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Electrochemical Cells

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    1.) Consider this overall redox process: Cu2+(aq)+Ba(s)→Cu(s)+Ba2+(aq)

    a.) Split the reaction into half reactions and determine their standard reduction potentials. Indicate which would be the anode and cathode.







     

    b.) Construct a cell diagram.









     

    c.) Give the line notation for this cell.




     

    d.) Calculate E°cell, the standard cell potential, which is given by E°red - E°ox.




     

    2.) Consider this overall redox process: Al(s)+Sn2+(aq)→Al3+(aq)+Sn(s)

    a.) Split the reaction into half reactions and determine their standard reduction potentials. Indicate which would be the anode and cathode.











     

    b.) Construct a cell diagram.







     

    c.) Give the line notation for this cell.



     

    d.) Calculate E°cell.

     

     

     

     

    3.) Consider a galvanic cell with Zn(s) and 0.25 M Zn(NO3)2(aq) in one compartment and Cu(s) and 0.25 M Cu(NO3)2(aq) in the other compartment.

    a.) Give the half-reactions and their standard reduction potentials.
     

    Reduction (cathode):
     
    Eocathode =

     

    Oxidation (anode):
     
    Eoanode =

     

    b.) Give the net, overall cell reaction and the standard cell potential:

     
     
    Eocell =

     

    c.) Now calculate the overall cell potential at the specific concentrations given.  You’ll need to use the Nernst equation: Ecell = Eocell – (0.0592/n)log Q







     

    d.) What would be the cell potential if the concentration of Zn(NO3)2 was increased to 2.5 M?







     

    4.) Consider a voltaic cell with Cr(s) and Cr3+(aq) in one compartment and Zn(s) and Zn2+(aq) in the other compartment.

    a.) Draw and label a diagram of this cell.
















     

    b.) Calculate the standard cell potential for the overall reaction.













     

    c.) If zinc is the anode and [Cr3+] = 0.010 M, what must the [Zn2+] be in order to achieve 0.050V?














     

    5.) A Zn/Zn2+ half-cell was coupled to a hydrogen electrode in which PH2 = 1 bar.  The [Zn2+] in the anode compartment was 0.10 M and the cell potential was 0.542 V.  Calculate the pH in the cathode compartment.














     

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    This page titled Electrochemical Cells was last modified on Wed, 28 Oct 2020 23:11:39 GMT and is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Contributor via source content that was edited to the style and standards of the LibreTexts platform.