Textbook Question
Classify each organic reaction as combustion, alkane substitution, alkene addition or hydrogenation, aromatic substitution, or alcohol substitution, elimination, or oxidation.
d.
Ch.22 - Organic Chemistry
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
Chapter 22, Problem 96
How many kilograms of CO2 does the complete combustion of 3.8 kg of n-octane produce?
Verified step by step guidance1
Step 1: Write down the balanced chemical equation for the combustion of n-octane (C8H18). The combustion reaction of n-octane with oxygen (O2) produces carbon dioxide (CO2) and water (H2O). The balanced equation is: 2C8H18 + 25O2 -> 16CO2 + 18H2O.
Step 2: Calculate the molar mass of n-octane and CO2. The molar mass of n-octane is approximately 114.22 g/mol and the molar mass of CO2 is approximately 44.01 g/mol.
Step 3: Convert the mass of n-octane from kilograms to grams. 1 kg = 1000 g, so multiply the given mass of n-octane by 1000.
Step 4: Use the stoichiometry of the balanced chemical equation to find the moles of CO2 produced from the combustion of n-octane. From the balanced equation, we can see that 2 moles of n-octane produce 16 moles of CO2.
Step 5: Convert the moles of CO2 to mass in kilograms. First, convert the moles of CO2 to grams by multiplying by the molar mass of CO2, then convert the mass from grams to kilograms by dividing by 1000.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Combustion Reaction
A combustion reaction is a chemical process in which a substance reacts rapidly with oxygen, producing heat and light. In the case of hydrocarbons like n-octane, the products are typically carbon dioxide (CO2) and water (H2O). Understanding this reaction is essential for calculating the amount of CO2 produced from a given mass of n-octane.
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Combustion Apparatus
Stoichiometry
Stoichiometry is the area of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. It allows us to use balanced chemical equations to determine how much of each substance is consumed or produced. In this question, stoichiometry will help convert the mass of n-octane into the mass of CO2 generated during combustion.
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Molar Mass
Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles, which is necessary for stoichiometric calculations. For n-octane and CO2, knowing their molar masses will enable accurate calculations of the mass of CO2 produced from the combustion of 3.8 kg of n-octane.
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Related Practice
Textbook Question
Classify each organic reaction as combustion, alkane substitution, alkene addition or hydrogenation, aromatic substitution, or alcohol substitution, elimination, or oxidation.
c.
Textbook Question
Determine whether the two structures are isomers or the same molecule drawn in two different ways. c.
Textbook Question
Determine the products of each reaction. d.
Textbook Question
Determine whether the two structures are isomers or the same molecule drawn in two different ways. b.