Domanda del libro di testo
Consider the reaction 2 NO2(g) → N2O4(g). (a) Using data from Appendix C, calculate ΔG° at 298 K. (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.40 atm and 1.60 atm, respectively.
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Ch.19 - Chemical Thermodynamics
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 19, Problema 78a
Consider the reaction 3 CH4(g) → C3H8(g) + 2 H2(g). (a) Using data from Appendix C, calculate ΔG° at 298 K.
Guida verificata passo dopo passo1
Identify the standard Gibbs free energy of formation (ΔG°f) for each compound involved in the reaction from Appendix C.
Write the balanced chemical equation: 3 CH_4(g) → C_3H_8(g) + 2 H_2(g).
Apply the formula for the standard Gibbs free energy change of the reaction: ΔG° = Σ(ΔG°f products) - Σ(ΔG°f reactants).
Calculate the ΔG° for the products: ΔG°(C_3H_8) + 2 * ΔG°(H_2).
Calculate the ΔG° for the reactants: 3 * ΔG°(CH_4) and subtract from the products' ΔG° to find the overall ΔG° for the reaction.
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Gibbs Free Energy (ΔG)
Gibbs Free Energy (ΔG) is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. It is a crucial concept in predicting the spontaneity of a reaction; a negative ΔG indicates that a reaction can occur spontaneously, while a positive ΔG suggests non-spontaneity.
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Percorso guidato
01:51
Gibbs Free Energy of Reactions
Standard Gibbs Free Energy Change (ΔG°)
The standard Gibbs Free Energy change (ΔG°) refers to the change in Gibbs Free Energy for a reaction under standard conditions, typically defined as 1 bar of pressure and a specified temperature, usually 298 K. It allows for the comparison of the thermodynamic favorability of different reactions under uniform conditions.
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00:32Standard Gibbs Free Energy and Temperature
Thermodynamic Data Tables
Thermodynamic data tables, such as those found in Appendix C, provide standard enthalpy (ΔH°) and standard entropy (S°) values for various substances. These values are essential for calculating ΔG° using the equation ΔG° = ΔH° - TΔS°, where T is the temperature in Kelvin, allowing for the determination of the spontaneity of the reaction.
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Percorso guidato
01:18First Law of Thermodynamics
Pratica correlata
Domanda del libro di testo
Consider the reaction 3 CH4(g) → C3H8(g) + 2 H2(g). (b) Calculate ΔG at 298 K if the reaction mixture consists of 40.0 atm of CH4, 0.0100 atm of C3H8(g), and 0.0180 atm of H2.
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Domanda del libro di testo
Using data from Appendix C, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K: (a) NaHCO3(s) ⇌ NaOH(s) + CO2(g)
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