14.4 Standard Cell Potentials
ε° = ε°cat - ε°an ε° = ε°redt - ε°ox
Zn2+ + Co → Zn + Co2+ ε° =
2Cr3+ + 3Cu → 2Cr + 3Cu2+ ε° =
| REDUCTION POTENTIALS | |
|---|---|
| Al3+ + 3e- → Al | -1.66V |
| Mn2+ + 2e- → Mn | -1.18V |
| Zn2+ + 2e- → Zn | -0.76V |
| Cr3+ + 3e- → Cr | -0.74V |
| Fe2+ + 2e- → Fe | -0.44V |
| Co2+ + 2e- → Co | -0.28V |
| 2H+ + 2e- → H2 | 0V |
| Cu2+ + 2e- → Cu | +0.34V |
| Ag+ + e- → Ag | +0.80V |
| Br2 + 2e- → 2Br- | +1.07V |
| Cl2 + 2e- → 2Cl- | +1.36V |
Write the balanced reaction and calculate E°cell for the voltaic cell produced from the Fe2+/Fe and Mn2+/Mn half cells.
Using the table of Reduction Potentials answer the following:
What is the strongest oxidizing agent?
What is the strongest reducing agent?
Which pairs will react spontaneously?
Al3+ / Mn2+ Al3+ / Mn
Al / Mn Al / Mn2+