Domanda del libro di testo
Sulfur dioxide reacts with strontium oxide as follows: SO2(g) + SrO(g) → SrSO3(s) (a) Without using thermochemical data, predict whether ΔG° for this reaction is more negative or less negative than ΔH°.
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Ch.19 - Chemical Thermodynamics
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 19, Problema 63a,b
Classify each of the following reactions as one of the four possible types summarized in Table 19.3: (i) spontanous at all temperatures; (ii) not spontaneous at any temperature; (iii) spontaneous at low T but not spontaneous at high T; (iv) spontaneous at high T but not spontaneous at low T.
(a) N2(g) + 3 F2(g) → 2 NF3(g) ΔH° = -249 kJ; ΔS° = -278 J/K
(b) N2(g) + 3 Cl2(g) → 2 NCl3(g) ΔH° = 460 kJ; ΔS° = -275 J/K
Guida verificata passo dopo passo1
Identify the Gibbs free energy equation: ΔG° = ΔH° - TΔS°. This equation helps determine the spontaneity of a reaction.
For reaction (a), N2(g) + 3 F2(g) → 2 NF3(g), note that ΔH° = -249 kJ and ΔS° = -278 J/K. Convert ΔS° to kJ by dividing by 1000, resulting in ΔS° = -0.278 kJ/K.
Substitute the values into the Gibbs free energy equation for reaction (a): ΔG° = -249 kJ - T(-0.278 kJ/K). Analyze the sign of ΔG° at different temperatures to determine spontaneity.
For reaction (b), N2(g) + 3 Cl2(g) → 2 NCl3(g), note that ΔH° = 460 kJ and ΔS° = -275 J/K. Convert ΔS° to kJ by dividing by 1000, resulting in ΔS° = -0.275 kJ/K.
Substitute the values into the Gibbs free energy equation for reaction (b): ΔG° = 460 kJ - T(-0.275 kJ/K). Analyze the sign of ΔG° at different temperatures to determine spontaneity.
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Gibbs Free Energy
Gibbs Free Energy (G) is a thermodynamic potential that helps predict the spontaneity of a reaction at constant temperature and pressure. The change in Gibbs Free Energy (ΔG) is calculated using the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. A negative ΔG indicates a spontaneous reaction, while a positive ΔG suggests non-spontaneity.
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01:51
Gibbs Free Energy of Reactions
Enthalpy and Entropy
Enthalpy (ΔH) is a measure of the total heat content of a system, while entropy (ΔS) quantifies the degree of disorder or randomness in a system. In chemical reactions, ΔH can be either positive (endothermic) or negative (exothermic), and ΔS can also be positive or negative depending on the change in disorder. The interplay between these two factors determines the spontaneity of a reaction across different temperature ranges.
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02:46Entropy in Thermodynamics
Temperature Dependence of Spontaneity
The spontaneity of a reaction can depend on temperature due to the relationship between enthalpy and entropy. Reactions that are exothermic (negative ΔH) and have positive entropy (positive ΔS) are spontaneous at all temperatures. Conversely, reactions that are endothermic with negative entropy are non-spontaneous at all temperatures. The temperature can shift the balance for reactions that are spontaneous at low or high temperatures, depending on the signs of ΔH and ΔS.
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01:24Kw Temperature Dependence
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Domanda del libro di testo
Classify each of the following reactions as one of the four possible types summarized in Table 19.3: (i) spontaneous at all temperatures; (ii) not spontaneous at any temperature; (iii) spontaneous at low T but not spontaneous at high T; (iv) spontaneous at high T but not spontaneous at low T.
(c) N2F4(g) ⟶ 2 NF2(g) ΔH° = 85 kJ; ΔS° = 198 J/K
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Domanda del libro di testo
From the values given for ΔH° and ΔS°, calculate ΔG° for each of the following reactions at 298 K. If the reaction is not spontaneous under standard conditions at 298 K, at what temperature (if any) would the reaction become spontaneous?
a. 2 PbS(s) + 3 O2(g) → 2 PbO(s) + 2 SO2(g) ΔH° = −844 kJ; ΔS° = −165 J/K
b. 2 POCl3(g) → 2 PCl3(g) + O2(g) ΔH° = 572 kJ; ΔS° = 179 J/K
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