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Chapter 50: Problem 16

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

Short Answer

Expert verified
The stronger oxidizing agent is determined by comparing the standard reduction potentials of \(\mathrm{Cu}^{2+}(\mathrm{aq})\) and \(\mathrm{H}^{+}(\mathrm{aq})\). Without the specific values from a standard electrode potential table, a definitive answer can't be given in this context. However, once the numbers are available, the ion with the higher reduction potential will be the stronger oxidizing agent.

Step by step solution

01

Refer to Standard Electrode Potential Table

Refer to a Standard Electrode Potential Table which will have reduction potentials listed for various half-reactions. The reduction potential values for \(\mathrm{H}^{+} \rightarrow \mathrm{H_{2}} (g)\) and \(\mathrm{Cu}^{2+} \rightarrow \mathrm{Cu} (s)\) are required.
02

Compare the Standard Reduction Potentials

Compare the standard reduction potentials. Use the values obtained from the standard electrode potential table. The species with the higher standard reduction potential will be the stronger oxidizing agent.
03

Draw a conclusion

The species with the higher standard reduction potential is the stronger oxidizing agent, because it is more prone to be reduced (gain electrons).

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Most popular questions from this chapter

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

The standard reduction potentials for \(\mathrm{Ag}^{+}(\mathrm{aq})\) and \(\mathrm{Au}^{+}(\mathrm{aq})\) are \(\begin{array}{lr} & E_{\mathrm{red}}^{\circ} \\ \mathrm{Ag}^{+}+1 \mathrm{e}^{-} \rightleftarrows \mathrm{Ag}(\mathrm{s}) & .80 \\\ \mathrm{Au}^{+}+1 \mathrm{e}^{-} \rightleftarrows \mathrm{Au}(\mathrm{s}) & 1.68\end{array}\) Which ion, \(\mathrm{Ag}^{+}(\mathrm{aq})\) or \(\mathrm{Au}^{+}(\mathrm{aq})\), exhibits the stronger pull on electrons?
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