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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 (NO鈧冣伝): Zn + 10H鈦� + 6NO鈧冣伝 -> 2Zn虏鈦� + 12NO鈧冣伝 + N鈧侽 + 6H鈧侽 The net ionic equation will be: Zn + 10H鈦� -> 2Zn虏鈦� + N鈧侽 + 6H鈧侽 ---------------------------------------------------------------- #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 (NO鈧冣伝): S + 6H鈦� + 6NO鈧冣伝 -> 2H鈦� + SO鈧劼测伝 + 6NO鈧� The net ionic equation will be: S + 6H鈦� -> SO鈧劼测伝 + 6NO2 + 4H鈦� Simplifying, we have: S + 2H鈦� -> SO鈧劼测伝 + 6NO鈧� ---------------------------------------------------------------- #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 (NO鈧冣伝): 2SO鈧� + 4H鈦� + 4NO鈧冣伝-> 4NO + 4H鈦� + 2SO鈧劼测伝 The net ionic equation will be: 2SO鈧� -> 4NO + 2SO鈧劼测伝 ---------------------------------------------------------------- #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 + CrO鈧劼测伝 + 4H2O -> N2 + Cr(OH)鈧勨伝

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Chemical Reactions
Chemical reactions are processes where reactants transform into one or more new products. These transformations involve breaking bonds in reactants and forming new bonds in products.
The process can be represented by a chemical equation, which not only shows substances involved but also their coefficients.
  • Reactants are on the left side.
  • Products are on the right side.
For example, in the reaction of zinc with nitric acid: Zn + HNO鈧� 鈫� Zn(NO鈧�)鈧� + N鈧侽 + H鈧侽.
Understanding what happens in a reaction helps us predict product formation and understand the reaction mechanism.
Balancing Chemical Equations
Balancing chemical equations is a crucial step in understanding chemical reactions. A balanced equation has equal numbers of each type of atom on both sides. This ensures the law of conservation of mass is followed.
To balance a chemical equation:
  • Write the unbalanced equation.
  • Adjust coefficients to have the same number of each atom on both sides.
For instance, consider the unbalanced equation used earlier: Zn + HNO鈧� 鈫� Zn(NO鈧�)鈧� + N鈧侽 + H鈧侽. We balance each atom, resulting in: 2Zn + 5HNO鈧� 鈫� 2Zn(NO鈧�)鈧� + N鈧侽 + 3H鈧侽.
Balancing equations helps predict the amount of reactants needed or products formed.
Oxidation-Reduction Reactions
Oxidation-reduction reactions, or redox reactions, are processes where electrons are transferred between substances. These reactions consist of two parts: oxidation, where a substance loses electrons, and reduction, where a substance gains electrons.
Consider this in the context of hydrazine reducing chromate ( CrO鈧刕{2-} ). Here, hydrazine ( N_{2}H_{4} ) is oxidized to nitrogen ( N_{2} ), and chromate is reduced to Cr(OH)鈧勨伝.
  • The oxidizing agent is the substance that gets reduced.
  • The reducing agent is the substance that gets oxidized.
Net ionic equations provide a clear picture of redox processes by showing only those entities that participate in the electron transfer.

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Most popular questions from this chapter

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 \(\mathrm{GeO}_{2}\).

Borazine, \((\mathrm{BH})_{3}(\mathrm{NH})_{3},\) is an analog of \(\mathrm{C}_{6} \mathrm{H}_{6},\) benzene. It can be prepared from the reaction of diborane with ammonia, with hydrogen as another product; or from lithium borohydride and ammonium chloride, with lithium chloride and hydrogen as the other products. (a) Write balanced chemical equations for the production of borazine using both synthetic methods. (b) Draw the Lewis dot structure of borazine. (c) How many grams of borazine can be prepared from \(2.00 \mathrm{~L}\) of ammonia at STP, assuming diborane is in excess?

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 \(\mathrm{SO}_{2}\), (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 \(2000 \mathrm{~kg}\) of \(\mathrm{H}_{2} \mathrm{SO}_{4} ?\)

Write a balanced equation for each of the following reactions: (a) hydrolysis of \(\mathrm{PCl}_{5},(\mathbf{b})\) dehydration of phosphoric acid (also called orthophosphoric acid) to form pyrophosphoric acid, \((\mathbf{c})\) reaction of \(\mathrm{P}_{4} \mathrm{O}_{10}\) with water.

Write a balanced equation for each of the following reactions: (a) Hydrogen cyanide is formed commercially by passing a mixture of methane, ammonia, and air over a catalyst at \(800^{\circ} \mathrm{C}\). Water is a by-product of the reaction. (b) Baking soda reacts with acids to produce carbon dioxide gas. (c) When barium carbonate reacts in air with sulfur dioxide, barium sulfate and carbon dioxide form.
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