염화요오드 수용액의 전극반응 = Electrode Reaction of Iodine Monochloride Aqueous Solution

다국어 초록 (Multilingual Abstract)

The electrode reactions of iodine monochloride aqueous solution on the platinum electrode were investigated to clarify the electrode reactions in the cathodic and the anodic processes using the anodic current density after applying the cathodic current density which came to the constant potential (the chronopotentiometric method). The essential current density range for investigating the electrode process was from 2.0 to 0.9 mΑ/㎠.
The cathodic reaction in electrolysis at the constant current density was found to be consisted of three successive steps, the EEE mechanism. Discharging of hydrogen ion to form the adsorbed hydrogen atom with regard to the first step proceeds as a diffusion controlled process, while the last step which occurs as a result of iodine reduction is more influenced by the adsorption than the second step. Thus the second is supposed as the electrochemical process of the hydrogen evolution reaction.
However, the anodic reaction takes place by a three-step mechanism (the ECE
mechanism) in which a chemical step is interposed between two charge transfers-i. e., the first step may be occurred by the adsorption of the reactant and the last step according to the kinetically controlled process.
The mechanisms of the cathodic electrode reaction at a high current density within 8.0-9.0mΑ/㎠ could be considered as follows:
The first step, ?; the second step, ?; the third step, Ⅰ₂(aq.)＋2e→?