Dioxygen cyclic voltammograms

Figure 27 Cyclic voltammograms recorded at a glassy carbon electrode in a CH2Cl2 solution of [Cu2(N3)]2+ (a) under dinitrogen atmosphere (b) after bubbling of dioxygen and subsequent bubbling of dinitrogen...

Fig. 30 Cyclic voltammograms (scan rate 2 mV s ) observed in 0.2 M Na2S04 + H2SO4 (pH 3) the working electrode was glassy carbon and the reference electrode was SCE. (a) M a2-P2Wi 5 M02CU. The choice of the reversal potentials help to distinguish the various steps, (b) dioxygen alone and 10 M q 2-P2Wi5Mo2Cu in the presence of different concentrations of dioxygen. For further details, see text (taken from Ref 161).

Figure 9.1 Electrochemical behavior of dioxygen (1 atm) in aqueous solutions (1 M NaC104) at a platinum electrode (area 0.458 cm2) A) the cyclic voltammogram was initiated at the rest potential with a scan rate of 0.1 V s-1 (B) the rotated-disk (400-rpm) voltammogram was obtained with a scan rate of 0.5 V min-1. 

Figure 9.2 Cyclic voltammogram for 5 mM dioxygen (02, at 1 atm) in pyridine (0.1 M tetrapropylammonium perchlorate) at a platinum electrode (area 0.23 cm2). Scan rate, 0.1 V s-1. Saturated calomel electrode (SCE) versus NHE, +0.244 V.

Reduction of O2 in the presence of excess zinc cation [ZnB(bpy)22+], (tetraphenylporphinato)iron(in) ion [(H2O)+Fe "TPP], and cuprous ion [Cul(MeCN)4 ] results in formation of metal-dioxygen adducts. Figures 2-11 and 2-12 illustrate the cyclic voltammograms for (Fe IlTPP)Cl and [CuI(MeCN)4]ClO4, respectively, in the absence and in the presence of 02- Reaction schemes for the three metal-O2 systems are outlined ... 

Fig. 6 Cyclic voltammogram obtained in a pH = 0.51 solution saturated with dioxygen. Scan rate 100 mV. Electrode surface area 0.07 cm. Dotted line freshly polished glassy carbon electrode solid line glassy carbon electrode modified in the presence of [PWi204o] as described in the text.

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