---
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 | $E^\\circ\\text{ (V)}$ | | :— | :— | | $\\text{Ag}^+\\text{(aq)} + e^- \\rightarrow \\text{Ag(s)}$ | $+0.80$ | | $\\text{Pb}^{2+}\\text{(aq)} + 2e^- \\rightarrow \\text{Pb(s)}$ | $-0.13$ |  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: "2026-08-19T12:39:39+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 | $E^\circ\text{ (V)}$ |
| :— | :— |
| $\text{Ag}^+\text{(aq)} + e^- \rightarrow \text{Ag(s)}$ | $+0.80$ |
| $\text{Pb}^{2+}\text{(aq)} + 2e^- \rightarrow \text{Pb(s)}$ | $-0.13$ |

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

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/*