Gas-phase oxidation of nitric oxide: Chemical kinetics and rate constant

Inhaled nitric oxide (NO) is gaining popularity as a selective pulmonary vasodilator. Because of the potential toxicity of NO and its oxidizing product nitrogen dioxide (NO2), any system for the delivery of inhaled NO must aim at predictable and reproducible levels of NO and at as low concentrations of NO2 as possible. This review describes the chemical kinetics and rate constant values k for the reaction 2NO + O-2 = 2NO(2). This reaction has been well established as a third-order homogeneous reaction. Published data support two equally plausible two-step mechanisms for the reaction between NO and O-2 over a wide range of temperature and pressure. The Arrhenius equation k (L-2 . mol(-2) . s(-1)) = 1.2 x 10(3) e(530/T) (=1.2 x 10(3) x 10(230/T)) gives the best fit to the experimental values of the rate constant thus far reported in a temperature range of 273 to 600 K. Using the reaction mechanism and the rate constant k, one can make reliable predictions about NO2 formation in any set of NO inhalation therapy conditions. It is also pointed out that NO2 the intermediate of one of the two mechanisms, deserves serious attention in NO inhalation therapy. (C) 1999 Academic Press.