Ammonia (NH3) is the primary feedstock for the manufacture of nitric acid and ammonium nitrate in chemical industries. The ammonia combustion is performed using a platinum catalyst at temperatures ranging from 800 to 900 °C in the presence of air to generate nitrogen oxides, principally NO, which is then progressively oxidised to nitric oxide absorber towers. This combustion process is one of the significant contributors to ozone depletion and global warming because it generates considerable amounts of N2O as a by-product. The decomposition of N2O has been widely researched over the last couple of decades. However, the catalytic decomposition of N2O still poses a great challenge. Considerable research has shown that a bed of Co3O4 catalyst above the Pt catalyst may decrease the formation of N2O. However, there is still a dearth of detailed knowledge about the promotion and activity of Pt, which is required to manipulate and then improve the reaction. This study is important because it highlights the combustion of NH3 as a critical step in the production of nitric monoxide (NO), which is subsequently used to produce nitric acid (HNO3) at an industrial scale. Until recently, pure oxygen, rather than air, has been employed as the oxidant in the burner, with steam acting as the thermal ballast; an alternative is the use of air in a process patented by Orica in collaboration with the University of Sydney (aka the JOHANNA Process). Extensive laboratory testing has confirmed the favourable operating characteristics of this process, including the achievement of low selectivity towards N2O. This study explores a methodology for simulating the kinetics of NH3 combustion on platinum surfaces with improved kinetic data and evaluating the conditions in which NH3 is oxidised to NO using O2. The NH3 combustion on Pt surfaces was mathematically simulated using Chemkin-Pro, where atomic chemistry and microkinetics serve as the foundation of the modelling. Atomic chemistry concepts were initially applied to propose elementary reactions in order to build a frame of the NH3 combustion’s reaction system. Microkinetics provided a method that was used to calculate the rates of reactions. Hence, the rates of reactions were obtained from the modelling, which indicated the performance of the reaction and also the catalyst. The kinetics of each reaction step was derived from a number of published resources, with the basic assumption that the initial reaction pathways stem from the parallel reactions between chemisorbed NH3 and oxygen. Density functional theory computations were also carried out when the data was either not available or was uncertain, especially when evaluating the coverage dependence on the thermodynamics of the surface species. The reaction mechanism of NH3 combustion involves several elementary steps that were studied in this work in terms of three different sub-mechanisms; these are presented schematically in Figure 1. Figure 1. Schematic representation of the NH3 reactions over platinum that are analysed in the present work. a) Nitrogen oxide decomposition, b) NH3 decomposition and NH3 combustion The thermodynamic parameters of the adsorbed species on Pt(111) and Pt(211) were obtained by applying the density functional theory at the PBE and HSE06; these parameters were properly presented using the NIST polynomial form, a format that is used in several engineering codes to study the reactivity, mass and heat transfer of catalytic processes. The kinetic parameters of the reaction were obtained via proper computational methods (CI-NEB and Dimer). The effect of the coverage dependence on NH3 conversion and yield of products was analysed in detail. This microkinetic model can account for ammonia decomposition in the absence of oxygen, and the accuracy of its results can be improved by considering lateral interactions in the form of coverage dependence. Some of the important surface species show stability in the temperature regions where previous experimental observations have been determined. We observed large uncertainties in describing the reactions in which O2 is a reactant, specifically in case of NO decomposition and NH3 oxidation. Such large uncertainties could have resulted from the improper treatment of complicated surface species such as O*, N*, and NO*. The calculated enthalpy of formation for each of this species varies by more than 50 kJ mol–1 when PBE and HSE06 are used. Additionally, the enthalpy of formation for almost all intermediates in the reaction changes very rapidly with small changes in the coverage, making the model highly dependent on the dynamic behaviour of the rate of reaction. The NH3 combustion starts at 300 oC, which is only 100 oC above the previous experimental observations. At low temperatures, the selectivity towards N2(g) is the highest, and NO(g) becomes the predominant product above 600 oC, as consistent with experimental observations. In effect, NO decomposition under the industrial conditions of NH3 combustion is very slow, but with a high selectivity towards N2(g).