Domanda del libro di testo
The change in internal energy for the combustion of 1.0 mol of octane at a pressure of 1.0 atm is 5084.3 kJ. If the change in enthalpy is 5074.1 kJ, how much work is done during the combustion?
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Ch.6 - Thermochemistry
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
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Capitolo 6, Problema 55
When 1 mol of a fuel burns at constant pressure, it produces 3452 kJ of heat and does 11 kJ of work. What are ΔE and ΔH for the combustion of the fuel?
Guida verificata passo dopo passo1
Identify the given values: heat produced (q) = -3452 kJ and work done (w) = -11 kJ. Note that both values are negative because the system is losing energy.
Recall the first law of thermodynamics, which states that the change in internal energy (ΔE) is given by ΔE = q + w.
Substitute the given values into the equation: ΔE = (-3452 kJ) + (-11 kJ).
Recognize that at constant pressure, the change in enthalpy (ΔH) is equal to the heat exchanged, so ΔH = q.
Substitute the given value for heat into the equation for ΔH: ΔH = -3452 kJ.
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Concetti chiave
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First Law of Thermodynamics
The First Law of Thermodynamics states that energy cannot be created or destroyed, only transformed from one form to another. In the context of chemical reactions, this principle implies that the change in internal energy (ΔE) of a system is equal to the heat added to the system minus the work done by the system on its surroundings.
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01:18
First Law of Thermodynamics
Enthalpy (ΔH)
Enthalpy (ΔH) is a thermodynamic quantity that represents the total heat content of a system at constant pressure. It accounts for the internal energy of the system plus the product of its pressure and volume. For reactions occurring at constant pressure, the change in enthalpy is equal to the heat absorbed or released during the reaction.
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02:34Enthalpy of Formation
Work in Thermodynamics
In thermodynamics, work refers to the energy transferred when a force is applied over a distance. For chemical reactions, work can be done by the system on the surroundings, such as when gases expand against external pressure. The work done affects the internal energy change and must be considered when calculating the overall energy changes in a reaction.
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01:18First Law of Thermodynamics
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Determine whether each process is exothermic or endothermic and indicate the sign of ΔH. a. natural gas burning on a stove b. isopropyl alcohol evaporating from skin c. water condensing from steam Indicate the sign of ΔH for the following processes.
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Determine whether each process is exothermic or endothermic and indicate the sign of ΔH. a. natural gas burning on a stove b. isopropyl alcohol evaporating from skin c. water condensing from steam Determine whether each of the following is exothermic or endothermic.
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Domanda del libro di testo
A gas is compressed from an initial volume of 5.55 L to a final volume of 1.22 L by an external pressure of 1.00 atm. During the compression the gas releases 124 J of heat. What is the change in internal energy of the gas?
2904
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