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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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 23
Is the total enthalpy (H) of the reactants for an endothermic reaction greater than or less than the total enthalpy of the products?
Verified step by step guidance1
Understand the concept of an endothermic reaction: In an endothermic reaction, energy is absorbed from the surroundings, meaning the system gains energy during the reaction.
Recall the relationship between enthalpy (H) and energy: Enthalpy is a measure of the total energy of a system, including internal energy and the energy required to make room for it by displacing its surroundings.
Analyze the energy flow in an endothermic reaction: Since energy is absorbed, the products of the reaction will have a higher energy content compared to the reactants.
Compare the enthalpy of reactants and products: For an endothermic reaction, the total enthalpy of the products is greater than the total enthalpy of the reactants because energy is added to the system.
Conclude: The total enthalpy (H) of the reactants is less than the total enthalpy (H) of the products in an endothermic reaction.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Enthalpy (H)
Enthalpy is a thermodynamic property that represents the total heat content of a system. It is defined as the sum of the internal energy and the product of pressure and volume. In chemical reactions, changes in enthalpy indicate whether a reaction absorbs or releases heat, which is crucial for understanding reaction energetics.
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Bond Energy Example 1
Endothermic Reaction
An endothermic reaction is a type of chemical reaction that absorbs heat from its surroundings. This results in a decrease in temperature of the surroundings and an increase in the internal energy of the reactants. In such reactions, the total enthalpy of the products is greater than that of the reactants, as energy is required to break bonds and form new ones.
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Comparison of Reactants and Products
In thermodynamics, comparing the total enthalpy of reactants and products helps determine the nature of a reaction. For endothermic reactions, the enthalpy of the products exceeds that of the reactants, indicating that energy has been absorbed. This comparison is essential for predicting reaction behavior and understanding energy flow in chemical processes.
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Related Practice
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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Textbook Question
The vaporization of Br2 from the liquid to the gas state requires 7.4 kcal/mol (31.0 kJ/mol).
a. What is the sign of ∆H for this process? Write a reaction showing heat as a product or reactant.
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Textbook Question
The vaporization of Br2 from the liquid to the gas state requires 7.4 kcal/mol (31.0 kJ/mol).
c. How many kilojoules are needed to evaporate 82 g of Br2?
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Textbook Question
Converting liquid water to solid ice releases 1.44 kcal/mol (6.02 kJ/mol).How many kilocalories are released by freezing 32 g of H2O?
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