---
title: "A galvanic cell is constructed at \\(298\\text{ K}\\) using zinc and copper half-cells connected by an external wire and a salt bridge containing \\(\\text{KNO}_3\\text{(aq)}\\), as shown in the diagram. The standard reduction potentials for the two half-reactions are given below.  \\[\\text{Zn}^{2+}\\text{(aq)} + 2\\,e^- \\rightarrow \\text{Zn(s)} \\quad E^\\circ = -0.76\\text{ V}\\] \\[\\text{Cu}^{2+}\\text{(aq)} + 2\\,e^- \\rightarrow \\text{Cu(s)} \\quad E^\\circ = +0.34\\text{ V}\\]  Which of the following correctly describes the direction of electron flow in the external circuit and the movement of ions from the salt bridge as the cell operates spontaneously?"
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url: "https://nerd-notes.com/ubq/119956/"
date_modified: "2026-08-21T08:24:53+00:00"
---

# A galvanic cell is constructed at \(298\text{ K}\) using zinc and copper half-cells connected by an external wire and a salt bridge containing \(\text{KNO}_3\text{(aq)}\), as shown in the diagram. The standard reduction potentials for the two half-reactions are given below.

\[\text{Zn}^{2+}\text{(aq)} + 2\,e^- \rightarrow \text{Zn(s)} \quad E^\circ = -0.76\text{ V}\]
\[\text{Cu}^{2+}\text{(aq)} + 2\,e^- \rightarrow \text{Cu(s)} \quad E^\circ = +0.34\text{ V}\]

Which of the following correctly describes the direction of electron flow in the external circuit and the movement of ions from the salt bridge as the cell operates spontaneously?

A galvanic cell is constructed at \(298\text{ K}\) using zinc and copper half-cells connected by an external wire and a salt bridge containing \(\text{KNO}_3\text{(aq)}\), as shown in the diagram. The standard reduction potentials for the two half-reactions are given below.

\[\text{Zn}^{2+}\text{(aq)} + 2\,e^- \rightarrow \text{Zn(s)} \quad E^\circ = -0.76\text{ V}\]
\[\text{Cu}^{2+}\text{(aq)} + 2\,e^- \rightarrow \text{Cu(s)} \quad E^\circ = +0.34\text{ V}\]

Which of the following correctly describes the direction of electron flow in the external circuit and the movement of ions from the salt bridge as the cell operates spontaneously?

![A schematic grayscale drawing of an electrochemical cell with two open beakers side by side. The left beaker is filled with a solution labeled \(1.0\text{ M Zn(NO}_3)_2\text{(aq)}\) and contains a vertical gray rectangular strip labeled \(\text{Zn(s)}\). The right beaker is filled with a solution labeled \(1.0\text{ M Cu(NO}_3)_2\text{(aq)}\) and contains a vertical stippled rectangular strip labeled \(\text{Cu(s)}\). An inverted U-shaped tube labeled \(\text{KNO}_3\text{(aq)}\) has its open ends immersed into the two solutions. A single line representing a wire connects the top of the \(\text{Zn(s)}\) strip to the top of the \(\text{Cu(s)}\) strip through a circular meter labeled \(\text{V}\). No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1787300693-OlYo8C.jpg)

- **A.** Electrons flow from the \(\text{Cu}\) electrode to the \(\text{Zn}\) electrode, while \(\text{K}^+\) ions migrate toward the \(\text{Zn}^{2+}\) solution and \(\text{NO}_3^-\) ions migrate toward the \(\text{Cu}^{2+}\) solution.
- **B.** Electrons flow from the \(\text{Zn}\) electrode to the \(\text{Cu}\) electrode, while \(\text{K}^+\) ions migrate toward the \(\text{Zn}^{2+}\) solution and \(\text{NO}_3^-\) ions migrate toward the \(\text{Cu}^{2+}\) solution.
- **C.** Electrons flow from the \(\text{Cu}\) electrode to the \(\text{Zn}\) electrode, while \(\text{NO}_3^-\) ions migrate toward the \(\text{Zn}^{2+}\) solution and \(\text{K}^+\) ions migrate toward the \(\text{Cu}^{2+}\) solution.
- **D.** Electrons flow from the \(\text{Zn}\) electrode to the \(\text{Cu}\) electrode, while \(\text{NO}_3^-\) ions migrate toward the \(\text{Zn}^{2+}\) solution and \(\text{K}^+\) ions migrate toward the \(\text{Cu}^{2+}\) solution.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119956/*