Question

Nitrogen monoxide, $\mathrm{NO}(g),$ reacts with phosphorus, $\mathrm{P}_{4}(s)$ , to produce nitrogen, $\mathrm{N}_{2}(g),$ and diphosphorus pentoxide, $\mathrm{P}_{2} \mathrm{O}_{5}$ Write the balanced equation for this reaction. Identify the atoms that have been oxidized and reduced, and identify the oxidizing and reducing agents.

          Nitrogen monoxide, $\mathrm{NO}(g),$ reacts with
phosphorus, $\mathrm{P}_{4}(s)$ , to produce nitrogen,
$\mathrm{N}_{2}(g),$ and diphosphorus pentoxide, $\mathrm{P}_{2} \mathrm{O}_{5}$
Write the balanced equation for this reaction. Identify the atoms that have been
oxidized and reduced, and identify the
oxidizing and reducing agents.

Added by Whitney M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ma Ednelyn Lim

04/11/2022

Step 1

Step 1:** Write the balanced chemical equation for the reaction: $$\mathrm{4NO(g) + P_{4}(s) \rightarrow 4N_{2}(g) + P_{2}O_{5}(s)}$$ ** Show more…

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Nitrogen monoxide, $\mathrm{NO}(g),$ reacts with phosphorus, $\mathrm{P}_{4}(s)$ , to produce nitrogen, $\mathrm{N}_{2}(g),$ and diphosphorus pentoxide, $\mathrm{P}_{2} \mathrm{O}_{5}$ Write the balanced equation for this reaction. Identify the atoms that have been oxidized and reduced, and identify the oxidizing and reducing agents.