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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

Explain the following observations: (a) For a given oxidation state, the acid strength of the oxyacid in aqueous solution decreases in the order chlorine \(>\) bromine \(>\) iodine.(b) Hydrofluoric acid cannot be stored in glass bottles. (c) HI cannot be prepared by treating Nal with sulfuric acid. ( \(\mathbf{d}\) ) The interhalogen ICl_ is known, but BrCl_ is not.

Account for the following observations: (a) \(\mathrm{H}_{3} \mathrm{PO}_{3}\) is a diprotic acid. (b) Nitric acid is a strong acid, whereas phosphoric acid is weak. (c) Phosphate rock is ineffective as a phosphate fertilizer. (d) Phosphorus does not exist at room temperature as diatomic molecules, but nitrogen does. (e) Solutions of \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) are quite basic.

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) sodium nitrite, (b) ammonia, (c) nitrous oxide, (d) sodium cyanide, (e) nitric acid, (f) nitrogen dioxide, (g) nitrogen, (h) boron nitride.

Complete and balance the following equations:$$ \begin{array}{l}{\text { (a) } \mathrm{ZnCO}_{3}(s) \stackrel{\Delta}{\longrightarrow}} \\ {\text { (b) } \mathrm{BaC}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { (c) } \mathrm{C}_{2} \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow}\end{array} $$ $$\begin{array}{l}{\text { (c) ~ } \mathrm{CS}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow} \\ {\text { (e) } \mathrm{Ca}(\mathrm{CN})_{2}(s)+\mathrm{HBr}(a q) \longrightarrow}\end{array}$$

What is the anhydride for each of the following acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4},(\mathbf{b}) \mathrm{HClO}_{3},(\mathbf{c}) \mathrm{HNO}_{2},(\mathbf{d}) \mathrm{H}_{2} \mathrm{CO}_{3},(\mathbf{e}) \mathrm{H}_{3} \mathrm{PO}_{4} ?\)
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