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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 28a
Capitolo 15, Problema 28a

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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1
Identify the relationship between the original reaction and the new reaction. The new reaction is obtained by dividing the original reaction by 2.
Understand that the equilibrium constant for a reaction that is multiplied or divided by a number can be calculated by raising the original equilibrium constant to the power of that number. In this case, since the reaction is divided by 2, the new Kp will be the square root of the original Kp.
Calculate the new Kp for the reaction COF2 (g) ⇌ 1/2 CO2(g) + 1/2 CF4(g) by taking the square root of the original Kp (2.2⨉106).
Compare the new Kp value to 1 to predict the direction of the equilibrium. If Kp > 1, the reaction favors the formation of products at equilibrium.
Conclude that since the new Kp is greater than 1, the reaction COF2 (g) ⇌ 1/2 CO2(g) + 1/2 CF4(g) will favor the formation of products (CO2 and CF4) at equilibrium.

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Equilibrium Constant (Kp)

The equilibrium constant, Kp, quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is expressed in terms of partial pressures for gaseous reactions. A large Kp value indicates that products are favored at equilibrium, while a small Kp suggests that reactants are favored.
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Equilibrium Constant Expressions

Reaction Stoichiometry

Reaction stoichiometry refers to the quantitative relationship between reactants and products in a chemical reaction, as represented by the balanced chemical equation. It is essential for calculating the equilibrium constant for different stoichiometric coefficients, as changing these coefficients alters the expression for Kp, affecting the equilibrium position.
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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 to counteract the change and restore a new equilibrium. This principle helps predict the direction in which the reaction will shift when the concentrations of reactants or products are altered, thereby influencing the favorability of reactants or products at equilibrium.
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Le Chatelier's Principle
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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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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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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. a. CH3OH(g) ⇌ CO(g) + 2 H2(g)

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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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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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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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