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title: "A student places a strip of solid zinc, \\(\\text{Zn}(s)\\), into an aqueous solution of silver nitrate, \\(\\text{AgNO}_3(aq)\\). Solid silver crystals form on the surface of the zinc strip as zinc ions enter the solution according to the following balanced chemical equation: \\[\\text{Zn}(s) + 2\\text{AgNO}_3(aq) \\rightarrow \\text{Zn(NO}_3)_2(aq) + 2\\text{Ag}(s)\\] Which species acts as the reducing agent in this reaction?"
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url: "https://nerd-notes.com/ubq/119207/"
date_modified: "2026-08-19T12:39:21+00:00"
---

# A student places a strip of solid zinc, \(\text{Zn}(s)\), into an aqueous solution of silver nitrate, \(\text{AgNO}_3(aq)\). Solid silver crystals form on the surface of the zinc strip as zinc ions enter the solution according to the following balanced chemical equation: \[\text{Zn}(s) + 2\text{AgNO}_3(aq) \rightarrow \text{Zn(NO}_3)_2(aq) + 2\text{Ag}(s)\] Which species acts as the reducing agent in this reaction?

A student places a strip of solid zinc, \(\text{Zn}(s)\), into an aqueous solution of silver nitrate, \(\text{AgNO}_3(aq)\). Solid silver crystals form on the surface of the zinc strip as zinc ions enter the solution according to the following balanced chemical equation: \[\text{Zn}(s) + 2\text{AgNO}_3(aq) \rightarrow \text{Zn(NO}_3)_2(aq) + 2\text{Ag}(s)\] Which species acts as the reducing agent in this reaction?

- **A.** \(\text{Ag}^+(aq)\)
- **B.** \(\text{Ag}(s)\)
- **C.** \(\text{Zn}(s)\)
- **D.** \(\text{NO}_3^-(aq)\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119207/*