---
title: "A student constructs a galvanic cell operating under standard conditions using the two half-reactions shown below.  \\(\\text{Ag}^+\\text{(aq)} + e^- \\rightarrow \\text{Ag(s)} \\quad E^\\circ = +0.80 \\text{ V}\\) \\(\\text{Zn}^{2+}\\text{(aq)} + 2 e^- \\rightarrow \\text{Zn(s)} \\quad E^\\circ = -0.76 \\text{ V}\\)  Which of the following balanced net-ionic equations represents the overall spontaneous reaction occurring in the cell?"
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url: "https://nerd-notes.com/ubq/119282/"
date_modified: "2026-08-19T12:39:38+00:00"
---

# A student constructs a galvanic cell operating under standard conditions using the two half-reactions shown below.

\(\text{Ag}^+\text{(aq)} + e^- \rightarrow \text{Ag(s)} \quad E^\circ = +0.80 \text{ V}\)
\(\text{Zn}^{2+}\text{(aq)} + 2 e^- \rightarrow \text{Zn(s)} \quad E^\circ = -0.76 \text{ V}\)

Which of the following balanced net-ionic equations represents the overall spontaneous reaction occurring in the cell?

A student constructs a galvanic cell operating under standard conditions using the two half-reactions shown below.

\(\text{Ag}^+\text{(aq)} + e^- \rightarrow \text{Ag(s)} \quad E^\circ = +0.80 \text{ V}\)
\(\text{Zn}^{2+}\text{(aq)} + 2 e^- \rightarrow \text{Zn(s)} \quad E^\circ = -0.76 \text{ V}\)

Which of the following balanced net-ionic equations represents the overall spontaneous reaction occurring in the cell?

- **A.** \(\text{Zn(s)} + 2\text{Ag}^+\text{(aq)} \rightarrow \text{Zn}^{2+}\text{(aq)} + 2\text{Ag(s)}\)
- **B.** \(\text{Zn(s)} + \text{Ag}^+\text{(aq)} \rightarrow \text{Zn}^{2+}\text{(aq)} + \text{Ag(s)}\)
- **C.** 2\(\text{Ag(s)} + \text{Zn}^{2+}\text{(aq)} \rightarrow 2\text{Ag}^+\text{(aq)} + \text{Zn(s)}\)
- **D.** \(\text{Ag(s)} + \text{Zn}^{2+}\text{(aq)} \rightarrow \text{Ag}^+\text{(aq)} + \text{Zn(s)}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119282/*