---
title: "A student uses concentrated nitric acid to dissolve copper from a metal sample. The net ionic equation for the reaction is shown below.  \\(\\text{Cu(s)} + 4\\text{H}^+\\text{(aq)} + 2\\text{NO}_3^-\\text{(aq)} \\rightarrow \\text{Cu}^{2+}\\text{(aq)} + 2\\text{NO}_2\\text{(g)} + 2\\text{H}_2\\text{O(l)}\\)  Which species is the oxidizing agent in the reaction?"
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url: "https://nerd-notes.com/ubq/119309/"
date_modified: "2026-08-19T12:39:44+00:00"
---

# A student uses concentrated nitric acid to dissolve copper from a metal sample. The net ionic equation for the reaction is shown below.

\(\text{Cu(s)} + 4\text{H}^+\text{(aq)} + 2\text{NO}_3^-\text{(aq)} \rightarrow \text{Cu}^{2+}\text{(aq)} + 2\text{NO}_2\text{(g)} + 2\text{H}_2\text{O(l)}\)

Which species is the oxidizing agent in the reaction?

A student uses concentrated nitric acid to dissolve copper from a metal sample. The net ionic equation for the reaction is shown below.

\(\text{Cu(s)} + 4\text{H}^+\text{(aq)} + 2\text{NO}_3^-\text{(aq)} \rightarrow \text{Cu}^{2+}\text{(aq)} + 2\text{NO}_2\text{(g)} + 2\text{H}_2\text{O(l)}\)

Which species is the oxidizing agent in the reaction?

- **A.** \(\text{Cu(s)}\)
- **B.** \(\text{H}^+\text{(aq)}\)
- **C.** \(\text{NO}_2\text{(g)}\)
- **D.** \(\text{NO}_3^-\text{(aq)}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119309/*