Domanda del libro di testo
Find and fix each mistake in the equilibrium constant expressions. a. 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = [H2][S2]/[H2S]
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Ch.15 - Chemical Equilibrium
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 15, Problema 6
Consider the reaction: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Kp = 0.0611 at 2000 K. A reaction mixture initially contains a CO partial pressure of 1344 torr and a H2O partial pressure of 1766 torr at 2000 K. Calculate the equilibrium partial pressures of each of the products.
Guida verificata passo dopo passo1
Convert the initial partial pressures from torr to atm by dividing each by 760, since 1 atm = 760 torr.
Set up an ICE (Initial, Change, Equilibrium) table to track the changes in partial pressures of each species. Let the change in pressure for CO and H2O be \(-x\), and for CO2 and H2 be \(+x\).
Write the expression for the equilibrium constant \(K_p\) in terms of partial pressures: \(K_p = \frac{P_{CO_2} \cdot P_{H_2}}{P_{CO} \cdot P_{H_2O}}\).
Substitute the equilibrium expressions from the ICE table into the \(K_p\) expression and solve for \(x\).
Calculate the equilibrium partial pressures by substituting \(x\) back into the expressions for each species: \(P_{CO} = P_{CO, initial} - x\), \(P_{H_2O} = P_{H_2O, initial} - x\), \(P_{CO_2} = x\), and \(P_{H_2} = x\).
Concetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
Equilibrium Constant (Kp)
The equilibrium constant (Kp) is a numerical value that expresses the ratio of the partial pressures of the products to the reactants at equilibrium for a given reaction at a specific temperature. For the reaction CO(g) + H2O(g) ⇌ CO2(g) + H2(g), Kp = 0.0611 indicates that at equilibrium, the products' partial pressures are relatively low compared to the reactants, reflecting the position of equilibrium.
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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 this context, if the initial concentrations of CO and H2O are high, the reaction will shift towards the products to reach equilibrium, affecting the partial pressures of CO2 and H2.
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07:32Le Chatelier's Principle
Partial Pressure
Partial pressure is the pressure exerted by a single component of a gas mixture. In this reaction, the total pressure is the sum of the partial pressures of CO, H2O, CO2, and H2. To find the equilibrium partial pressures of the products, one must apply the initial conditions and the equilibrium constant to calculate how much of each gas is present at equilibrium.
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00:48Partial Pressure Calculation