Galvanic Cells Worksheet

 

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  1. What is a galvanic cell?

    2.  

     

  2. Draw a galvanic cell and label all its components.

    3.  

     

  3. Why is a salt bridge necessary to complete the circuit?

    4.  

     

  4. What do the following acronyms mean?

      5.  

    • RED-CAT

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    • OX-AN

     

     

  5. What is the unit measure for cell potential?

    6.  

     

  6. What are standard conditions?

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  7. You must break the redox reaction into ______   _________   in order to determine the anode and cathode.

    8.  

     

  8. For a galvanic cell the value of ε°­cell must be _________ as it indicates _________.

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  9. What overall reaction would happen between based on the reduction potentials of each half reaction.?

      10.  

    • Mn2+ + 2e-→Mn     ε° = -1.18V

       

      Cu2++e-      →Cu             ε°=0.34V

      •  

    • Mn2+ + 2e-→Mn     ε° = -1.18V

       

      Fe3+ + 3e-      →Fe         ε° = -0.036V

     

     

  10. Answer the following using standard reduction potential values

      11.  

    • Is H+(aq) capable of dissolving Cu(s) to Cu2+(aq)?

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    • Is Fe3+(aq) capable of oxidizing I-(aq)?

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    • Is H2(g) capable of reducing Ag+(aq)?

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    • Is Fe2+(aq) capable of reducing Cr3+(aq)­ to Cr2+(aq)?

     

     

  11. Using the standard reduction potential and considering

    Na+, Cl-, Ag+, Ag, Zn2+, Zn and Pb

    answer the following

      12.  

    • Which is the strongest oxidizing agent?

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    • Which is the strongest reducing agent?

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    • Which species can be oxidized by SO42-(aq) in acid?

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    • Which species can be reduced by Al(s)?

     

     

  12. What equation relates ε° and ∆G°?

      13.  

    • What is F?

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    • What is n?


  13. Just as the value of  ∆G is dependent upon the concentrations of reactants/products – ε is as well.  Leading to the following equations:

      14.  

    • For non standard cells:

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    • At equilibrium:

     

     

  14. Calculate the values of ∆G° and K for the following cell

    H2O2 + 2H+ + 2e-    → 2H2O             ε°= 1.78V

     

    O2 + 2H+ +2e-    → H2O2                    ε° = 0.68V

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  15. Consider the following galvanic cell at 25°C:

    Pt|Cr2+(0.30 M), Cr3+(2.0M)|| Co2+(0.20M)|Co                      K=2.79 x 107

    Calculate the cell potential and ∆G for this galvanic cell.    

    16.  

     

  16. Consider the cell described below

    Al|Al3+(1.00M)||Pb2+(1.00M)|Pb

    Calculate the cell potential after the reaction has operated long enough for the [Al3+] to have changed by 0.60 mol/L.  (assume T=25°C)

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