For the redox reaction Zn(s) + Cu^(2+) (1M) --> Cu (1M) + Zn^(2+) (1M)
1. Write oxidation and reduction half-equations and a balanced overall equation
2. Write a cell diagram for a voltaic cell in which this reaction occurs. Label the anode and cathode.
3. Calculate E^o cell. Given the standard electrode potential E^o (Cu2+/Cu) = 0.34 V, E^o (Zn2/Zn) = -0.77 V
Redox reactions???? PLEASE HELP!!?
2016-07-03 6:06 pm
回答 (1)
2016-07-03 7:07 pm
✔ 最佳答案
1.Oxidation half-equation : Zn(s) → Zn²⁺(1M) + 2e⁻
Reduction half-equation : Cu²⁺(1M) + 2e⁻ → Cu(s)
Overall equation : Zn(s) + Cu²⁺(1M) → Cu(s) + Zn²⁺(1M)
====
2.
(Anode) Zn(s) | Zn²⁺(1M) || Cu²⁺(1 M) | Cu(s) (Cathode)
====
3.
E°cell
= E°(Cu²⁺|Cu) - E°(Zn²⁺|Zn)
= (+0.34 V) - (-0.77 V)
= +1.11 V
收錄日期: 2021-04-18 15:12:24
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