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 13
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?
Guida verificata passo dopo passo1
Identify the rate constants for the forward reaction (A → B) and the reverse reaction (B → A). The rate constant for A → B is 4.7×10−3 s−1 and for B → A is 5.8×10−1 s−1.
Understand that at equilibrium, the rate of the forward reaction (A → B) equals the rate of the reverse reaction (B → A). This can be expressed as kf[A] = kr[B], where kf and kr are the rate constants for the forward and reverse reactions, respectively, and [A] and [B] are the concentrations of A and B.
Rearrange the equilibrium expression to find the ratio of the concentrations of B to A at equilibrium: [B]/[A] = kf/kr.
Substitute the given rate constants into the expression to find the ratio: [B]/[A] = (4.7×10−3 s−1) / (5.8×10−1 s−1).
Compare the ratio [B]/[A] to determine which is greater at equilibrium. If [B]/[A] > 1, then [B] is greater; if [B]/[A] < 1, then [A] is greater.
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Equilibrium Constant
The equilibrium constant (K) for a reaction at equilibrium is defined as the ratio of the concentrations (or partial pressures) of the products to the reactants, each raised to the power of their stoichiometric coefficients. For the reactions A ⇌ B, K can be calculated using the rate constants of the forward (k₁) and reverse (k₂) reactions: K = k₁/k₂. This constant helps determine the relative amounts of A and B at equilibrium.
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Percorso guidato
01:14
Equilibrium Constant K
Rate Constants
Rate constants (k) are specific to each reaction and indicate the speed at which a reaction proceeds. In this case, the rate constant for the forward reaction (A → B) is 4.7×10⁻³ s⁻¹, while for the reverse reaction (B → A) it is 5.8×10⁻¹ s⁻¹. The magnitude of these constants influences the equilibrium position, with larger constants favoring the formation of products or reactants.
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Percorso guidato
00:45Rate Constant Units
Le Chatelier's Principle
Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust to counteract the disturbance and restore a new equilibrium. In the context of the given reactions, knowing the rate constants allows us to predict which species will be favored at equilibrium, as the system will shift towards the side with the lower energy or higher stability based on the rate constants.
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07:32Le Chatelier's Principle
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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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Domanda del libro di testo
The reaction A2 + B2 ⇌ 2 AB has an equilibrium constant Kc = 1.5. The following diagrams represent reaction mixtures containing A2 molecules (red), B2 molecules (blue), and AB molecules. (a) Which reaction mixture is at equilibrium?
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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 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
When lead(IV) oxide is heated above 300°C, it decomposes according to the reaction, 2 PbO2(𝑠)⇌2PbO(𝑠)+O2(𝑔). Consider the two sealed vessels of PbO2 shown here. If both vessels are heated to 400°C and allowed to come to equilibrium, which of the following statements is or are true? c. The partial pressure of O2(𝑔) will be the same in vessels A and B. [Section 15.4]