Citation: TsungYu Lee, Hsunling Bai. Low temperature selective catalytic reduction of NOx with NH3 over Mn-based catalyst: A review[J]. AIMS Environmental Science, 2016, 3(2): 261-289. doi: 10.3934/environsci.2016.2.261
[1] | Wenjie Qin, Jiamin Zhang, Zhengjun Dong . Media impact research: a discrete SIR epidemic model with threshold switching and nonlinear infection forces. Mathematical Biosciences and Engineering, 2023, 20(10): 17783-17802. doi: 10.3934/mbe.2023790 |
[2] | Cunjuan Dong, Changcheng Xiang, Wenjin Qin, Yi Yang . Global dynamics for a Filippov system with media effects. Mathematical Biosciences and Engineering, 2022, 19(3): 2835-2852. doi: 10.3934/mbe.2022130 |
[3] | Rajanish Kumar Rai, Pankaj Kumar Tiwari, Yun Kang, Arvind Kumar Misra . Modeling the effect of literacy and social media advertisements on the dynamics of infectious diseases. Mathematical Biosciences and Engineering, 2020, 17(5): 5812-5848. doi: 10.3934/mbe.2020311 |
[4] | Arvind Kumar Misra, Rajanish Kumar Rai, Yasuhiro Takeuchi . Modeling the control of infectious diseases: Effects of TV and social media advertisements. Mathematical Biosciences and Engineering, 2018, 15(6): 1315-1343. doi: 10.3934/mbe.2018061 |
[5] | Xuejuan Lu, Shaokai Wang, Shengqiang Liu, Jia Li . An SEI infection model incorporating media impact. Mathematical Biosciences and Engineering, 2017, 14(5&6): 1317-1335. doi: 10.3934/mbe.2017068 |
[6] | Bruno Buonomo, Eleonora Messina . Impact of vaccine arrival on the optimal control of a newly emerging infectious disease: A theoretical study. Mathematical Biosciences and Engineering, 2012, 9(3): 539-552. doi: 10.3934/mbe.2012.9.539 |
[7] | Zehan Liu, Daoxin Qiu, Shengqiang Liu . A two-group epidemic model with heterogeneity in cognitive effects. Mathematical Biosciences and Engineering, 2025, 22(5): 1109-1139. doi: 10.3934/mbe.2025040 |
[8] | Dongmei Li, Bing Chai, Weihua Liu, Panpan Wen, Ruixue Zhang . Qualitative analysis of a class of SISM epidemic model influenced by media publicity. Mathematical Biosciences and Engineering, 2020, 17(5): 5727-5751. doi: 10.3934/mbe.2020308 |
[9] | Pengfei Liu, Yantao Luo, Zhidong Teng . Role of media coverage in a SVEIR-I epidemic model with nonlinear incidence and spatial heterogeneous environment. Mathematical Biosciences and Engineering, 2023, 20(9): 15641-15671. doi: 10.3934/mbe.2023698 |
[10] | Xin-You Meng, Tao Zhang . The impact of media on the spatiotemporal pattern dynamics of a reaction-diffusion epidemic model. Mathematical Biosciences and Engineering, 2020, 17(4): 4034-4047. doi: 10.3934/mbe.2020223 |
Coal oxidation at ambient temperatures is considered the main reason for products quality and energy losses. Chemisorption and oxidation occur when coal is exposed to air at relatively low temperatures (below 100 °C). Moreover, as such processes are exothermal, this may also lead to self-heating (accelerating the oxidation reaction) and spontaneous combustion events during production, storage, transportation and utilization of coal [1,2,3].
There exist a certain amount of instrumental methods and techniques for characterization of coals propensity to self-heating at oxidation. The most widely used one is the so-called R70 method [4,5]. The essence of this method is as follows. The grinded (with particle sizes of <212 µm) coal sample is dried in adiabatic oven at temperature of 105-110 °C for 15 hours under inert gas flow, then cooled to 40 °C in the same environment, and after that is being stored in the oxygen-rich air flow at the temperature of 40 °C. Under the latter conditions, coal oxidation is being initiated and the processes of self-heating are observed. The average rate of the coal heating from 40 to 70 °C is considered to be the index R70 (°C/h). The higher the value of such index, the more prone the coal is to spontaneous combustion. Such method is the most efficient one with respect to simple characterization of coals propensity to oxidation and self-heating, but unfortunately there exist some disadvantages connected with the method of samples preparation, namely, their drying at high temperatures which may lead to irreversible alterations of coals properties.
Crossing Point Temperature (CPT) is another method widely applied for characterization of coals propensity to spontaneous combustion [6,7]. Here, the coal sample is placed in the oven which is being heated with constant rate. Within this method, a rate of coal sample heating is compared with the rate of the oven walls heating at the condition of constant air supply to the sample. In comparison with the aforementioned R70 method, CPT allows in situ coals samples testing, but still there are some disadvantages connected with the samples moisture, particles sizes, etc.
Other promising methods of characterization of coals spontaneous combustion due to oxidation are thermogravimetric analysis (TGA) [8] and differential scanning calorimetry [9]. Despite the fact that these approaches also allow studying of coal in situ, they also have disadvantages, namely, the oxidation effects are observed here at the temperatures much higher than ambient (over 200 °C).
In order to completely describe the behavior of systems prone to spontaneous combustion, one should have sufficient information on the mechanism and kinetics of the characteristic chemical reactions considering also temperature and the conditions of heat loss to the surroundings. The activity of processes in the system depends on numerous factors, including the chemical composition, supramolecular structure, and porosity of the coal, as well as ambient conditions (air humidity, air flow, etc.). Many authors report experimental data on the effects of individual factors on the chemical activity of coal and use them as the basis for kinetic models of self-heating (e.g. see [1,2,10,11,12,13] for review). Although, it seems difficult to develop a complete kinetic model allowing the behavior of coal under real conditions to be predicted.
In order to simplify the description of the self-heating process, the interaction of coal with air is assumed to be a single exothermal reaction. The chemical activity of coal is estimated from apparent kinetic constants of the reaction, namely, the activation energy and the pre-exponential factor. They are commonly estimated using thermal methods [11,12,13,14,15,16,17,18] based on the results of direct laboratory measurements of thermal effects during oxidation. Kinetic constants evaluation within the thermal steady-state method is based on Frank-Kamenetskii (F-K) analysis [19] which was originally developed to determine the critical conditions of spontaneous combustion when the kinetics of the process is known. Thermal methods solve the inverse problem, i.e., determination of the kinetic constants when the parameters corresponding to the critical conditions of the system are known. This requires estimation of the relationship between the characteristic temperature and the critical F-K parameter (δсr) determining the critical conditions under which a steady-state temperature profile in the system becomes impossible. The parameter δсr is preliminarily calculated for the laboratory reactor used in the study; the characteristic temperature is estimated from the results of a thermal experiment on coal heating in the reactor with the temperature on its surface maintained constant.
One of the most useful methods for evaluation of the relationship between δсr and the critical ambient temperature (Ts cr) (at which the temperature at the center of the sample drastically rises) is the traditional steady-state thermal method [3]. The kinetic constants are determined from the plot of versus 1/Tscr (where R is the characteristic size of the reactor) based on experimental data obtained for different sizes of laboratory reactors with the δсr parameter known for each of them. In thermal experiments, the crushed coal in a cylindrical laboratory reactor is placed into an oven where the constant temperature is maintained. The experiments are usually carried out at temperatures above 100 °C, because rapid heat loss to the surroundings of the sample makes it impossible to observe sample heating caused by the exothermal reaction at lower temperatures. It takes a series of thermal experiments to determine the critical temperature for each reactor.
In order to reduce the number of experiments, a transient method (the Chen method) has been proposed [17,18]. The estimation of the kinetic constants in this method is based on determining the rate of temperature change at the center of the reactor at the moment of time when the thermal conduction term of the equation of heat balance near the center becomes zero. The temperature corresponding to this moment is estimated experimentally from the condition of equality of the temperatures at the center and a point near it; it is termed the crossing point temperature. This method is described in detail as applied to cylindrical reactors in the study [17]. In this study, the estimation of the crossing point temperature was based on determining the moment when only the radial component of the thermal conduction term became zero. Strictly speaking, however, the moment when the sum of the radial and vertical components of the thermal conduction term is equal to zero should be used in the calculations. As further development of the Chen method, a procedure has been suggested for estimating the kinetic parameters from the dependence of the dimensionless crossing point temperature (θcpt) on the F-K parameter [19]. This dependence for an infinite slab has been shown to have the form θcpt = 0.1δ.
These transient methods for estimation of the kinetic parameters have allowed the number of experiments to be reduced compared to the steady-state method. The aim of the current work is to present a possibility of the same reduction in the context of the steady-state approach using experiments where critical conditions are not reached. To this end, a modified method for estimation of the kinetic parameters from the temperature at the center of a laboratory reactor in the steady-state mode is proposed. It was also established how the calculated values of the kinetic constants depend on whether or not the oxygen consumption in the oxidation reaction is taken into account.
As noted above, the traditional steady-state approach to the estimation of the kinetic constants requires that the critical conditions characterized by the critical F-K parameter (δсr) be found. These conditions for each reactor are determined in a series of experiments at different temperatures on the sample surface. Let us consider how the results of a thermal experiment where the system goes to a steady state without reaching the critical conditions can be used for determining the kinetic constants. It is suggested that the relationship between the F-K parameter and the dimensionless temperature (θс) is used in the steady-state mode at the center of the laboratory reactor, where heating is the most intense.
Coal heating is described by an unsteady-state energy balance equation for the case of an internal heat source:
$\rho {{C}_{p}}\frac{\partial T}{\partial t}=k\Delta T+QW(T),$ | (1) |
where T is the temperature (K), ρ is the bulk density of coal (kg m−3), Cp specific heat capacity of coal (J kg−1 K−1), k is the thermal conductivity of coal (W m−1 K−1), Q is the heat of oxidation (J kg−1) released as a result of the reaction. It is assumed that the reaction rate depends on temperature according to the Arrhenius law: W(T) = A exp(-E/RgT), where A is the pre-exponential factor (s−1) which includes the concentration of the reagents and E is the apparent activation energy (J mol−1), Rg is the universal gas constant (8.314 J mol−1 K−1). The consumption of the reagents in the course of oxidation is not taken into account, because this would substantially complicate the task. The use of Eq. (1) requires preliminary determination of parameters of the coal, including its density, thermal conductivity, and heat of reaction. In analyzing the results of thermal experiments, it is convenient to go from Eq. (1) to the equation describing the rate of temperature change:
$\frac{\partial T}{\partial t}=a\Delta T+B\exp \left( -E/{{R}_{g}}T \right).$ | (2) |
Here a is the temperature conductivity coefficient (m2/s), B = QA/(Cpρ) is a parameter that includes the constant characterizing the reaction rate and the thermophysical constants of the system (Ks−1); B determines the rate of temperature rise as a result of the exothermal oxidation reaction under adiabatic conditions. Equation (2) allows calculation of the kinetic parameters E and B provided that the coefficient a is known. The number of variables in Eq. (2) can be reduced using the F-K approximation to the Arrhenius term [19]. In order to obtain scaled dimensionless variables the dimensional variables are divided by their scales: length, ξ = x/R, where R is the characteristic size (the radius of the reactor); time, τ = at/R2; and temperature, $\theta =E\left( T-{{T}_{s}} \right)/{{R}_{g}}{{T}_{s}}^{2}$, where Ts is the temperature of the reactor walls. Equation (2) in dimensionless variables takes the form
$\frac{\partial \theta }{\partial t}={{\Delta }_{\xi }}\theta +\delta \exp \left( \theta \right)$ | (3) |
Here, Δξ is the Laplacian operator written in dimensionless variables and $\delta =\frac{E{{R}^{2}}B}{{{R}_{g}}{{T}_{s}}^{2}}\exp \left( -\frac{E}{{{R}_{g}}{{T}_{s}}} \right)$ is the dimensionless F-K parameter. The solutions of Eq. (3) are determined by the F-K parameter. The conditions of combustion are characterized by the critical value δсr. The condition δ = δсr corresponds to the critical state where steady-state distribution becomes impossible. At δ < δсr, a steady-state temperature distribution is formed in the system; at δ > δсr, heat generation exceeds heat loss to the surroundings, which leads to self-heating of the system followed by spontaneous combustion. The parameter δсr is calculated for a given system with known thermophysical parameters and a prespecified geometry.
Following F-K method it is possible to obtain the correlation between parameter and a dimensionless temperature θс in a steady state inside the central point of the laboratory reactor. To do this it is suffice to solve the steady state temperature distribution problem taking into account the chemical reaction:
${{\Delta }_{\xi }}\theta =-\delta {{e}^{\theta }}$ | (4) |
The solution of the equation (4) corresponds to a steady state temperature distribution. Numerical solution of Eq. (4) has yielded the values of the dimensionless temperature at the center of the reactor (θc) at different values of δ for a cylindrical reactor with a height-to-diameter ratio of h/d = 1 (Table 1). The boundary condition at the sample surface is θc = 0. It is convenient to represent the solution of this equation in a plot as the dependence δ = f (θc) (Fig.1, curve 1). It is possible to approximate this dependence with the function
$\delta =3.15(1-\exp \left( -\theta /0.55 \right)),$ | (5) |
where $\delta =\frac{E{{R}^{2}}B}{{{T}_{s}}^{2}{{R}_{g}}a}\exp \left( -\frac{E}{{{T}_{s}}{{R}_{g}}} \right)$ and $\theta =\frac{E\left( {{T}_{C}}-{{T}_{S}} \right)}{{{T}_{s}}^{2}{{R}_{g}}}$, Tc is the temperature at the center of the reactor in the steady-state mode, TS is the temperature of the reactor walls. Figure 1 also shows the relation between dimensionless temperature (θc) and δ for cylindrical reactors with h/d = 2 and h/d = 5 (Fig.1, curves 2 and 3, respectively). The parameters of the equation δ = f(θc) have been found for δ<δcr, i.e., for the case where critical conditions have not been reached. The critical values of the F-K parameter for cylindrical reactors with finite length can be obtained by solving the equation (4) numerically. In the extreme case of h $\gg $ d, the parameter δcr should approach the critical value for an infinite cylinder, δcr = 2 [19].
δ | θC | δ | θC |
0 | 0 | 2.1 | 0.664 |
0.25 | 0.052 | 2.2 | 0.7242 |
0.5 | 0.1082 | 2.3 | 0.792 |
0.75 | 0.1693 | 2.4 | 0.8704 |
1 | 0.2365 | 2.5 | 0.9644 |
1.25 | 0.3112 | 2.6 | 1.0842 |
1.5 | 0.3956 | 2.65 | 1.1617 |
1.75 | 0.4932 | 2.7 | 1.2615 |
2 | 0.6098 | 2.75 | 1.4143 |
The explicit form of the equation F(δ, θc) = 0 in the unknown parameters E and B is obtained by substituting the expressions for δ and θ into Eq. (5). The temperature at the center of the reactor (Tc) when the steady-state mode is established should be estimated from the results of a thermal experiment under the conditions of a constant temperature at the walls (Ts). The experiment should be performed several times at different Ts values. In this way, the pairs of temperatures (Ts1, Tc1), (Ts2, Tc2), etc. are determined. Each (Ts, Tc) pair should be substituted into the equation F(δ, θc) = 0. This yields a set of simultaneous algebraic equations whose solution allows the apparent kinetic constants to be determined.
Let us consider an example where the procedure described above is used to calculate the kinetic parameters E and B for a cylindrical reactor with h/d = 1. The values of the kinetic parameters can be determined from the results of two thermal experiments. The temperatures at the center of the reactor (Tc1 and Tc2) in the steady-state mode can be estimated by numerically solving Eq. (1). The calculations have been performed for a cylindrical reactor with equal height and diameter of h = d = 0.1 m. In this study, the thermophysical parameters have been taken from [17]: E = 101.7 kJ/mol and B = 1.1 * 1011 K/s, a = 1.5 •10-7 m2/s. In our calculations, the temperature at the sample surface has been taken to be Ts1 = 373.15K (100 °C) in the first case and Ts2 =383.15K (110 °C) (in the second case); in the center, the symmetry condition has been assumed to be satisfied. The calculated temperatures at the center of the reactor are Tc1 = 376.05K (102.9 °C) and Tc2 = 392.85K (119.7 °C), respectively.
In order to determine the parameters E and B, let us rewrite Eq. (5) explicitly:
$\frac{E{{R}^{2}}B}{{{T}_{s}}^{2}{{R}_{g}}a}\exp \left( -\frac{E}{{{T}_{s}}{{R}_{g}}} \right)=3.15(1-\exp \left( -\frac{E\left( {{T}_{C}}-{{T}_{S}} \right)}{0.55\cdot {{T}_{s}}^{2}{{R}_{g}}} \right)),$ | (6) |
which allows us to substitute the temperatures (Ts1, Tc1) and (Ts2, Tc2). The result is a system of two equations with two unknowns, E and B. By dividing the first equation of the set of equations by the second we will get the equation in only one unknown E. It is convenient to solve this equation using a graphical calculation. Then we will evaluate the parameter B. The following kinetic parameters were obtained using this procedure for the aforementioned system of equations: E = 99.7 kJ/mol and B = 1 * 1011 K/s. The value of the activation energy obtained by solving the inverse problem differs from that used in calculating the temperature by about 1%.
For a discriminating comparison between the temperatures used in Chen's method and in a proposed method we consider the temperature profiles in the reactor for the cases when the crossing point temperature occurs (Fig.2, curve 1) and when the steady state is established (Fig.2, curve 2) at 110 °C (Ts). As seen from Fig.2, in an experiment where critical conditions are not reached, the crossing point temperature only slightly differs from the temperature at the reactor wall, which is inconvenient for analysis of the experimental data. The temperature at the center of the reactor in the steady-state mode is much higher; therefore, it is more suitable to use this value as a characteristic temperature.
In our modified method for estimating the kinetic constants of coal oxidation, the temperature in the steady-state mode, where the critical conditions are not reached, serves as a characteristic temperature. One should only experimentally measure the temperature at the center of the sample and know the temperature conductivity coefficient to determine the unknown parameters.
The solution of the heat conductivity Eq. (1) yields the relationships from which the kinetic constants can only be determined if the concentrations of the reagents are assumed to be constant. This limits the use of thermal methods based on the F-K analysis. To use this approximation, one should estimate the conditions of its applicability. For this purpose, let us recalculate the temperature in the sample during the heating, now with the oxygen consumption in the oxidation reaction taken into account. It is assumed that there is no forced convection, oxygen transport being accounted for by molecular diffusion.
Let us consider heating of coal in a cylindrical basket-type reactor, which ensures air supply to the coal. Numerical calculations will be performed for a system with the same parameters as in the system considered above, where the oxygen expenditure was not taken into consideration. It is assumed that, at the initial moment of time, oxygen is evenly distributed in the pores between granules throughout the rector. The coal in the reactor is considered as a quasi-homogeneous medium with an effective coefficient of diffusion. The initial oxygen concentration in the sample (C0) is determined from the condition of equilibrium with the ambient air; the porosity factor is assumed to be 30%.
Within the quasi-homogeneous approximation, the process of heating is described by the equations of thermal conduction and diffusion containing a reaction term; the reaction is assumed to be of the first order with respect to oxygen:
$ρCp∂T∂t=k∇2T+QAexp(−ERgT)⋅CC0,ε∂C∂t=D∇2C−Aexp(−ERgT)⋅CC0. $
|
(7) |
Where C is the oxygen concentration (mol L−1) (it is taken into consideration that the pre-exponential factor includes the concentration C0); D is the diffusion coefficient in the porous medium, ε - porosity. The system of equations (7) was numerically solved under the boundary conditions of constant temperature Ts and oxygen concentration C0. In the calculations, the kinetic parameters of the coal from the study [17] (see above) was used; it is suggested that they correspond to the characteristic of coal saturated with oxygen. The temperatures at the surface of the sample were specified as Ts1 = 373.15 K (100 °C) and Ts2 = 383.15K (110 °C).
The calculations have shown that, when the steady-state mode has been reached, the oxygen concentration in the center of the sample is decreased by about 4% in the first case and about 10% in the second case (Fig.3, curve 1). This oxygen "deficit" leads to a decrease in temperature. In the steady-state mode, the temperature is settled at Tc1 = 375.95K (102.8 °C) and Tc2 = 391.75 K (118.6 °C) in the first and second cases, respectively (Fig.3, curve 2). For comparison, the respective temperatures obtained for this system without oxygen consumption taken into account are 376.05K and 392.85K (see above).
Let us estimate how the decrease in the Tc-Ts value due to the decrease in oxygen concentration affects the values of the kinetic constants calculated by the modified method. For this purpose, let us use the temperatures (Ts1, Tc1) and (Ts2, Tc2) calculated with the oxygen consumption in the sample taken into account. The kinetic parameters determined by our method are E = 100 kJ/mol and B = 1.3·1011 K/s. This example shows that the consideration of the change in Tc due to oxygen consumption under the given conditions only slightly affects the values of the kinetic constants calculated by the modified method. In the general case, a thermal experiment should be carried out under the conditions that ensure a negligibly small consumption of the reagents.
The modified method proposed here allows the kinetic constants of coal oxidation to be determined from the temperatures at the center and surface of the sample in a steady-state mode, where the critical conditions are not reached. The method is based on the dependence of the dimensionless temperature on the F-K parameter. This approach makes it possible to substantially reduce the number of experiments compared to the traditional steady-state method. The kinetic constants evaluation procedure was shown for the case of numerical experiment (as an example).
The work was supported by the Federal Target Program "Research and development on priority directions of Russia scientific-technological complex for 2014-2020", event 1.2. Unique identifier of the project RFMEF157514X0062.
All authors declare no conflicts of interest in this paper
[1] | Busca G, Lietti L, Ramis G, et al. (1998) Chemical and mechanistic aspects of the selective catalytic reduction of NOx by ammonia over oxide catalysts: A review. Appl Catal B-Environ 18: 1-36. |
[2] |
Roy S, Hegde MS, Madras G (2009) Catalysis for NOx abatement. Appl Energ 86: 2283-2297. doi: 10.1016/j.apenergy.2009.03.022
![]() |
[3] |
Kompio PGWA, Bruckner A, Hipler F, et al. (2012) A new view on the relations between tungsten and vanadium in V2O5-WO3/TiO2 catalysts for the selective reduction of NO with NH3. J Catal 286: 237-247. doi: 10.1016/j.jcat.2011.11.008
![]() |
[4] | Balle P, Geiger B, Kureti S (2009) Selective catalytic reduction of NOx by NH3 on Fe/HBEA zeolite catalysts in oxygen-rich exhaust. Appl Catal B-Environ 85: 109-119. |
[5] |
Li L, Diao YF, Liu X (2014) Ce-Mn mixed oxides supported on glass-fiber for low-temperature selective catalytic reduction of NO with NH3. J Rare Earth 32: 409-415. doi: 10.1016/S1002-0721(14)60086-7
![]() |
[6] |
Lee SM, Kim SS, Hong SC (2012) Systematic mechanism study of the high temperature SCR of NOx by NH3 over a W/TiO2 catalyst. Chem Eng Sci 79: 177-185. doi: 10.1016/j.ces.2012.05.032
![]() |
[7] |
Garcia-Bordeje E, Pinilla JL, Lazaro MJ, et al. (2005) Role of sulphates on the mechanism of NH3-SCR of NO at low temperatures over presulphated vanadium supported on carbon-coated monoliths. J Catal 233: 166-175. doi: 10.1016/j.jcat.2005.04.032
![]() |
[8] |
Bai HL, Lee SH, Lin CH, et al. (2001) Field study, design, and catalyst cost of selective catalytic reduction process. J Environ Eng-Asce 127: 735-740. doi: 10.1061/(ASCE)0733-9372(2001)127:8(735)
![]() |
[9] |
Bai HL, Chwu JW (1997) Theoretical analysis of selective catalytic reduction catalysts. J Environ Eng-Asce 123: 431-436. doi: 10.1061/(ASCE)0733-9372(1997)123:5(431)
![]() |
[10] |
Chen L, Si ZC, Wu XD, et al. (2014) Rare earth containing catalysts for selective catalytic reduction of NOx with ammonia: A Review. J Rare Earth 32: 907-917. doi: 10.1016/S1002-0721(14)60162-9
![]() |
[11] | Singoredjo L, Korver R, Kapteijn F, et al. (1992) Alumina Supported Manganese Oxides for the Low-Temperature Selective Catalytic Reduction of Nitric-Oxide with Ammonia. Appl Catal B-Environ 1: 297-316. |
[12] | Kapteijn F, Singoredjo L, Andreini A, et al. (1994) Activity and Selectivity of Pure Manganese Oxides in the Selective Catalytic Reduction of Nitric-Oxide with Ammonia. Appl Catal B-Environ 3: 173-189. |
[13] | Smirniotis PG, Pena DA, Uphade BS (2001) Low-temperature selective catalytic reduction (SCR) of NO with NH3 by using Mn, Cr, and Cu oxides supported on Hombikat TiO2. Angew Chem Int Edit 40: 2479-+. |
[14] | Shen BX, Wang YY, Wang FM, et al. (2014) The effect of Ce-Zr on NH3-SCR activity over MnOx(0.6)/Ce0.5Zr0.5O2 at low temperature. Chem Eng J 236: 171-180. |
[15] |
Zhao WR, Tang Y, Wan YP, et al. (2014) Promotion effects of SiO2 or/and Al2O3 doped CeO2/TiO2 catalysts for selective catalytic reduction of NO by NH3. J Hazard Mater 278: 350-359. doi: 10.1016/j.jhazmat.2014.05.071
![]() |
[16] | Thirupathi B, Smirniotis PG (2011) Co-doping a metal (Cr, Fe, Co, Ni, Cu, Zn, Ce, and Zr) on Mn/TiO2 catalyst and its effect on the selective reduction of NO with NH3 at low-temperatures. Appl Catal B-Environ 110: 195-206. |
[17] |
Wu ZB, Jin RB, Wang HQ, et al. (2009) Effect of ceria doping on SO2 resistance of Mn/TiO2 for selective catalytic reduction of NO with NH3 at low temperature. Catal Commun 10: 935-939. doi: 10.1016/j.catcom.2008.12.032
![]() |
[18] | Xie GY, Liu ZY, Zhu ZP, et al. (2004) Simultaneous removal of SO2 and NOx from flue gas using a CuO/Al2O3 catalyst sorbent I. Deactivation of SCR activity by SO2 at low temperatures. J Catal 224: 36-41. |
[19] | Kijlstra WS, Biervliet M, Poels EK, et al. (1998) Deactivation by SO2 of MnOx/Al2O3 catalysts used for the selective catalytic reduction of NO with NH3 at low temperatures. Appl Catal B-Environ 16: 327-337. |
[20] | Huang JH, Tong ZQ, Huang Y, et al. (2008) Selective catalytic reduction of NO with NH3 at low temperatures over iron and manganese oxides supported on mesoporous silica. Appl Catal B-Environ 78: 309-314. |
[21] | Shu Y, Aikebaier T, Quan X, et al. (2014) Selective catalytic reaction of NOx with NH3 over Ce-Fe/TiO2-loaded wire-mesh honeycomb: Resistance to SO2 poisoning. Appl Catal B-Environ 150: 630-635. |
[22] | Yu J, Guo F, Wang YL, et al. (2010) Sulfur poisoning resistant mesoporous Mn-base catalyst for low-temperature SCR of NO with NH3. Appl Catal B-Environ 95: 160-168. |
[23] | Liu FD, Asakura K, He H, et al. (2011) Influence of sulfation on iron titanate catalyst for the selective catalytic reduction of NOx with NH3. Appl Catal B-Environ 103: 369-377. |
[24] | Kwon DW, Nam KB, Hong SC (2015) The role of ceria on the activity and SO2 resistance of catalysts for the selective catalytic reduction of NOx by NH3. Appl Catal B-Environ 166: 37-44. |
[25] |
Tang XL, Hao JM, Xu WG, et al. (2007) Low temperature selective catalytic reduction of NOx with NH3 over amorphous MnOx catalysts prepared by three methods. Catal Commun 8: 329-334. doi: 10.1016/j.catcom.2006.06.025
![]() |
[26] | Jin RB, Liu Y, Wang Y, et al. (2014) The role of cerium in the improved SO2 tolerance for NO reduction with NH3 over Mn-Ce/TiO2 catalyst at low temperature. Appl Catal B-Environ 148: 582-588. |
[27] |
Jin RB, Liu Y, Wu ZB, et al. (2010) Relationship between SO2 poisoning effects and reaction temperature for selective catalytic reduction of NO over Mn-Ce/TiO2 catalyst. Catal Today 153: 84-89. doi: 10.1016/j.cattod.2010.01.039
![]() |
[28] |
Wang YL, Li XX, Zhan L, et al. (2015) Effect of SO2 on Activated Carbon Honeycomb Supported CeO2-MnOx Catalyst for NO Removal at Low Temperature. Ind Eng Chem Res 54: 2274-2278. doi: 10.1021/ie504074h
![]() |
[29] |
Sheng ZY, Hu YF, Xue JM, et al. (2012) SO2 poisoning and regeneration of Mn-Ce/TiO2 catalyst for low temperature NOx reduction with NH3. J Rare Earth 30: 676-682. doi: 10.1016/S1002-0721(12)60111-2
![]() |
[30] | Kato A, Matsuda S, Kamo T, et al. (1981) Reaction between Nox and Nh3 on Iron Oxide-Titanium Oxide Catalyst. J Phys Chem 85: 4099-4102. |
[31] | Duffy BL, Curryhyde HE, Cant NW, et al. (1994) Isotopic Labeling Studies of the Effects of Temperature, Water, and Vanadia Loading on the Selective Catalytic Reduction of No with Nh3 over Vanadia-Titania Catalysts. J Phys Chem 98: 7153-7161. |
[32] |
Heck RM, Chen JM, Speronello BK (1994) Operating Characteristics and Commercial Operating Experience with High-Temperature Scr Nox Catalyst. Environmental Progress 13: 221-225. doi: 10.1002/ep.670130410
![]() |
[33] |
Koebel M, Madia G, Elsener M (2002) Selective catalytic reduction of NO and NO2 at low temperatures. Catal Today 73: 239-247. doi: 10.1016/S0920-5861(02)00006-8
![]() |
[34] | Amblard M, Burch R, Southward BWL (1999) The selective conversion of ammonia to nitrogen on metal oxide catalysts under strongly oxidising conditions. Appl Catal B-Environ 22: L159-L166. |
[35] |
Lippits MJ, Gluhoi AC, Nieuwenhuys BE (2008) A comparative study of the selective oxidation of NH3 to N-2 over gold, silver and copper catalysts and the effect of addition of Li2O and CeOx. Catal Today 137: 446-452. doi: 10.1016/j.cattod.2007.11.021
![]() |
[36] |
Deboer M, Huisman HM, Mos RJM, et al. (1993) Selective Oxidation of Ammonia to Nitrogen over Sio2-Supported Moo3 Catalysts. Catal Today 17: 189-200. doi: 10.1016/0920-5861(93)80023-T
![]() |
[37] |
Tuenter G, Vanleeuwen WF, Snepvangers LJM (1986) Kinetics and Mechanism of the Nox Reduction with Nh3 on V2o5-Wo3-Tio2 Catalyst. Ind Eng Chem Prod Res Dev 25: 633-636. doi: 10.1021/i300024a607
![]() |
[38] |
Kang M, Park ED, Kim JM, et al. (2007) Manganese oxide catalysts for NOx reduction with NH3 at low temperatures. Appl Catal a-Gen 327: 261-269. doi: 10.1016/j.apcata.2007.05.024
![]() |
[39] | Hu H, Cai SX, Li HR, et al. (2015) In Situ DRIFTs Investigation of the Low-Temperature Reaction Mechanism over Mn-Doped Co3O4 for the Selective Catalytic Reduction of NOx with NH3. J Phys ChemC 119: 22924-22933. |
[40] |
Zhou GY, Zhong BC, Wang WH, et al. (2011) In situ DRIFTS study of NO reduction by NH3 over Fe-Ce-Mn/ZSM-5 catalysts. Catal Today 175: 157-163. doi: 10.1016/j.cattod.2011.06.004
![]() |
[41] |
Shu Y, Sun H, Quan X, et al. (2012) Enhancement of Catalytic Activity Over the Iron-Modified Ce/TiO2 Catalyst for Selective Catalytic Reduction of NOx with Ammonia. J Phys Chem C 116: 25319-25327. doi: 10.1021/jp307038q
![]() |
[42] |
Wang WC, McCool G, Kapur N, et al. (2012) Mixed-Phase Oxide Catalyst Based on Mn-Mullite (Sm, Gd)Mn2O5 for NO Oxidation in Diesel Exhaust. Science 337: 832-835. doi: 10.1126/science.1225091
![]() |
[43] |
Ruggeri MP, Grossale A, Nova I, et al. (2012) FTIR in situ mechanistic study of the NH3-NO/NO2 "Fast SCR" reaction over a commercial Fe-ZSM-5 catalyst. Catal Today 184: 107-114. doi: 10.1016/j.cattod.2011.10.036
![]() |
[44] | Jiang BQ, Li ZG, Lee SC (2013) Mechanism study of the promotional effect of O-2 on low-temperature SCR reaction on Fe-Mn/TiO2 by DRIFT. Chem Eng J 225: 52-58. |
[45] |
Yang SJ, Xiong SC, Liao Y, et al. (2014) Mechanism of N2O Formation during the Low-Temperature Selective Catalytic Reduction of NO with NH3 over Mn-Fe Spinel. Environ Sci Technol 48: 10354-10362. doi: 10.1021/es502585s
![]() |
[46] |
Long RQ, Yang RT (2002) Reaction mechanism of selective catalytic reduction of NO with NH3 over Fe-ZSM-5 catalyst. J Catal 207: 224-231. doi: 10.1006/jcat.2002.3528
![]() |
[47] | Lin CH, Bai H (2003) Surface acidity over vanadia/titania catalyst in the selective catalytic reduction for NO removal - in situ DRIFTS study. Appl Catal B-Environ 42: 279-287. |
[48] | Qi GS, Yang RT, Chang R (2004) MnOx-CeO2 mixed oxides prepared by co-precipitation for selective catalytic reduction of NO with NH3 at low temperatures. Appl Catal B-Environ 51: 93-106. |
[49] | Yang SJ, Wang CZ, Li JH, et al. (2011) Low temperature selective catalytic reduction of NO with NH3 over Mn-Fe spinel: Performance, mechanism and kinetic study. Appl Catal B-Environ 110: 71-80. |
[50] |
Yang SJ, Fu YW, Liao Y, et al. (2014) Competition of selective catalytic reduction and non selective catalytic reduction over MnOx/TiO2 for NO removal: the relationship between gaseous NO concentration and N2O selectivity. Catal Sc Technol 4: 224-232. doi: 10.1039/C3CY00648D
![]() |
[51] | Qi GS, Yang RT (2003) A superior catalyst for low-temperature NO reduction with NH3. Chem Commun 2003: 848-849. |
[52] |
Hu H, Cai SX, Li HR, et al. (2015) Mechanistic Aspects of deNO(x) Processing over TiO2 Supported Co-Mn Oxide Catalysts: Structure-Activity Relationships and In Situ DRIFTs Analysis. Acs Catalysis 5: 6069-6077. doi: 10.1021/acscatal.5b01039
![]() |
[53] |
Pena DA, Uphade BS, Reddy EP, et al. (2004) Identification of surface species on titania-supported manganese, chromium, and copper oxide low-temperature SCR catalysts. J Phys Chem B 108: 9927-9936. doi: 10.1021/jp0313122
![]() |
[54] |
Ettireddy PR, Ettireddy N, Boningari T, et al. (2012) Investigation of the selective catalytic reduction of nitric oxide with ammonia over Mn/TiO2 catalysts through transient isotopic labeling and in situ FT-IR studies. J Catal 292: 53-63. doi: 10.1016/j.jcat.2012.04.019
![]() |
[55] |
Chen L, Li JH, Ge MF (2009) Promotional Effect of Ce-doped V2O5-WO3/TiO2 with Low Vanadium Loadings for Selective Catalytic Reduction of NOx by NH3. J Phys Chem C 113: 21177-21184. doi: 10.1021/jp907109e
![]() |
[56] |
Jin RB, Liu Y, Wu ZB, et al. (2010) Low-temperature selective catalytic reduction of NO with NH3 over Mn-Ce oxides supported on TiO2 and Al2O3: A comparative study. Chemosphere 78: 1160-1166. doi: 10.1016/j.chemosphere.2009.11.049
![]() |
[57] | Su Y, Dong GJ, Zhao Y, et al. (2015) FeOx-VOx-WOx-MnOx-CeOx/TiO2 as a catalyst for selective catalytic reduction of NOx with NH3 and the role of iron. Indian J Chem Section a-Inorganic Bio-Inorganic Physical Theoretical & Analytical Chemistry 54: 744-751. |
[58] | Kong ZJ, Wang C, Ding ZN, et al. (2015) Enhanced activity of MnxW0.05Ti0.95 (-) O-x(2) (-) (delta) for selective catalytic reduction of NOx with ammonia by self-propagating high-temperature synthesis. Catal Commun 64: 27-31. |
[59] | Putluru SSR, Schill L, Godiksen A, et al. (2016) Promoted V2O5/TiO2 catalysts for selective catalytic reduction of NO with NH3 at low temperatures. Appl Catal B-Environ 183: 282-290. |
[60] |
Xu HD, Zhang QL, Qiu CT, et al. (2012) Tungsten modified MnOx-CeO2/ZrO2 monolith catalysts for selective catalytic reduction of NOx with ammonia. Chem Eng Sci 76: 120-128. doi: 10.1016/j.ces.2012.04.012
![]() |
[61] |
Pappas DK, Boningari T, Boolchand P, et al. (2016) Novel manganese oxide confined interweaved titania nanotubes for the low-temperature Selective Catalytic Reduction (SCR) of NOx by NH3. J Catal 334: 1-13. doi: 10.1016/j.jcat.2015.11.013
![]() |
[62] | Liu FD, He H, Ding Y, et al. (2009) Effect of manganese substitution on the structure and activity of iron titanate catalyst for the selective catalytic reduction of NO with NH3. Appl Catal B-Environ 93: 194-204. |
[63] |
Liu FD, Shan WP, Lian ZH, et al. (2013) Novel MnWOx catalyst with remarkable performance for low temperature NH3-SCR of NOx. Catal Sci Technol 3: 2699-2707. doi: 10.1039/c3cy00326d
![]() |
[64] | Qiu L, Pang DD, Zhang CL, et al. (2015) In situ IR studies of Co and Ce doped Mn/TiO2 catalyst for low-temperature selective catalytic reduction of NO with NH3. Appl Surf Sci 357: 189-196. |
[65] | Magdalena JABŁOŃSKA LC, Agnieszka WĘGRZYN (2013) Selective catalytic oxidation (SCO) of ammonia into nitrogen and water vapour over hydrotalcite originated mixed metal oxides ? a short review. CHEMIK 67: 701-710. |
[66] |
Park KH, Lee SM, Kim SS, et al. (2013) Reversibility of Mn Valence State in MnOx/TiO2 Catalysts for Low-temperature Selective Catalytic Reduction for NO with NH3. Catal Lett 143: 246-253. doi: 10.1007/s10562-012-0952-8
![]() |
[67] | Qu RY, Gao X, Cen KF, et al. (2013) Relationship between structure and performance of a novel cerium-niobium binary oxide catalyst for selective catalytic reduction of NO with NH3. Appl Catal B-Environ142: 290-297. |
[68] |
Kwon DW, Nam KB, Hong SC (2015) Influence of tungsten on the activity of a Mn/Ce/W/Ti catalyst for the selective catalytic reduction of NO with NH3 at low temperatures. Appl Catal a-Gen 497: 160-166. doi: 10.1016/j.apcata.2015.01.013
![]() |
[69] |
Cao F, Xiang J, Su S, et al. (2015) Ag modified Mn-Ce/gamma-Al2O3 catalyst for selective catalytic reduction of NO with NH3 at low-temperature. Fuel Process Technol 135: 66-72. doi: 10.1016/j.fuproc.2014.10.021
![]() |
[70] |
Xu HD, Fang ZT, Cao Y, et al. (2012) Influence of Mn/(Mn plus Ce) Ratio of MnOx-CeO2/WO3-ZrO2 Monolith Catalyst on Selective Catalytic Reduction of NOx with Ammonia. Chinese J Catal 33: 1927-1937. doi: 10.1016/S1872-2067(11)60467-1
![]() |
[71] |
Liu FD, He H, Zhang CB, et al. (2011) Mechanism of the selective catalytic reduction of NOx with NH3 over environmental-friendly iron titanate catalyst. Catal Today 175: 18-25. doi: 10.1016/j.cattod.2011.02.049
![]() |
[72] | Lee SM, Park KH, Hong SC (2012) MnOx/CeO2-TiO2 mixed oxide catalysts for the selective catalytic reduction of NO with NH3 at low temperature. Chem Eng J 195: 323-331. |
[73] |
Wang P, Sun H, Quan X, et al. (2016) Enhanced catalytic activity over MIL-100(Fe) loaded ceria catalysts for the selective catalytic reduction of NOx with NH3 at low temperature. J Hazard Mater 301: 512-521. doi: 10.1016/j.jhazmat.2015.09.024
![]() |
[74] | Cao F, Xiang J, Su S, et al. (2014) The activity and characterization of MnOx-CeO2-ZrO2/gamma-Al2O3 catalysts for low temperature selective catalytic reduction of NO with NH3. Chem Eng J 243: 347-354. |
[75] |
Zhang P, Chen TH, Zou XH, et al. (2014) V2O5/hematite catalyst for low temperature selective catalytic reduction of NOx with NH3. Chinese J Catal 35: 99-107. doi: 10.1016/S1872-2067(12)60719-0
![]() |
[76] |
Zuo JL, Chen ZH, Wang FR, et al. (2014) Low-Temperature Selective Catalytic Reduction of NOx with NH3 over Novel Mn-Zr Mixed Oxide Catalysts. Ind Eng Chem Res 53: 2647-2655. doi: 10.1021/ie404224y
![]() |
[77] |
Li JH, Chang HZ, Ma L, et al. (2011) Low-temperature selective catalytic reduction of NOx with NH3 over metal oxide and zeolite catalysts-A review. Catal Today 175: 147-156. doi: 10.1016/j.cattod.2011.03.034
![]() |
[78] | Apostolescu N, Geiger B, Hizbullah K, et al. (2006) Selective catalytic reduction of nitrogen oxides by ammonia on iron oxide catalysts. Appl Catal B-Environ 62: 104-114. |
[79] |
Shen BX, Liu T, Zhao N, et al. (2010) Iron-doped Mn-Ce/TiO2 catalyst for low temperature selective catalytic reduction of NO with NH3. J Environ Sci-China 22: 1447-1454. doi: 10.1016/S1001-0742(09)60274-6
![]() |
[80] |
Shen BX, Yao Y, Ma HQ, et al. (2011) Ceria Modified MnOx/TiO2-Pillared Clays Catalysts for Selective Catalytic Reduction of NO with NH3 at Low Temperature. Chinese J Catal 32: 1803-1811. doi: 10.1016/S1872-2067(10)60269-0
![]() |
[81] |
Yao Y, Zhang SL, et al. (2011) Low-temperature Selective Catalytic Reduction of NO over Manganese Supported on TiO2 Nanotubes. J Fuel Chem Technol 39: 694-701. doi: 10.1016/S1872-5813(11)60042-X
![]() |
[82] |
Schill L, Putluru SSR, Jensen AD, et al. (2015) MnFe/Al2O3 Catalyst Synthesized by Deposition Precipitation for Low-Temperature Selective Catalytic Reduction of NO with NH3. Catal Lett 145: 1724-1732. doi: 10.1007/s10562-015-1576-6
![]() |
[83] | Qu L, Li CT, Zeng GM, et al. (2014) Support modification for improving the performance of MnOx-CeOy/gamma-Al2O3 in selective catalytic reduction of NO by NH3. Chem Eng J 242: 76-85. |
[84] |
Gao RH, Zhang DS, Liu XG, et al. (2013) Enhanced catalytic performance of V2O5-WO3/Fe2O3/TiO2 microspheres for selective catalytic reduction of NO by NH3. Catal Sci Technol 3: 191-199. doi: 10.1039/C2CY20332D
![]() |
[85] |
Xu WQ, He H, Yu YB (2009) Deactivation of a Ce/TiO2 Catalyst by SO2 in the Selective Catalytic Reduction of NO by NH3. J Phys Chem C 113: 4426-4432. doi: 10.1021/jp8088148
![]() |
[86] |
Yang R, Huang HF, Chen YJ, et al. (2015) Performance of Cr-doped vanadia/titania catalysts for low-temperature selective catalytic reduction of NOx with NH3. Chinese J Catal 36: 1256-1262. doi: 10.1016/S1872-2067(15)60884-1
![]() |
[87] | Huang ZG, Zhu ZP, Liu ZY (2002) Combined effect of H2O and SO2 on V2O5/AC catalysts for NO reduction with ammonia at lower temperatures. Appl Catal B-Environ 39: 361-368. |
[88] |
Huang ZG, Zhu ZP, Liu ZY, et al. (2003) Formation and reaction of ammonium sulfate salts on V2O5/AC catalyst during selective catalytic reduction of nitric oxide by ammonia at low temperatures. J Catal 214: 213-219. doi: 10.1016/S0021-9517(02)00157-4
![]() |
[89] |
Zhu ZP, Liu ZY, Niu HX, et al. (1999) Promoting effect of SO2 on activated carbon-supported vanadia catalyst for NO reduction by NH3 at low temperatures. J Catal 187: 245-248. doi: 10.1006/jcat.1999.2605
![]() |
[90] |
Zhu ZP, Liu ZY, Niu HX, et al. (2001) Mechanism of SO2 promotion for NO reduction with NH3 over activated carbon-supported vanadium oxide catalyst. J Catal 197: 6-16. doi: 10.1006/jcat.2000.3052
![]() |
[91] |
Jiang BQ, Wu ZB, Liu Y, et al. (2010) DRIFT Study of the SO2 Effect on Low-Temperature SCR Reaction over Fe-Mn/TiO2. J Phys Chem C 114: 4961-4965. doi: 10.1021/jp907783g
![]() |
[92] | Chen L, Li JH, Ge MF (2011) The poisoning effect of alkali metals doping over nano V2O5-WO3/TiO2 catalysts on selective catalytic reduction of NOx by NH3. Chem Eng J 170: 531-537. |
[93] | Yu WC, Wu XD, Si ZC, et al. (2013) Influences of impregnation procedure on the SCR activity and alkali resistance of V2O5-WO3/TiO2 catalyst. Appl Surf Sci 283: 209-214. |
[94] |
Putluru SSR, Jensen AD, Riisager A, et al. (2011) Heteropoly acid promoted V2O5/TiO2 catalysts for NO abatement with ammonia in alkali containing flue gases. Catal Sc Technol 1: 631-637. doi: 10.1039/c1cy00081k
![]() |
[95] | Zhang LJ, Cui SP, Guo HX, et al. (2014) The influence of K+ cation on the MnOx-CeO2/TiO2 catalysts for selective catalytic reduction of NOx with NH3 at low temperature. J Mol Catal a-Chem 390: 14-21. |
[96] | Guo RT, Wang QS, Pan WG, et al. (2015) The poisoning effect of Na and K on Mn/TiO2 catalyst for selective catalytic reduction of NO with NH3: A comparative study. Appl Surf Sci 325: 262-262. |
[97] |
Yu YK, Meng XR, Chen JS, et al. (2016) Deactivation mechanism and feasible regeneration approaches for the used commercial NH3-SCR catalysts. Environ Technol 37: 828-836. doi: 10.1080/09593330.2015.1088070
![]() |
[98] | Pourkhalil M, Moghaddam AZ, Rashidi A, et al. (2013) Preparation of highly active manganese oxides supported on functionalized MWNTs for low temperature NOx reduction with NH3. Appl Surf Sci 279: 250-259. |
[99] |
Shen BX, Zhang XP, Ma HQ, et al. (2013) A comparative study of Mn/CeO2, Mn/ZrO2 and Mn/Ce-ZrO2 for low temperature selective catalytic reduction of NO with NH3 in the presence of SO2 and H2O. J Environ Sci-China 25: 791-800. doi: 10.1016/S1001-0742(12)60109-0
![]() |
[100] |
Qi GS, Yang RT (2004) Characterization and FTIR studies of MnOx-CeO2 catalyst for low-temperature selective catalytic reduction of NO with NH3. J Phys ChemB 108: 15738-15747. doi: 10.1021/jp048431h
![]() |
[101] |
Fang D, He F, Mei D, et al. (2014) Thermodynamic calculation for the activity and mechanism of Mn/TiO2 catalyst doped transition metals for SCR at low temperature. Catal Commun 52: 45-48. doi: 10.1016/j.catcom.2014.04.010
![]() |
[102] |
Xie JL, Fang D, He F, et al. (2012) Performance and mechanism about MnOx species included in MnOx/TiO2 catalysts for SCR at low temperature. Catal Commun 28: 77-81. doi: 10.1016/j.catcom.2012.08.022
![]() |
[103] |
Zhang YP, Zhao XY, Xu HT, et al. (2011) Novel ultrasonic-modified MnOx/TiO2 for low-temperature selective catalytic reduction (SCR) of NO with ammonia. J Colloid Interface Sci 361: 212-218. doi: 10.1016/j.jcis.2011.05.012
![]() |
[104] |
Boningari T, Ettireddy PR, Somogyvari A, et al. (2015) Influence of elevated surface texture hydrated titania on Ce-doped Mn/TiO2 catalysts for the low-temperature SCR of NOx under oxygen-rich conditions. J Catal 325: 145-155. doi: 10.1016/j.jcat.2015.03.002
![]() |
[105] |
Jiang BQ, Liu Y, Wu ZB (2009) Low-temperature selective catalytic reduction of NO on MnOx/TiO2 prepared by different methods. J Hazard Mater 162: 1249-1254. doi: 10.1016/j.jhazmat.2008.06.013
![]() |
[106] | Park TS, Jeong SK, Hong SH, et al. (2001) Selective catalytic reduction of nitrogen oxides with NH3 over natural manganese ore at low temperature. Ind Eng Chem Res 40: 4491-4495. |
[107] |
Zhuang K, Qiu J, Tang FS, et al. (2011) The structure and catalytic activity of anatase and rutile titania supported manganese oxide catalysts for selective catalytic reduction of NO by NH3. Phys Chem Chem Phys 13: 4463-4469. doi: 10.1039/c0cp02288h
![]() |
[108] | Chen XB, Cen CP, Tang ZX, et al. (2013) The Key Role of pH Value in the Synthesis of Titanate Nanotubes-Loaded Manganese Oxides as a Superior Catalyst for the Selective Catalytic Reduction of NO with NH3. J Nanomater 2013: 871528. |
[109] |
Pan WG, Hong JN, Guo RT, et al. (2014) Effect of support on the performance of Mn-Cu oxides for low temperature selective catalytic reduction of NO with NH3. J Ind Engin Chem 20: 2224-2227. doi: 10.1016/j.jiec.2013.09.054
![]() |
[110] |
Panahi PN, Niaei A, Tseng HH, et al. (2015) Modeling of catalyst composition-activity relationship of supported catalysts in NH3-NO-SCR process using artificial neural network. Neural Comput Appl 26: 1515-1523. doi: 10.1007/s00521-014-1781-z
![]() |
[111] |
Lv G, Bin F, Song CL, et al. (2013) Promoting effect of zirconium doping on Mn/ZSM-5 for the selective catalytic reduction of NO with NH3. Fuel 107: 217-224. doi: 10.1016/j.fuel.2013.01.050
![]() |
[112] |
Wang X, Zheng YY, Lin JX (2013) Highly dispersed Mn-Ce mixed oxides supported on carbon nanotubes for low-temperature NO reduction with NH3. Catal Commun 37: 96-99. doi: 10.1016/j.catcom.2013.03.035
![]() |
[113] |
Lu XL, Zheng YY, Zhang YB, et al. (2015) Low-temperature selective catalytic reduction of NO over carbon nanotubes supported MnO2 fabricated by co-precipitation method. Micro Nano Lett 10: 666-669. doi: 10.1049/mnl.2015.0247
![]() |
[114] |
Zhang XP, Shen BX, Wang K, et al. (2013) A contrastive study of the introduction of cobalt as a modifier for active components and supports of catalysts for NH3-SCR. J Ind Engin Chem 19: 1272-1279. doi: 10.1016/j.jiec.2012.12.028
![]() |
[115] |
Su W, Lu XN, Jia SH, et al. (2015) Catalytic Reduction of NOX Over TiO2-Graphene Oxide Supported with MnOX at Low Temperature. Catal Lett 145: 1446-1456. doi: 10.1007/s10562-015-1550-3
![]() |
[116] |
Fan XY, Qiu FM, Yang HS, et al. (2011) Selective catalytic reduction of NOx with ammonia over Mn-Ce-O-x/TiO2-carbon nanotube composites. Catal Commun 12: 1298-1301. doi: 10.1016/j.catcom.2011.05.011
![]() |
[117] |
Liu ZM, Yi Y, Zhang SX, et al. (2013) Selective catalytic reduction of NOx with NH3 over Mn-Ce mixed oxide catalyst at low temperatures. Catal Today 216: 76-81. doi: 10.1016/j.cattod.2013.06.009
![]() |
[118] | Fang D, He F, Li D, et al. (2013) First principles and experimental study of NH3 adsorptions on MnOx surface. Appl Surf Sci 285: 215-219. |
[119] | Fang D, Xie JL, Hu H, et al. (2015) Identification of MnOx species and Mn valence states in MnOx/TiO2 catalysts for low temperature SCR. Chem Eng J 271: 23-30. |
[120] |
Li Y, Wan Y, Li YP, et al. (2016) Low-Temperature Selective Catalytic Reduction of NO with NH3 over Mn2O3-Doped Fe2O3 Hexagonal Microsheets. Acs Appl Mater Inter 8: 5224-5233. doi: 10.1021/acsami.5b10264
![]() |
[121] |
Boningari T, Pappas DK, Ettireddy PR, et al. (2015) Influence of SiO2 on MiTiO(2) (M = Cu, Mn, and Ce) Formulations for Low-Temperature Selective Catalytic Reduction of NOx with NH3: Surface Properties and Key Components in Relation to the Activity of NOx Reduction. Ind Eng Chem Res 54: 2261-2273. doi: 10.1021/ie504709j
![]() |
[122] |
Sultana A, Sasaki M, Hamada H (2012) Influence of support on the activity of Mn supported catalysts for SCR of NO with ammonia. Catal Today 185: 284-289. doi: 10.1016/j.cattod.2011.09.018
![]() |
[123] | Zhao WW, Li CT, Lu P, et al. (2013) Iron, lanthanum and manganese oxides loaded on gamma-Al2O3 for selective catalytic reduction of NO with NH3 at low temperature. Environ Technol 34: 81-90. |
[124] |
Smirniotis PG, Sreekanth PM, Pena DA, et al. (2006) Manganese oxide catalysts supported on TiO2, Al2O3, and SiO2: A comparison for low-temperature SCR of NO with NH3. Ind Eng Chem Res 45: 6436-6443. doi: 10.1021/ie060484t
![]() |
[125] |
Wang YL, Ge CZ, Zhan L, et al. (2012) MnOx-CeO2/Activated Carbon Honeycomb Catalyst for Selective Catalytic Reduction of NO with NH3 at Low Temperatures. Ind Eng Chem Res 51: 11667-11673. doi: 10.1021/ie300555f
![]() |
[126] | Zhou CC, Zhang YP, Wang XL, et al. (2013) Influence of the addition of transition metals (Cr, Zr, Mo) on the properties of MnOx-FeOx catalysts for low-temperature selective catalytic reduction of NOx by Ammonia. J Colloid Interface Sci 392: 319-324. |
[127] |
Wang XY, Wu W, Chen ZL, et al. (2015) Bauxite-supported Transition Metal Oxides: Promising Low-temperature and SO2-tolerant Catalysts for Selective Catalytic Reduction of NOx. Scientific Reports 5: 9766. doi: 10.1038/srep09766
![]() |
[128] |
Fang D, Xie JL, Mei D, et al. (2014) Effect of CuMn2O4 spinel in Cu-Mn oxide catalysts on selective catalytic reduction of NOx with NH3 at low temperature. Rsc Advances 4: 25540-25551. doi: 10.1039/c4ra02824d
![]() |
[129] | Zhi-jian KONG CW, Zheng-nan DING, Yin-fei CHEN, Ze-kai ZHANG (2014) Li-modified MnO2 catalyst and LiMn2O4 for selective catalytic reduction of NO with NH3. J Fuel Chem Technol 12: 1447-1454. |
[130] |
Wu ZB, Jin RB, Liu Y, et al. (2008) Ceria modified MnOx/TiO2 as a superior catalyst for NO reduction with NH3 at low-temperature. Catal Commun 9: 2217-2220. doi: 10.1016/j.catcom.2008.05.001
![]() |
[131] | Liu L, Gao X, Song H, et al. (2014) Study of the Promotion Effect of Iron on Supported Manganese Catalysts for No Oxidation. Aerosol Air Qual Res 14: 1038-1046. |
[132] |
Shen BX, Liu T, Zhao N, et al. (2010) Iron-doped Mn-Ce/TiO2 catalyst for low temperature selective catalytic reduction of NO with NH3. J Environ Sci 22: 1447-1454. doi: 10.1016/S1001-0742(09)60274-6
![]() |
[133] | Shen K, Zhang YP, Wang XL, et al. (2013) Influence of chromium modification on the properties of MnOx-FeOx catalysts for the low-temperature selective catalytic reduction of NO by NH3. J Energ Chem 22: 617-623. |
[134] | Gu TT, Jin RB, Liu Y, et al. (2013) Promoting effect of calcium doping on the performances of MnOx/TiO2 catalysts for NO reduction with NH3 at low temperature. Appl Catal B-Environ 129: 30-38. |
[135] |
Thirupathi B, Smirniotis PG (2012) Nickel-doped Mn/TiO2 as an efficient catalyst for the low-temperature SCR of NO with NH3: Catalytic evaluation and characterizations. J Catal 288: 74-83. doi: 10.1016/j.jcat.2012.01.003
![]() |
[136] |
Zhang SL, Liu XX, Zhong Q, et al. (2012) Effect of Y doping on oxygen vacancies of TiO2 supported MnOX for selective catalytic reduction of NO with NH3 at low temperature. Catal Commun 25: 7-11. doi: 10.1016/j.catcom.2012.03.026
![]() |
1. | C. W. Chukwu, M. L. Juga, Z. Chazuka, J. Mushanyu, Mathematical Analysis and Sensitivity Assessment of HIV/AIDS-Listeriosis Co-infection Dynamics, 2022, 8, 2349-5103, 10.1007/s40819-022-01458-3 | |
2. | Hengki Tasman, Dipo Aldila, Putri A. Dumbela, Meksianis Z. Ndii, Faishal F. Herdicho, Chidozie W. Chukwu, Assessing the Impact of Relapse, Reinfection and Recrudescence on Malaria Eradication Policy: A Bifurcation and Optimal Control Analysis, 2022, 7, 2414-6366, 263, 10.3390/tropicalmed7100263 | |
3. | Dipo Aldila, Basyar Lauzha Fardian, Chidozie Williams Chukwu, Muhamad Hifzhudin Noor Aziz, Putri Zahra Kamalia, Improving tuberculosis control: assessing the value of medical masks and case detection—a multi-country study with cost-effectiveness analysis, 2024, 11, 2054-5703, 10.1098/rsos.231715 | |
4. | Lin Hu, Linfei Nie, Stability and Hopf Bifurcation Analysis of a Multi-Delay Vector-Borne Disease Model with Presence Awareness and Media Effect, 2023, 7, 2504-3110, 831, 10.3390/fractalfract7120831 | |
5. | C.W. Chukwu, S.Y. Tchoumi, M.L. Diagne, A simulation study to assess the epidemiological impact of pneumonia transmission dynamics in high-risk populations, 2024, 10, 27726622, 100423, 10.1016/j.dajour.2024.100423 | |
6. | Dipo Aldila, Nadya Awdinda, Faishal F. Herdicho, Meksianis Z. Ndii, Chidozie W. Chukwu, Optimal control of pneumonia transmission model with seasonal factor: Learning from Jakarta incidence data, 2023, 9, 24058440, e18096, 10.1016/j.heliyon.2023.e18096 |
δ | θC | δ | θC |
0 | 0 | 2.1 | 0.664 |
0.25 | 0.052 | 2.2 | 0.7242 |
0.5 | 0.1082 | 2.3 | 0.792 |
0.75 | 0.1693 | 2.4 | 0.8704 |
1 | 0.2365 | 2.5 | 0.9644 |
1.25 | 0.3112 | 2.6 | 1.0842 |
1.5 | 0.3956 | 2.65 | 1.1617 |
1.75 | 0.4932 | 2.7 | 1.2615 |
2 | 0.6098 | 2.75 | 1.4143 |