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Chapter 22: Problem 56

Write complete balanced half-reactions for (a) reduction of nitrate ion to NO in acidic solution, (b) oxidation of \(\mathrm{HNO}_{2}\) to \(\mathrm{NO}_{2}\) in acidic solution.

Short Answer

Expert verified
(a) \(NO_3^- + 3e^- + 4H^+ -> NO + 2H_2O\) (b) \(HNO_2 + H^+ -> NO_2 + 2H_2O + 2e^-\)

Step by step solution

01

For the reduction reaction (a), the nitrate ion (NO3-) will be reduced to nitric oxide (NO), and for the oxidation reaction (b), nitrous acid (HNO2) will be oxidized to nitrogen dioxide (NO2). (a) NO3- -> NO (b) HNO2 -> NO2 #Step 2: Balance the elements other than oxygen and hydrogen#

In both cases, nitrogen is already balanced, as there is one nitrogen atom on each side of the reactions. (a) NO3- -> NO (b) HNO2 -> NO2 #Step 3: Balance oxygen atoms by adding water molecules#
02

We will add water molecules to balance the oxygen atoms. (a) NO3- -> NO + 2H2O (b) HNO2 -> NO2 + H2O #Step 4: Balance hydrogen atoms by adding H+ ions#

Let's balance the hydrogen atoms by adding H+ ions to the reactions. (a) NO3- + 4H+ -> NO + 2H2O (b) HNO2 + H+ -> NO2 + 2H2O #Step 5: Balance the charges by adding electrons#
03

Now, we will balance the charges by adding electrons to the appropriate side of the reactions. (a) NO3- + 3e- + 4H+ -> NO + 2H2O (b) HNO2 + H+ -> NO2 + 2H2O + 2e- #Step 6: Write the balanced half-reactions#

We can now write the balanced half-reactions for each case. (a) NO3- + 3e- + 4H+ -> NO + 2H2O (b) HNO2 + H+ -> NO2 + 2H2O + 2e- The balanced half-reactions for the reduction of nitrate ion to NO in acidic solution are given by (a) and for the oxidation of HNO2 to NO2 in acidic solution by (b) respectively.

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Most popular questions from this chapter

Manganese silicide has the empirical formula \(\mathrm{MnSi}\) and melts at \(1280^{\circ} \mathrm{C}\). It is insoluble in water but does dissolve in aqueous HF. (a) What type of compound do you expect \(\mathrm{MnSi}\) to be: metallic, molecular, covalent-network, or ionic? (b) Write a likely balanced chemical equation for the reaction of MnSi with concentrated aqueous \(\mathrm{HF}\).

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Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) sodium azide, (b) ammonium ion, (c) nitrous acid, \((\mathbf{d})\) magnesium nitride, \((\mathbf{e})\) diazene, \((\mathbf{f})\) sodium nitrate, (g) nitrogen trifluoride, (h) nitric acid.

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