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Electrochemistry assessment
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1) Consider the following materials and galvanic cell diagram: silver, aluminum, nickelelectrodes, 1.0 M AgNO3(aq) solution, 1.0 M Al(NO3)3 solution, 1.0 M Ni(NO3)2 solution
From the above list, select the materials that are capable of producing the greatest voltage: Silver
and aluminum.
Label the diagram:
Calculate the initial voltage for the electrochemical cell
Ag+ + e- → Ag 0.80 (Reduction)
Reverse reduction to oxidation: Al3+ + 3e- → Al(s) 1.88
E cell = E reduction + E oxidation:
= 0.80V + 1.88V
= 2.46V
Write the complete balanced redox reaction for the cell:
Oxidation reaction - Keep the same: Al3+ + 3e- → Al(s)
Reduction reaction - Multiply by 3: 3Ag+ + 3e- → 3Ag
Redox reaction: Al3+ + 3Ag+ → Al(s) + 3Ag
Which 2 metals from the above list would produce an electrochemical cell with the smallest
initial voltage? Aluminum and nickel
2) A trophy manufacturer electroplates an iron trophy with gold.
Write the equation for the half reaction that occurs at the iron trophy. There is no half reaction
given.
Identify the cathode: Gold
Explain how to maintain a constant metal ion concentration in the electrolyte. A constant metal
ion concentration can be maintained by electroplating with a small amount of gold at a time.
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