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^+