Textbook Question
For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆H = –43 kcal/mol (–180 kJ/mol).
b. Under what conditions would you expect this process to be spontaneous?
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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 44
Why does increasing concentration generally increase the rate of a reaction?
Verified step by step guidance1
Understand the concept of reaction rate: The rate of a chemical reaction refers to how quickly reactants are converted into products. It depends on the frequency and energy of collisions between reactant molecules.
Recall the collision theory: According to collision theory, for a reaction to occur, reactant molecules must collide with sufficient energy (activation energy) and proper orientation.
Relate concentration to collision frequency: Increasing the concentration of reactants means there are more molecules or ions in a given volume. This increases the likelihood of collisions between reactant particles.
Explain the effect on reaction rate: With more frequent collisions, the number of successful collisions (those with sufficient energy and correct orientation) also increases, leading to a faster reaction rate.
Summarize the relationship: In general, a higher concentration of reactants results in a higher reaction rate because it increases the probability of effective collisions as described by the collision theory.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Collision Theory
Collision theory posits that for a reaction to occur, reactant particles must collide with sufficient energy and proper orientation. Increasing the concentration of reactants raises the number of particles in a given volume, leading to more frequent collisions. This increased frequency enhances the likelihood of effective collisions, thereby accelerating the reaction rate.
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Atomic Theory
Reaction Rate
The reaction rate refers to the speed at which reactants are converted into products in a chemical reaction. It is influenced by several factors, including concentration, temperature, and the presence of catalysts. Higher concentrations typically result in a higher reaction rate due to the increased number of reactant molecules available to participate in the reaction.
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Equilibrium Shift
In reversible reactions, increasing the concentration of reactants can shift the equilibrium position according to Le Chatelier's principle. This shift favors the formation of products, thus increasing the rate at which products are formed. Understanding this concept is crucial for predicting how changes in concentration affect the dynamics of a chemical reaction.
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Related Practice
Textbook Question
The following reaction is used in the industrial synthesis of polyvinyl chloride (PVC) polymer:
Cl2(g) + H2C=CH2(g) → ClCH2CH2Cl(l) ∆H = –52 kcal/mol (–218 kJ/mol)
a. Is ∆S positive or negative for this process?
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Textbook Question
Which reaction is faster, one with Eact = +10 kcal/mol(+41.8 kJ/mol) or one with Eact = +5 kcal/mol(+20.9 kJ/mol)? Explain.
2017
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Textbook Question
What is a catalyst, and what effect does it have on the activation energy of a reaction?
2017
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Textbook Question
If a catalyst changes the activation energy of a forward reaction from 28.0 kcal/mol to 23.0 kcal/mol, what effect does it have on the reverse reaction?
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Textbook Question
For the reaction C(s, diamond) → C(s, graphite), ∆G = -0.693 kcal/mol (-2.90 kJ/mol) at 25 °C.
a. According to this information, do diamonds spontaneously turn into graphite?
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