14.4 Standard Cell Potentials

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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+