Ch.15 - Chemical Equilibrium

Problem 28b

Chapter 15, Problem 28b

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

Verified step by step guidance

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 K_p value. Since the new reaction is three times the original, raise the original K_p to the power of 3.

Calculate K_p for the new reaction using the formula K_p,new = (K_p,original)^3.

Predict whether reactants or products are favored by comparing the magnitude of the new K_p. If K_p is much greater than 1, products are favored; if K_p is much less than 1, reactants are favored.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

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.

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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Related Practice

Textbook Question

This reaction has an equilibrium constant of K_p = 2.26⨉10⁴ at 298 K. CO(g) + 2 H₂(g) ⇌ CH₃OH(g) Calculate K_p 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)

Textbook Question

c. 2 CH₃OH(g) ⇌ 2 CO(g) + 4 H₂(g)

Textbook Question

This reaction has an equilibrium constant of K_p = 2.2⨉10⁶ at 298 K. 2 COF₂(g) ⇌ CO₂(g) + CF₄(g) Calculate K_p 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)

Textbook Question

c. 2 CO₂(g) + 2 CF₄(g) ⇌ 4 COF₂(g)

Textbook Question

Consider the reactions and their respective equilibrium

constants:

NO(g) + 1/2 Br (g) ⇌ NOBr(g) K_p = 5.3

2 NO(g) ⇌ N₂(g) + O₂(g) K_p = 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)

Textbook Question

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