Textbook Question
Consider the reaction 4 NH3(π) + 5 O2(π) β 4 NO(π) + 6 H2O(π), Ξπ» = β904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (e) add a catalyst
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Ch.15 - Chemical Equilibrium
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 15, Problem 61f
Consider the following equilibrium, for which Ξπ»<0
2 SO2(π) + O2(π) β 2 SO3(π)
(f) How will each of the following changes affect an equilibrium mixture of the three gases: SO3(π) is removed from the system?
Verified step by step guidance1
insert step 1> Identify the type of reaction and the effect of removing a product on the equilibrium. This is an exothermic reaction (Ξπ» < 0), and removing a product will shift the equilibrium to the right according to Le Chatelier's Principle.
insert step 2> Apply Le Chatelier's Principle: When a product (SO3) is removed, the system will try to counteract this change by producing more SO3.
insert step 3> Predict the shift in equilibrium: The equilibrium will shift to the right, favoring the formation of more SO3 from SO2 and O2.
insert step 4> Consider the effect on concentrations: As the equilibrium shifts to the right, the concentration of SO2 and O2 will decrease, while the concentration of SO3 will increase.
insert step 5> Conclude the effect on the system: The removal of SO3 results in the system adjusting to restore equilibrium by producing more SO3, thus shifting the equilibrium to the right.
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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, removing SOβ will decrease its concentration, prompting the equilibrium to shift to the right to produce more SOβ, thereby restoring balance.
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Le Chatelier's Principle
Equilibrium Constant (K)
The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction provided, K is determined by the concentrations of SOβ, SOβ, and Oβ. Changes in concentration, such as the removal of SOβ, can affect the system's ability to reach a new equilibrium state.
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Endothermic vs. Exothermic Reactions
Reactions are classified as endothermic or exothermic based on the heat exchange with the surroundings. The given reaction is exothermic (ΞH < 0), meaning it releases heat. Understanding this helps predict how temperature changes might affect the equilibrium; for instance, removing a product like SOβ can shift the equilibrium to the right, potentially releasing heat and favoring the formation of more products.
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Related Practice
Textbook Question
Consider the reaction 4 NH3(π) + 5 O2(π) β 4 NO(π) + 6 H2O(π), Ξπ» = β904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (d) decrease the volume of the container in which the reaction occurs
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Textbook Question
Consider the reaction 4 NH3(π) + 5 O2(π) β 4 NO(π) + 6 H2O(π), Ξπ» = β904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (a) increase [NH3] (b) increase [H2O] (c) decrease [O2]
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Textbook Question
At 80Β°C, πΎπ = 1.87Γ10β3 for the reaction PH3BCl3(π ) β PH3(π) + BCl3(π) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80Β°C and decomposes until equilibrium is reached. (b) If the flask has a volume of 0.250 L, what is the minimum mass of PH3BCl3(π ) that must be added to the flask to achieve equilibrium?
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