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Chapter 8: Problem 16

What are some of the characteristics of each of these five common chemical reactions? $$ \begin{array}{l}{\text { a. combustion }} \\ {\text { b. synthesis }} \\\ {\text { c. decomposition }} \\ {\text { d. displacement }} \\ {\text { e. double-displacement }}\end{array} $$

Short Answer

Expert verified
Combustion reactions involve reacting a substance with oxygen. Synthesis reactions combine different compounds to form a new compound. Decomposition reactions break down a compound into simpler substances. Displacement reactions involve a more reactive element replacing a less reactive element in a compound. Double-Displacement reactions involve the positive ions of two different compounds exchange places to form two new compounds.

Step by step solution

01

Define Combustion

Combustion is a chemical reaction that involves the reaction of a substance with an oxidizing element, usually oxygen, to release energy. It's a kind of reaction where the substance burns in oxygen to release energy. Thus, the generic representation would be: \( X + O_2 \to Y \), where \(X\) is the substance and \(Y\) is the new compound formed.
02

Define Synthesis

A synthesis reaction or direct combination reaction, is one of the most straightforward types of chemical reactions. It is a reaction in which two or more chemical compounds combine to form a more complex compound. Thus, its general representation can be: \( A + B \to Z \), where \(A\) and \(B\) are different reactants joining together to create a new compound \(Z\).
03

Define Decomposition

Decomposition is a type of chemical reaction wherein one compound breaks down into two or more simpler substances. Its general form would look like: \( X \to A + B \), where \(X\) is the complex compound and \( A \) and \( B \) are simpler products.
04

Define Displacement

In a displacement reaction, a more reactive element displaces a less reactive element from its compound. Its generic representation is: \( A + BX \to AX + B \), where \(A\) is the more reactive element that replaces \( B \) in \(BX\) to yield \(AX\) and release \(B\).
05

Define Double-Displacement

Double displacement reactions, also known as exchange reactions, are reactions in which the positive ions of two different compounds exchange places to form two new compounds. Here's its generic form: \( AX + BY \to AY + BX \), where elements \(A\) and \( B \) exchange partners.

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Key Concepts

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

Combustion Reaction
In a combustion reaction, a substance combines with an oxidizing element, such as oxygen, and releases energy, often in the form of heat and light. This is why burning wood in a fireplace or gasoline in an engine produces flames and heat. The general equation for a combustion reaction is:

\( X + O_2 \rightarrow Y + \text{energy} \), where \(X\) is the substance being burned and \(Y\) is the product, usually including carbon dioxide (\(CO_2\)) and water (\(H_2O\)) if the fuel is a hydrocarbon. It's crucial that there is enough oxygen because insufficient oxygen can lead to incomplete combustion, resulting in carbon monoxide (\(CO\)) and even soot.
Synthesis Reaction
A synthesis reaction, also known as a direct combination reaction, occurs when two or more reactants combine to form a single product. An everyday example of this type of reaction is the formation of water from hydrogen and oxygen gases.

The synthesis reaction is represented by: \( A + B \rightarrow Z \), where \(A\) and \(B\) are the reactants that come together to form the new compound \(Z\). It’s a process akin to creating a building from bricks; the reactants are the bricks which when combined, result in a new, larger structure. This type of reaction is fundamental in the formation of many compounds in chemistry.
Decomposition Reaction
Decomposition reactions involve a single compound breaking apart into two or more simpler substances. This reaction can be caused by heating, light, or electricity. For instance, when an electric current is passed through water, it decomposes into hydrogen and oxygen gases.

The general form for a decomposition reaction is: \( X \rightarrow A + B \), where \(X\) is the compound that decomposes into simpler products \(A\) and \(B\). One classic demonstration of a decomposition reaction is the breakdown of potassium chlorate into potassium chloride and oxygen gas when heated.
Displacement Reaction
In a displacement reaction, a more reactive element swaps places with a less reactive element in a compound. The reactivity series of metals can predict whether a displacement reaction will occur, as a more reactive metal will displace a less reactive metal from a solution of its salt.

The representation is: \( A + BX \rightarrow AX + B \), where \(A\) is the more reactive element that replaces \(B\) in compound \(BX\) to form a new compound \(AX\) and release \(B\) as a separate element. This kind of reaction is significant in many industrial processes, such as the extraction of metals from their ores.
Double-Displacement Reaction
Double-displacement reactions, also known as exchange reactions, involve the exchange of ions between two compounds to form two new products. This kind of reaction is common in solutions where ions can move freely to new combinations.

The general equation is: \( AX + BY \rightarrow AY + BX \), where elements \(A\) and \(B\) exchange partners. These reactions often result in the formation of a precipitate, a gas or a molecular compound like water, marking the completion of the reaction. An example is the neutralization of an acid with a base to form a salt and water.

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Most popular questions from this chapter

Write a balanced equation for each of the following: $$\begin{array}{c}{\text { a. copper(II) sulfate }+\text { ammonium sulfide } \rightarrow} \\ {\text { copper(II) sulfide + ammonium sulfate }} \\ {\text { b. nitric acid + barium hydroxide } \rightarrow} \\ {\text { water + barium nitrate }}\end{array}$$ $$ \begin{array}{c}{\text { c. barium chloride + phosphoric acid } \rightarrow} \\\ {\text { barium phosphate + hydrochloric acid }}\end{array} $$

Predict the products for each of the following reactions. Write a total ionic equation and a net ionic equation for each reaction. If no reaction occurs, write "no reaction." $$\begin{array}{l}{\text { a. } \mathrm{Li}_{2} \mathrm{CO}_{3}(a q)+\mathrm{BaBr}_{2}(a q) \longrightarrow} \\ {\text { b. } \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q) \rightarrow} \\ {\text { c. } \mathrm{Al}(s)+\mathrm{NiCl}_{2}(a q) \rightarrow} \\ {\text { d. } \mathrm{K}_{2} \mathrm{CO}_{3}(a q)+\mathrm{FeCl}_{3}(a q) \rightarrow}\end{array}$$

Define each of the following terms: $$\begin{array}{l}{\text { a. decomposition reaction }} \\ {\text { b. double-displacement reaction }} \\ {\text { c. spectator ions }} \\ {\text { d. activity series }}\end{array}$$

A student writes the following statement in a lab report: "During the reaction, the particles of the reactants are lost. The reaction creates energy and particles of the products" $$\begin{array}{l}{\text { a. Explain the scientific inaccuracies in the }} \\\ {\text { student's statement. }} \\ {\text { b. How could the student correct the }} \\ {\text { inaccurate statement? }}\end{array}$$

Complete and balance the equation for the complete combustion of each of the following. $$ \begin{array}{ll}{\text { a. } C_{3} \mathrm{H}_{6}} & {\text { c. } C \mathrm{H}_{3} \mathrm{OH}} \\ {\text { b. } C_{5} \mathrm{H}_{12}} & {\text { d. } C_{12} \mathrm{H}_{22} \mathrm{O}_{11}}\end{array} $$
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