Domanda del libro di testo
Consider this reaction occurring at 298 K: N2O(g) + NO2(g) ⇌ 3 NO(g) a. Show that the reaction is not spontaneous under standard conditions by calculating ΔG°rxn.
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Ch.19 - Free Energy & Thermodynamics
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 19, Problema 94a
Consider this reaction occurring at 298 K: BaCO3(s) ⇌ BaO(s) + CO2(g) a. Show that the reaction is not spontaneous under standard conditions by calculating ΔG°rxn.
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insert step 1> Calculate the standard Gibbs free energy of formation (\( \Delta G_f^\circ \)) for each substance involved in the reaction: BaCO3(s), BaO(s), and CO2(g). These values can be found in a standard thermodynamic table.
insert step 2> Use the formula for the standard Gibbs free energy change of the reaction: \( \Delta G_{rxn}^\circ = \sum \Delta G_f^\circ (\text{products}) - \sum \Delta G_f^\circ (\text{reactants}) \).
insert step 3> Substitute the \( \Delta G_f^\circ \) values for BaO(s) and CO2(g) as products and BaCO3(s) as the reactant into the equation from Step 2.
insert step 4> Perform the arithmetic to find \( \Delta G_{rxn}^\circ \).
insert step 5> Interpret the result: If \( \Delta G_{rxn}^\circ > 0 \), the reaction is non-spontaneous under standard conditions.
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Gibbs Free Energy (ΔG)
Gibbs Free Energy is a thermodynamic potential that helps predict the spontaneity of a reaction. A negative ΔG indicates that a reaction can occur spontaneously, while a positive ΔG suggests non-spontaneity. The standard Gibbs free energy change (ΔGrxn °) is calculated under standard conditions (1 atm, 298 K) and is essential for determining the favorability of the reaction.
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01:51
Gibbs Free Energy of Reactions
Standard State Conditions
Standard state conditions refer to a set of specific conditions used to measure the properties of substances, typically at 1 bar (or 1 atm) pressure and a specified temperature, usually 298 K. These conditions provide a consistent basis for comparing thermodynamic data, such as enthalpy, entropy, and Gibbs free energy, which are crucial for calculating ΔGrxn °.
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01:10Standard Reduction Potentials
Equilibrium Constant (K)
The equilibrium constant (K) is a dimensionless value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction. It is related to the standard Gibbs free energy change by the equation ΔGrxn ° = -RT ln(K). Understanding K helps in assessing the position of equilibrium and the spontaneity of the reaction under standard conditions.
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Percorso guidato
01:14Equilibrium Constant K
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Living organisms use energy from the metabolism of food to create an energy-rich molecule called adenosine triphosphate (ATP). The ATP acts as an energy source for a variety of reactions that the living organism must carry out to survive. ATP provides energy through its hydrolysis, which can be symbolized as follows: ATP(aq) + H2O(l) → ADP(aq) + Pi(aq) ΔGrxn ° = -30.5 kJ where ADP represents adenosine diphosphate and Pi represents an inorganic phosphate group (such as HPO42-). a. Calculate the equilibrium constant, K, for the given reaction at 298 K.
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Domanda del libro di testo
Consider this reaction occurring at 298 K: N2O(g) + NO2(g) ⇌ 3 NO(g) c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, what temperature is required to make the reaction spontaneous under standard conditions?
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Domanda del libro di testo
Consider this reaction occurring at 298 K: N2O(g) + NO2(g) ⇌ 3 NO(g) b. If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous?
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Domanda del libro di testo
Consider this reaction occurring at 298 K: BaCO3(s) ⇌ BaO(s) + CO2( g) b. If BaCO3 is placed in an evacuated flask, what is the partial pressure of CO2 when the reaction reaches equilibrium?
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Domanda del libro di testo
Consider this reaction occurring at 298 K: BaCO3(s) ⇌ BaO(s) + CO2(g) c. Can the reaction be made more spontaneous by an increase or decrease in temperature? If so, at what temperature is the partial pressure of carbon dioxide 1.0 atm?
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