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Chapter 22: Problem 56

Write a balanced net ionic equation for each of the following reactions: (a) Dilute nitric acid reacts with zinc metal with formation of nitrous oxide. (b) Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide. (c) Concentrated nitric acid oxidizes sulfur dioxide with formation of nitric oxide. (d) Hydrazine is burned in excess fluorine gas, forming \(\mathrm{NF}_{3}\). (e) Hydrazine reduces \(\mathrm{CrO}_{4}^{2-}\) to \(\mathrm{Cr}(\mathrm{OH})_{4}^{-}\) in base (hydrazine is oxidized to \(\mathrm{N}_{2}\) ).

Short Answer

Expert verified
(a) \(Zn + 4H^+ + 4NO^-_2 \rightarrow Zn^{2+} + 2NO + 2NO_2 + 2H_2O\) (b) \(6H^+ + 6NO^-_3 + S \rightarrow 2H^+ + SO^{2-}_4 + 6NO_2 + 2H_2O\) (c) \(2NO^-_3 + SO_2 \rightarrow NO + NO_2 + SO^{2-}_4\) (d) \(2F_2 + N_2H_4 \rightarrow 4NF_3\) (e) \(N_2H_4 + 2Cr^{6+} + 8O^{2-} + OH^- \rightarrow N_2 + 2Cr^{3+} + 8OH^-\)

Step by step solution

01

Reaction (a) - Dilute nitric acid reacts with zinc metal with formation of nitrous oxide

First, write the balanced molecular equation: \(Zn + 4HNO_2 \rightarrow Zn^{2+} + 2NO + 2NO_2 + 2H_2O\) Now, break apart the strong electrolytes into their ions to get the total ionic equation: \(Zn + 4H^+ + 4NO^-_2 \rightarrow Zn^{2+} + 2NO + 2NO_2 + 2H_2O\) Group the same ions on both sides and cross out the spectator ions (none in this case). The remaining equation is the net ionic equation: \(Zn + 4H^+ + 4NO^-_2 \rightarrow Zn^{2+} + 2NO + 2NO_2 + 2H_2O\)
02

Reaction (b) - Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide

First, write the balanced molecular equation: \(6HNO_3 + S \rightarrow H_2SO_4 + 6NO_2 + 2H_2O\) Next, break apart the strong electrolytes into their ions to get the total ionic equation: \(6H^+ + 6NO^-_3 + S \rightarrow 2H^+ + SO^{2-}_4 + 6NO_2 + 2H_2O\) Group the same ions on both sides and cross out the spectator ions (none in this case). The remaining equation is the net ionic equation: \(6H^+ + 6NO^-_3 + S \rightarrow 2H^+ + SO^{2-}_4 + 6NO_2 + 2H_2O\)
03

Reaction (c) - Concentrated nitric acid oxidizes sulfur dioxide with formation of nitric oxide

First, write the balanced molecular equation: \(2HNO_3 + SO_2 \rightarrow NO + NO_2 + H_2SO_4\) Next, break apart the strong electrolytes into their ions to get the total ionic equation: \(2H^+ + 2NO^-_3 + SO_2 \rightarrow NO + NO_2 + 2H^+ + SO^{2-}_4\) Group the same ions on both sides and cross out the spectator ions (H^+ in this case). The remaining equation is the net ionic equation: \(2NO^-_3 + SO_2 \rightarrow NO + NO_2 + SO^{2-}_4\)
04

Reaction (d) - Hydrazine is burned in excess fluorine gas, forming \(\mathrm{NF}_{3}\)

First, write the balanced molecular equation: \(2F_2 + N_2H_4 \rightarrow 4NF_3\) This reaction does not involve ions, so no further decomposition is needed. The net ionic equation is the same as the molecular equation: \(2F_2 + N_2H_4 \rightarrow 4NF_3\)
05

Reaction (e) - Hydrazine reduces \(\mathrm{CrO}_{4}^{2-}\) to \(\mathrm{Cr}(\mathrm{OH})_{4}^{-}\) in base (hydrazine is oxidized to \(\mathrm{N}_{2}\) )

First, write the balanced molecular equation: \(N_2H_4 + 2CrO^{2-}_4 + OH^- \rightarrow N_2 + 2Cr(OH^-)_4\) Next, break apart the strong electrolytes into their ions to get the total ionic equation: \(N_2H_4 + 2Cr^{6+} + 8O^{2-} + OH^- \rightarrow N_2 + 2Cr^{3+} + 8OH^-\) Group the same ions on both sides and cross out the spectator ions (none in this case). The remaining equation is the net ionic equation: \(N_2H_4 + 2Cr^{6+} + 8O^{2-} + OH^- \rightarrow N_2 + 2Cr^{3+} + 8OH^-\)

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Most popular questions from this chapter

The atomic and ionic radii of the first three group \(6 \mathrm{~A}\) elements are (a) Explain why the atomic radius increases in moving downward in the group. (b) Explain why the ionic radii are larger than the atomic radii. (c) Which of the three anions would you expect to be the strongest base in water? Explain. [Sections 22.5 and 22.6\(]\)

Write a balanced equation for each of the following reactions: (a) Diborane reacts with water to form boric acid and molecular hydrogen. (b) Upon heating, boric acid undergoes a condensation reaction to form tetraboric acid. (c) Boron oxide dissolves in water to give a solution of boric acid.

(a) Draw the Lewis structures for at least four species that have the general formula $$ [: X=Y:]^{n} $$ where \(\mathrm{X}\) and \(\mathrm{Y}\) may be the same or different, and \(n\) may have a value from +1 to -2 . (b) Which of the compounds is likely to be the strongest Bronsted base? Explain. [Sections \(22.1,22.7,\) and 22.9\(]\)

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.

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.
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