---
title: "A standard galvanic cell is constructed using two half-cells connected by a salt bridge and an external wire with a voltmeter at \\(298\\text{ K}\\). The standard reduction potentials for the two half-reactions are given below.  \\[\\text{Fe}^{2+}\\text{(aq)} + 2\\,\\text{e}^- \\rightarrow \\text{Fe(s)} \\quad E^\\circ = -0.44\\text{ V}\\] \\[\\text{Ag}^+\\text{(aq)} + \\text{e}^- \\rightarrow \\text{Ag(s)} \\quad E^\\circ = +0.80\\text{ V}\\]  Which of the following correctly identifies the direction of electron flow through the external wire and the standard cell potential, \\(E^\\circ_{\\text{cell}}\\), when the cell operates spontaneously?"
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url: "https://nerd-notes.com/ubq/121414/"
date_modified: "2026-08-23T05:02:09+00:00"
---

# A standard galvanic cell is constructed using two half-cells connected by a salt bridge and an external wire with a voltmeter at \(298\text{ K}\). The standard reduction potentials for the two half-reactions are given below.

\[\text{Fe}^{2+}\text{(aq)} + 2\,\text{e}^- \rightarrow \text{Fe(s)} \quad E^\circ = -0.44\text{ V}\]
\[\text{Ag}^+\text{(aq)} + \text{e}^- \rightarrow \text{Ag(s)} \quad E^\circ = +0.80\text{ V}\]

Which of the following correctly identifies the direction of electron flow through the external wire and the standard cell potential, \(E^\circ_{\text{cell}}\), when the cell operates spontaneously?

A standard galvanic cell is constructed using two half-cells connected by a salt bridge and an external wire with a voltmeter at \(298\text{ K}\). The standard reduction potentials for the two half-reactions are given below.

\[\text{Fe}^{2+}\text{(aq)} + 2\,\text{e}^- \rightarrow \text{Fe(s)} \quad E^\circ = -0.44\text{ V}\]
\[\text{Ag}^+\text{(aq)} + \text{e}^- \rightarrow \text{Ag(s)} \quad E^\circ = +0.80\text{ V}\]

Which of the following correctly identifies the direction of electron flow through the external wire and the standard cell potential, \(E^\circ_{\text{cell}}\), when the cell operates spontaneously?

- **A.** | From the \(\text{Fe}\) electrode to the \(\text{Ag}\) electrode | \(+0.36\text{ V}\) |
- **B.** | From the \(\text{Fe}\) electrode to the \(\text{Ag}\) electrode | \(+1.24\text{ V}\) |
- **C.** | From the \(\text{Ag}\) electrode to the \(\text{Fe}\) electrode | \(+1.24\text{ V}\) |
- **D.** | From the \(\text{Ag}\) electrode to the \(\text{Fe}\) electrode | \(+2.04\text{ V}\) |

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121414/*