A voltaic cell is based on the Co2+/Co and AgCl/Ag half-cells. Explain how to identify the anode and cathode. Next, calculate the standard cell potential.Given: Co2+ (aq) + 2 e- → Co (s) E° = -0.277 VAgCl (s) + e- → Ag (s) + Cl- (aq) E° = +0.222 V
The size of the different numbers.0.499V
To identify the anode and cathode in a voltaic cell based on the given half-cells, we need to compare the standard reduction potentials of each half-cell. The half-cell with the more positive reduction potential will be reduced, thus acting as the cathode. Conversely, the half-cell with the less positive reduction potential will oxidize and act as the anode.
In this case, the AgCl/Ag half-cell has a higher standard reduction potential of +0.222 V compared to the Co2+/Co half-cell, which has a standard reduction potential of -0.277 V. Therefore, AgCl/Ag will be reduced and act as the cathode, while Co2+/Co will be oxidized and act as the anode.
To calculate the standard cell potential, we can use the formula:
E°cell = E°cathode – E°anode
where E°cathode and E°anode are the standard reduction potentials of the cathode and anode, respectively.
Plugging in the values for our half-cells, we get:
E°cell = +0.222 V – (-0.277 V) = +0.499 V
Therefore, the standard cell potential for the Co2+/Co and AgCl/Ag voltaic cell is +0.499 V.
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