Kinetics and mechanism of the electrochemical oxidation of the NO−<sub>2</sub> ion on platinum in AgNO<sub>2</sub>-acetonitrile solution
The anodic oxidation of NO−2 ion dissolved as AgNO2 in ACN, in the range − 12° to 68°C, is investigated using platinum electrodes. Single and multiple linear potential sweep and rotating disc electrode techniques are used. The electrochemical reaction is interpreted with the following sequence of re...
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| Autores principales: | , , |
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| Formato: | Articulo |
| Lenguaje: | Inglés |
| Publicado: |
1974
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| Materias: | |
| Acceso en línea: | http://sedici.unlp.edu.ar/handle/10915/121709 |
| Aporte de: |
| Sumario: | The anodic oxidation of NO−2 ion dissolved as AgNO2 in ACN, in the range − 12° to 68°C, is investigated using platinum electrodes. Single and multiple linear potential sweep and rotating disc electrode techniques are used. The electrochemical reaction is interpreted with the following sequence of reactions:
rds
(1) NO<sub>2</sub> = NO<sub>2</sub> + e
(2) [2 NO<sub>2</sub> ⇋ N<sub>2</sub>O<sub>4</sub>]
(3) NO<sub>2</sub> + NO<sub>2</sub> = NO + NO<sub>3</sub>
(4) NO = NO- + e
(5) NO+ + NO<sub>2</sub> = N<sub>2</sub>O<sub>3</sub>
(6) [N<sub>2</sub>O<sub>3</sub> ⇋ NO + NO<sub>2</sub>]
Step (1) behaves as an irreversible step which at high potentials is diffusion controlled, while step (4) corresponds to a reversible charge transfer step. The chemical reactions are fast processes. The postulated reaction mechanism for the anodic discharge of the NO−<sub>2</sub> ion implies the preferential reaction of the initial product with a NO−<sub>2</sub> ion instead of a solvent molecule as it occurred with solutions employing other aprotic solvents. |
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