Li(s)|Li+ (aq,1 M)||Zn2+(aq, 1 M)|Zn(s) A.Write half-reactions occurring in the electrochemical cell B.Which reaction is occurring at the cathode? Which reaction is occurring at the anode? C.Write a fully balanced redox reaction based on your half-reactions D.Based on the table of standard reduction potentials (see document on Canvas), calculate E°cell.
Li(s)|Li+ (aq,1 M)||Zn2+(aq, 1 M)|Zn(s)
A.Write half-reactions occurring in the
B.Which reaction is occurring at the cathode? Which reaction is occurring at the anode?
C.Write a fully
D.Based on the table of standard reduction potentials (see document on Canvas), calculate E°cell.
E.As the reaction progresses, 4.52g of the lithium electrode corrodes and 21.3 g of zinc is deposited on your zinc electrode. Assuming both solutions in your cell are 1 L and 298 K, what would be the cell potential (Ecell) at this point?
F.Based on Question E, how much time is necessary to run a 12.5A current through your Li+solution to reduce it ALL to lithium metal
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