13. The standard reduction potential of several half-cell reactions are shown below. \( \mathrm{Ag}^{+}(\mathrm{aq})+ \) é \( \rightarrow \mathrm{Ag}(\mathrm{s}) \quad \mathrm{E}^{\circ} \mathrm{Ag}^{+} / \mathrm{Ag}= \) +0.80 V \( \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{e} \rightarrow \mathrm{Cu}(\mathrm{s}) \quad \mathrm{E}^{\circ} \mathrm{Cu}^{2+} / \mathrm{Cu}= \) +0.34 V \( \mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{e} \rightarrow 2 \mathrm{Cl}-(\mathrm{aq}) \quad \mathrm{E}^{\circ} \mathrm{Cl}_{2} / \mathrm{Cl}^{-}=+ \) 1.36 V \( \mathrm{Au}^{3+}(\mathrm{aq})+3 \mathrm{é} \rightarrow \mathrm{Au}(\mathrm{s}) \quad \mathrm{E}^{\circ} \mathrm{Au}^{3+} / \mathrm{Au}= \) +1.50 V

Imagine a time when the discovery of metals shaped economies and practices worldwide! Silver (Ag), copper (Cu), and gold (Au) have been treasured since ancient civilizations, not just for their beauty but for their reactivity. Their standard reduction potentials tell a riveting story of which metals are more likely to gain electrons—thus becoming reduced—versus those that are less likely. Gold has the highest potential among the listed metals, making it a sought-after choice for various applications from jewelry to electronics, due to its stability and conductivity. When thinking about how these potentials translate into the real world, consider batteries! The strongest reduction potentials indicate the most potent oxidizing agents available in electrochemical cells. For instance, pairing gold with a less noble metal could create an efficient galvanic cell, generating electricity in practical applications like powering gadgets or even in biodata sensors. This fascinating integration of chemistry not only illustrates fundamental principles but also drives technological advancements in energy solutions.