Using a table of standard electrode potentials (such as the one in your textbook), calculate the standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is connected by an electrolyte to a Ag+(aq) solution containing a silver electrode. Show your work.
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To calculate the standard cell potential for the given cell, we need to use the standard electrode potentials for the reduction half-reactions of the two electrodes involved. Here's how you can do it:
Step 1: Find the reduction half-reactions for both zinc and silver. In this case, the reduction half-reactions are:
Zn2+(aq) + 2e- -> Zn(s)
Ag+(aq) + e- -> Ag(s)
Step 2: Look up the standard electrode potentials for these half-reactions in your textbook or a table of standard electrode potentials. Let's assume the values are:
E°(Zn2+/Zn) = -0.76 V
E°(Ag+/Ag) = 0.80 V
Step 3: Since the zinc electrode is undergoing oxidation (losing electrons) and the silver electrode is undergoing reduction (gaining electrons), we need to flip the sign of the zinc half-reaction:
Zn(s) -> Zn2+(aq) + 2e-
Step 4: Now, add the two half-reactions and their potentials together:
Zn(s) -> Zn2+(aq) + 2e- (E° = -0.76 V) (reversed)
Ag+(aq) + e- -> Ag(s) (E° = 0.80 V)
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Zn(s) + Ag+(aq) -> Zn2+(aq) + Ag(s) (E°cell)
Step 5: Add the two voltages together to obtain the standard cell potential (E°cell):
E°(cell) = -0.76 V + 0.80 V
E°(cell) = 0.04 V
Therefore, the standard cell potential for the given cell is 0.04 V.