Reaction of silver(I) oxide with nitrogen monoxide

Abstract

The reaction of Ag₂O with NO has been studied in the range 333–473 K with flow and batch reactors. The reaction products are Ag[NO₂], Ag[NO₃], Ag, and NO₂. A change in the products with reaction times reveals that [AgNO₂] is the primary product by reaction (i), Ag₂O + NO → Ag[NO₂]+ Ag, and then decomposes to Ag[NO₃] with the evolution of NO by reaction (ii), 2 Ag[NO₂]→ Ag[NO₃]+ Ag + NO. When Ag[NO₂] is a starting material, reaction (iii), Ag[NO₂]→ Ag + NO₂, occurs together with (ii). Reaction (i) occurs mainly at ⩽353 K and the reaction order with respect to [NO] is close to unity. Reactions (ii) and (iii) proceed at 353 K and are inhibited by NO. At 453 K in the flow system, Ag[NO₃] reacts further with NO through (iv), Ag[NO₃]+ NO → Ag + 2NO₂. In the static system, on the other hand, (iv) does not proceed. This difference is suggested to result from NO₂ inhibition of reaction (iv).