Rates and products of the (3 + α)NO + CH4 ⇒ 1/2(3 + α)N2 + (1 − α)CO + αCO2 + 2H2O (0 ≤ α ≤ 1)
reaction were determined in low-pressure (NO/CH4/O2) mixtures ([NO] < 1 μM, [CH4] < 10[NO], [O2] ≤
[NO]; 1 μM = 82 ppm at 1 atm, 1000 K) flowing over Sm2O3 between 1000 and 1200 K. Samaria pretreated
with CH4 (or H2) at reaction temperatures instantly releases N2 when exposed to NO. Prompt CO formation
also occurs on methane-conditioned samples. In contrast, stationary outflow gas compositions attain only
after several reactor residence times following step (NO + CH4) injections to the untreated catalyst. Nitric
oxide reduction rates R
-
NO are roughly proportional to ([CH4] × [NO])1/2 but do not extrapolate to zero at
[NO] → 0 and always increase with T. We infer that: (1) there is no direct reaction between CH4 and NO
on the catalyst surface; (2) instead, NO is reduced to N2 by reaction with oxygen vacancies V, and with
nonvolatile carbon-containing Cs species created in the heterogeneous oxidation/decomposition of CH4,
respectively; (3) the entire mass, rather than just the surface, of catalyst microparticles participate in this
phenomenon. We propose a purely heterogeneous mechanism in which physisorbed NO reacts with either
vacancies in equilibrium with the active oxygen OR species responsible for CH4 oxidation or with Cs species.
The derived kinetic law: R
-
NO = k
A([NO]s[CH4])1/2 + k
B[CH4], with [NO]s = [NO]/(K
8
-1 + [NO]), in
conjunction with the reported Arrhenius parameters, closely fits rates measured under anoxic conditions.
The fact that R
-
NO is unaffected by O2 up to F
O
2
∼ 0.3F
NO but drops at larger F
O
2
inflows, even if O2 is fully
consumed in CH4 oxidation, is consistent with the competition of NO and O2 for vacancies. The dissimilar
observations made in experiments performed in the Torr range strongly suggest that solid catalysts promote
combustion at such relatively high pressures.