---
title: "An electrolytic cell is set up using inert platinum electrodes immersed in a \\(1.0\\text{ M }\\text{NaBr(aq)}\\) solution at \\(298\\text{ K}\\). A direct current is applied to drive the nonspontaneous process.  | Half-reaction | \\(E^\\circ\\text{ at } 298\\text{ K}\\) | |—|—| | \\(\\text{Na}^+\\text{(aq)} + e^- \\rightarrow \\text{Na(s)}\\) | \\(-2.71\\text{ V}\\) | | \\(2\\text{H}_2\\text{O}(l) + 2e^- \\rightarrow \\text{H}_2\\text{(g)} + 2\\text{OH}^-\\text{(aq)}\\) | \\(-0.83\\text{ V}\\) | | \\(\\text{Br}_2(l) + 2e^- \\rightarrow 2\\text{Br}^-\\text{(aq)}\\) | \\(+1.07\\text{ V}\\) | | \\(\\text{O}_2\\text{(g)} + 4\\text{H}^+\\text{(aq)} + 4e^- \\rightarrow 2\\text{H}_2\\text{O}(l)\\) | \\(+1.23\\text{ V}\\) |  Based on the standard reduction potentials in the table, which of the following correctly identifies the chemical species reduced at the cathode and the chemical species oxidized at the anode?"
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date_modified: "2026-08-23T04:23:23+00:00"
---

# An electrolytic cell is set up using inert platinum electrodes immersed in a \(1.0\text{ M }\text{NaBr(aq)}\) solution at \(298\text{ K}\). A direct current is applied to drive the nonspontaneous process.

| Half-reaction | \(E^\circ\text{ at } 298\text{ K}\) |
|—|—|
| \(\text{Na}^+\text{(aq)} + e^- \rightarrow \text{Na(s)}\) | \(-2.71\text{ V}\) |
| \(2\text{H}_2\text{O}(l) + 2e^- \rightarrow \text{H}_2\text{(g)} + 2\text{OH}^-\text{(aq)}\) | \(-0.83\text{ V}\) |
| \(\text{Br}_2(l) + 2e^- \rightarrow 2\text{Br}^-\text{(aq)}\) | \(+1.07\text{ V}\) |
| \(\text{O}_2\text{(g)} + 4\text{H}^+\text{(aq)} + 4e^- \rightarrow 2\text{H}_2\text{O}(l)\) | \(+1.23\text{ V}\) |

Based on the standard reduction potentials in the table, which of the following correctly identifies the chemical species reduced at the cathode and the chemical species oxidized at the anode?

An electrolytic cell is set up using inert platinum electrodes immersed in a \(1.0\text{ M }\text{NaBr(aq)}\) solution at \(298\text{ K}\). A direct current is applied to drive the nonspontaneous process.

| Half-reaction | \(E^\circ\text{ at } 298\text{ K}\) |
|---|---|
| \(\text{Na}^+\text{(aq)} + e^- \rightarrow \text{Na(s)}\) | \(-2.71\text{ V}\) |
| \(2\text{H}_2\text{O}(l) + 2e^- \rightarrow \text{H}_2\text{(g)} + 2\text{OH}^-\text{(aq)}\) | \(-0.83\text{ V}\) |
| \(\text{Br}_2(l) + 2e^- \rightarrow 2\text{Br}^-\text{(aq)}\) | \(+1.07\text{ V}\) |
| \(\text{O}_2\text{(g)} + 4\text{H}^+\text{(aq)} + 4e^- \rightarrow 2\text{H}_2\text{O}(l)\) | \(+1.23\text{ V}\) |

Based on the standard reduction potentials in the table, which of the following correctly identifies the chemical species reduced at the cathode and the chemical species oxidized at the anode?

- **A.** Cathode: \(\text{Na}^+\text{(aq)}\); Anode: \(\text{Br}^-\text{(aq)}\)
- **B.** Cathode: \(\text{Na}^+\text{(aq)}\); Anode: \(\text{H}_2\text{O}(l)\)
- **C.** Cathode: \(\text{H}_2\text{O}(l)\); Anode: \(\text{Br}^-\text{(aq)}\)
- **D.** Cathode: \(\text{H}_2\text{O}(l)\); Anode: \(\text{H}_2\text{O}(l)\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120358/*