Domanda del libro di testo
Ethanol (C2H5OH) is blended with gasoline as an automobile fuel. (d) Calculate the mass of CO2 produced per kJ of heat emitted.
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Ch.5 - Thermochemistry
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 5, Problema 81c
Ethanol (C2H5OH) is blended with gasoline as an automobile fuel. (c) Calculate the heat produced per liter of ethanol by combustion of ethanol under constant pressure. Ethanol has a density of 0.789 g/mL.
Guida verificata passo dopo passo1
Identify the chemical reaction for the combustion of ethanol: \[ \text{C}_2\text{H}_5\text{OH} + 3\text{O}_2 \rightarrow 2\text{CO}_2 + 3\text{H}_2\text{O} \].
Determine the molar mass of ethanol (C2H5OH) by adding the atomic masses of its constituent atoms.
Use the density of ethanol (0.789 g/mL) to convert 1 liter of ethanol to grams.
Convert the mass of ethanol obtained in the previous step to moles using the molar mass of ethanol.
Use the standard enthalpy of combustion for ethanol to calculate the heat produced per mole, then multiply by the number of moles to find the heat produced per liter.
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Combustion Reaction
A combustion reaction is a chemical process in which a substance reacts rapidly with oxygen, releasing energy in the form of heat and light. In the case of ethanol, the reaction produces carbon dioxide and water as byproducts. Understanding the stoichiometry of this reaction is essential for calculating the heat produced during combustion.
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Percorso guidato
02:24
Combustion Apparatus
Heat of Combustion
The heat of combustion is the amount of energy released when a substance undergoes complete combustion with oxygen. It is typically expressed in kilojoules per mole (kJ/mol). For ethanol, this value can be found in tables of thermodynamic data and is crucial for determining the total heat produced when a specific volume of ethanol is burned.
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Percorso guidato
02:24Combustion Apparatus
Density and Volume Conversion
Density is defined as mass per unit volume and is crucial for converting between the volume of a liquid and its mass. In this case, the density of ethanol (0.789 g/mL) allows us to calculate the mass of ethanol in a liter, which is necessary for determining the total heat produced during combustion based on the heat of combustion per mole.
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Percorso guidato
05:30Density Conversion Example
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Methanol (CH3OH) is used as a fuel in race cars. (c) Calculate the heat produced by combustion per liter of methanol. Methanol has a density of 0.791 g/mL.
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Domanda del libro di testo
Methanol (CH3OH) is used as a fuel in race cars. (b) Calculate the standard enthalpy change for the reaction, assuming H2O(g) as a product.
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Diethyl ether, C4H10O(l), a flammable compound that was once used as a surgical anesthetic, has the structure The complete combustion of 1 mol of C4H10O(l) to CO2(g) and H2O(l) yields ΔH° = -2723.7 kJ. (a) Write a balanced equation for the combustion of 1 mol of C4H10O(l).
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