AP Chemistry
4.9 Oxidation-Reduction (Redox) Reactions
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?
\(\text{Cu(s)} + 4\text{H}^+\text{(aq)} + 2\text{NO}_3^-\text{(aq)} \rightarrow \text{Cu}^{2+}\text{(aq)} + 2\text{NO}_2\text{(g)} + 2\text{H}_2\text{O(l)}\)
Which species is the oxidizing agent in the reaction?
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