31Aug/08Off
Nickel Silver
A galvanic cell is constructed with a silver-silver chloride electrode, and a nickel strip immersed in a beake
A galvanic cell is constructed with a silver-silver chloride electrode, and a nickel strip immersed in a beaker containing 1.56x 10-2 M solution of NiCl2. Determine the balanced cell reaction and calculate the potential of the cell. Enter in volts. (assume a temperature of 25oC)
First, the reduction reactions for both species are:
AgCl + e- » Ag + Cl- [0.22 V]
Ni(2+) + 2e- » Ni [-0.23 V]
now, one of the equation needs to be reversed to become the oxidation reaction and to make the potential positive.
The second one will become oxidated.
AgCl + e- » Ag + Cl- [0.22 V]
Ni » Ni(2+) + 2e- [0.23 V]
Then, the first reaction needs to multiplied by two to make the electrons disappear in the overall equation. The potential is left alone.
2AgCl + 2e- » 2Ag +2Cl- [0.22 V]
Ni » Ni(2+) + 2e- [0.23 V]
Add the equations together and get...
2AgCl + Ni » 2Ag +2Cl- + Ni(2+) [0.45 V]
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