In a galvanic cell, a spontaneous redox reaction occurs. However, the reactants

Question

In a galvanic cell, a spontaneous redox reaction occurs. However, the reactants are separated such that the transfer of electrons is forced to occur across a wire. The resulting electricity is measured in volts (V) and is the sum of the potentials of the oxidation and reduction half-reactions:

E?cell=E?red+E?ox

Which is sometimes also written as:

E?cell=E?red(cathode)?E?red(anode)

A table of standard reduction potentials gives E?red values for common half-reactions.

By reversing any of these reduction half-reactions, you get the corresponding oxidation half-reaction, for which E?ox has the opposite sign of E?red.

Calculate the standard potential for the following galvanic cell:

Fe(s) | Fe2+(aq) || Ag+(aq) | Ag(s)

Reduction half-reaction E? (V) Ag+(aq)+e??Ag(s) 0.80 Cu2+(aq)+2e??Cu(s) 0.34 Ni2+(aq)+2e??Ni(s) ?0.26 Fe2+(aq)+2e??Fe(s) ?0.45 Zn2+(aq)+2e??Zn(s) ?0.76

Explanation / Answer

the standard potential for the following galvanic cell: 0.8 - (-0.45) = 1.25 V

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