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Ch.4 - Reactions in Aqueous Solution
All textbooksBrown 14th EditionCh.4 - Reactions in Aqueous SolutionProblem 96a
Chapter 4, Problem 96a

The commercial production of nitric acid involves the following chemical reactions:
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
2 NO(g) + O2(g) → 2 NO2(g)
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
(a) Which of these reactions are redox reactions?

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Identify the oxidation states of each element in the reactants and products for each reaction.
For the first reaction: 4 NH_3(g) + 5 O_2(g) → 4 NO(g) + 6 H_2O(g), determine the change in oxidation states for nitrogen and oxygen.
For the second reaction: 2 NO(g) + O_2(g) → 2 NO_2(g), determine the change in oxidation states for nitrogen and oxygen.
For the third reaction: 3 NO_2(g) + H_2O(l) → 2 HNO_3(aq) + NO(g), determine the change in oxidation states for nitrogen.
Identify which reactions involve a change in oxidation states, indicating they are redox reactions.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Redox Reactions

Redox reactions, or reduction-oxidation reactions, involve the transfer of electrons between substances. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Identifying redox reactions requires analyzing changes in oxidation states of the elements involved.
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Oxidation States

Oxidation states (or oxidation numbers) are assigned to atoms in a compound to indicate their degree of oxidation or reduction. The oxidation state helps in determining which atoms are oxidized and which are reduced in a reaction. For example, in the reaction of ammonia with oxygen, nitrogen in NH3 has an oxidation state of -3, which changes to +2 in NO.
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Balancing Chemical Reactions

Balancing chemical reactions is essential to ensure that the number of atoms of each element is conserved throughout the reaction. This involves adjusting coefficients in front of the reactants and products. In redox reactions, balancing also includes ensuring that the total charge is the same on both sides of the equation, which is crucial for identifying the electron transfer.
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Related Practice
Open Question
Suppose you have a solution that might contain any or all of the following cations: Ni2+, Ag+, Sr2+, and Mn2+. Addition of HCl solution causes a precipitate to form. After filtering off the precipitate, H2SO4 solution is added to the resulting solution and another precipitate forms. This is filtered off, and a solution of NaOH is added to the resulting solution. No precipitate is observed. Which of the four ions listed above must be absent from the original solution?
Open Question
You choose to investigate some of the solubility guidelines for two ions not listed in Table 4.1, the chromate ion (CrO₄²⁻) and the oxalate ion (C₂O₄²⁻). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: When these solutions are mixed, the following observations are made:
(a) Write a net ionic equation for the reaction that occurs in the first experiment. (b) Identify the precipitate formed in the first experiment. (c) Write a net ionic equation for the reaction that occurs in the third experiment. (d) Identify the precipitate formed in the third experiment. (e) Write a net ionic equation for the reaction that occurs in the fourth experiment. (f) Identify the precipitate formed in the fourth experiment. (g) Write a net ionic equation for the reaction that occurs in the fifth experiment. (h) Identify the precipitate formed in the fifth experiment. (i) Write a net ionic equation for the reaction that occurs in the sixth experiment. (j) Identify the precipitate formed in the sixth experiment.
Textbook Question

Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the aqueous HCl in the stomach and each of the following substances used in various antacids: (d) NaAl1CO3)1OH221s2

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Textbook Question

The commercial production of nitric acid involves the following chemical reactions:

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

2 NO(g) + O2(g) → 2 NO2(g)

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

(b) Identify the element undergoing oxidation and the element undergoing reduction. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

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Textbook Question

The commercial production of nitric acid involves the following chemical reactions:

4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)

2 NO(g) + O2(g) → 2 NO2(g)

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

(c) How many grams of ammonia must you start with to make 1000.0 L of a 0.150 M aqueous solution of nitric acid? Assume all the reactions give 100% yield.

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Textbook Question

Consider the following reagents: zinc, copper, mercury (density 13.6 g/mL), silver nitrate solution, nitric acid solution. (a) Given a 500-mL Erlenmeyer flask and a balloon, can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon?

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