Domanda del libro di testo
The equilibrium constant for the dissociation of molecular iodine, I2(g) ⇌ 2 I(g), at 800 K is Kc = 3.1 × 10–5. (a) Which species predominates at equilibrium I2 or I?
Ch.15 - Chemical Equilibrium
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 15, Problema 15e
Write the expression for Kc for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous.
(a) 3 NO(g) ⇌ N2O(g) + NO2(g)
(b) CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g)
(c) Ni(CO)4(g) ⇌ Ni(s) + 4 CO(g)
(d) HF(aq) ⇌ H+(aq) + F-(aq)
(e) 2Ag(s) + Zn2+(aq) ⇌ 2 Ag+(aq) + Zn(s)
(f) H2O(l) ⇌ H+(aq) + OH-(aq)
(g) 2 H2O(l) ⇌ 2 H+(aq) + 2 OH-(aq)
Guida verificata passo dopo passo1
Identify the reactants and products in the reaction. For the given reaction, the reactants are Ag(s) and Zn2+(aq), and the products are Ag+(aq) and Zn(s).
Write the expression for the equilibrium constant, Kc, using the concentrations of the aqueous species. For each species, raise the concentration to the power of its stoichiometric coefficient in the balanced equation.
Since Ag(s) and Zn(s) are solids, their activity is considered to be 1 and they do not appear in the expression for Kc.
The expression for Kc is therefore: Kc = [Ag+]^2 / [Zn2+]
Determine the type of reaction: Since the reaction involves both solid and aqueous species, it is a heterogeneous reaction.
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Equilibrium Constant (Kc)
The equilibrium constant, Kc, is a numerical value that expresses the ratio of the concentrations of products to the concentrations of reactants at equilibrium for a given reaction at a specific temperature. It is calculated using the formula Kc = [products]^[coefficients] / [reactants]^[coefficients]. Understanding Kc is essential for predicting the direction of a reaction and the extent to which reactants are converted to products.
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03:20
Equilibrium Constant Expressions
Homogeneous vs. Heterogeneous Reactions
Homogeneous reactions occur when all reactants and products are in the same phase (solid, liquid, or gas), while heterogeneous reactions involve reactants and products in different phases. This distinction is important because it affects how concentrations are expressed in the Kc expression. In heterogeneous reactions, only the concentrations of species in the aqueous or gaseous phase are included in the Kc expression, while solids and liquids are omitted.
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03:05Ksp vs Q in Precipitation
Phase Representation in Reactions
In chemical equations, the physical state of each substance is indicated by symbols: (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous solutions. This representation is crucial for determining the correct form of the Kc expression. For example, in the given reaction, only the aqueous ions are included in the Kc expression, as the solid metals do not contribute to the equilibrium concentrations.
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03:22Phase Changes in Diagrams
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