Nitrogen monoxide reactions

The reaction between copper and nitric acid, 1 part concentrated acid and 1 part water, gives impure nitrogen monoxide ... 

Electrons are shared when nitrogen monoxide combines with oxygen, a spontaneous reaction, to give nitrogen dioxide... 

If this reaction takes place in air, the evolved nitrogen monoxide is oxidised to the dioxide and this dissolves again as in equation (9.1) hence virtually complete conversion of nitrogen dioxide to nitric acid can occur (see nitric acid, below). With alkalis, a mixture of nitrite and nitrate is formed ... 

Our experience conditions us to focus on the organic components of the reaction—l arginine and l citrul line—and to give less attention to the inorganic one—nitric oxide (nitrogen monoxide NO) To do so however would lead us to overlook one of the most important discoveries in biology in the last quarter of the twentieth century... 

The measurement of NO concentration is based on chemiluminescence this is light generation due to a chemical reaction. This occurs when nitrogen monoxide and ozone react with each other. 

The chemiluminescence reaction between nitrogen monoxide and ozone is formulated as ... 

Self-Test M.3B Suppose that 28 g of NOz and 18 g of water are allowed to react to produce nitric acid and nitrogen monoxide. If 22 g of nitric acid is produced in the reaction, what is the percentage yield ... 

C. At that temperature some endothermic reactions take place that at lower temperatures are not spontaneous under standard conditions (pure substances, each at I bar). Estimate the temperatures at which the following stratospheric reactions become spontaneous under standard conditions. Which ones could occur during re-entry of the space shuttle (a) The formation of nitrogen monoxide from nitrogen and oxygen ... 

Other reactions of small inorganic molecules are the oxidation of chloride ion at a Nafion electrode impregnated with a ruthenium 0x0 complex and the reduction of nitrogen monoxide to ammonia at a Co phthalocyanine modified electrode... 

NO. Nitric oxide, or nitrogen monoxide, is a colorless gas at room temperature. As we have already seen, it is industrially produced by the oxidation of ammonia. However, with respect to the urban envirorunent, a more significant process is the high temperature reaction of N2 with O2 (as in a car engine) to produce NO. 

The experimental results imply that the main reaction (eq. 1) is an equilibrium reaction and first order in nitrogen monoxide and iron chelate. The equilibrium constants at various temperatures were determined by modeling the experimental NO absorption profile using the penetration theory for mass transfer. Parameter estimation using well established numerical methods (Newton-Raphson) allowed detrxmination of the equilibrium constant (Fig. 1) as well as the ratio of the diffusion coefficients of Fe"(EDTA) andNO[3]. 

A very attractive method for the preparation of nitroalkenes, which is based on the reaction with NO, has been reported. Treatment of alkenes at ambient pressure of nitrogen monoxide (NO) at room temperature gives the corresponding nitroalkenes in fairly good yields along with P-nitroalcohols in a ratio of about 8 to 2. The nitroalcohol by-products are converted into the desired nitroalkenes by dehydration with acidic alumina in high total yield. This simple and convenient nitration procedure is applied successfully to the preparation of nitroalkenes derived from various terminal alkenes or styrenes (Eq. 2.27).53 This process is modified by the use of HY-zeolites instead of alumina. The lack of corrosiveness and the ability to regenerate and reuse the catalyst make this an attractive system (Eq. 2.28).54... 

Fig. 4.2 Comparison of amino acid yields using CH4, CO and CO2 as carbon sources with the addition of varying amounts of H2. The yields were calculated on the basis of the amount of carbon present in the reaction mixture. In all cases, the partial pressures of nitrogen, methane, carbon monoxide and carbon dioxide were lOOmmHg. For the reactions using nitrogen, the reaction vessel contained 100 mL of water, but no ammonia. Reactions involving nitrogen and ammonia were carried out using 100 mL of ammonium chloride (0.05 M). The electrical discharge experiments took 48 hours at room temperature (Schlesinger and Miller, 1983)...

Another example is the use of catalytic metals (platinum and rhodium) in the catalytic converter of a motor car. These solid metals catalyse the reaction between the pollutant gases carbon monoxide and nitrogen monoxide. 

Herold, S., Rock, G., Reactions of deoxy-, oxy-, and methemoglobin with nitrogen monoxide. Mechanistic studies of the S-nitrosothiol formation under different mixing conditions, /. Biol. Chem. 278 (2003), p. 6623-34... 

Some metals can have different oxidation numbers in different compounds. In the following reactions of iron with concentrated nitric acid, assume that one of the products in each case is gaseous nitrogen monoxide. 

NO (nitrogen monoxide) is the primary NO component in the flue gas meaning that the first equation above is the more significant one. Stoichiometry reveals that one mole of ammonia is required to reduce one mole of NO and convert it to nitrogen and water. Reaction rates are indicative of the Arrhenius equation that describes temperature dependent reactions. 

If the procedure is carried out under an atmosphere of nitrogen, oxidation of nitrogen monoxide to nitrogen dioxide is prevented and the reaction mixture remains colorless, but the yield is not improved. 

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