Nitric oxide (NO) reduction by methanol was studied over La2O3 in the presence and absence of oxygen. In the absence of O-2, CH3OH reduced NO to both N2O and N-2, with selectivity to dinitrogen formation decreasing from around 85% at 623 K to 50-70% at 723 K. With 1% O-2 in the feed, rates were 4-8 times higher, but the selectivity to N-2 dropped from 50% at 623 K to 10% at 723 K. The specific activities with La2O3 for this reaction were higher than those for other reductants; for example, at 773 K with hydrogen a specific activity of 35 mu mol NO/s m(2) was obtained whereas that for methanol was 600 mu mol NO/s m(2). The Arrhenius plots were linear under differential reaction conditions, and the apparent activation energy was consistently near 14 kcal/mol with CH3OH. Linear partial pressure dependencies based on a power rate law were obtained and showed a near-zero order in CH3OH and a near-first order in H-2. In the absence of O-2, a Langmuir-Hinshelwood type model assuming a surface reaction between adsorbed CH3OH and adsorbed NO as the slow step satisfactorily fitted the data, and the model invoking two types of sites provided the best fit and gave thermodynamically consistent rate constants. In the presence of O-2 a homogeneous gas-phase reaction between O-2, NO, and CH3OH occurred to yield methyl nitrite. This reaction converted more than 30% of the methanol at 300 K and continued to occur up to temperatures where methanol was fully oxidized. Quantitative kinetic studies of the heterogeneous reaction with O-2 present were significantly complicated by this homogeneous reaction.