Figure 1. NOx conversion of NMO as function of time at 423 K : (a) NO conversion, (b) NO2 concentration, (c) NH3 concentration (S.V. : 30,000 h-1, NO : 424 ppm, NO2 : 7 ppm, NH3 : 480 ppm).
Figure 2. Grid of experimental conditions for NO and NH3 at 3 kPa of O2 carried out at 393, 423, and 455 K : NMO, MnO2, Mn2O3. (Exp. Condition: Loaded Cat.: 25 , 50, 100 mg Temp : 393, 423, 455 K, Variable : PNO, PNH3, PO2)
Figure 3. Observed NO conversion as a function of the space time for various partial pressures at 423 K : (a) NMO, (b) MnO3, (c) Mn2O3. (PNH3: 40.5 Pa, PO2: 3 kPa).
Figure 4. Observed NO conversion as a function of a partial NH3 pressure for various space times at 423 K : (a) NMO, (b) MnO3, (c) Mn2O3. (PO2 : 3 kPa, PNO : 40.5 Pa).
Figure 5. Observed NO conversion as a function of a partial O2 pressure for various space times at 423 K : (a) NMO, (b) MnO3, (c) Mn2O3. (PNH3: 40.5 Pa, PNO: 40.5 Pa).
Figure 6. The dependence of the NO conversion on the temperature over (a) NMO, (b) MnO3, (c) Mn2O3 (loaded cat: 50 mg, PNH3 : 40.5 Pa, PNH3 : 40.5 pa, PO2 : 3 kPa).
Figure 7. Error as a function of calculated rate at 393 K : (a) NMO, (b) MnO3, (c) Mn2O3.
Table 1. The experimental conditions
Table 2. Thermal stabilities absorbed NO complexes
Table 3. Reaction orders of Mn oxides
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