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Ch.15 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.15 - Chemical EquilibriumProblema 28b
Capitolo 15, Problema 28b

This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.
b. 6 COF2(g) ⇌ 3 CO2(g) + 3 CF4(g)

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Identify the relationship between the original reaction and the new reaction. The new reaction is essentially three times the original reaction.
Use the rule for equilibrium constants when a reaction is multiplied by a factor. If a balanced equation is multiplied by a factor 'n', the new equilibrium constant K' is the original K raised to the power of 'n'.
Apply the rule to the given Kp value. Since the new reaction is three times the original, raise the original Kp to the power of 3.
Calculate Kp for the new reaction using the formula Kp,new = (Kp,original)^3.
Predict whether reactants or products are favored by comparing the magnitude of the new Kp. If Kp is much greater than 1, products are favored; if Kp is much less than 1, reactants are favored.

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Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is calculated using the partial pressures of gases involved in the reaction. A large Kp value (greater than 1) indicates that products are favored at equilibrium, while a small Kp value (less than 1) suggests that reactants are favored.
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Equilibrium Constant Expressions

Reaction Stoichiometry

Reaction stoichiometry refers to the quantitative relationship between the amounts of reactants and products in a chemical reaction, as described by the balanced chemical equation. It is essential for calculating the equilibrium constant for different stoichiometric coefficients. In the given reaction, the stoichiometry must be adjusted to determine how the equilibrium constant changes when the coefficients of the reactants and products are altered.
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Stoichiometry Concept

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. This principle helps predict the direction in which a reaction will shift when changes in concentration, pressure, or temperature occur. Understanding this principle is crucial for determining whether reactants or products will be favored at equilibrium based on the given equilibrium constant.
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Le Chatelier's Principle
Pratica correlata
Domanda del libro di testo

Consider the reactions and their respective equilibrium

constants:

NO(g) + 1/2 Br (g) ⇌ NOBr(g) Kp = 5.3

2 NO(g) ⇌ N2(g) + O2(g) Kp = 2.1⨉1030

Use these reactions and their equilibrium constants to predict

the equilibrium constant for the following reaction: N2(g) + O2(g) + Br2(g) ⇌ 2 NOBr(g)

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Domanda del libro di testo

This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

c. 2 CO2(g) + 2 CF4(g) ⇌ 4 COF2(g)

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Domanda del libro di testo

Calculate Kc for each reaction. a. I2(g) ⇌ 2I(g) Kp = 6.26⨉10-22 (at 298K)

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Domanda del libro di testo

This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

a. COF2 (g) ⇌ 1/2 CO2(g) + 1/2 CF4(g)

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Domanda del libro di testo

This reaction has an equilibrium constant of Kp = 2.26⨉104 at 298 K. CO(g) + 2 H2(g) ⇌ CH3OH(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

c. 2 CH3OH(g) ⇌ 2 CO(g) + 4 H2(g)

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Domanda del libro di testo

This reaction has an equilibrium constant of Kp = 2.26⨉104 at 298 K. CO(g) + 2 H2(g) ⇌ CH3OH(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

b. 1/2 CO(g) + H2 (g) ⇌ 1/2 CH3OH(g)

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