Textbook Question
Is the yield of SO3 at equilibrium favored by a higher or lower pressure? By a higher or lower temperature?
2 SO2(g) + O2 ⇌ 2 SO3(g) ∆H = -47 kcal/mol
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Ch.7 Chemical Reactions: Energy, Rate and Equilibrium
McMurry8th EditionFundamentals of GOBISBN: 9780134015187
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Table of contents
- Ch.1 Matter and Measurements27
- Ch.2 Atoms and the Periodic Table20
- Ch.3 Ionic Compounds8
- Ch.4 Molecular Compounds23
- Ch.5 Classification & Balancing of Chemical Reactions12
- Ch.6 Chemical Reactions: Mole and Mass Relationships28
- Ch.7 Chemical Reactions: Energy, Rate and Equilibrium64
- Ch.8 Gases, Liquids and Solids24
- Ch.9 Solutions52
- Ch.10 Acids and Bases25
- Ch.11 Nuclear Chemistry22
- Ch.12 Introduction to Organic Chemistry: Alkanes57
- Ch.13 Alkenes, Alkynes, and Aromatic Compounds47
- Ch.14 Some Compounds with Oxygen, Sulfur, or a Halogen50
- Ch.15 Aldehydes and Ketones45
- Ch.16 Amines42
- Ch.17 Carboxylic Acids and Their Derivatives57
- Ch.18 Amino Acids and Proteins82
- Ch.19 Enzymes and Vitamins63
- Ch.20 Carbohydrates44
- Ch.21 The Generation of Biochemical Energy65
- Ch.22 Carbohydrate Metabolism45
- Ch.23 Lipids42
- Ch.24 Lipid Metabolism33
- Ch.25 Protein and Amino Acid Metabolism24
- Ch.26 Nucleic Acids and Protein Synthesis45
Chapter 7, Problem 16c
What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?
C(s) + 2 H2(g) ⇌ CH4(g) ∆H = -18 kcal/mol (-75kJ/mol)
c. Allowing CH4 to escape continuously from the reaction vessel
Verified step by step guidance1
Identify the type of reaction: The reaction is exothermic (∆H = -18 kcal/mol), meaning it releases heat as it proceeds in the forward direction.
Understand the equilibrium principle: According to Le Chatelier's Principle, if a change is made to a system at equilibrium, the system will adjust to counteract that change and restore equilibrium.
Analyze the effect of CH4 escaping: If CH4 (a product) is continuously removed from the reaction vessel, the concentration of CH4 decreases. This disrupts the equilibrium by reducing the product concentration.
Predict the shift in equilibrium: To counteract the removal of CH4, the equilibrium will shift to the right (toward the products) to produce more CH4 and restore balance.
Conclude the effect: Allowing CH4 to escape continuously will drive the reaction forward, increasing the consumption of C(s) and H2(g) to produce more CH4(g).
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Le Chatelier's Principle
Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In the context of the given reaction, allowing CH4 to escape continuously reduces its concentration, prompting the equilibrium to shift to the right to produce more CH4, thereby attempting to restore balance.
Equilibrium Position
The equilibrium position of a reaction refers to the relative concentrations of reactants and products at equilibrium. In the reaction C(s) + 2 H2(g) ⇌ CH4(g), the position can be influenced by changes in concentration, pressure, or temperature. Understanding how these factors affect the equilibrium position is crucial for predicting the outcome of the reaction when CH4 is allowed to escape.
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The Equilibrium Constant Example 1
Endothermic and Exothermic Reactions
Reactions can be classified as endothermic or exothermic based on heat exchange. The given reaction is exothermic (∆H = -18 kcal/mol), meaning it releases heat. This characteristic is important because changes in temperature can also affect the equilibrium; for exothermic reactions, increasing temperature shifts the equilibrium to favor reactants, while decreasing temperature favors products.
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Related Practice
Textbook Question
What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?
C(s) + 2 H2(g) ⇌ CH4(g) ∆H = -18 kcal/mol (-75kJ/mol)
a. Increasing temperature
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Textbook Question
What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?
C(s) + 2 H2(g) ⇌ CH4(g) ∆H = -18 kcal/mol (-75kJ/mol)
b. Increasing pressure by decreasing volume
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Textbook Question
Two curves are shown in the following energy diagram:
b. Which curve represents the spontaneous reaction, and which the nonspontaneous?
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Textbook Question
The following diagram portrays a reaction of the type A(s) → B(g) + C(g), where the different-colored spheres represent different molecular structures. Assume that the reaction has ∆H = +9.1 kcal/mol (+38.1 kJ/mol).
a. What is the sign of ∆S for the reaction?
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Textbook Question
The following diagram portrays a reaction of the type A(s) → B(g) + C(g), where the different-colored spheres represent different molecular structures. Assume that the reaction has ∆H = +9.1 kcal/mol (+38.1 kJ/mol).
b. Is the reaction likely to be spontaneous at all temperatures, nonspontaneous at all temperatures, or spontaneous at some but nonspontaneous at others?
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