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
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 15, Problema 14b
The equilibrium constant for the dissociation of molecular iodine, I2(g) ⇌ 2 I(g), at 800 K is Kc = 3.1×10−5. (b) Assuming both forward and reverse reactions are elementary reactions, which reaction has the larger rate constant, the forward or the reverse reaction?
Guida verificata passo dopo passo1
Identify the reaction and its reverse: The given reaction is I2(g) ⇌ 2 I(g). The forward reaction is the dissociation of I2 into 2 I atoms, and the reverse reaction is the recombination of 2 I atoms to form I2.
Understand the equilibrium constant (Kc): Kc is defined as the ratio of the rate constant of the forward reaction (kf) to the rate constant of the reverse reaction (kr). The formula is Kc = kf / kr.
Analyze the value of Kc: Given that Kc = 3.1×10−5, which is a small number, it indicates that the equilibrium heavily favors the reactants over the products at 800 K.
Determine the larger rate constant: Since Kc is small and represents the ratio of kf to kr, this implies that kr (rate constant for the reverse reaction) is much larger than kf (rate constant for the forward reaction).
Conclude which reaction has the larger rate constant: The reverse reaction, which is the recombination of I atoms to form I2, has the larger rate constant compared to the forward reaction of dissociation of I2 into I atoms.
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Equilibrium Constant (Kc)
The equilibrium constant, Kc, quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the dissociation of I2, Kc = [I]^2 / [I2]. A small Kc value, like 3.1×10^−5, indicates that at equilibrium, the concentration of reactants (I2) is much greater than that of products (I), suggesting the reaction favors the reactants.
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03:20
Equilibrium Constant Expressions
Rate Constants and Reaction Rates
Rate constants (k) are specific to each reaction and temperature, determining the speed of the reaction. The forward reaction rate constant (k_forward) relates to the formation of products, while the reverse reaction rate constant (k_reverse) relates to the formation of reactants. The relationship between Kc and the rate constants is given by Kc = k_forward / k_reverse, which helps in comparing their magnitudes.
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00:45Rate Constant Units
Elementary Reactions
Elementary reactions are single-step processes where reactants convert directly to products without intermediates. Each elementary reaction has a specific rate law that reflects its molecularity. In this case, both the forward and reverse reactions are assumed to be elementary, allowing for a straightforward comparison of their rate constants based on the equilibrium constant.
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03:06Reaction Mechanism Overview
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