is of great significance to its safe application.
At present, some scholars have carried out detailed studies on the deflagration characteristics of DME or H2 single gas, but research on DME/H2-blended gas is still insufficient. Youn et al. [13] studied the effect of DME fuel on the performance of a four-cylinder diesel engine and found that the peak combustion pressure and ignition delay of DME fuel were higher and faster than that of ultra-low sulfur diesel, respectively. Ying et al. [14] carried out experimental studies on the combustion and emissions of a DME compression ignition engine. With the increase in the equivalence ratio (Φ), the peak values of pressure and temperature in the engine increased; NOx emissions decreased at first and then remained unchanged, while CO and HC emissions increased. Huang et al. [15] used high-speed ripple photography to measure the laminar flame speed of DME/air mixtures at different initial pressures and Φ. The results showed that the Markstein number decreased with increasing Φ. Wang et al. [16] conducted experimental and simulation studies on the propagation and extinguishing of DME/air-premixed flames and found that the high-temperature reaction of DME was mainly determined by intermediate products, and the effect of reaction kinetics on flame extinguishing was greater than that on flame propagation. Moradi et al. [17] studied the effect of H2 on the combustion characteristics of a natural gas HCCI engine and found that H2 improved engine efficiency, accelerated natural gas combustion, and reduced the ignition delay time and HC and CO emissions. Li et al. [18] studied the combustion characteristics of NH3/DME/H2 using the spherical iso-volume combustion method and optimized the simplified kinetic mechanism, finding that H2 can effectively improve the laminar combustion rate of the NH3/DME/air mixture and that the laminar flame speed shows a non-monotonous increasing trend with Φ at different H2 additions. Cong et al. [19] studied the combustion and emission characteristics of DME/H2 and found that the addition of DME increased the engine power output while significantly reducing NOx emissions, but CO and HC emissions increased. Pan et al. [20] studied the variation in the ignition delay time of DME/H2 mixtures with Φ and the hydrogen-blended ratio (λ) using a combination of experiments and numerical simulations and found that the ignition delay time increased with Φ and gradually decreased and then rapidly decreased with λ. Shi et al. [21] analyzed a dilute DME/H2 mixture with Φ = 0.3~0.5 and a hydrogen mole fraction of 0~85% based on the pyrolysis oxidation mechanism model of NUI Aramco Mech 2.0 and found that when the mole fraction of H2 was more than 70% and the pressure was low, while the effect of H2 on the ignition delay was clearer, and there were three stages of exothermic behavior under the condition of extremely lean combustion (Φ = 0.3).
Up until now, scholars at home and abroad have extensively studied the chain reaction mechanism of pure DME and pure H2; however, there are relatively few studies on the pyrolysis and chemical kinetic parameters of DME/H2-blended gas in the air. It is very important to reveal the risk of deflagration of DME/H2-blended gas under different Φ and λ conditions from the microscopic mechanism. In this paper, a model of the pyrolysis oxidation mechanism of DME/H2-blended gas was constructed by conducting research in the literature, and this model was validated based on the ignition delay time to determine the optimal pyrolysis oxidation mechanism model. Based on the mechanism model, adiabatic flame temperature, equilibrium molar concentration, laminar flame speed, the chemical reaction path, and related elementary reaction sensitivities were analyzed successively, and the intrinsic effects of Φ and λ on the deflagration characteristics of DME/H2-blended gas were revealed from the mechanism.

2. Research Methods and Pyrolysis Oxidation Mechanism Model

2.1. Research Methods

Based on the chemical reaction kinetic mechanism model of DME/H2-blended gas deflagration, it was assumed that 79% nitrogen and 21% oxygen would be present in the air. An equilibrium closed homogeneous 0-D reactor and premixed laminar flame-speed calculation model were adopted. The adiabatic flame temperature, laminar flame speed, equilibrium analysis, chemical reaction path, and related elementary reactions of DME/H2-blended gas with different Φ and λ at the initial temperature of 298 K and initial pressure of 1 atm were analyzed. We selected Φ = 0.6, 0.8, 1.0, 1.2, 1.4, 1.6, 1.8, 2.0, λ = 0%, 10%, 30%, 50%, 70%, 90%, 100%.
Φ is defined as the ratio of theoretical air consumption (V0) to the actual air consumption (VS) when burning 1 kg of fuel, i.e.,
Φ = V 0 V S
λ = V H 2 V H 2 + V DME

2.2. Modeling and Validation of Pyrolytic Oxidation Mechanism

In this paper, based on the UC San Diego DME model constructed by the UC San Diego 14-step DME chemical kinetic reaction model and the GRI-Mech 3.0 mechanism (containing 53 substances and 325 elementary reactions) [22], the UC San Diego 2016 model containing the H2 oxidation reaction mechanism from UC San Diego is embedded [23]; thus, the DME/H2-blended gas chain reaction mechanism model was obtained. Here, the reaction mechanism model of DME/H2-blended gas is called the UC San Diego 2016 model. Through an experimental study on parameters such as the ignition delay time, explosion overpressure, and explosion temperature, many scholars at home and abroad have verified the accuracy of the UC San Diego 2016 model to predict the chemical kinetic properties of common C1-C4 substances under specific conditions. However, there are few reports on the accuracy of the UC San Diego 2016 model in predicting the chemical kinetic characteristics of DME/H2-blended gas. Therefore, it is compared with the AramcoMech 2.0 model of the National University of Galway, Ireland, which was constructed by Galway University Center for Combustion Chemistry in combination with the H2 gas mixture pyrolysis oxidation mechanism of A. Kéromnès, Y. Zhang, and M. Ó Conaire et al [24,25].
Ignition delay time is one of the most fundamental, important, and sensitive parameters of chemical kinetics [26,27,28,29]. Pan et al. [20] revealed the ignition delay time of DME/H2-blended gas with Φ = 0.5 and an initial pressure of 1.2 atm by shock tube experiments, so the results of this experiment can be used to validate the combustion model in this paper. As shown in Figure 1, detailed comparisons of experimental and simulated values of the ignition delay time for DME/H2-doped gas under different λ conditions at Φ = 0.5 and an initial pressure of 1.2 atm are demonstrated so as to verify the accuracy of the UC San Diego 2016 model. Here, the blue solid line, green solid line, and red sphere represent the numerical results of the UC San Diego 2016 model, the AramcoMech2.0 model, and the experimental results of Pan et al. [20] in the State Key Laboratory of Power Engineering of Xi’an Jiaotong University, respectively.
As can be seen from Figure 1, when the UC San Diego 2016 model and AramcoMech2.0 model are used to simulate the ignition process of DME single fuel and DME/H2-blended gas, the calculation results of the AramcoMech2.0 model are slightly larger than that of the UC San Diego 2016 model, and the calculation result of the UC San Diego 2016 model is closer to the experimental results of the State Key Laboratory of Power Engineering Multiphase flow of Xi’an Jiaotong University. The UC San Diego 2016 model shows a better ability to predict the ignition delay with higher accuracy. Therefore, in this paper, the UC San Diego 2016 model was selected as a model to study the reaction mechanism of DME/H2-blended gas.

3. Results and Discussion

3.1. Adiabatic Flame Temperature

The adiabatic flame temperature not only reflects the exothermic performance of the blended gas but also has an important influence on flame propagation and extinguishment, the ignition limit, and the formation of combustion pollutants [30,31]. Meanwhile, the adiabatic flame temperature can also reflect the laminar flame speed to a certain extent in order to help select appropriate materials and design appropriate protective measures. The adiabatic flame temperature of DME/H2-blended gas under the action of different Φ and λ at normal pressure and temperature is shown in Figure 2.
From Figure 2, it can be seen that the adiabatic flame temperature first increases and then decreases with the increase in Φ at different λ and reaches a maximum value between Φ = 1.0 and 1.1, and the maximum value ranges from 2338 to 2436 K. At the same time, because the calorific value of DME is smaller than H2, and there are C-O and C-C bonds in the molecular structure of CH3OCH3 with a high bond energy, which requires larger energy to break it, the combustion reaction of H2 is relatively simple and involves only the chemical reaction of hydrogen itself. Therefore, the adiabatic flame temperature increases with the increase in λ under the same conditions.
The effect degree of H2 on blended gas at a lean burn concentration is much less than that of blended gas with a rich burn concentration. When Φ = 0.6–2.0, with the increase in λ, the growth rate of the adiabatic flame temperature is 5.36%, 4.35%, 4.17%, 6.10%, 8.69%, 11.33%, 14.07%, and 17.01%, respectively. The growth rate of adiabatic flame temperature first decreases and then increases with the increase in Φ, reaching a minimum value at Φ = 1.0.

3.2. Laminar Flame Speed

The laminar flame speed is the velocity of a one-dimensional adiabatic plane flame surface relative to incoming unburned premixed gas. The laminar flame speed is one of the most important parameters that reflect the combustion characteristics of the fuel. The trend in laminar flame speed of DME/H2-blended gas with Φ and λ is shown in Figure 3.
The laminar flame speed of the doped gas increases with larger λ, which means that increasing λ can increase the laminar flame speed of DME/H2-doped gas. Meanwhile, with the increase in λ, the peak laminar flame speed of the blended gas corresponds to the increase in Φ, which means that the peak laminar flame speed moves to the rich combustion condition with the addition of H2. When λ = 100%, the laminar flame speed of blended gas increases with the increase in Φ, and when λ < 100%, the laminar flame speed increases at first and then decreases with the increase in Φ. When λ ≤ 0.3, the laminar flame speed and evolution trend under all values of λ are almost the same. When the laminar flame speed increases with the increase in Φ and the same Φ variation, the greater the λ, and the greater the increase in laminar flame speed.

3.3. Equilibrium Molar Concentration

The risk of deflagration can be inferred by studying the equilibrium molar concentrations of reactants, which are key free radicals of the intermediate products and main products [32,33,34]. Figure 4 shows the equilibrium molar fraction waterfall diagram of the reactant O2 at different Φ and λ.
It can be seen from Figure 4 that when λ is the same, the equilibrium mole fraction of O2 decreases rapidly with the increase in Φ. When Φ = 1, there is still partial O2 in the reaction system, which is due to the reverse reaction, which leads to the re-conversion of the product into reactants, resulting in the existence of partial O2 in the reaction system after the end of the reaction. The value of Φ > 1 is present in the oxygen-lean condition, in which the sufficient blended gas results in almost the complete combustion of O2, and the equilibrium mole fraction is close to zero.
When Φ is the same, the equilibrium mole fraction of O2 decreases slightly with the increase in λ, which means that the addition of H2 increases the consumption of O2, promotes the forward reaction of the reaction system, and increases the risk of deflagration of DME/H2-blended gas. At the same time, when burning the same mole of gas, the oxygen consumption of H2 is much less than that of DME. Combined with Figure 2, the addition of H2 leads to a continuous increase in adiabatic flame temperature. It also shows that H2 has a “brightening effect”, which can drive the less combustible components of DME gas to burn further and consume more oxides.
H radicals can react with O2, H2, and other gasses to release a large amount of heat energy. OH radicals have a stronger oxidation ability in the reaction, and they can accelerate the reaction rate through the chain reaction, thus making the reaction more intense. Figure 5 shows the equilibrium molar fraction waterfall diagram of H and OH radicals at different Φ and λ.
It can be seen from Figure 5 that both H and OH radicals increase gradually with the increase in λ, while the OH radicals rise significantly more than H radicals with the increase in Φ; however, they all increase at first and then decrease with the increase in Φ, reaching the maximum at Φ = 1.2 and Φ = 1.0, respectively. Therefore, the overall risk of the reaction system increases with the increase in λ, and when Φ = 1.0–1.2, the concentration of key radicals of H and OH is the highest, and the risk is the highest. Clearly, H2 greatly increases the concentration of activated radicals in the reaction system and promotes a positive reaction.
In the whole reaction system, complete combustion and incomplete combustion often exist at the same time due to the change in reaction conditions and reactant characteristics. Figure 6 shows the equilibrium mole fraction waterfall diagram of the complete combustion products CO2 and H2O and the incomplete combustion products CO and H2 under different λ and Φ.
It can be seen from Figure 6 that the equilibrium concentration of CO2 and H2O increases at first and then decreases with the increase in Φ and peaks near Φ = 1, when the proportion of complete reaction is the largest. With the increase in Φ, the equilibrium concentration of CO and H2 approaches 0 at first and then increases rapidly, and incomplete combustion is especially obvious under oxygen-lean conditions.
With the increase in λ, the equilibrium mole fraction of H2O increases, while the equilibrium mole fraction of CO2 decreases. It is clear that the continuous addition of H2 reduces the emissions of CO2 while promoting complete combustion. When Φ > 1.0, the equilibrium concentration of CO decreases with the increase in λ. On the one hand, the increase in H2 leads to the decrease in DME supply in the reaction system, which leads to a decrease in the reaction product CO; on the other hand, it is due to the catalytic effect of H2 on CO, so that H2 reacts with CO to produce H2O and CO2, releasing a large amount of heat, which results in the content of CO, which then decreases gradually.

3.4. Sensitivity Analysis of Elementary Reactions

In order to understand the reaction process, the temperature sensitivity of DME/H2-blended gasses was analyzed from the point of view of the main elementary reactions [35,36]. Figure 7 shows the temperature sensitivity coefficient distribution of different H2 blending degrees (λ = 0%, 50%, 70%, 100%) at Φ = 1, including initial temperature at 298 K and initial pressure at 1 atm. Here, the positive value means promoting the reaction process, while the negative value means inhibiting the reaction process. The greater the absolute value of the sensitivity coefficient, the stronger the corresponding promotion or inhibition ability.
As can be seen from Figure 7, among the 16 highly sensitive radical reactions, the main reactions that promote the deflagration of DME/H2-blended gas are as follows:
CH3OCH3(+M) <=> CH3O + CH3(+M)
CH3 + O2 <=> CH2O + O
H + O2 <=> OH + O
The two elementary reactions of R52 and R1 consumed O2 and produced highly active OH free radicals, which increased the concentration of active free radicals and promoted the positive chemical reaction. Among the 16 highly sensitive radical reactions, those that had an inhibitory role on the DME/H2-blended gas reaction acted as follows:
2CH3(+M) <=> C2H6(+M)
CH3OCH3 + H <=> CH3OCH2 + H2
The reaction consumes highly active H and CH3 radicals, produces relatively stable ethane and H2, reduces the concentration of the activation center, and inhibits the positive process of the reaction system. At the same time, the incorporation of H2 brings about two new and highly sensitive elementary reactions that promote the forward reaction process of DME/H2-blended gas, as follows:
CH4 + H <=> H2 + CH3
H2 + OH <=> H2O + H
When H2 is incorporated, the number of elementary reactions that promote the positive reaction increases by two, but the number of elementary reactions that inhibit the positive reaction does not increase, and the R1, R41, R52, R275, and R276 elementary reactions are dominant. When λ = 0% and 100%, the temperature sensitivity of the R1 elementary reaction is low, but when DME and H2 exist at the same time, the temperature sensitivity increases greatly, which leads to a significant increase in the active free radical OH and the reaction rate of the system. Meanwhile, it can be seen from Figure 7 that the temperature sensitivity of the promoted and inhibited elementary reactions increase with the incorporation of H2, and the absolute value of the number of promoting reactions and the absolute value of the temperature sensitivity coefficient is always larger than that of inhibitory reactions as a whole, which shows that the addition of H2 can promote the chemical reaction of blended gas.

3.5. Chemical Reaction Path

In order to elaborate the cause and process of deflagration and to reveal the key steps in the chain reaction [37], the main pathways of the DME/H2-blended gas deflagration reaction and the main radicals, such as H, OH, O, and CH3, in each branch of the reaction were analyzed at Φ = 1.0, λ = 10%, 30%, 50%, and 70% with the initial temperature at 298 K and the initial pressure at 1 atm. The main reaction path and the radicals of the products or reactants in each branch reaction are shown in Figure 8.
From Figure 8, the main chemical reaction path of DME is CH3OCH3→CH3OCH2→CH2O→HCO→CO→CO2. For DME, about 100% of CH3OCH3 undergoes dehydrogenation to form dimethyl carbonate (CH3OCH2), and H and OH are highly active radicals that play a major role in this process, in which CH3OCH3 reacts with OH to form H2O.CH3OCH2 completely through the cracking reaction to produce CH3 and the relatively stable intermediate product formaldehyde (CH2O). CH2O reacts with various radicals, such as OH and H, to produce an important intermediate product aldehyde group (HCO), and most HCO is produced by reacting with H, OH, O2, and CH3 to produce CO, which finally forms CO2 via an oxidation reaction.
With the increase in λ, the main reaction path of CH3OCH3 did not change in any obvious way; only the consumption proportion of radicals changed slightly. With the increase in λ, the dehydrogenation of CH3OCH3 increased from 98.9% to 99.9%, in which the H radical, which participated in the reaction, increased from 60.4% to 66.8%, CH3 continued to decrease, and the proportion of OH radicals in the main reaction pathway continued to increase. The addition of H2 increased the reaction rate of most reactions in the DME reaction process, which promoted the combustion of DME.

4. Conclusions

The adiabatic flame temperature increases with the increase in λ; it first increases and then decreases with an increase in Φ and reaches the maximum value between Φ = 1.0 and 1.1, and the maximum value ranges from 2338 to 2436 K. Meanwhile, the larger the λ, the greater the laminar flame speed of the blended gas, and with the increase in λ, the Φ corresponding to the peak laminar flame speed of the blended gas increases.
When Φ = 1.0–1.2, the equilibrium mole fraction of H and OH-activated radicals is the highest, the activation degree of the reaction is the highest, and the risk is the greatest. The addition of H2 increases the consumption of O2 and promotes complete combustion with a decrease in CO, and H2 plays a catalytic role in CO, which makes H2 react with CO to form H2O and CO2, promotes the forward reaction and increases the risk of deflagration of DME/H2-blended gas.
The elementary reactions that play a promoting role in the deflagration of DME/H2-blended gas are mainly R1, R52, and R271, while R57 and R275 play an inhibitory role. After the addition of H2, the number of promoted elementary reactions increases by two, while the number of inhibited elementary reactions does not increase. Meanwhile, the sensitivity coefficient of promoting and inhibiting the elementary reaction of DME/H2-blended gas deflagration increases with the addition of H2, which also confirms that the addition of H2 increases the risk of deflagration of blended gas from the reaction mechanism.
The main chemical reaction path of DME is CH3OCH3→CH3OCH2→CH2O→HCO→CO→CO2. With the increase in λ, the main reaction path of CH3OCH3 does not clearly change; only the consumption proportion of radicals change slightly. With the increase in λ, the dehydrogenation of CH3OCH3 increases from 98.9% to 99.9%, in which the H radical, which participates in the reaction, increases from 60.4% to 66.8%, CH3 continues to decrease, and the proportion of OH radicals in the main reaction pathway continues to increase. The addition of H2 increases the reaction rate of most reactions in the DME reaction process and promotes the positive progress of DME, which promotes the positive process of DME and increases the risk of the reaction system.

Author Contributions

Y.Z.: Project administration, Methodology. Y.K.: Writing—Original draft, Data curation, Writing—Review and Editing. Q.Z.: Methodology, Funding acquisition. Q.H.: Investigation. Z.W.: Software, Data curation. H.L.: Data curation. All authors have read and agreed to the published version of the manuscript.

Funding

This work was financially supported by the Opening Project of State Key Laboratory of Explosion Science and Technology, Beijing Institute of Technology (Grant no. KFJJ23-23M).

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

The original contributions presented in this study are included in the article, further inquiries can be directed to the corresponding author.

Conflicts of Interest

Author Yong Zhou was employed by the company National Energy Group Wuhai Energy Co., Ltd. The remaining authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

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Figure 1. Comparison of experimental and theoretical values of ignition delay time for DME/H2-blended gas at different λ.
Figure 1. Comparison of experimental and theoretical values of ignition delay time for DME/H2-blended gas at different λ.
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Figure 2. Adiabatic flame temperature evolution curves. (a). Adiabatic flame temperature evolution at different λ; (b). Adiabatic flame temperature evolution at different Φ.
Figure 2. Adiabatic flame temperature evolution curves. (a). Adiabatic flame temperature evolution at different λ; (b). Adiabatic flame temperature evolution at different Φ.
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Figure 3. Evolution relationship between laminar flame speed, Φ, and λ.
Figure 3. Evolution relationship between laminar flame speed, Φ, and λ.
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Figure 4. Equilibrium molar fraction of reactants of O2 for different Φ and λ.
Figure 4. Equilibrium molar fraction of reactants of O2 for different Φ and λ.
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Figure 5. Equilibrium molar fraction waterfall diagram of H and OH radicals for different Φ and λ.
Figure 5. Equilibrium molar fraction waterfall diagram of H and OH radicals for different Φ and λ.
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Figure 6. Equilibrium molar fraction waterfall diagram of the main products for different Φ and λ.
Figure 6. Equilibrium molar fraction waterfall diagram of the main products for different Φ and λ.
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Figure 7. Sensitivity of DME/H2-blended gas reaction system under different λ.
Figure 7. Sensitivity of DME/H2-blended gas reaction system under different λ.
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Figure 8. Schematic diagram of the DME reaction path.
Figure 8. Schematic diagram of the DME reaction path.
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MDPI and ACS Style

Zhou, Y.; Kong, Y.; Zhang, Q.; Huang, Q.; Wei, Z.; Lu, H. Study on Explosion Mechanism of Dimethyl Ether/H2-Blended Gas Based on Chemical Kinetics Method. Fire 2024, 7, 328. https://doi.org/10.3390/fire7090328

AMA Style

Zhou Y, Kong Y, Zhang Q, Huang Q, Wei Z, Lu H. Study on Explosion Mechanism of Dimethyl Ether/H2-Blended Gas Based on Chemical Kinetics Method. Fire. 2024; 7(9):328. https://doi.org/10.3390/fire7090328

Chicago/Turabian Style

Zhou, Yong, Yang Kong, Qi Zhang, Qi Huang, Zhikai Wei, and Huaheng Lu. 2024. "Study on Explosion Mechanism of Dimethyl Ether/H2-Blended Gas Based on Chemical Kinetics Method" Fire 7, no. 9: 328. https://doi.org/10.3390/fire7090328

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