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Chapter 48: Problem 20

What value (in volts) should be assigned as the standard reduction potential, \(E_{\text {red }}^{\circ}\), of the \(\mathrm{Cu} / \mathrm{Cu}^{2+}\) half-cell?

Short Answer

Expert verified
The standard reduction potential, \(E_{\text{red}}^{\circ}\), of the Cu/Cu2+ half-cell is +0.34V.

Step by step solution

01

Understand the terms

Standard reduction potential, expressed as \(E_{\text{red}}^{\circ}\) is a measure of the tendency of a chemical species to be reduced, that is, to gain electrons. A half-cell, in this case the Cu/Cu2+ half-cell, comprises of the oxidation or reduction reaction of the species in question.
02

Look up the standard reduction potential

For the Cu/Cu2+ half-cell, we consult a Table of Standard Reduction Potentials. This lists the \(E_{\text{red}}^{\circ}\) values for a variety of half-cells.
03

Identify the correct value

From this table, the standard reduction potential for the Cu/Cu2+ half-cell, \(E_{\text{red}}^{\circ}\), can be found to be +0.34V.

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Most popular questions from this chapter

Which is the stronger oxidizing agent, \(\mathrm{Cu}^{2+}(\mathrm{aq})\) or \(\mathrm{H}^{+}(\mathrm{aq})\) ?

The standard reduction potentials for \(\mathrm{Ag}^{+}(\mathrm{aq})\) and \(\mathrm{Au}^{+}(\mathrm{aq})\) are $$ \begin{array}{lr} \mathrm{Ag}^{+}+\mathrm{le}^{-} \rightleftarrows \mathrm{Ag}(\mathrm{s}) & .80 \\\ \mathrm{Au}^{+}+\mathrm{le}^{-} \rightleftharpoons \mathrm{Au}(\mathrm{s}) & 1.68 \end{array} $$ Which ion, \(\mathrm{Ag}^{+}(\mathrm{aq})\) or \(\mathrm{Au}^{+}(\mathrm{aq})\), exhibits the stronger pull on electrons?

What use(s) could be made of the flow of electrons in the wire?
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