Domanda del libro di testo
Using values from Appendix C, calculate the value of H for each of the following reactions: (a) NiO(s) + 2 HCl(g) → NiCl2(s) + H2O(g)
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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 77
Complete combustion of 1 mol of acetone (C3H6O) liberates 1790 kJ: C3H6O(l) + 4 O2(g) → 3 CO2(g) + 3 H2O(l) ΔH° = -1790 kJ Using this information together with the standard enthalpies of formation of O2(g), CO2(g), and H2O(l) from Appendix C, calculate the standard enthalpy of formation of acetone.
Guida verificata passo dopo passo1
Identify the given reaction and the enthalpy change: C_3H_6O(l) + 4 O_2(g) → 3 CO_2(g) + 3 H_2O(l) with ΔH° = -1790 kJ.
Recall that the standard enthalpy change of a reaction (ΔH°_rxn) is calculated using the formula: ΔH°_rxn = ΣΔH°_f(products) - ΣΔH°_f(reactants).
List the standard enthalpies of formation (ΔH°_f) for the products and reactants: ΔH°_f[CO_2(g)] = -393.5 kJ/mol, ΔH°_f[H_2O(l)] = -285.8 kJ/mol, and ΔH°_f[O_2(g)] = 0 kJ/mol (since O_2 is in its standard state).
Set up the equation using the enthalpy of formation values: -1790 kJ = [3(-393.5) + 3(-285.8)] - [ΔH°_f[C_3H_6O(l)] + 4(0)].
Solve for the standard enthalpy of formation of acetone (ΔH°_f[C_3H_6O(l)]) by rearranging the equation and performing the necessary arithmetic operations.
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Standard Enthalpy of Formation
The standard enthalpy of formation (ΔH°f) is the change in enthalpy when one mole of a compound is formed from its elements in their standard states. It is a crucial concept in thermodynamics, as it allows for the calculation of the energy changes associated with chemical reactions. The values are typically tabulated and can be used to determine the enthalpy changes for reactions using Hess's law.
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02:34
Enthalpy of Formation
Hess's Law
Hess's Law states that the total enthalpy change for a chemical reaction is the same, regardless of the number of steps taken to achieve the reaction. This principle allows chemists to calculate the enthalpy change of a reaction by using known enthalpy changes of other reactions. In the context of the question, it enables the calculation of the standard enthalpy of formation of acetone by using the enthalpy of combustion and the enthalpies of formation of the products.
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02:03Hess's Law
Combustion Reaction
A combustion reaction is a chemical reaction that typically involves a hydrocarbon reacting with oxygen to produce carbon dioxide and water, releasing energy in the form of heat. In this case, the complete combustion of acetone is represented by the given reaction, which provides the enthalpy change associated with the process. Understanding the stoichiometry of combustion reactions is essential for calculating energy changes and determining the enthalpy of formation of reactants.
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02:24Combustion Apparatus
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