While performing Lab 11, Electrochemistry, students connected 1 M solutions of the following metals and used electrodes to monitor the cell potential.  Using the table of theoretical values and what you know of the metals to fill in the blanks below.   When writing equations: Use spaces only before and after a plus sign. For example, the reaction: Fe2++2e−→FeFe2++2e-→Fe  would be entered as:  Fe^2+ + 2e^- →→ Fe Galvanic Cell Consisting of:   Zn2++2e−Zn2++2e- →→  ZnZn -0.76   Al3++3e−Al3++3e- →→  AlAl -1.66 E0cell Measured   0.79 Write the equation occuring at the anode. →→   Write the equation occurring at the cathode. →→    Shorthand Notation for the Cell:  l  lI  l  Oxidizing Agent: Al Zn2+ Zn `Al3+ Reducing Agent: Zn Zn2+ `Al3+ Al   E0cell from Table Values (Theoretical Numbers above).   E0cell Percent Error

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