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The cyclic voltammetry and the potential-time curve after galvanostatic electrolysis were used to study the electrode processes of Cu(n) in CH3OH solution and DMSO solution. The electroreduction of Cu(Ⅱ) to Cu on a Pt electrode proceeds in two steps: Cu(Ⅱ) + e = Cu(Ⅰ); Cu(I) + e = Cu. The reduction potential of Cu(n) in DMSO solution is more negative than that in CH3OH solution, and the diffusion coefficient of Cu(Ⅱ) ion in DMSO solution is larger than that in CH3OH solution because the polarity of DMSO is larger than that of CH3OH observably and has a stronger solvating power.
The cyclic voltammetry and the potential-time curve after galvanostatic electrolysis were used to study the electrode processes of Cu (n) in CH3OH solution and DMSO solution. The electrokineduction of Cu (II) to Cu on a Pt electrode proceeds in two steps: Cu (II) + e = Cu (I); Cu (I) + e = Cu. The reduction potential of Cu (n) in DMSO solution is more negative than that in CH3OH solution, and the diffusion coefficient of Cu in DMSO solution is larger than that in CH3OH solution because the polarity of DMSO is larger than that of CH3OH observably and has a stronger solvating power.