Reactive Molecular Dynamics Study of Pollutant Formation Mechanism in Hydrogen/Ammonia/Methanol Ternary Carbon-Neutral Fuel Blend Combustion

Hydrogen, ammonia, and methanol are typical carbon-neutral fuels. Combustion characteristics and pollutant formation problems can be significantly improved by their blending. In this paper, reactive molecular dynamics were used to investigate the pollutant formation characteristics of hydrogen/ammonia/methanol blended fuel combustion and to analyze the mechanisms of CO, CO2, and NOX formation at different temperatures and blending ratios. It was found that heating can significantly increase blending and combustion efficiency, leading to more active oxidizing groups and thus inhibiting N2 production. Blended combustion pollutant formation was affected by coupling effects. NH3 depressed the rate of CO production when CH4O was greater than 30%, but the amount of CO and CO2 was mainly determined by CH4O. This is because CH4O provides more OH, H, and carbon atoms for CO and CO2 to collide efficiently. CH4O facilitates the combustion of NH3 by simplifying the reaction pathway, making it easier to form NOX.


Introduction
Currently, the global transportation industry relies mainly on fossil energy sources [1], but the combustion of these traditional fossil energy sources causes a lot of pollution.To fundamentally solve this problem, finding clean energy sources that can replace traditional energy sources has become one of the most important research topics [2,3].
H 2 and NH 3 are both ideal clean and renewable fuels that have received a lot of attention from scholars at home and abroad.H 2 can be produced renewably from green energy by electrolyzing water.In addition, it is characterized by good combustibility, low ignition energy, and fast combustion rates [4,5].However, difficulties in storage and transportation, its excessive combustion rate, and its high combustion temperature producing NO X pollution have limited the practical promotion of pure H 2 fuel use [6].NH 3 , as a good zero-carbon H 2 storage carrier, can be obtained from fossil fuels, biomass, or other renewable sources.This is why NH 3 has received a great deal of attention from the combustion community in recent years and is considered a sustainable fuel that can be remotely transported and applied [7].NH 3 is currently used as a fuel in a wide range of applications, such as vehicle engines [8], marine engines [9], and combustion engines for power generators [10].The low viscosity of NH 3 helps in fuel atomization and droplet formation during fuel injection [11].In addition, NH 3 has a high octane rating, which makes it suitable for engines with high compression ratios and reduced detonation [12].However, NH 3 has the disadvantages of a low combustion rate [13], high autoignition temperature [14], and narrow flammability limits, often leading to incomplete combustion.This contributes to poor engine performance, making it difficult to use as a single fuel for direct combustion [15,16].The use of H 2 as a combustion aid and NH 3 blending has been found to be one of the ways to improve the efficiency of NH 3 combustion [17].This not only leads to improved in-cylinder combustion [18] but also reduces the requirement for engine modifications (material compatibility), thus ensuring a cost-effective transition to H 2 [19].Wang et al. [20] found that engine exhaust heat can crack some of the NH 3 into H 2 and nitrogen to provide energy, making this method much more maneuverable.However, a study by Alam et al. [21] pointed out that although H 2 -NH 3 blending reduces carbon emissions, including CO, etc., in diesel internal combustion engines, incomplete fuel combustion and higher NO X were observed.
Blending oxygenated fuels as combustion aids is also an effective way to improve combustion performance and pollutant emissions in diesel engines [22].In a study of LPG-diesel-and CNG-diesel-fueled diesel engines using the high-cetane fuel diethyl ether, improved combustion was observed [23].Wang et al. [24] performed numerical simulations of ethanol and diesel blends on their combustion and emission characteristics.It was found that ethanol/diesel blends significantly reduced CO 2 and soot emissions compared to diesel.Soot and CO 2 emissions were reduced by 63.25% and 17.24% respectively at 100% load, but Nox was increased by 1.39%.Feng et al. [25] analyzed a methanol/diesel/nbutanol replacement blend.The results show that the thermal efficiency and the blending efficiency of diesel and alcohol fuel increase with an increase in the alcohol fuel blending ratio (0-15%), and irreversible loss also increases.Increasing the load on a diesel engine can improve its thermal efficiency.Wang et al. [26] investigated DGE as an oxygenated fuel and combustion enhancer to improve the combustion emissions of NH 3 and H 2 blends.It was found that when 60-70% of diesel fuel was replaced with DGE, H 2 , and NH 3 , CO 2 was reduced by 50% and synergistic effects were found between DGE and H 2 and NH 3 , reducing PM, NO X , HC, and CO emissions.
CH 4 O, as the saturated monohydric alcohol with the simplest structure, is inexpensive and simple to synthesize.It is a high-quality representative for the study of combustionenhancing effects on oxygenated fuels.Li et al. [27] found that blending a small amount of CH 4 O into NH 3 combustion made the blend more reactive, due to the enrichment of the O/H radical pool by the addition of CH 4 O. Species in this sequence can also react directly with NH 3 combustion-associated species, thereby consuming NH 3 and promoting spontaneous combustion.Xu et al. [28] simulated the combustion characteristics of NH 3 /CH 4 O blends and found that CH 4 O makes a significant contribution to the laminar combustion rate of NH 3 , and NO X emission analysis showed that the blending of 60% CH 4 O leads to the highest NO X emissions.Lu et al. [29] investigated the effect of CH 4 O doping on NH 3 combustion and emissions by modeling the chemical reaction mechanisms of an NH 3 /CH 4 O blend.The results showed that CH 4 O doping significantly increased the chemical reaction activity of NH 3 and significantly reduced the ignition delay time.
Because of the complexity of the engine in cylinder combustion and its pollutant formation characteristics, it is not favorable to explore the chemical reaction kinetics and blended fuel combustion pollutant laws under different operating parameters in isolation [30,31].In this paper, CH 4 O is used as a representative of oxygenated fuels.Reactive molecular dynamics are used to investigate the effect of CH 4 O on the combustion pollutant formation characteristics of H 2 and NH 3 combustion-reforming gases in diesel engines.This study analyzes the pollutant formation mechanisms of CO, CO 2 , and NO X formations at different temperatures and fuel ratios at the molecular level.This study is of great theoretical and practical significance to enhance the application of carbon-neutral fuels in engines and other practical combustion equipment.

Temperature Effects on Ternary Blended Combustion Components and Pollutant Formation
2.1.1.Temperature Effects on Ternary Blended Combustion Components and Free Radicals Figure 1 shows the effects of different temperatures on the four reactant components CH4O, NH3, H2, and O2 in the ternary blended combustion process.From the figure, it can be seen that heating significantly accelerated the decomposition rate of CH4O, NH3, H2, and O2.The insignificant rises for H2 and O2 at high temperatures may be caused by the decomposition of H2O due to the intensification of molecular collisions at high temperatures.Figure 2a,b shows the effects of different temperatures on the formation of H2O and N2 in the combustion process.From Figure 2a, it can be seen that the growth rate of H2O slows down significantly after a rapid increase to a certain level.Heating accelerates the rate of H2O formation during combustion.However, the effect of heating is not obvious when the temperature is further increased above 2000 K. Above 2500 K, H2O shows an insignificant decreasing trend, which may be due to the decomposition of H2O at high temperatures.This conclusion is consistent with the above conclusion that high temperatures lead to a slowly increasing trend for H2 and O2 at the late stage of the reaction.In Figure 2b, it is visible that the variation rule for N2 at different temperatures is not strictly temperature-dependent.The maximum amount of N2 generated by the reactants is at 1000 K. Above 2500 K and 1500 K, the amount of N2 generated increases with an increase in Figure 2a,b shows the effects of different temperatures on the formation of H 2 O and N 2 in the combustion process.From Figure 2a, it can be seen that the growth rate of H 2 O slows down significantly after a rapid increase to a certain level.Heating accelerates the rate of H 2 O formation during combustion.However, the effect of heating is not obvious when the temperature is further increased above 2000 K. Above 2500 K, H 2 O shows an insignificant decreasing trend, which may be due to the decomposition of H 2 O at high temperatures.This conclusion is consistent with the above conclusion that high temperatures lead to a slowly increasing trend for H 2 and O 2 at the late stage of the reaction.In Figure 2b, it is visible that the variation rule for N 2 at different temperatures is not strictly temperaturedependent.The maximum amount of N 2 generated by the reactants is at 1000 K. Above 2500 K and 1500 K, the amount of N 2 generated increases with an increase in temperature.However, in the case of 2000 K, the amount of N 2 is significantly lower than for other temperatures.This is because N from NH 3 generates more NO X at 2000 K.
temperature.However, in the case of 2000 K, the amount of N2 is significantly lower than for other temperatures.This is because N from NH3 generates more NOX at 2000 K. Figure 2c,d shows the effects of different temperatures on the formation of H and OH during blended combustion.It can be seen that the formation of H and OH is slow at low temperatures and the quantity is depleted as the reaction continues.High temperatures increase the amounts of H and OH.The difference is that H peaks rapidly and then decreases as the reaction proceeds, while OH peaks and then stabilizes as the reaction proceeds.The peak H at 3000 K is five times higher than that at 1500 K. Heating significantly increases the H and OH concentrations in the combustion reaction.

Temperature Effects on CO and CO2 Formation in Blended Combustion
Figure 3a,b shows CO and CO2 formation during the blended combustion process at different temperatures.Heating increases the rate of CO production, where CO is formed rapidly and then decreases slowly at temperatures of 2000 K and higher.At 1500 K and 1000 K, CO has still not peaked at the end of the reaction and is in a state of continuous growth.As the temperature increases the CO2 production rate increases, and the peak state remains almost stable.However, some of the CO is further oxidized to CO2 at high temperatures.Heating significantly accelerates the production of CO and CO2.The decrease in CO2 at 3000 K is because the high temperature promotes the reduction of more CO2 to CO. Figure 2c,d shows the effects of different temperatures on the formation of H and OH during blended combustion.It can be seen that the formation of H and OH is slow at low temperatures and the quantity is depleted as the reaction continues.High temperatures increase the amounts of H and OH.The difference is that H peaks rapidly and then decreases as the reaction proceeds, while OH peaks and then stabilizes as the reaction proceeds.The peak H at 3000 K is five times higher than that at 1500 K. Heating significantly increases the H and OH concentrations in the combustion reaction.

Temperature Effects on CO and CO 2 Formation in Blended Combustion
Figure 3a,b shows CO and CO 2 formation during the blended combustion process at different temperatures.Heating increases the rate of CO production, where CO is formed rapidly and then decreases slowly at temperatures of 2000 K and higher.At 1500 K and 1000 K, CO has still not peaked at the end of the reaction and is in a state of continuous growth.As the temperature increases the CO 2 production rate increases, and the peak state remains almost stable.However, some of the CO is further oxidized to CO 2 at high temperatures.Heating significantly accelerates the production of CO and CO 2 .The decrease in CO 2 at 3000 K is because the high temperature promotes the reduction of more CO 2 to CO. Figure 4 shows the effects of temperature on the formation of NOX (NO, NO2, and NO3) in the combustion of ternary carbon-neutral fuel blends.From Figure 4a, it can be seen that, as the reaction proceeds, NO is first generated rapidly.NO at low temperatures is gradually depleted after reaching the peak value, but the amount of NO at high temperatures is relatively stable.As the temperature increases, the NO peak is gradually shifted forward, and the peak value increases.
Figure 4b shows the change in NO2 with combustion, and its change rule in the range of 2000 K to 3000 K is opposite to that of NO, in which the largest amount of NO2 exists at 2000 K, followed by 2500 K, with the least at 3000 K, which may be caused by part of NO2 being reduced at a high temperature.NO2 at 1500 K shows the same trend of increasing and then decreasing as NO in this condition.The time of peak NO coincides with the time of a rapid increase in NO2, and the time of a large amount of NO consumption coincides with the time of peak NO2, so the consumed NO2 is further oxidized to NO3.
Figure 4c represents the variation in NO3 as the combustion reaction proceeds, with almost no change for the two high-temperature conditions.Its rise at 2000 K is followed by a steady rise and a rapid and sustained rise in the low-temperature condition.
Figure 4d represents the rapid formation and gradual stabilization of NOX as the blended combustion reaction proceeds.The effect of heating on the NOX peak is nonlinear.The NOX peak growth rate slows down with increasing temperature and reaches a peak at 2000 K.The NOX peak growth rate is also shown in Figure 4d, which shows that NOX formation is rapid and stabilizes under ternary combustion.2.1.3.Temperature Effects on NO X Formation from the Blended Combustion of Ternary Carbon-Neutral Fuels Figure 4 shows the effects of temperature on the formation of NO X (NO, NO 2 , and NO 3 ) in the combustion of ternary carbon-neutral fuel blends.From Figure 4a, it can be seen that, as the reaction proceeds, NO is first generated rapidly.NO at low temperatures is gradually depleted after reaching the peak value, but the amount of NO at high temperatures is relatively stable.As the temperature increases, the NO peak is gradually shifted forward, and the peak value increases.Heating accelerates the formation of NOX, but high temperature inhibits the formation of NOX when the temperature is higher than 2000 K.At low temperatures, NOX exists mainly in the form of NO3.At high temperatures, the main form of NOX is NO.At 2000 K, NO2 is the main form of NOX.This is probably because high temperature accelerates the reduction of NOX. Figure 4b shows the change in NO 2 with combustion, and its change rule in the range of 2000 K to 3000 K is opposite to that of NO, in which the largest amount of NO 2 exists at 2000 K, followed by 2500 K, with the least at 3000 K, which may be caused by part of NO 2 being reduced at a high temperature.NO 2 at 1500 K shows the same trend of increasing and then decreasing as NO in this condition.The time of peak NO coincides with the time of a rapid increase in NO 2 , and the time of a large amount of NO consumption coincides with the time of peak NO 2 , so the consumed NO 2 is further oxidized to NO 3 .
Figure 4c represents the variation in NO 3 as the combustion reaction proceeds, with almost no change for the two high-temperature conditions.Its rise at 2000 K is followed by a steady rise and a rapid and sustained rise in the low-temperature condition.
Figure 4d represents the rapid formation and gradual stabilization of NO X as the blended combustion reaction proceeds.The effect of heating on the NO X peak is nonlinear.The NO X peak growth rate slows down with increasing temperature and reaches a peak at 2000 K.The NO X peak growth rate is also shown in Figure 4d, which shows that NO X formation is rapid and stabilizes under ternary combustion.
Heating accelerates the formation of NO X , but high temperature inhibits the formation of NO X when the temperature is higher than 2000 K.At low temperatures, NO X exists mainly in the form of NO 3 .At high temperatures, the main form of NO X is NO.At 2000 K, NO 2 is the main form of NO X .This is probably because high temperature accelerates the reduction of NO X .

Influence of Blending Ratio on Combustion Composition and Pollutant Formation 2.2.1. Influence of Blending Ratio on Combustion Components and Free Radicals
A comparison and analysis of different blending ratios were carried out to obtain the formation patterns of reactants and NO X in ternary blended combustion under different blending ratios.Figure 5 shows the changes in reactants with time under different blending ratios.When the proportion of CH 4 O is more than 30%, the lower the proportion of NH 3 , the faster and more complete the reaction.When the proportion of CH 4 O is less than 30%, the reaction rate of CH 4 O is faster in the case of H 2 /NH 3 being more than 1, which is because H 2 promotes the decomposition of CH 4 O.Therefore, NH 3 inhibits CH 4 O combustion and H 2 promotes CH 4 O combustion in blended fuel combustion.When the proportion of CH 4 O is more than 30%, NH 3 plays a major role.When the proportion of CH 4 O is less than 30%, H 2 plays a major role.
As shown in Figure 5b, the higher the CH 4 O percentage, the higher the NH 3 reaction rate and the more complete the reaction.When the amount of NH 3 is determined, the working NH 3 reaction rate is faster for CH 4 O/H 2 greater than 1.This is because CH 4 O can promote the combustion of NH 3 .As shown in Figure 5c, the lower the NH 3 percentage the higher the H 2 reaction rate and the more complete the reaction.This is because NH 3 inhibits H 2 combustion.When the amount of H 2 is determined, the H 2 reaction rate is faster for the working condition of CH 4 O/NH 3 greater than 1, which also indicates that NH 3 inhibits H 2 combustion during the combustion of blended fuels.
From Figure 6a, it can be seen that the growth rate of H 2 O slows down significantly after a rapid rise to a certain level.With the increase in the proportion of H 2 , the rate of H 2 O generation is accelerated, and it can be seen that H 2 accelerates the rate of H 2 O formation in the combustion process.Through Figure 6b, it can be found that with the reaction, N 2 rises rapidly to a certain degree and then stabilizes, and N 2 rises with an increase in NH 3 content under different doping ratios.Because H 2 and NH 3 have a competitive relationship in the combustion process, and N 2 is a product of NH 3 combustion, when NH 3 is the same, the smaller the proportion of H 2 the faster N 2 rises and the larger the peak.However, in the case of a H 2 /NH 3 /CH 4 O ratio of 1:2:3, the amount of N 2 is significantly lower than a ratio of 3:2:1, which may be due to the large amount of CH 4 O affecting the conversion of NH 3 to N 2 during combustion, which will be further verified at the molecular level in Section 3.4.As shown in Figure 5b, the higher the CH4O percentage, the higher the NH3 reaction rate and the more complete the reaction.When the amount of NH3 is determined, the working NH3 reaction rate is faster for CH4O/H2 greater than 1.This is because CH4O can promote the combustion of NH3.As shown in Figure 5c, the lower the NH3 percentage the higher the H2 reaction rate and the more complete the reaction.This is because NH3 inhibits H2 combustion.When the amount of H2 is determined, the H2 reaction rate is faster for the working condition of CH4O/NH3 greater than 1, which also indicates that NH3 inhibits H2 combustion during the combustion of blended fuels.
From Figure 6a, it can be seen that the growth rate of H2O slows down significantly after a rapid rise to a certain level.With the increase in the proportion of H2, the rate of H2O generation is accelerated, and it can be seen that H2 accelerates the rate of H2O formation in the combustion process.Through Figure 6b, it can be found that with the reaction, N2 rises rapidly to a certain degree and then stabilizes, and N2 rises with an increase in NH3 content under different doping ratios.Because H2 and NH3 have a competitive relationship in the combustion process, and N2 is a product of NH3 combustion, when NH3 is the same, the smaller the proportion of H2 the faster N2 rises and the larger the peak.However, in the case of a H2/NH3/CH4O ratio of 1:2:3, the amount of N2 is significantly lower than a ratio of 3:2:1, which may be due to the large amount of CH4O affecting the conversion of NH3 to N2 during combustion, which will be further verified at the molecular level in Section 3.4.Figure 6c,d, on the other hand, shows the effect of different blending ratios on the formation of H and OH during the ternary hybrid combustion.It can be seen that H shows an increasing and then decreasing trend as the reaction proceeds.The conclusion is that the peak H value increases with increasing CH4O percentage.When the proportion of CH4O in the blending fuel remains constant, H2 has a certain promotion effect on H peak generation, and NH3 has a certain inhibition effect.When the proportion of CH4O is more Figure 6c,d, on the other hand, shows the effect of different blending ratios on the formation of H and OH during the ternary hybrid combustion.It can be seen that H shows an increasing and then decreasing trend as the reaction proceeds.The conclusion is that the peak H value increases with increasing CH 4 O percentage.When the proportion of CH 4 O in the blending fuel remains constant, H 2 has a certain promotion effect on H peak generation, and NH 3 has a certain inhibition effect.When the proportion of CH 4 O is more than half, the inhibitory effect is greater than the promotion effect, and OH grows to the peak and then decreases slowly as the reaction, which is almost stable, proceeds.The peak rises with the increase in CH 4 O percentage.When the proportion of CH 4 O in the blending fuel remains constant, unlike H, NH 3 promotes the generation of OH while H 2 inhibits it, and the inhibitory effect is greater than the promotional effect when the proportion of H 2 is more than half.Therefore, the concentration of radicals H and OH in the ternary blended combustion reaction is mainly affected by CH 4 O.

Influence of the Blending Ratio on CO and CO 2 Formation in Blended Combustion
Figure 7a,b shows CO and CO 2 formation during the ternary fuel blending process at different blending ratios, respectively.As the CH 4 O combustion reaction proceeds, the rate of CO formation is mainly affected by NH 3 , which slows down the rate of CO formation at a CH 4 O share of more than 30%.However, the amount of CO production is mainly influenced by CH 4 O, which increased with the increase in CH 4 O percentage.When the proportion of CH 4 O in the blending fuel remains constant, the larger the proportion of H 2 , the larger the peak of CO, which may be due to the combustion process of H 2 to promote the production of CO.CO 2 , in the progress of the reaction, shows a continuous increase in the trend of the rate, and the amount of CO 2 production is mainly affected by the proportion of CH 4 O.When the proportion of CH 4 O in the blending fuel remains constant, the higher the proportion of H 2 , the faster the reaction, and the greater the amount of formation, indicating that H 2 plays a role in promoting the formation of CO 2 , while NH 3 , and CH 4 O have a competitive relationship.
Molecules 2023, 28, x FOR PEER REVIEW 9 of 23 increase in the trend of the rate, and the amount of CO2 production is mainly affected by the proportion of CH4O.When the proportion of CH4O in the blending fuel remains constant, the higher the proportion of H2, the faster the reaction, and the greater the amount of formation, indicating that H2 plays a role in promoting the formation of CO2, while NH3, and CH4O have a competitive relationship.In summary, it is shown that the production of CO and CO2 during the combustion of a blend of ternary carbon-neutral fuels is not simply influenced by CH4O alone but is a result of the coupling of three fuels, H2, NH3, and CH4O, which will be examined on a molecular level in a detailed pathway analysis in Section 3.4.

Influence of Blending Ratio on NOX Formation in Blended Combustion
Figure 8 shows the influence of the NH3 blending ratio on the formation of NOX (NO, NO2, and NO3) during the blended combustion of ternary carbon-neutral fuels.Figure 8a shows that, as the reaction proceeds, NO is first generated rapidly and then gradually depleted.The NO formation rates and the peak values are in the ratios 2:3:1, 1:3:2, 1:2:3, 3:2:1, 2:1:3, and 3:1:2 from large to small, respectively.The time of peak appearance is positively correlated with the size of the peaks.The rate of NO formation and the magnitude of the peak are mainly influenced by NH3 in the fuel blends.When NH3 is quantized, In summary, it is shown that the production of CO and CO 2 during the combustion of a blend of ternary carbon-neutral fuels is not simply influenced by CH 4 O alone but is a result of the coupling of three fuels, H 2 , NH 3 , and CH 4 O, which will be examined on a molecular level in a detailed pathway analysis in Section 3.4.

Influence of Blending Ratio on NO X Formation in Blended Combustion
Figure 8 shows the influence of the NH 3 blending ratio on the formation of NO X (NO, NO 2 , and NO 3 ) during the blended combustion of ternary carbon-neutral fuels.Figure 8a shows that, as the reaction proceeds, NO is first generated rapidly and then gradually depleted.The NO formation rates and the peak values are in the ratios 2:3:1, 1:3:2, 1:2:3, 3:2:1, 2:1:3, and 3:1:2 from large to small, respectively.The time of peak appearance is positively correlated with the size of the peaks.The rate of NO formation and the magnitude of the peak are mainly influenced by NH 3 in the fuel blends.When NH 3 is quantized, CH 4 O promotes NH 3 combustion.Figure 8b represents the change in NO 2 with the combustion reaction process, and the NO 2 reaction fluctuates up and down around the peak value after a certain stage.The trend of the magnitude of the stabilization value with the blending ratio is similar to that of NO, and the rate of NO 2 formation and the magnitude of the peak are mainly affected by the NH 3 in the blended fuels.Comparing 1:2:3 and 3:2:1, it can be seen that CH 4 O promotes the combustion of NH 3 but increases the formation of NO 2 .Figure 8c represents the variation in NO 3 as the combustion reaction proceeds, showing a continuous growth trend as the reaction proceeds, but the growth rate is slow and then fast.The variation in the blending ratio is also similar to that of NO. Figure 8d shows the rapid formation and gradual stabilization of NOX as the combustion reaction proceeds.As the NH3 percentage increases, the NOX peak increases.When NH3 is quantized, the higher the CH4O content, the higher the NOX peak.Based on the NH3 percentage, it was hypothesized that there should be little difference between the ratio of 1:2:3 and the ratio of 3:2:1 NOX quantities, but the result was unexpected.The NOX value of 1:2:3 was 25% higher than that of 3:2:1, which may be due to the fact that CH4O increased the conversion rate of NH3 to NOX.In order to gain insight into the effects of doping ratio on NOX formation, reaction pathway analysis will be carried out at the molecular level in the following.

Analysis of the Mechanisms of CO, CO2, and NOX Formation in the Combustion of Blended Fuels as Affected by Temperature
This section will further discuss temperature-influenced ternary blended fuel com- Figure 8d shows the rapid formation and gradual stabilization of NO X as the combustion reaction proceeds.As the NH 3 percentage increases, the NO X peak increases.When NH 3 is quantized, the higher the CH 4 O content, the higher the NO X peak.Based on the NH 3 percentage, it was hypothesized that there should be little difference between the ratio of 1:2:3 and the ratio of 3:2:1 NO X quantities, but the result was unexpected.The NO X value of 1:2:3 was 25% higher than that of 3:2:1, which may be due to the fact that CH 4 O increased the conversion rate of NH 3 to NO X .In order to gain insight into the effects of doping ratio on NO X formation, reaction pathway analysis will be carried out at the molecular level in the following.

Analysis of the Mechanisms of CO, CO 2 , and NO X Formation in the Combustion of Blended Fuels as Affected by Temperature
This section will further discuss temperature-influenced ternary blended fuel combustion in the mechanism of CO, CO 2 , and NO X formation.In this section, the N and C migration paths during ternary blended fuel combustion simulated by ReaxFF MD at different temperatures are generated and discussed for Case 1, Case 2, and Case 5 as examples.Figure 9a-c represents the network diagrams for NO X formation reaction paths during the combustion of ternary fuel at temperatures of 1000 K, 2000 K, and 3000 K.The percentages in the network diagrams indicate the reactant conversion rates.In order to highlight the main paths of the reaction network, reaction paths with a conversion rate of less than 15% are ignored in all network diagrams in this study.Comparative analysis of the graphs in Figure 9 reveals that the complexity of the paths appears to be greater and then lesser as the temperature increases; the paths are most complex at 2000 K.The complexity of the paths is greater when the temperature is too low.This may be because the reaction is incomplete and molecular activity is low at Comparative analysis of the graphs in Figure 9 reveals that the complexity of the paths appears to be greater and then lesser as the temperature increases; the paths are most complex at 2000 K.The complexity of the paths is greater when the temperature is too low.This may be because the reaction is incomplete and molecular activity is low at 1000 K. Therefore, many molecules do not have the opportunity to collide with each other, so there are fewer intermediate products and the path is simpler.At 3000 K, because of the high temperature, the reactants are very active, especially the O molecules, so that many reactions can occur in a very short period of time.The oxidation of NH 3 by OH during the conversion of NH 3 molecules to NH 2 decreases from 66.7% to less than 10%, but O increases rapidly from 33% to 67%.The intermediates required for the conversion of NH 3 molecules to NO are gradually reduced from three to direct oxidation without intermediates.Thus, higher temperatures significantly contribute to the NH 3 combustion reaction rate.By comparing Figure 9a-c, it is found that, as the temperature is further increased to 3000 K, the high temperature leads to the disappearance of the pathway for NH 3 to generate NiHi, which cannot generate N 2 but directly generates NO, and the significant increase in H and OH concentrations also contributes to the generation of NO from NH 3 to a certain extent.This analysis validates the conclusion in Section 3.1 of this paper about heating.Although accelerating the formation of NO X is not conducive to the formation of NH 3 , the conclusion is that high temperature inhibits NO X formation when the temperature is higher than 2000 K.The results of this analysis are summarized in Figure 2c.
Analyzing the redox process for NO X , it was found that NO X is all formed by NO conversion.At low temperatures (1000 K), 50% of NO is oxidized directly to NO 3 , while 25% of NO is oxidized to NO 2 .A total of 50% of NO 3 can be reduced to NO 2 , but NO 2 and NO 3 cannot be reduced directly to NO.Therefore, at low temperatures, NO X exists mainly as NO 3 .At 2000 K, the direct oxidation path from NO to NO 3 disappears, and it needs to pass through NO 2 to form NO 3 .Overall, 91% of NO is oxidized directly or indirectly to NO 2 , and the reduction of NO 3 to NO 2 is as high as 67%.Therefore, at 2000 K, NO 2 is the main form of NO X .At high temperatures (3000 K), the pathway to generate NO 3 disappears, and 68% of NO is oxidized directly or indirectly to NO 2 .The reduction rate for NO 2 is as high as 71%.Therefore, NO X mainly exists in the form of NO at high temperatures.
Figure 10a-c represents the network diagrams of CO 2 formation reaction paths during combustion of ternary fuels at temperatures of 1000 K, 2000 K, and 3000 K. From Figure 10a  Figure 10b represents the main reaction paths of CO and CO2 formation by combustion of ternary hybrid fuel at a temperature of 2000 K.It can be seen that 73% of CH4O molecules will collide to form CH3O by the H2 extraction reaction.CH3O continues to collide with OH and O2 to form CH2O by a dehydrogenation reaction, while 27% of CH4O is oxidized by O2 to form CH2O. Unlike at 1000 K, the path from CH2O to CHO2 has expanded by two pathways: 64% of CH2O will collide with OH to form CHO first, and then collide with groups such as OH or H2O to form CHO2, while 18% of CH2O collides directly with O to form CHO2. The proportion of CH2O2 formation through collision with O to form CHO2 and then CHO2 (as at 1000 K) has decreased from 100% to 18%.CHO2 collides with groups such as OH and O2 to form CO2. CO2 is formed in the presence of groups such as OH, O2, O, and so forth.CO and CO3 ultimately flow to CO2.CO2 remains relatively stable in the form of an end product.
Figure 10c shows the main reaction paths for CO2 formation from the combustion of ternary hybrid fuels at a temperature of 3000 K.It is found that 60% of CH4O reacts with OH to form CH3O at the beginning of the combustion process at a temperature of 3000 K, and 40% of CH4O is directly formed into CH2O under the action of O.The proportions of CH4O reacting with OH to form CH3O at temperatures of 1000 K and 2000 K are 90% and  Through further comparative analysis, it was found that with an increase in temperature, as for the N migration path, the complexity of the C migration path appeared to become larger and then smaller.The path is most complex at 2000 K.The consumption of CH 4 O molecules decreases the percentage of flow to CH 3 O from 90% to 60%, a decrease of 30%.The proportion of flow to CH 2 O increases from 0 to 40%, an increase of 40%.Thus, higher temperatures significantly contribute to the NH 3 combustion reaction rate.By comparing Figure 10a-c, it is found that the percentage of CO formation is very small at low temperatures.At 2000 K, a CO formation pathway emerges from the reduction of 40% CO 2 and the combination of 90% of this with OH to form CHO 2 .At a high temperature, unlike at low and medium temperatures, CO 2 is not the only source of CO, which is not only derived from 50% CO 2 , but also from 50% CHO.In addition, the consumption of CO also decreases from 90% to 67%.Therefore, with further increases in temperature, the rate of CO and CO 2 formation rises, and the CO peak increases.Reaction path analysis explains the phenomenon in Section 3.1 of this paper that heating accelerates the rate of CO and CO 2 formation and the increase in peak CO with increasing temperature.

Mechanism and Reaction Path Analysis of CO, CO 2 , and NO X Formation in Blended Fuel Combustion as Affected by Blending Ratio
This section will further discuss the influence of blending ratio in the combustion of ternary blended fuel on the mechanisms of CO, CO 2 , and NO X formation.In this paper, the N and C migration paths of ternary blended fuel combustion are simulated by ReaxFF MD with different blending ratios generated and discussed for Case 1, Case 6, Case 7, and Case 9 as examples.Figure 11a-d represents the NO X formation reaction path network diagrams during the combustion of ternary fuels with H 2 /NH 3 /CH 4 O blending ratios of 2:2:2, 1:2:3, 1:3:2, and 2:3:1.
From Figure 11a, it can be found that NH and H 3 NO generate NO by oxidizing to produce HNO and H 2 NO.A total of 55% of the NO collides with OH to produce HNO 2 , whose continued collision with OH leads to the formation of NO 2 .Meanwhile, 36% of NO is oxidized directly to NO 2 .A total of 85% of the NO 2 collides with OH to produce HNO 3 , and 64% of the HNO 3 is dehydrogenated to produce NO 3 before it is reduced to NO 2 by NO, while 27% of the HNO 3 is directly reduced back to NO 2 by collision with OH.A total of 25% of the NO 2 remains relatively stable in the form of an end product.
Figure 11b shows the main reaction pathways for the formation of NO X from blended combustion with a ratio of 1:2:3.HNO is oxidized to NO by O 2 , while 25% of NH is directly oxidized to NO by collision with OH.Subsequently, 14% of the NO remains relatively stable as an end product; 50% of the NO collides with OH to form HNO 2 , which is then reduced to NO 2 by the continued collision with OH and O 2 ; 36% of the NO is directly oxidized to NO 2 ; and 38% of the NO is dehydrogenated with OH to form HNO 3 .A total of 60% of the HNO 3 is dehydrogenated to NO 3 and then reduced to NO 2 by O.A total of 40% of HNO 3 is dehydrogenated to NO 3 before being reduced to NO 2 by O.
Figure 11c shows the main reaction paths of NO X formation for blended combustion with a ratio of 1:3:2.A total of 37.5% of the NH 2 collides and combines with NH 2 groups to form N 2 H 4 .It continues to collide with groups such as OH, O 2 , etc., to eventually form N 2 .Meanwhile, 25% of the NH 2 collides with OH in a dehydrogenation reaction to form NH. NH collides with oxidizing groups such as O 2 , HO 2 , and O to form HNO. HNO collides with OH to form NO. A total of 12% of the NO remains relatively stable as an end product; 75.68% of the NO is oxidized to NO 2 ; 37% of the NO 2 combines with OH to form HNO 3 .HNO 3 continues to collide with OH to form NO 3 .A total of 44% of the NO 3 is reduced to NO 2 by groups such as O and OH, but HNO 3 is not the only source of NO 3 .This is because 25% of NH 2 forms NO 3 through H 3 NO as well.
Figure 11d represents the main reaction pathways for NO X formation in blended combustion with a ratio of 2:3:1.HNO is oxidized to NO by groups such as HO 2 and OH.A total of 20% of the NH 2 collides with OH to form NH; 67% of the NH is oxidized directly to NO by groups such as O and O 2 ; 25% of the NH is oxidized directly to NO by collisions with OH.In total, 33% of the NO and of the OH produce NO 2 indirectly via HNO 2 , while 42% of the NO is oxidized directly to NO 2 .Overall, 22% of the NO 2 collides with OH to produce NO 3 ; 80% of the NO 3 is reduced directly back to NO 2 by collisions with O and NO.From Figure 11a, it can be found that NH and H3NO generate NO by oxidizing to produce HNO and H2NO.A total of 55% of the NO collides with OH to produce HNO2, whose continued collision with OH leads to the formation of NO2.Meanwhile, 36% of NO is oxidized directly to NO2.A total of 85% of the NO2 collides with OH to produce HNO3, and 64% of the HNO3 is dehydrogenated to produce NO3 before it is reduced to NO2 by Comparison of Figure 11a,b reveals that the main path of NO X formation does not change much when the amount of NH 3 fuel is the same.The reaction path is simpler at 1:2:3 compared to the 2:2:2 blending ratio.The conversion ratio of NH 3 to NO also increases from 36.3% to 53.2%.This indicates that CH 4 O makes the NH 3 reaction path simpler and NO X formation easier.This is consistent with the conclusion in Section 3.2 that CH 4 O promotes NH 3 combustion.Comparison of Figure 11a,c reveals that when the amount of CH 4 O fuel is certain, the proportion of NH 3 is greater in the case of the ratio 1:3:2, which increases the reaction of NiHi to produce N 2 and NO 3 .The conversion of NH 3 to NO X increases from 36.3% to 51.5%.The conclusion that NO X is mainly determined by NH 3 is confirmed.This conclusion is similarly confirmed in the comparative analysis of Figure 11a,d.The 2:3:1 pathway is simpler when the number of H 2 fuels is the same.The conversion of NH 3 to NO does not require a stepwise dehydrogenation reaction, and the conversion efficiency is increased to 50.6%.
Figure 12a-d shows the network diagrams of CO 2 formation reaction paths during the combustion of ternary fuels with H 2 /NH 3 /CH 4 O blending ratios of 2:2:2, 1:2:3, 1:3:2, and 2:3:1.Figure 12a shows the main reaction paths for the formation of CO and CO 2 in blended combustion with a ratio of 2:2:2.CHO 2 collides with groups such as OH and O 2 to form CO 2 .The CO and CO 3 formed by CO 2 in the presence of groups such as OH, O 2 , and O ultimately flow back to CO 2 .The CO 2 remains relatively stable in the form of an end product.Figure 12b represents the main reaction path for the formation of CO and CO2 from blended combustion at a ratio of 1:2:3.It can be seen that CHO2 collides with OH and other groups to generate CO2.CO2 is formed under the action of OH, O2, O and other groups of CO and CO3.Compared with the different times at 2:2:2, CH2O2 can collide directly with OH to generate CO at this ratio, and the reaction path is more complex.Figure 12b represents the main reaction path for the formation of CO and CO 2 from blended combustion at a ratio of 1:2:3.It can be seen that CHO 2 collides with OH and other groups to generate CO 2 .CO 2 is formed under the action of OH, O 2 , O and other groups of CO and CO 3 .Compared with the different times at 2:2:2, CH 2 O 2 can collide directly with OH to generate CO at this ratio, and the reaction path is more complex.
Figure 12c shows the main reaction paths for CO and CO 2 formation in blended combustion when the ratio is 1:3:2.Overall, 33% of CH 2 O collides with free radicals, such as O, to form CO; 56% of CH 2 O collides with OH to form CHO; and the two portions of 33% of CHO collide with OH to form CH 2 O 2 and CO, respectively.
Figure 12d shows the main reaction paths for CO and CO 2 formation from the combustion of ternary blends at a ratio of 2:3:1.It is found that 78% of CH 4 O starts to react with OH and O to form CH 3 O at the ratio of 2:3:1.Overall, 78% of CH 3 O forms CH 2 O in the presence of O 2 ; 57% of CH 2 O collides with free radicals such as OH to form CHO; 29% of CH 2 O collides with O 2 to form CO 2 ; and CHO generates CO and CO 2 directly or indirectly.
Comparison of Figure 12a,b shows that when the amount of NH 3 fuel is fixed, more CH 4 O is converted to CH 2 O with a ratio of 1:2:3 compared to 2:2:2.This may be due to the fact that H 2 promotes the oxidation of CH 4 O.There were more reaction pathways for CO and CO 2 formation compared to the 2:2:2 ratio of 1:2:3.This may be caused by the high number of OH radicals in the reaction.
Comparison of Figure 12a,c reveals that the two paths do not differ much when the amount of CH 4 O fuel is the same.This indicates that the reactions of CO and CO 2 during the combustion of ternary fuels are mainly influenced by CH 4 O.
Comparison of Figure 12a,d reveals that when the number of H 2 fuels is the same, the path with a ratio of 2:3:1 is more complex.However, it does not mean that the oxidation of carbon-containing fuels in ternary fuels is more intense.Analyzing the percentage of oxidizing groups in the pathway reveals that, on the contrary, it is the oxidation of carboncontaining fuels at 2:3:1 that does not have enough O and OH groups.This time more intermediate OH groups are needed.From the analysis of OH groups mainly influenced by CH 4 O it can be concluded that CO and CO 2 are mainly determined by CH 4 O.

Reactive Force-Field Molecular Dynamics (ReaxFF MD)
ReaxFF MD combines molecular dynamics simulation with the calculation of reactive force fields.Its reactive force-field potential function is derived from experimental data and density functional theory, so the accuracy is close to quantum computation and does not require the predetermination of chemical reaction paths in the system [32].ReaxFF is parameterized against QM-based training sets and is dependent on the bond order, while the bond order is a function of interatomic distance and updates at every iteration.Therefore, ReaxFF can describe bond formation and dissociation and provide highly accurate simulation results.ReaxFF MD has been widely used in the study of pyrolysis [33], combustion [34], explosions [35], oxidation [36], catalysis [37], and other systems involving physical chemistry.It provides a promising means of exploring the chemical behavior of complex molecular systems.Bond-order-dependent characterization is achieved by detailed parameterization of the atomic, bonding, angular, and torsional properties of each particle, and the interactions within the system [38].The total energy of the system can be calculated by summing all partial energy terms as described in R1: E system = E bond + E over + E under + E val + E pen + E tors + E conj + E vdWaals + E coulomb (1) where E bond , E over , E under , E val , E pen , E tors , and E conj correspond to bond energy, overcoordination energy, under-coordination energy, bond angle energy, compensation energy, torsion energy, and four-body conjugation energy.The non-bonding terms mainly consist of van der Waals force energy (E vdWaals ) and Coulomb force energy (E coulomb ).When calculating non-bonding interactions, the charged atoms cross the truncation radius of the non-bonding interactions, thus leading to a jump in energy.Therefore, ReaxFF is additionally corrected by introducing a seventh-order polynomial Taper function, which ensures that, at the truncation radius, the non-bonding interaction's first-, second-, and third-order derivatives of the energy term are all zero [39].ReaxFF also takes better account of charge polarization by employing the electronegativity equalization method [40] and updates the atomic charges at each time step [41].The detailed meaning of the ReaxFF parameters, the setup of the molecular structure, and the applicability of the reaction force field have been described in detail in a previous study [42].

Case Set-Ups
Table 1 lists all H 2 /NH 3 /CH 4 O blend combustion ReaxFF MD simulation cases in the high-pressure environment of this paper.The system density (ρ), equivalence ratio (ϕ), and simulation time are 0.05 g/cm 3 , 0.5, and 1.25 ns, where more air (ϕ = 0.5) is used to ensure complete fuel combustion.Cases 1 to 5 represent the combustion of H 2 /NH 3 /CH 4 O blended fuel at 2000 K, 1000 K, 1500 K, 2500 K, and 3000 K. Cases 6 to 11 represent combustion at the same temperature with H 2 /NH 3 /CH 4 O ratios of 1:2:3, 1:3:2, 2:1:3, 2:3:1, 3:1:2, and 3:2:1.Three replicates with different initial configurations were simulated for individual cases.All the results reported in this work are ensemble-averaged from them.Through further comparative analysis, the mechanisms of CO, CO 2 , and NO X formation at different temperatures and fuel ratios are analyzed at the molecular level.

Computational Details and Post-Processing
All the cases listed in Table 1 were analyzed in the ReaxFF module of AMS [43][44][45].In this study, the HE2.ff force field [46] and the regular system with constant atomic number, volume, and temperature (NVT) were used.To ensure the overall stability of hydrocarbon fuel combustion, the energy and configuration of all simulated cases were first optimized using the "Geometry Optimization" and "Energy Optimization" plugins.Figure 13 shows the optimized systematic for Case 1, which shows that fuel and oxidant are uniformly blended, similar to a premixed flame, and similar to the cyclone burner we previously employed [47].A Berendsen thermostat was used to control the temperature with a time step of 0.25 fs.Periodic boundary conditions were applied in all three xyz directions and the soot intermediate components and product distributions were analyzed from trajectories using a 0.3 Å bond level cutoff.All simulations were done on a server with an Intel(R) Xeon(R) Platinum 8352Y CPU @ 2.20 GHz, 64-core CPU, and 256 GB of RAM, and each set of conditions simulated for 1 ns required approximately 30 h of CPU time.

Validation of the ReaxFF MD Method
The reliability and validity of the ReaxFF MD method have been widely tested and verified in previous studies [38,39,[48][49][50][51]].Among them, Wang et al. [39] constructed the reaction pathways in high-pressure combustion by tracking the trajectories of reacting atoms through ReaxFF MD to understand NOX formation mechanisms in NH3/CH4 combustion at different temperatures and pressures.The results showed that a high temperature accelerated the rate of ammonia consumption, which was consistent with the experimental results.High pressure complicated the reaction pathway in NH3/CH4 combustion with the emergence of new intermediates and primitive reactions.In addition, they pointed out that ReaxFF MD is a valuable tool to reveal the underlying reaction mechanisms in combustion and pollutant formation.Liu et al. [51] investigated the chemical reactivity effects of NO on the oxidation of CH4 using ReaxFF MD simulations and found that increasing the blending ratio of NO accelerated the rate of CH4 consumption.This is mainly due to the fact that, on the one hand, conversion of NO to NO2 generates OH radicals, which accelerates CH4 consumption, while, on the other hand, NO can also inhibit CH4 consumption by combining with reactive radicals.Wang et al. [48] applied ReaxFF MD and Py-GC/MS to investigate the characteristics of soot particulate formation in the process of the hydrogen-doped combustion of methane and ethylene.Both experimental and numerical results reflected that PAHs and ethylene were not the most important pollutants in the combustion process of CH4.The experimental and numerical results reflect the evolution of PAHs and initial soot particles, as well as the different chemical effects of hydrogen doping on PAHs and soot formation.

Conclusions
In this paper, the effects of different reactant temperatures and blending ratios on combustion reaction rates and the formation characteristics of CO, CO2, and NOX in the combustion of H2/NH3/CH4O ternary carbon-neutral blended fuels were investigated for the first time using ReaxFF MD.The mechanisms of CO, CO2, and NOX formation in ternary blended fuels at different temperatures and blending ratios were investigated.The conclusions of this paper are summarized as follows: (1) Heating accelerates the rate of H2, NH3, CH4O, and O2 consumption during ternary fuel combustion.However, the effect of heating on products such as N2 and H2O is not linear.The lowest amount of N2 was produced and the most amount of NOX was generated at 2000 K.The reaction rate and formation of CO and CO2 increased with temperature.The CO peak shifted forward with increasing temperature.Free radical analysis revealed that CO, CO2, and NOX may be closely related to large amounts of OH.The predominant form present in NOX changed with temperature.However, CO2 has been the main form present in carbonaceous pollutants.

Validation of the ReaxFF MD Method
The reliability and validity of the ReaxFF MD method have been widely tested and verified in previous studies [38,39,[48][49][50][51]].Among them, Wang et al. [39] constructed the reaction pathways in high-pressure combustion by tracking the trajectories of reacting atoms through ReaxFF MD to understand NO X formation mechanisms in NH 3 /CH 4 combustion at different temperatures and pressures.The results showed that a high temperature accelerated the rate of ammonia consumption, which was consistent with the experimental results.High pressure complicated the reaction pathway in NH 3 /CH 4 combustion with the emergence of new intermediates and primitive reactions.In addition, they pointed out that ReaxFF MD is a valuable tool to reveal the underlying reaction mechanisms in combustion and pollutant formation.Liu et al. [51] investigated the chemical reactivity effects of NO on the oxidation of CH 4 using ReaxFF MD simulations and found that increasing the blending ratio of NO accelerated the rate of CH 4 consumption.This is mainly due to the fact that, on the one hand, conversion of NO to NO 2 generates OH radicals, which accelerates CH 4 consumption, while, on the other hand, NO can also inhibit CH 4 consumption by combining with reactive radicals.Wang et al. [48] applied ReaxFF MD and Py-GC/MS to investigate the characteristics of soot particulate formation in the process of the hydrogen-doped combustion of methane and ethylene.Both experimental and numerical results reflected that PAHs and ethylene were not the most important pollutants in the combustion process of CH 4 .The experimental and numerical results reflect the evolution of PAHs and initial soot particles, as well as the different chemical effects of hydrogen doping on PAHs and soot formation.

Conclusions
In this paper, the effects of different reactant temperatures and blending ratios on combustion reaction rates and the formation characteristics of CO, CO 2 , and NO X in the combustion of H 2 /NH 3 /CH 4 O ternary carbon-neutral blended fuels were investigated for the first time using ReaxFF MD.The mechanisms of CO, CO 2 , and NO X formation in ternary blended fuels at different temperatures and blending ratios were investigated.The conclusions of this paper are summarized as follows: (1) Heating accelerates the rate of H 2 , NH 3 , CH 4 O, and O 2 consumption during ternary fuel combustion.However, the effect of heating on products such as N 2 and H 2 O is not linear.The lowest amount of N 2 was produced and the most amount of NO X was generated at 2000 K.The reaction rate and formation of CO and CO 2 increased with temperature.The CO peak shifted forward with increasing temperature.Free radical analysis revealed that CO, CO 2 , and NO X may be closely related to large amounts of OH.The predominant form present in NO X changed with temperature.However, CO 2 has been the main form present in carbonaceous pollutants.
(2) Pollutant formation during the combustion of H 2 /NH 3 /CH 4 O ternary carbonneutral blends was influenced by the coupling of H 2 , NH 3 , and CH 4 O. NH 3 suppressed the CO formation rate when the percentage of CH 4 O was greater than 30%.However, the amount of CO and CO 2 formation was mainly determined by CH 4 O, which increased the NH 3 combustion rate, causing NH 3 combustion to form more NO X .In the ternary blended combustion process, NH 3 inhibits H 2 combustion, but CH 4 O promotes H 2 combustion, in which NH 3 plays a major role.
(3) Analysis of the formation mechanisms of pollutants from the combustion of ternary carbon-neutral blended fuels at different temperatures reveals that high temperatures lead to more active oxidizing groups such as O in the reaction, which inhibits N 2 formation.The pathway of NO X is more complicated at 2000 K. NO X is formed by the conversion of NO.At low temperatures, half of the NO is oxidized directly to NO 3 , but NO 2 and NO 3 cannot be reduced to NO directly.At 2000 K, NO needs to pass through NO 2 to form NO 3 .A large amount of NO is oxidized to NO 2 , and the reduction of NO 3 to NO 2 is higher.At high temperatures, the pathway to generate NO 3 disappears, and NO 2 has a higher reduction rate.Therefore, the main form of NO X exists differently in different temperature states.Higher temperatures lead to the emergence of more CO formation paths, making CO and CO 2 be produced more quickly.
(4) By analyzing the formation mechanisms of pollutants in the combustion of ternary carbon-neutral blends with different blending ratios, it was found that CH 4 O promotes the combustion of NH 3 .This makes the reaction path simpler and easier for the generation of NO X .CH 4 O not only provides more carbon atoms involved in collisions for CO and CO 2 formation, but also leads to more OH and H formation.Therefore, the amount of CO and CO 2 formation is mainly determined by CH 4 O.

Figure 3 .
Figure 3. CO and CO 2 formation with time for blended combustion at different temperatures (a) CO; (b) CO 2 .

Figure 4 .
Figure 4. Distribution of NO X during the combustion of ternary carbon-neutral fuel blends.(a) NO; (b) NO 2 ; (c) NO 3 ; (d) NO X .

Figure 6 .
Figure 6.Variation in combustion components and free radicals in ternary carbon-neutral fuel blends with time at different blending ratios.(a) H 2 O; (b) N 2 ; (c) H; (d) OH.

Figure 7 .
Figure 7. CO and CO2 formation over time for blended combustion at different blending ratios (a) CO; (b) CO2.

Figure 7 .
Figure 7. CO and CO 2 formation over time for blended combustion at different blending ratios (a) CO; (b) CO 2 .

Figure 8 .
Figure 8. Distribution of NO X during the combustion of ternary carbon-neutral fuel blends at different blending ratios.(a) NO; (b) NO 2 ; (c) NO 3 ; (d) NO X .

Figure 10 .
Figure 10.Mechanisms of CO and CO2 formation in the blended combustion of ternary carbonneutral fuels at different temperatures.(a) 1000 K; (b) 2000 K; (c) 3000 K.

Figure 10 .
Figure 10.Mechanisms of CO and CO 2 formation in the blended combustion of ternary carbonneutral fuels at different temperatures.(a) 1000 K; (b) 2000 K; (c) 3000 K.

Figure
Figure10cshows the main reaction paths for CO 2 formation from the combustion of ternary hybrid fuels at a temperature of 3000 K.It is found that 60% of CH 4 O reacts with OH to form CH 3 O at the beginning of the combustion process at a temperature of 3000 K, and 40% of CH 4 O is directly formed into CH 2 O under the action of O.The proportions of CH 4 O reacting with OH to form CH 3 O at temperatures of 1000 K and 2000 K are 90% and 73%, respectively.The present reaction is only at 60%, and the proportions of CH 4 O directly oxidized into CH 2 O are 0 and 27% respectively, growing to 40% in the present case.Therefore, in this study, it was found that the oxidation of CH 4 O molecules during the combustion of ternary blended fuels is more pronounced as the temperature increases.This is mainly due to the fact that as the temperature increases the ternary fuel combustion reaction contains more free OH and O.The temperature also means the reactant movement is more violent, allowing more molecules to collide and participate in the pyrolysis reaction.A temperature of 3000 K generated 80% of CH 2 O by direct O oxidation to CHO; CHO and OH collision generated under half of the formation of CO and half of the formation of CO 2 .Through further comparative analysis, it was found that with an increase in temperature, as for the N migration path, the complexity of the C migration path appeared to become larger and then smaller.The path is most complex at 2000 K.The consumption of CH 4 O molecules decreases the percentage of flow to CH 3 O from 90% to 60%, a decrease of 30%.The proportion of flow to CH 2 O increases from 0 to 40%, an increase of 40%.
2.1.Temperature Effects on Ternary Blended Combustion Components and Pollutant Formation 2.1.1.Temperature Effects on Ternary Blended Combustion Components and Free Radicals Figure 1 shows the effects of different temperatures on the four reactant components CH 4 O, NH 3 , H 2 , and O 2 in the ternary blended combustion process.From the figure, it can be seen that heating significantly accelerated the decomposition rate of CH 4 O, NH 3 , H 2 , and O 2 .The insignificant rises for H 2 and O 2 at high temperatures may be caused by the decomposition of H 2 O due to the intensification of molecular collisions at high temperatures.
, it can be found that 90% of CH 4 O molecules first collide with OH from O 2 decomposition to form CH 3 O.A total of 75% of CH 3 O collides with HO 2 and O to form CH 2 O, which is oxidized by O to form CH 2 O 2 .CH 2 O 2 is oxidized by NO 2 and O to form CHO 2 , which collides with OH to form CO 2 .The reaction paths are chain-shaped in this case.The path is chain-shaped and has a simple structure.Figure 10b represents the main reaction paths of CO and CO 2 formation by combustion of ternary hybrid fuel at a temperature of 2000 K.It can be seen that 73% of CH 4 O molecules will collide to form CH 3 O by the H 2 extraction reaction.CH 3 O continues to collide with OH and O 2 to form CH 2 O by a dehydrogenation reaction, while 27% of CH 4 O is oxidized by O 2 to form CH 2 O. Unlike at 1000 K, the path from CH 2 O to CHO 2 has expanded by two pathways: 64% of CH 2 O will collide with OH to form CHO first, and then collide with groups such as OH or H 2 O to form CHO 2 , while 18% of CH 2 O collides directly with O to form CHO 2 .The proportion of CH 2 O 2 formation through collision with O to form CHO 2 and then CHO 2 (as at 1000 K) has decreased from 100% to 18%.CHO 2 collides with groups such as OH and O 2 to form CO 2 .CO 2 is formed in the presence of groups such as OH, O 2 , O, and so forth.CO and CO 3 ultimately flow to CO 2 .CO 2 remains relatively stable in the form of an end product.