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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 are: (a) Oxidation of HNO2 to NO3- in acidic solution: \(HNO_{2} + H_{2}O \rightarrow NO_{3}^{-} + 3H^{+} + 2e^{-}\) (b) Oxidation of N2 to N2O in acidic solution: \(N_{2} + H_{2}O \rightarrow N_{2}O + 2H^{+} + 2e^{-}\)

Step by step solution

01

Identify the species being oxidized

The species being oxidized in this process is nitrous acid (HNO2), and the product is the nitrate ion (NO3-).
02

Balance elements excluding oxygen and hydrogen

There is only one nitrogen atom on both sides, so the nitrogen atoms are already balanced: \(HNO_{2} \rightarrow NO_{3}^{-}\)
03

Balance oxygen atoms

There are two oxygen atoms in HNO2 and three in NO3-. Add one H2O molecule to the left side to balance the oxygens: \(HNO_{2} + H_{2}O \rightarrow NO_{3}^{-}\)
04

Balance hydrogen atoms

There are now three hydrogen atoms on the left side of the equation and none on the right side. Add three H+ ions to the right side to balance the hydrogens: \(HNO_{2} + H_{2}O \rightarrow NO_{3}^{-} + 3H^{+}\)
05

Balance electrical charges

The left side has a total charge of 0 while the right side has a total charge of +2. Add two electrons (e-) to the right side to balance the electrical charges: \(HNO_{2} + H_{2}O \rightarrow NO_{3}^{-} + 3H^{+} + 2e^{-}\)
06

Verify the balanced half-reaction

The resulting balanced half-reaction looks like this: \(HNO_{2} + H_{2}O \rightarrow NO_{3}^{-} + 3H^{+} + 2e^{-}\) We can verify that it is correctly balanced, as there is an equal number of atoms of each element on both sides of the equation, and the overall charges are equal. ##Oxidation of N2 to N2O in acidic solution##
07

Identify the species being oxidized

The species being oxidized in this process is nitrogen gas (N2), and the product is nitrous oxide (N2O).
08

Balance elements excluding oxygen and hydrogen

There are two nitrogen atoms on both sides, so the nitrogen atoms are already balanced: \(N_{2} \rightarrow N_{2}O\)
09

Balance oxygen atoms

There are no oxygen atoms in N2, but one in N2O. Add one H2O molecule to the left side to balance the oxygen: \(N_{2} + H_{2}O \rightarrow N_{2}O\)
10

Balance hydrogen atoms

There are two hydrogen atoms on the left side of the equation and none on the right side. Add two H+ ions to the right side to balance the hydrogens: \(N_{2} + H_{2}O \rightarrow N_{2}O + 2H^{+}\)
11

Balance electrical charges

The left side has a total charge of 0 while the right side has a total charge of +2. Add two electrons (e-) to the right side to balance the electrical charges: \(N_{2} + H_{2}O \rightarrow N_{2}O + 2H^{+} + 2e^{-}\)
12

Verify the balanced half-reaction

The resulting balanced half-reaction looks like this: \(N_{2} + H_{2}O \rightarrow N_{2}O + 2H^{+} + 2e^{-}\) We can verify that it is correctly balanced, as there is an equal number of atoms of each element on both sides of the equation, and the overall charges are equal.

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Most popular questions from this chapter

Select the more acidic member of each of the following pairs: (a) \(\mathrm{Mn}_{2} \mathrm{O}_{7}\) and \(\mathrm{MnO}_{2},(\mathbf{b}) \mathrm{SnO}\) and \(\mathrm{SnO}_{2},(\mathbf{c}) \mathrm{SO}_{2}\) and \(\mathrm{SO}_{3},(\mathbf{d}) \mathrm{SiO}_{2}\) and \(\mathrm{SO}_{2},(\mathbf{e}) \mathrm{Ga}_{2} \mathrm{O}_{3}\) and \(\mathrm{In}_{2} \mathrm{O}_{3},(\mathbf{f}) \mathrm{SO}_{2}\) and \(\mathrm{SeO}_{2} .\)

The maximum allowable concentration of \(\mathrm{H}_{2} \mathrm{S}(g)\) in air is 20 mg per kilogram of air \((20\) ppm by mass). How many grams of FeS would be required to react with hydrochloric acid to produce this concentration at 1.00 atm and \(25^{\circ} \mathrm{C}\) in an average room measuring 12 \(\mathrm{ft} \times 20 \mathrm{ft} \times 8 \mathrm{ft}\) ? (Under these conditions, the average molar mass of air is 29.0 \(\mathrm{g} / \mathrm{mol.} )\)

Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the nitrogen: (a) \(\mathrm{NH}_{4}^{+},(\mathbf{b}) \mathrm{NO}_{2}^{-},(\mathbf{c}) \mathrm{N}_{2} \mathrm{O},(\mathbf{d}) \mathrm{NO}_{2}\)

Indicate whether each of the following statements is true or false (a) \(\mathrm{H}_{2}(g)\) and \(\mathrm{D}_{2}(g)\) are allotropic forms of hydrogen. (b) \(\mathrm{ClF}_{3}\) is an interhalogen compound. (c) MgO(s) is an acidic anhydride. (d) \(\mathrm{SO}_{2}(g)\) is an acidic anhydride. (e) \(2 \mathrm{H}_{3} \mathrm{PO}_{4}(l) \rightarrow \mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7}(l)+\mathrm{H}_{2} \mathrm{O}(g)\) is an example of a condensation reaction. (f) Tritium is an isotope of the element hydrogen. (g) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{SO}_{3}(g)\) is an example of a disproportionation reaction.

A sulfuric acid plant produces a considerable amount of heat. This heat is used to generate electricity, which helps reduce operating costs. The synthesis of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) consists of three main chemical processes: (a) oxidation of S to SO, (b) oxidation of \(\mathrm{SO}_{2}\) to \(\mathrm{SO}_{3},\) (c) the dissolving of \(\mathrm{SO}_{3}\) in \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and the subsequent reaction with water to form \(\mathrm{H}_{2} \mathrm{SO}_{4}\) . If the third process produces \(130 \mathrm{kJ} / \mathrm{mol},\) how much heat is produced in preparing a mole of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from a mole of S? How much heat is produced in preparing 5000 pounds of \(\mathrm{H}_{2} \mathrm{SO}_{4} ?\)
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