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Spontaneous vs Non-spontaneous Redox Reactions

Some Standard Reduction Potentials

Oxidants

  

Reductants

E0
(volts)
Weakest
Oxidant		 K++e K(s) -2.94 Strongest
Reductant
↓ Ba2++2e Ba(s) -2.91 ↑
↓ Ca2++2e Ca(s) -2.87 ↑
↓ Na++e Na(s) -2.71 ↑
↓ Mg2++2e Mg(s) -2.36 ↑
↓ Al3++3e Al(s) -1.68 ↑
↓ Mn2++2e Mn(s) -1.18 ↑
↓ Zn2++2e Zn(s) -0.76 ↑
↓ Fe2++2e Fe(s) -0.44 ↑
↓ Ni2++2e Ni(s) -0.24 ↑
↓ Sn2++2e Sn(s) -0.14 ↑
↓ Pb2++2e Pb(s) -0.13 ↑
↓ Cu2++2e Cu(s) 0.34 ↑
Strongest
Oxidant		 Ag++e Ag(s) 0.80 Weakest
Reductant

Key Concepts

  • Eo(redox reaction) =
    Eo(reduction reaction) + Eo(oxidation reaction)

  • If Eo(redox reaction) is positive, redox reaction is spontaneous

  • If Eo(redox reaction) is negative, redox reaction is not spontaneous (non-spontaneous)

  • If a redox reaction is spontaneous it proceeds in the forward direction as written.

  • If a redox reaction is not spontaneous it does not proceed in the forward direction as written.
 

Examples of Determinig if a Redox Reaction is Spontaneous

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