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Chapter 17: Problem 19

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.

Short Answer

Expert verified
The balanced equation is \(5NO + P_4 \rightarrow 2N_2 + P_2O_5\). Nitrogen is reduced, phosphorus is oxidized, \(NO\) is the oxidizing agent, and \(P_4\) is the reducing agent.

Step by step solution

01

Write the Unbalanced Chemical Equation

The reaction involves nitrogen monoxide (\(NO\)) and phosphorus (\(P_4\)) reacting to form nitrogen (\(N_2\)) and diphosphorus pentoxide (\(P_2O_5\)). So the unbalanced chemical equation is: \(NO + P_4 \rightarrow N_2 + P_2O_5\)
02

Balance the Chemical Equation

Balance the equation by adjusting coefficients. The balanced equation is: \(5NO + P_4 \rightarrow 2N_2 + P_2O_5\)
03

Identify the Oxidized and Reduced Atoms

In the reaction, the nitrogen in NO is reduced to N2 (the oxidation state goes from +2 in NO to 0 in N2). Therefore, Nitrogen (\(N\)) is reduced. The phosphorus in P4 is oxidized to P in P2O5 (the oxidation state goes from 0 in P4 to +5 in P2O5). Therefore, Phosphorus (\(P\)) is oxidized.
04

Identify the Oxidizing and Reducing Agents

The oxidizing agent is the substance that gets reduced (gains electrons), so nitrogen monoxide (\(NO\)) is the oxidizing agent. The reducing agent is the substance that gets oxidized (loses electrons), so phosphorus (\(P_4\)) is the reducing agent.

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