Domanda del libro di testo
(c) In each case, indicate whether K should increase or decrease with increasing temperature. (i) 2 Mg(s) + O2 (g) ⇌ 2 MgO(s) (ii) 2 KI(s) ⇌ 2 K(g) + I2(g) (iii) Na2(g) ⇌ 2 Na(g) (iv) 2 V2O5(s) ⇌ 4 V(s) + 5 O2(g)
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 97b
(b) Based on your general chemical knowledge, predict which of these reactions will have K>1. (i) 2 Mg(s) + O2 (g) ⇌ 2 MgO(s) (ii) 2 KI(s) ⇌ 2 K(g) + I2(g) (iii) Na2(g) ⇌ 2 Na(g) (iv) 2 V2O5(s) ⇌ 4 V(s) + 5 O2(g)
Guida verificata passo dopo passo1
Understand the concept of equilibrium constant (K): The equilibrium constant, K, indicates the extent to which a reaction proceeds to form products. If K > 1, the reaction favors the formation of products at equilibrium.
Analyze reaction (i): 2 Mg(s) + O_2(g) ⇌ 2 MgO(s). This is a combustion reaction where magnesium reacts with oxygen to form magnesium oxide, a stable compound. Such reactions typically have K > 1 as they favor product formation.
Analyze reaction (ii): 2 KI(s) ⇌ 2 K(g) + I_2(g). This reaction involves the decomposition of a solid into gaseous elements. Decomposition reactions of stable ionic solids like KI generally have K < 1, as they do not favor the formation of gaseous products.
Analyze reaction (iii): Na_2(g) ⇌ 2 Na(g). This reaction involves the dissociation of a diatomic molecule into atoms. The stability of Na_2 compared to individual Na atoms will determine K. Typically, such dissociation reactions have K < 1.
Analyze reaction (iv): 2 V_2O_5(s) ⇌ 4 V(s) + 5 O_2(g). This is a decomposition reaction of a stable oxide into its elements. Such reactions usually have K < 1, as they do not favor the formation of gaseous products from stable solids.
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Equilibrium Constant (K)
The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. A K value greater than 1 indicates that products are favored at equilibrium, while a K value less than 1 suggests that reactants are favored. Understanding K helps predict the direction of a reaction and its extent.
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Equilibrium Constant K
Gibbs Free Energy (ΔG)
Gibbs free energy (ΔG) is a thermodynamic potential that predicts the spontaneity of a reaction. A negative ΔG indicates that a reaction is spontaneous and will proceed in the forward direction, often correlating with a K value greater than 1. Conversely, a positive ΔG suggests non-spontaneity, aligning with a K value less than 1.
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01:51Gibbs Free Energy of Reactions
Phase States and Their Influence on K
The phase states of reactants and products (solid, liquid, gas) significantly influence the equilibrium constant. Only gases and solutes in solution are included in the K expression, while solids and liquids are omitted. Recognizing the phase states helps in determining the correct K value and understanding how changes in conditions affect the equilibrium position.
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03:19States of Matter of Phase Diagrams
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