Reference no: EM13178767
Write the equations describing the electrode reactions and the net cell reaction for this electrochemical cell containing copper and silver: Cu(s) | Cu^2+(aq) || Ag^+(aq) | Ag(s)
Anode: ?
Cathode: ?
Net cell reaction: ?
Using the following data:
1. Cu^3+ + 2e^- ---> Cu^+ E1^degree= 1.28 V
2. Cu^2+ + e^- ----> Cu^+ E2^degree= 0.15V
3. Cu^2+ + 2e^- ---> Cu(s) E3^degree= 0.34V
4. Cu^+ + e^- ---> Cu(s) E4^degree= 0.52V
Calculate the standard reduction potential for the reaction for the reaction Cu(III) to Cu(II).
= ? V
Balance the following equation in acidic conditions.
Cu + NO3^- ---> Cu^2+ + NO
Complete and balance the equation for this reaction in acidic solution.
A) ZnS + NO3^- --> Zn^2+ + S + NO
B) MnO4^- + HNO2 ----> NO3^- + Mn^2+
In a particular redox reaction, ClO2^- is oxidized to ClO4^- and Cu^2+ is reduced to Cu^+. Complete and balance the eqaution for this reaction in acidic solution.
ClO2^- + Cu^2+ ---> ClO4^- + Cu^+
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: Calculate the standard reduction potential for the reaction for the reaction Cu(III) to Cu(II).
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