Indicate what type, or types, of reaction each of the following represents: (a) \(\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{C}(s) \longrightarrow \mathrm{CO}(g)+\mathrm{H}_{2}(g)\) (b) \(2 \mathrm{KClO}_{3}(s) \longrightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}(a q)+3 \mathrm{HCl}(a q) \longrightarrow \mathrm{AlCl}_{3}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l)\) (d) \(\operatorname{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+2 \mathrm{HNO}_{3}(a q)\)

Short Answer

Expert verified
(a) Redox reaction, (b) Decomposition reaction, (c) Acid-base neutralization, (d) Precipitation reaction (double displacement).

Step by step solution

01

Identify Reaction Type for (a)

Inspect the reactants and products in (a) to determine the reaction type. Here, a compound and an element react to form two new compounds, which characterizes a redox reaction. The carbon is being oxidized, and the water is being reduced.
02

Identify Reaction Type for (b)

Examine the reactants and products in (b) to classify the reaction. This reaction involves the decomposition of potassium chlorate (KClO3) into potassium chloride (KCl) and oxygen gas (O2). Decomposition reactions involve a single compound breaking down into two or more simpler substances.
03

Identify Reaction Type for (c)

Evaluate the reactants and products in (c) to ascertain the reaction type. Since an acid (HCl) reacts with a base (Al(OH)3) to produce a salt (AlCl3) and water (H2O), this reaction is an acid-base neutralization.
04

Identify Reaction Type for (d)

Look at the reactants and products in (d) for reaction classification. Two aqueous compounds are reacting to form one solid product (PbSO4) in a double displacement reaction, also known as a precipitation reaction, since a precipitate is formed.

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Key Concepts

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

Redox Reaction
Redox reactions, or oxidation-reduction reactions, are a fundamental type of chemical reaction where the oxidation state of atoms changes. Oxidation is the process of losing electrons, and reduction is the gain of electrons. In a redox reaction, one substance is oxidized while another is reduced.

To get a clearer picture, let's consider the given example (a) \(\mathrm{H}_{2} \mathrm{O}(g) + \mathrm{C}(s) \longrightarrow \mathrm{CO}(g) + \mathrm{H}_{2}(g)\). This reaction involves the transfer of electrons between chemical species. The carbon \(C\) is oxidized as it gains oxygen to form carbon monoxide \(CO\), while water \(H_2O\) is reduced to hydrogen gas \(H_2\).

Recognizing redox reactions is critical for students because these reactions are prevalent in both laboratory chemistry and in everyday processes such as combustion, respiration, and corrosion.
Decomposition Reaction
Decomposition reactions entail a single compound breaking apart into two or more simpler substances. These reactions often require an input of energy in the form of heat, light, or electricity.

The example (b) \(2 \mathrm{KClO}_{3}(s) \longrightarrow 2 \mathrm{KCl}(s) + 3 \mathrm{O}_{2}(g)\) illustrates a classical decomposition reaction. Here, potassium chlorate \(KClO_3\) decomposes into potassium chloride \(KCl\) and oxygen gas \(O_2\) when heated.

Decomposition reactions are important to understand for processes like the breakdown of organic matter, the digestion of food, and the production of metals from ores.
Acid-Base Neutralization
An acid-base neutralization is a type of chemical reaction where an acid and a base react to form water and a salt. This process is driven by the combination of H+ ions from the acid and OH- ions from the base to produce water.

The reaction shown in (c) \(\mathrm{Al}(\mathrm{OH})_{3}(aq) + 3 \mathrm{HCl}(aq) \longrightarrow \mathrm{AlCl}_{3}(aq) + 3 \mathrm{H}_{2} \mathrm{O}(l)\) is a perfect example. The hydrochloric acid \(HCl\) and aluminum hydroxide \(Al(OH)_3\) react to form aluminum chloride \(AlCl_3\), which is the salt, and water \(H_2O\).

Understanding neutralization is essential because it's widely used in various applications, including the treatment of acid reflux, the neutralization of soil acidity in agriculture, and in wastewater treatment.
Precipitation Reaction
Precipitation reactions occur when two aqueous solutions react to form an insoluble solid, known as a precipitate. These reactions are a subset of double displacement reactions and are important for identifying the presence of certain ions in a solution.

In the provided example (d) \(\operatorname{Pb}(\mathrm{NO}_{3})_{2}(aq) + \mathrm{H}_{2} \mathrm{SO}_{4}(aq) \longrightarrow \mathrm{PbSO}_{4}(s) + 2 \mathrm{HNO}_{3}(aq)\), lead nitrate and sulfuric acid react to form lead sulfate, which precipitates from the solution, and nitric acid.

Recognizing precipitation reactions helps in understanding processes like the purification of water, the formation of geological formations such as stalactites and stalagmites, and in medical diagnostics for the detection of certain ions in bodily fluids.

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Most popular questions from this chapter

50\. What mass of silver oxide, \(\mathrm{Ag}_{2} \mathrm{O}\), is required to produce \(25.0 \mathrm{g}\) of silver sulfadiazine, \(\mathrm{AgC}_{10} \mathrm{H}_{9} \mathrm{N}_{4} \mathrm{SO}_{2}\), from the reaction of silver oxide and sulfadiazine? \(2 \mathrm{C}_{10} \mathrm{H}_{10 \mathrm{N}_{4}} \mathrm{SO}_{2}+\mathrm{Ag}_{2} \mathrm{O} \longrightarrow 2 \mathrm{AgC}_{10} \mathrm{H}_{9} \mathrm{N}_{4} \mathrm{SO}_{2}+\mathrm{H}_{2} \mathrm{O}\)

Identify the atoms that are oxidized and reduced, the change in oxidation state for each, and the oxidizing and reducing agents in each of the following equations: (a) \(\mathrm{Mg}(s)+\mathrm{NiCl}_{2}(a q) \rightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{Ni}(s)\) (b) \(\mathrm{PCl}_{3}(l)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{PCl}_{5}(s)\) (c) \(\mathrm{C}_{2} \mathrm{H}_{4}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\) (d) \(\mathrm{Zn}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{ZnSO}_{4}(a q)+\mathrm{H}_{2}(g)\) (e) \(2 \mathrm{K}_{2} \mathrm{S}_{2} \mathrm{O}_{3}(s)+\mathrm{I}_{2}(s) \longrightarrow \mathrm{K}_{2} \mathrm{S}_{4} \mathrm{O}_{6}(s)+2 \mathrm{KI}(s)\) (f) \(3 \mathrm{Cu}(s)+8 \mathrm{HNO}_{3}(a q) \rightarrow 3 \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{NO}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)\) 21\. Complete and balance the following acid-base equations: (a) HCl gas reacts with solid Ca(OH) \(_{2}(s)\). (b) A solution of \(\operatorname{Sr}(\mathrm{OH})_{2}\) is added to a solution of \(\mathrm{HNO}_{3}\).

Lithium hydroxide may be used to absorb carbon dioxide in enclosed environments, such as manned spacecraft and submarines. Write an equation for the reaction that involves 2 mol of LiOH per 1 mol of \(\mathrm{CO}_{2}\). (Hint: Water is one of the products.)

I_ \(_{2}\) is produced by the reaction of 0.4235 mol of \(\mathrm{CuCl}_{2}\) according to the following equation: \(2 \mathrm{CuCl}_{2}+4 \mathrm{KI} \longrightarrow 2 \mathrm{CuI}+4 \mathrm{KCl}+\mathrm{I}_{2}\) (a) How many molecules of I \(_{2}\) are produced? (b) What mass of I \(_{2}\) is produced?

Outline the steps needed to determine the limiting reactant when 0.50 mol of \(\mathrm{Cr}\) and \(0.75 \mathrm{mol}\) of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) react according to the following chemical equation. \(2 \mathrm{Cr}+2 \mathrm{H}_{3} \mathrm{PO}_{4} \longrightarrow 2 \mathrm{CrPO}_{4}+3 \mathrm{H}_{2}\) Determine the limiting reactant.

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