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Ch.16 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.16 - Chemical EquilibriumProblem 29c
Chapter 16, Problem 29c

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)

Verified step by step guidance
1
Identify the relationship between the given reaction and the reaction in part c. The reaction in part c is the reverse of the given reaction, and it is also multiplied by a factor of 2.
Recall that the equilibrium constant for the reverse reaction is the reciprocal of the equilibrium constant for the forward reaction. Mathematically, if the forward reaction has an equilibrium constant K, then the reverse reaction has an equilibrium constant of 1/K.
Since the reaction in part c is also multiplied by 2, remember that when a reaction is multiplied by a factor, the equilibrium constant is raised to the power of that factor. If a reaction is multiplied by n, then the new equilibrium constant K' = K^n.
Apply these principles to calculate the new equilibrium constant Kp for the reaction in part c. Use the formula Kp' = (1/Kp)^2, where Kp is the equilibrium constant of the original reaction.
Predict whether reactants or products will be favored at equilibrium by comparing the magnitude of Kp' to 1. If Kp' > 1, products are favored; if Kp' < 1, reactants are favored.

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 larger Kp value indicates that products are favored at equilibrium, while a smaller Kp suggests that reactants are favored.
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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, thus influencing the favorability of reactants or products.
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Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction, as represented by the balanced chemical equation. Understanding stoichiometry is essential for calculating equilibrium constants for different reactions, as it allows for the proper adjustment of coefficients when deriving Kp for reactions that differ from the original equation.
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Related Practice
Textbook Question

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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Textbook Question

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)

790
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Textbook Question

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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Textbook Question

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
comments
Textbook Question

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)

3230
views
Textbook Question

H2 and I2 are combined in a flask and allowed to react according to the reaction: H2(g) + I2(g) ⇌ 2 HI(g) Examine the figures (sequential in time) and answer the questions: a. Which figure represents the point at which equilibrium is reached?

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