---
title: "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?"
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url: "https://nerd-notes.com/ubq/123918/"
date_modified: "2026-09-28T12:32:11+00:00"
---

# 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?

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?

- **A.** \(\text{Br}_2\text{(l)}\) at the cathode
- **B.** \(\text{H}_2\text{(g)}\) at the anode
- **C.** \(\text{Br}^-\text{(aq)}\) at the anode
- **D.** \(\text{H}^+\text{(aq)}\) at the cathode

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123918/*