AP Chemistry
9.9 Cell Potential and Free Energy
9.8 Galvanic (Voltaic) and Electrolytic Cells
A galvanic cell operates spontaneously under standard conditions at \(298\text{ K}\). One half-cell consists of a standard hydrogen electrode (\(\text{Pt(s)} \mid \text{H}_2\text{(g)} \mid \text{H}^+\text{(aq)}\)), and the other half-cell consists of an inert platinum electrode in contact with liquid bromine and aqueous bromide ions (\(\text{Pt(s)} \mid \text{Br}_2\text{(l)} \mid \text{Br}^-\text{(aq)}\)). The standard reduction potentials are shown below.
\[ \begin{aligned} \text{Br}_2(l) + 2\,\text{e}^- &\rightarrow 2\,\text{Br}^-(aq) & E^\circ &= +1.07\text{ V} \\ 2\,\text{H}^+(aq) + 2\,\text{e}^- &\rightarrow \text{H}_2(g) & E^\circ &= 0.00\text{ V} \end{aligned} \]
Which species acts as the reducing agent in the overall cell reaction, and at which electrode does it react?
\[ \begin{aligned} \text{Br}_2(l) + 2\,\text{e}^- &\rightarrow 2\,\text{Br}^-(aq) & E^\circ &= +1.07\text{ V} \\ 2\,\text{H}^+(aq) + 2\,\text{e}^- &\rightarrow \text{H}_2(g) & E^\circ &= 0.00\text{ V} \end{aligned} \]
Which species acts as the reducing agent in the overall cell reaction, and at which electrode does it react?
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