---
title: "A student constructs a galvanic cell operating under standard conditions using silver and lead electrodes submerged in standard \\(1.0 \\, \\text{M}\\) nitrate solutions. The relevant standard reduction potentials are given in the table below.  | Half-Reaction | \\(E^\\circ \\, \\text{(V)}\\) | | :— | :— | | \\(\\text{Ag}^+(\\text{aq}) + e^- \\rightarrow \\text{Ag}(\\text{s})\\) | \\(+0.80\\) | | \\(\\text{Pb}^{2+}(\\text{aq}) + 2e^- \\rightarrow \\text{Pb}(\\text{s})\\) | \\(-0.13\\) |  What is the standard cell potential, \\(E^\\circ_{\\text{cell}}\\), for the galvanic cell?"
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url: "https://nerd-notes.com/ubq/119285/"
date_modified: "2026-08-21T18:12:28+00:00"
---

# A student constructs a galvanic cell operating under standard conditions using silver and lead electrodes submerged in standard \(1.0 \, \text{M}\) nitrate solutions. The relevant standard reduction potentials are given in the table below.

| Half-Reaction | \(E^\circ \, \text{(V)}\) |
| :— | :— |
| \(\text{Ag}^+(\text{aq}) + e^- \rightarrow \text{Ag}(\text{s})\) | \(+0.80\) |
| \(\text{Pb}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Pb}(\text{s})\) | \(-0.13\) |

What is the standard cell potential, \(E^\circ_{\text{cell}}\), for the galvanic cell?

A student constructs a galvanic cell operating under standard conditions using silver and lead electrodes submerged in standard \(1.0 \, \text{M}\) nitrate solutions. The relevant standard reduction potentials are given in the table below.

| Half-Reaction | \(E^\circ \, \text{(V)}\) |
| :--- | :--- |
| \(\text{Ag}^+(\text{aq}) + e^- \rightarrow \text{Ag}(\text{s})\) | \(+0.80\) |
| \(\text{Pb}^{2+}(\text{aq}) + 2e^- \rightarrow \text{Pb}(\text{s})\) | \(-0.13\) |

What is the standard cell potential, \(E^\circ_{\text{cell}}\), for the galvanic cell?

- **A.** \(-0.93\text{ V}\)
- **B.** \(+0.67\text{ V}\)
- **C.** \(+0.93\text{ V}\)
- **D.** \(+1.73\text{ V}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119285/*