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Chapter 22: Problem 54

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
\(a) Zn + 10H^+ \rightarrow 2Zn^{2+} + N_2O + 6H_2O\) \(b) S + 2H^+ \rightarrow SO_4^{2-} + 6NO_2\) \(c) 2SO_2 \rightarrow 4NO + 2SO_4^{2-}\) \(d) N_2H_4 + 3F_2 \rightarrow 4NF_3\) \(e) N_2H_4 + CrO_4^{2-} + 4H_2O \rightarrow N_2 + Cr(OH)_4^-\)

Step by step solution

01

Write the unbalanced chemical equation

Identify the reactants and products of the reaction: Zn + HNO3 -> Zn(NO3)2 + N2O + H2O
02

Balance the chemical equation

Balance the equation by adjusting the coefficients of the reactants and products: 2Zn + 5HNO3 -> 2Zn(NO3)2 + N2O + 3H2O
03

Write the net ionic equation

Break down the ionic compounds and eliminate spectator ions (NO₃⁻): Zn + 10H⁺ + 6NO₃⁻ -> 2Zn²⁺ + 12NO₃⁻ + N₂O + 6H₂O The net ionic equation will be: Zn + 10H⁺ -> 2Zn²⁺ + N₂O + 6H₂O ---------------------------------------------------------------- #b) Concentrated nitric acid reacts with sulfur#
04

Write the unbalanced chemical equation

Identify the reactants and products of the reaction: S + HNO3 -> H2SO4 + NO2
05

Balance the chemical equation

Balance the equation by adjusting the coefficients of the reactants and products: S + 6HNO3 -> H2SO4 + 6NO2
06

Write the net ionic equation

Break down the ionic compounds and eliminate spectator ions (NO₃⁻): S + 6H⁺ + 6NO₃⁻ -> 2H⁺ + SO₄²⁻ + 6NO₂ The net ionic equation will be: S + 6H⁺ -> SO₄²⁻ + 6NO2 + 4H⁺ Simplifying, we have: S + 2H⁺ -> SO₄²⁻ + 6NO₂ ---------------------------------------------------------------- #c) Concentrated nitric acid oxidizes sulfur dioxide#
07

Write the unbalanced chemical equation

Identify the reactants and products of the reaction: SO2 + HNO3 -> NO + H2SO4
08

Balance the chemical equation

Balance the equation by adjusting the coefficients of the reactants and products: 2SO2 + 4HNO3 -> 4NO + 2H2SO4
09

Write the net ionic equation

Break down the ionic compounds and eliminate the spectator ions (NO₃⁻): 2SO₂ + 4H⁺ + 4NO₃⁻-> 4NO + 4H⁺ + 2SO₄²⁻ The net ionic equation will be: 2SO₂ -> 4NO + 2SO₄²⁻ ---------------------------------------------------------------- #d) Hydrazine is burned in excess fluorine gas#
10

Write the unbalanced chemical equation

Identify the reactants and products of the reaction: N2H4 + F2 -> NF3
11

Balance the chemical equation

Balance the equation by adjusting the coefficients of the reactants and products: N2H4 + 3F2 -> 4NF3
12

Write the net ionic equation

There are no ionic compounds in this reaction, so the net ionic equation is the same as the balanced chemical equation: N2H4 + 3F2 -> 4NF3 ---------------------------------------------------------------- #e) Hydrazine reduces CrO4 2- in base#
13

Write the unbalanced chemical equation

Identify the reactants and products of the reaction: N2H4 + CrO4 2- -> N2 + Cr(OH)4^-
14

Balance the chemical equation

Balance the equation by adjusting the coefficients of the reactants and products (balance the oxygens using water molecules): N2H4 + CrO4 2- + 4H2O -> N2 + Cr(OH)4^-
15

Write the net ionic equation

The net ionic equation will be: N2H4 + CrO₄²⁻ + 4H2O -> N2 + Cr(OH)₄⁻

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Most popular questions from this chapter

(a) Determine the number of calcium ions in the chemical formula of the mineral hardystonite, $\mathrm{Ca}_{x} \mathrm{Zn}\left(\mathrm{Si}_{2} \mathrm{O}_{7}\right)$. (b) Determine the number of hydroxide ions in the chemical formula of the mineral pyrophyllite, $\mathrm{Al}_{2}\left(\mathrm{Si}_{2} \mathrm{O}_{5}\right)_{2}(\mathrm{OH})_{x}$.

(a) The \(\mathrm{P}_{4}, \mathrm{P}_{4} \mathrm{O}_{6}\) and $\mathrm{P}_{4} \mathrm{O}_{10}$ molecules have a common structural feature of four \(\mathrm{P}\) atoms arranged in a tetrahedron (Figures 22.27 and 22.28 ). Does this mean that the bonding between the \(\mathrm{P}\) atoms is the same in all these cases? Explain. (b) Sodium trimetaphosphate $\left(\mathrm{Na}_{3} \mathrm{P}_{3} \mathrm{O}_{9}\right)$ and sodium tetrametaphosphate \(\left(\mathrm{Na}_{4} \mathrm{P}_{4} \mathrm{O}_{12}\right)\) are used as water-softening agents. They contain cyclic $\mathrm{P}_{3} \mathrm{O}_{9}^{3-}\( and \)\mathrm{P}_{4} \mathrm{O}_{12}{ }^{4-}$ ions, respectively. Propose reasonable structures for these ions.

Ultrapure germanium, like silicon, is used in semiconductors. Germanium of "ordinary" purity is prepared by the high-temperature reduction of \(\mathrm{GeO}_{2}\) with carbon. The Ge is converted to \(\mathrm{GeCl}_{4}\) by treatment with \(\mathrm{Cl}_{2}\) and then purified by distillation; \(\mathrm{GeCl}_{4}\) is then hydrolyzed in water to \(\mathrm{GeO}_{2}\) and reduced to the elemental form with \(\mathrm{H}_{2}\). The element is then zone refined. Write a balanced chemical equation for each of the chemical transformations in the course of forming ultrapure Ge from \(\mathrm{GeO}_{2}\).

Write balanced equations for each of the following reactions. (a) When mercury(II) oxide is heated, it decomposes to form \(\mathrm{O}_{2}\) and mercury metal. ( \(\mathbf{b}\) ) When copper(II) nitrate is heated strongly, it decomposes to form copper(II) oxide, nitrogen dioxide, and oxygen. (c) Lead(II) sulfide, \(\mathrm{PbS}(s)\) reacts with ozone to form \(\mathrm{PbSO}_{4}(s)\) and \(\mathrm{O}_{2}(g) .\) (d) When heated in air, \(\mathrm{ZnS}(s)\) is converted to \(\mathrm{ZnO}\). (e) Potassium peroxide reacts with \(\mathrm{CO}_{2}(g)\) to give potassium carbonate and \(\mathrm{O}_{2}\). (f) Oxygen is converted to ozone in the upper atmosphere.

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.
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