Textbook Question
Methanol (CH3OH) can be made by the reaction of CO with H2: CO(π) + 2 H2(π) β CH3OH(π) (b) To maximize the equilibrium yield of methanol, would you use a high or low temperature?
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Ch.15 - Chemical Equilibrium
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 15, Problem 69b
(b) If the temperature is raised by 100 K, does the equilibrium constant for this reaction increase or decrease?
Verified step by step guidance1
insert step 1> Identify the type of reaction (endothermic or exothermic) using the enthalpy change (\( \Delta H \)) of the reaction.
insert step 2> Recall Le Chatelier's Principle, which states that a system at equilibrium will adjust to counteract any changes imposed on it.
insert step 3> Understand that for an endothermic reaction (\( \Delta H > 0 \)), increasing temperature shifts the equilibrium to the right, favoring the formation of products, thus increasing the equilibrium constant (\( K \)).
insert step 4> Conversely, for an exothermic reaction (\( \Delta H < 0 \)), increasing temperature shifts the equilibrium to the left, favoring the formation of reactants, thus decreasing the equilibrium constant (\( K \)).
insert step 5> Conclude whether the equilibrium constant increases or decreases based on the reaction's enthalpy change and the temperature increase.
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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. This principle helps predict how changes in temperature, pressure, or concentration will affect the position of equilibrium in a chemical reaction.
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Le Chatelier's Principle
Temperature and Equilibrium Constant
The equilibrium constant (K) of a reaction is temperature-dependent. For exothermic reactions, increasing the temperature typically decreases K, while for endothermic reactions, increasing the temperature usually increases K. Understanding the nature of the reaction (exothermic or endothermic) is crucial to predicting how K will change with temperature.
Exothermic and Endothermic Reactions
Exothermic reactions release heat, resulting in a negative change in enthalpy (ΞH < 0), while endothermic reactions absorb heat, leading to a positive change in enthalpy (ΞH > 0). The classification of a reaction as exothermic or endothermic is essential for determining how the equilibrium constant will respond to temperature changes.
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Related Practice
Textbook Question
(a) Is the dissociation of fluorine molecules into atomic fluorine, F2(π) β 2 F(π), an exothermic or endothermic process?
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Textbook Question
(c) If the temperature is raised by 100 K, does the forward rate constant kf increase by a larger or smaller amount than the reverse rate constant kr?
Textbook Question
When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(g) β SO2(g) + Cl2(g) (a) Calculate Kc for this reaction at this temperature.
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Textbook Question
Ozone, O3, decomposes to molecular oxygen in the stratosphere according to the reaction 2 O3(π) βΆ 3 O2(π). Would increasing the pressure by decreasing the size of the reaction vessel favor the formation of ozone or of oxygen?