The right battery symbol of the reaction of Cu(s) + 2H+ (0.01 mol/L) = Cu2+ (0.1 mol/L ) + H2 (0.9×1.013×105 Pa) is
A. (–) Cu(s) | Cu2+ (0.1 mol/L) || H+ (0.01mol/L) |H2 (0.9×1.013×105 Pa) | Pt(s) (+).
B. (–) Pt(s) | H+ (0.01mol/L) | H2 (0.9×1.013×105 Pa) || Cu2+ (0.1 mol/L) | Cu(s) (+).
C. (–) Cu(s) | Cu2+ (0.1 mol/L) | H+ (0.01mol/L) || H2 (0.9×1.013×105 Pa) | Pt(s) (+).
D. (–) Pt(s) | H2 (0.9×1.013×105 Pa) || H+ (0.01mol/L) |Cu2+ (0.1 mol/L) | Cu(s) (+).
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Which of the following statements about primary cell is wrong?
A. In principle, any spontaneous redox reaction can be designed as a primary cell.
B. A primary cell can be constructed with Cu and Cu2+ without other redox substances.
Change the pH value of the solution, the electromotive force of the primary cell will change.
D. The temperature rises, the electromotive force of the primary cell increases.
The oxidation numbers of Cl in Cl2O and S in S4O62– are
A. +1 and + 6, respectively.
B. +1 and + 4, respectively.
C. +1 and + 2.5, respectively.
D. –1 and + 6, respectively.
The greater the electromotive force, the faster the redox reaction rate.
The larger the electrode potential E value, the stronger the oxidation state of the oxidized substance in the electric pair.
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