Textbook Question
When the following equilibria are disturbed by increasing the pressure, does the concentration of reaction products increase, decrease, or remain the same?
a. 2 CO2(g) ⇌ 2 CO(g) + O2(g)
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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 65b
The reaction H2(g) + I2(g) ⇌ 2 HI(g) has ∆H = -2.2 kcal/mol (-9.2 kJ/mol). Will the equilibrium concentration of HI increase or decrease when
b. H2 is removed?
Verified step by step guidance1
Identify the type of reaction: The reaction is exothermic because the enthalpy change (∆H) is negative (-2.2 kcal/mol). This means heat is released as the reaction proceeds forward.
Understand the effect of removing H2: According to Le Châtelier's Principle, if a reactant (H2 in this case) is removed, the equilibrium will shift to counteract the change by producing more H2. This means the reaction will shift to the left (toward the reactants).
Analyze the impact on HI concentration: Since the reaction shifts to the left, the concentration of the product (HI) will decrease as the system works to re-establish equilibrium.
Summarize the relationship: Removing H2 reduces the availability of one of the reactants, which forces the equilibrium to favor the reverse reaction, thereby decreasing the concentration of HI.
Conclude the answer: The equilibrium concentration of HI will decrease when H2 is removed, as the system shifts to restore balance by producing more H2 and I2.
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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 system will adjust to counteract the change and restore a new equilibrium. In this case, removing H2 will shift the equilibrium position to favor the production of H2 to compensate for its loss.
Equilibrium Constant (K)
The equilibrium constant (K) 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. Changes in concentration of reactants or products can affect the position of equilibrium but not the value of K itself.
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Reaction Quotient (Q)
The reaction quotient (Q) is a measure of the relative concentrations of products and reactants at any point in time, not just at equilibrium. By comparing Q to K, one can predict the direction in which the reaction will shift to reach equilibrium. If H2 is removed, Q will change, prompting the system to shift towards the reactants.
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Related Practice
Textbook Question
For the following equilibria, use Le Châtelier's principle to predict the direction of the reaction when the pressure is increased by decreasing the volume of the equilibrium mixture.
a. C(s) + H2O(g) ⇌ CO(g) + H2(g)
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Textbook Question
The reaction CO(g) + H2O(g) ⇌ CO2(g) + H2(g) has ∆H = -9.8 kcal/mol (-41 kJ/mol). Does the amount of H2 in an equilibrium mixture increase or decrease when the temperature is decreased?
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Textbook Question
The reaction H2(g) + I2(g) ⇌ 2 HI(g) has ∆H = -2.2 kcal/mol (-9.2 kJ/mol). Will the equilibrium concentration of HI increase or decrease when
c. A catalyst is added?
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Textbook Question
The reaction Fe3+(aq) + Cl-(aq) ⇌ FeCl2+(aq) is endothermic. How will the equilibrium concentration of FeCl2+ change when
b. Cl- is precipitated by addition of AgNO3?
2017
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Textbook Question
For the unbalanced combustion reaction shown, 1 mol of ethanol, C2H5OH, releases 327 kcal (1370 kJ):
C2H5OH + O2 → CO2 + H2O
e. If the density of ethanol is 0.789 g/mL, calculate the combustion energy of ethanol in kilocalories/milliliter and kilojoules/milliliter
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