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Ch.15 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.15 - Chemical EquilibriumProblem 27b
Chapter 15, Problem 27b

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)

Verified step by step guidance
1
Step 1: Understand the relationship between the original reaction and the new reaction. In this case, the new reaction is the original reaction divided by 2.
Step 2: Use the rule that if a reaction is divided by a factor, the equilibrium constant for the new reaction is the square root of the original equilibrium constant. This is because the equilibrium constant is a ratio of the concentrations of the products to the reactants, each raised to the power of their stoichiometric coefficients. When the coefficients are halved, the powers in the ratio are also halved, which is equivalent to taking the square root.
Step 3: Calculate the new equilibrium constant, Kp', by taking the square root of the original Kp. The square root of 2.26⨉104 will give you Kp' for the new reaction.
Step 4: Determine whether the reactants or products are favored at equilibrium. If Kp' is greater than 1, the products are favored. If Kp' is less than 1, the reactants are favored.
Step 5: Compare the calculated Kp' with 1 to determine whether the reactants or products are favored at equilibrium.

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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, 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 larger Kp value indicates that products are favored at equilibrium, while a smaller Kp suggests that reactants are favored.
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Reaction Stoichiometry

Reaction stoichiometry refers to the quantitative relationship between reactants and products in a chemical reaction, as represented by the balanced equation. It is essential for calculating the equilibrium constant for reactions with different stoichiometric coefficients, as changes in coefficients affect the equilibrium expression and the value of Kp.
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Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions (such as concentration, pressure, or temperature), 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 equilibrium is altered, indicating whether reactants or products will be favored.
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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)

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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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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.

c. 2 CH3OH(g) ⇌ 2 CO(g) + 4 H2(g)

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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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Textbook Question

Ethene (C2H4) can be halogenated by this reaction: C2H4(g) + X2(g) ⇌ C2H4X2(g) where X2 can be Cl2 (green), Br2 (brown), or I2 (purple). Examine the three figures representing equilibrium concentrations in this reaction at the same temperature for the three different hal- ogens. Rank the equilibrium constants for the three reactions from largest to smallest.

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