Domanda del libro di testo
The diagram shown here represents the equilibrium state for the reaction A2(𝑔) + 2B(𝑔) ⇌ 2AB(𝑔). (a) Assuming the volume is 2 L, calculate the equilibrium constant 𝐾𝑐 for the reaction.
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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 14a
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?
Guida verificata passo dopo passo1
Understand the equilibrium expression for the reaction: I2(g) ⇌ 2 I(g). The equilibrium constant, Kc, is given for this reaction.
Write the expression for the equilibrium constant Kc: . This expression relates the concentrations of the products and reactants at equilibrium.
Consider the value of Kc = 3.1 × 10–5. A small Kc value indicates that the equilibrium position favors the reactants over the products.
Analyze the equilibrium position: Since Kc is much less than 1, the concentration of I2(g) is greater than the concentration of I(g) at equilibrium.
Conclude which species predominates: Given the small value of Kc, I2(g) predominates at equilibrium over I(g).
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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 the products (I), suggesting that the reaction favors the formation of reactants.
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Percorso guidato
03:20
Equilibrium Constant Expressions
Le Chatelier's Principle
Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. In the context of the dissociation of I2, if the concentration of I is increased or the temperature is altered, the equilibrium will shift to either the right (producing more I) or the left (producing more I2) to minimize the disturbance.
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07:32Le Chatelier's Principle
Predominance of Species at Equilibrium
To determine which species predominates at equilibrium, one must compare the concentrations of the reactants and products using the equilibrium constant. A Kc value significantly less than 1 indicates that the reactants are favored, meaning that at equilibrium, the concentration of I2 will be much higher than that of I, confirming that I2 predominates in this reaction.
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Percorso guidato
03:03Amphoteric Species
Pratica correlata
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. (b) Assuming both forward and reverse reactions are elementary reactions, which reaction has the larger rate constant, the forward or the reverse reaction?
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Domanda del libro di testo
Write the expressions for Kc for the following reactions. In each case indicate whether the reaction is homogeneous or heterogeneous.
(a) 2 O3(g) ⇌ 3 O2(g)
(c) 2 C2H4(g) + 2 H2O(g) ⇌ 2 C2H6(g) + O2(g)
(d) C(s) + 2 H2(g) ⇌ CH4(g)
(e) 4 HCl(aq) + O2(g) ⇌ 2 H2O(l) + 2 Cl2(g)
(f) 2 C8H18(l) + 25 O2(g) ⇌ 16 CO2(g) + 18 H2O(g)
(g) 2 C8H18(l) + 25 O2(g) ⇌ 16 CO2(g) + 18 H2O(l)
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Domanda del libro di testo
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)
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Domanda del libro di testo
Suppose that the gas-phase reactions A → B and B → A are both elementary reactions with rate constants of 4.7×10−3 s−1 and 5.8×10−1 s−1, respectively. (a) What is the value of the equilibrium constant for the equilibrium A(g) ⇌ B(g)? (b) Which is greater at equilibrium, the partial pressure of A or the partial pressure of B?
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