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Chapter 22: Problem 55

Write complete balanced half-reactions for (a) oxidation of nitrous acid to nitrate ion in acidic solution, (b) oxidation of \(\mathrm{N}_{2}\) to \(\mathrm{N}_{2} \mathrm{O}\) in acidic solution.

Short Answer

Expert verified
The balanced half-reactions for the given processes are: (a) Oxidation of nitrous acid to nitrate ion in an acidic solution: \(HNO_2 + H_2O \rightarrow NO_3^- + 2H^+ + e^-\) (b) Oxidation of N2 to N2O in an acidic solution: \(N_2 + H_2O \rightarrow N_2O + 2H^+ + 2e^-\)

Step by step solution

01

Write Down the Unbalanced Half-reaction

Identify the reactants and products: \(HNO_2 \rightarrow NO_3^-\)
02

Balance Atoms Except H and O

The nitrogen atoms are already balanced in the half-reaction.
03

Balance Oxygen Atoms With Water

Add 1 water molecule to the left side to balance the oxygen atoms: \(HNO_2 + H_2O \rightarrow NO_3^-\)
04

Balance Hydrogen Atoms With H+ Ions

Add 2 H+ ions to the right side to balance the hydrogen atoms: \(HNO_2 + H_2O \rightarrow NO_3^- + 2H^+\)
05

Balance Charge With Electrons

Add 1 electron to the right side to balance the charges: \(HNO_2 + H_2O \rightarrow NO_3^- + 2H^+ + e^-\)
06

Check the Balance

Atoms: 1 N, 3 O, and 3 H on each side. Charge: 0 on both sides. Thus, the balanced half-reaction for oxidation of nitrous acid to nitrate ion in an acidic solution is: \(HNO_2 + H_2O \rightarrow NO_3^- + 2H^+ + e^-\) (b) Oxidation of N2 to N2O in an acidic solution
07

Write Down the Unbalanced Half-reaction

Identify the reactants and products: \(N_2 \rightarrow N_2O\)
08

Balance Atoms Except H and O

The nitrogen atoms are already balanced in the half-reaction.
09

Balance Oxygen Atoms With Water

Add 1 water molecule to the left side to balance the oxygen atoms: \(N_2 + H_2O \rightarrow N_2O\)
10

Balance Hydrogen Atoms With H+ Ions

Add 2 H+ ions to the right side to balance the hydrogen atoms: \(N_2 + H_2O \rightarrow N_2O + 2H^+\)
11

Balance Charge With Electrons

Add 2 electrons to the right side to balance the charges: \(N_2 + H_2O \rightarrow N_2O + 2H^+ + 2e^-\)
12

Check the Balance

Atoms: 2 N, 1 O, and 2 H on each side. Charge: 0 on both sides. Thus, the balanced half-reaction for oxidation of N2 to N2O in an acidic solution is: \(N_2 + H_2O \rightarrow N_2O + 2H^+ + 2e^-\)

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Most popular questions from this chapter

Write a balanced equation for each of the following reactions: (a) Sulfur dioxide reacts with water. (b) Solid zinc sulfide reacts with hydrochloric acid. (c) Elemental sulfur reacts with sulfite ion to form thiosulfate. (d) Sulfur trioxide is dissolved in sulfuric acid.

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) dinitrogen trioxide, (b) dinitrogen pentoxide, (c) hydrogen cyanide, (d) ammonium nitrate, (e) iron(III) nitrite, \((\mathbf{f})\) nitrogen trichloride.

Write the chemical formula for each of the following, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) krypton tetrafluoride, (b) hexafluoroantimonate ion, \((\mathbf{c})\) sodium hypoiodite, \((\mathbf{d})\) perbromic acid, (e) aluminum perchlorate, (f) iron(II) iodite.

Identify the following hydrides as ionic, metallic, or molecular: $(\mathbf{a}) \mathrm{H}_{2} \mathrm{~S},(\mathbf{b}) \mathrm{LiH},(\mathbf{c}) \mathrm{VH}_{0.56}$.

The dissolved oxygen present in any highly pressurized, high-temperature steam boiler can be extremely corrosive to its metal parts. Hydrazine, which is completely miscible with water, can be added to remove oxygen by reacting with it to form nitrogen and water. (a) Write the balanced equation for the reaction between gaseous hydrazine and oxygen. (b) Calculate the enthalpy change accompanying this reaction. (c) Oxygen in air dissolves in water to the extent of 9.1 ppm at \(20^{\circ} \mathrm{C}\) at sea level. How many grams of hydrazine are required to react with all the oxygen in $3.0 \times 10^{4} \mathrm{~L}$ (the volume of a small swimming pool) under these conditions?
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