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By Glenn Dryhurst (Auth.)

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According to Parker [74], the individual l e " transfer steps cannot be separated or distinguished even by very rapid electrochemical techniques. 4 V vs. SCE. This potential does not agree with results from earlier studies [71 ] in which, with tetraethylammonium perchlorate as the supporting electrolyte, neutral p-benzoquinone gives rise to a reduction peak at - 0 . 5 5 V vs. , peak l l c , Figs. 25 and 26). The reason that p-benzoquinone can be detected by fast-sweep voltammetry, according to Parker [74], is because the protonation of the latter compound to give compound VII [Eq.

17b)]. Thus, the peak occurring at approximately - 0 . 1 to - 0 . 2 V was thought to be an HeHe process [Eq. (17a,b)]. 7 to + 0 . 8 V (Table VI) was due to oxidation of ubiquinol-5, formed by the reaction sequence shown in Eq. (17a,b), back to ubiquinone5. Detailed studies of the electrochemical oxidation of ubiquinol-5 in acetonitrile have not been carried out. Cauquis and Marbach [84] have carried out a similar but more extensive study than that of Marcus and Hawley [82]. These workers utilized ubiquinone-30 (vitamin Q-6) and studied the behavior of this compound in acetonitrile.

1 M N a C I 0 4 as supporting electrolyte in the presence of 2,6-lutidine. 0 m M . Sweep rate: 156 mV s . ) Ill c and oxidation peak lll a [Fig. 29(c)-(f)] until they become the predominant peaks. Constant-current coulometric oxidation of p-benzohydroquinone in the presence of 2 equivalents of 2,6-lutidine was found to be a 2e~ per molecule process, and the only voltammetric peak in the product solution was reduction peak lll c . The height of the latter peak was just slightly greater than that initially observed for p-benzoquinone in the presence of base.

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