Anodic Oxidation Of Hydrazine Research Articles

Anodic oxidation of hydrazine and its derivatives Part IV. The oxidation of methylhydrazine (MH) on gold electrodes in acid solution

The electrooxidation of methylhydrazine on a gold electrode in H2SO4 has been studied. Linear sweep, steady state and quasi steady-state methods were used to evaluate the various parameters for the oxidation process and a mechanism is proposed. It involves two fast de-electronation reactions and the rate-determining step is an activated desorption step.

Anodic oxidation of hydrazine and its derivatives III. The oxidation of methylhydrazine on mercury electrodes in alkaline solutions

Summary The electro-oxidation of methylhydrazine in alkaline solutions has been studied on a mercury electrode. Polarography and cyclic voltammetry were used to determine the parameters of the oxidation process. A mechanism which fits the experimental results is proposed in which the rds consists of the reaction of an adsorbed OH radical with a methylhydrazine molecule.

Anodic oxidation of hydrazine and its derivatives: III. The oxidation of methylhydrazine on mercury electrodes in alkaline solutions

The electro-oxidation of methylhydrazine in alkaline solutions has been studied on a mercury electrode. Polarography and cyclic voltammetry were used to determine the parameters of the oxidation process. A mechanism which fits the experimental results is proposed in which the rds consists of the reaction of an adsorbed OH radical with a methylhydrazine molecule.

Anodic oxidation of hydrazine and its derivatives: Part IL the oxidation of 1,1-dimethyl-hydrazine (DMH) on gold electrodes in acid solution

The anodic oxidation of 1,1-dimethylhydrazine has been studied in 0.5–1 N H 2SO 4. From potential-sweep measurements in the range −0.400 to +1.00 V ( vs. mercury—mercurous sulfate) three oxidation peaks were obtained. The first peak is a well-defined irreversible peak which has a corresponding reduction peak. Tafel relationships, reaction orders, and pH effects, were studied and a mechanism proposed for the first oxidation step. This involves two fast charge-transfer steps which are in quasi-equilibrium and a slow non-activated desorption step which is the rate-determining step.

Anodic oxidation of hydrazine and its derivatives: Part I. The oxidation of hydrazine on gold electrodes in acid solutions

The anodic oxidation of hydrazine on gold electrodes has been studied in acid solutions (0.5–2N H2SO4). The electrode pretreatment consisted of electropolishing, followed by a sequence of potentials (0.90V,−0.20V) before each measurement. The Tafel slope was determined by four independent techniques (shift of the peak potential with sweep rate in linear potential sweep, foot of the current/potential curve in the same measurement, galvanostatic and steady state potentiostatic) all of which gave values in the range of 90–100 mV. The reaction order and pH effects were 0.3 and 0.8, respectively.

Anodic oxidation of hydrazine and its derivatives Part I. The oxidation of hydrazine on gold electrodes in acid solutions

The anodic oxidation of hydrazine on gold electrodes has been studied in acid solutions (0.5–2 N H 2 SO 4 ). The electrode pretreatment consisted of electropolishing, followed by a sequence of potentials (0.90V,−0.20V) before each measurement. The Tafel slope was determined by four independent techniques (shift of the peak potential with sweep rate in linear potential sweep, foot of the current/potential curve in the same measurement, galvanostatic and steady state potentiostatic) all of which gave values in the range of 90–100 mV. The reaction order and pH effects were 0.3 and 0.8, respectively. The mechanism proposed involves fast equilibrium in the first discharge step in which an adsorbed N 2 H 3 radical is formed. Desorption of this radical with formation of N 2 H 2 in solution is believed to be rate determining. The surface coverage by N 2 H 3 radicals is intermediate and a Frumkin type adsorption isotherm is applicable, with correction for the energy of displacement of water molecules from the surface, according to the theory of Bockris et al. for electrosorption of neutral organic species.