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Is it possible for a reaction to be nonspontaneous yet exo-thermic? Explain.
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Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
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McMurry 8th EditionCh.18 - Thermodynamics: Entropy, Free Energy & EquilibriumProblema 124d
McMurry 8th EditionCh.18 - Thermodynamics: Entropy, Free Energy & EquilibriumProblema 124dCapitolo 18, Problema 124d
Consider the Haber synthesis of gaseous NH3 (∆H°f = -46.1 kJ/mol; ∆G°f = -16.5 kJ/mol: (d) What are the equilibrium constants Kp and Kc for the reaction at 350 K? Assume that ∆H° and ∆S° are independent of temperature.
Guida verificata passo dopo passo1
First, write down the balanced chemical equation for the Haber process: N2(g) + 3 H2(g) ⇌ 2 NH3(g).
Use the given standard Gibbs free energy of formation (∆G°f) to calculate the standard Gibbs free energy change for the reaction (∆G°rxn) using the formula: ∆G°rxn = ∑∆G°f(products) - ∑∆G°f(reactants).
Calculate the equilibrium constant K at 350 K using the relationship between Gibbs free energy and the equilibrium constant, K = e(-∆G°rxn / RT), where R is the gas constant (8.314 J/mol·K) and T is the temperature in Kelvin.
To find Kp, use the equation Kp = Kc(RT)Δn, where Δn is the change in moles of gas (moles of gaseous products minus moles of gaseous reactants) for the reaction.
To find Kc, use the relationship Kc = Kp / (RT)Δn. Calculate Kc using the value of Kp obtained in the previous step and the same values for R and T.
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Haber Synthesis
The Haber synthesis is a chemical reaction that combines nitrogen gas (N₂) and hydrogen gas (H₂) to produce ammonia (NH₃). This process is crucial for producing fertilizers and is represented by the equation N₂(g) + 3H₂(g) ⇌ 2NH₃(g). Understanding this reaction involves recognizing its enthalpy change (∆H°) and Gibbs free energy change (∆G°), which indicate the energy dynamics and spontaneity of the reaction.
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Percorso guidato
03:49
Born Haber Cycle
Equilibrium Constants (Kp and Kc)
Equilibrium constants, Kp and Kc, quantify the ratio of products to reactants at equilibrium for a given reaction. Kp is used for gas-phase reactions and is expressed in terms of partial pressures, while Kc is used for reactions in solution and is expressed in terms of molar concentrations. The relationship between Kp and Kc can be derived from the ideal gas law and the reaction's stoichiometry, and they are temperature-dependent.
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02:06Kp vs. Kc Formula
Gibbs Free Energy and Temperature
Gibbs free energy (G) is a thermodynamic potential that helps predict the direction of chemical reactions. The change in Gibbs free energy (∆G) at a given temperature indicates whether a reaction is spontaneous (∆G < 0) or non-spontaneous (∆G > 0). The relationship between Gibbs free energy and equilibrium constants is given by the equation ∆G° = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin, allowing for the calculation of Kp and Kc at specific temperatures.
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00:32Standard Gibbs Free Energy and Temperature
Pratica correlata
Domanda del libro di testo
Trouton's rule says that the ratio of the molar heat of vaporization of a liquid to its normal boiling point (in kelvin) is approximately the same for all liquids: ∆Hvap/Tbp ≈ 88 J/(K*mol) (b) Explain why liquids tend to have the same value of ∆Hvap/Tbp.
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Domanda del libro di testo
Ammonium nitrate is dangerous because it decomposes (sometimes explosively) when heated:
(a) Using the data in Appendix B, show that this reaction is spontaneous at 25 °C.
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Domanda del libro di testo
Use the data in Appendix B to calculate the equilibrium pressure of CO2 in a closed 1 L vessel that contains each of the following samples:
(a) 15 g of MgCO3 and 1.0 g of MgO at 25 °C
(b) 15 g of MgCO3 and 1.0 g of MgO at 280 °C .
Assume that ∆H° and ∆S° are independent of temperature.
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Domanda del libro di testo
Trouton's rule says that the ratio of the molar heat of vaporization of a liquid to its normal boiling point (in kelvin) is approximately the same for all liquids: ∆Hvap/Tbp ≈ 88 J/(K*mol) (a) Check the reliability of Trouton's rule for the liquids listed in the following table.
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