Domanda del libro di testo
If 2.0 mol CH3CH2CH2COOH, 2.0 mol C4H10, and 2.0 mol C6H6 are completely combusted in oxygen, which one produces the largest number of moles of H2O?
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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
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Brown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 88b
Brown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblema 88bCapitolo 3, Problema 88b
If 2.0 mol CH3CH2CH2COOH, 2.0 mol C4H10, and 2.0 mol C6H6 are completely combusted in oxygen, which one produces the least? Explain.
Guida verificata passo dopo passo1
Identify the chemical formulas for each compound: CH3CH2CH2COOH (butanoic acid), C4H10 (butane), and C6H6 (benzene).
Write the balanced chemical equations for the complete combustion of each compound: \( \text{CH}_3\text{CH}_2\text{CH}_2\text{COOH} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \), \( \text{C}_4\text{H}_{10} + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \), \( \text{C}_6\text{H}_6 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \).
Determine the number of moles of \( \text{CO}_2 \) produced per mole of each compound by using the stoichiometry from the balanced equations.
Calculate the total moles of \( \text{CO}_2 \) produced for 2.0 moles of each compound by multiplying the moles of \( \text{CO}_2 \) per mole of compound by 2.0.
Compare the total moles of \( \text{CO}_2 \) produced by each compound to determine which one produces the least amount of \( \text{CO}_2 \).
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Combustion Reaction
A combustion reaction is a chemical process in which a substance reacts with oxygen to produce heat and light. Typically, hydrocarbons combust to form carbon dioxide and water. The amount of energy released during combustion depends on the structure of the hydrocarbon and the number of carbon and hydrogen atoms present.
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02:24
Combustion Apparatus
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the moles of products formed from a given amount of reactants. In this case, knowing the stoichiometric coefficients for the combustion of each hydrocarbon will help us compare the total moles of carbon dioxide produced.
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01:16Stoichiometry Concept
Energy Content of Fuels
The energy content of fuels, often measured in kilojoules per mole, indicates how much energy is released during combustion. Different hydrocarbons have varying energy contents based on their molecular structure. By comparing the energy released per mole of each compound during combustion, we can determine which fuel produces the least energy and, consequently, the least amount of products.
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01:26Nature of Energy
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