Textbook Question
At 2000Β°C, the equilibrium constant for the reaction 2 NO(π) β N2(π) + O2(π) is πΎπ = 2.4Γ103. If the initial concentration of NO is 0.175 M, what are the equilibrium concentrations of NO, N2, and O2?
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Ch.15 - Chemical Equilibrium
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 (SO<sub>3</sub>) is removed, the system will try to counteract this change by producing more SO<sub>3</sub>.
insert step 3> Predict the shift in equilibrium: The equilibrium will shift to the right, favoring the formation of more SO<sub>3</sub> from SO<sub>2</sub> and O<sub>2</sub>.
insert step 4> Consider the effect on concentrations: As the equilibrium shifts to the right, the concentration of SO<sub>2</sub> and O<sub>2</sub> will decrease, while the concentration of SO<sub>3</sub> will increase.
insert step 5> Conclude the effect on the system: The removal of SO<sub>3</sub> results in the system adjusting to restore equilibrium by producing more SO<sub>3</sub>, 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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01:14Equilibrium Constant K
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
For the equilibrium Br2(π) + Cl2(π) β 2 BrCl(π) at 400 K, πΎπ = 7.0. If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentrations of Br2, Cl2, and BrCl?
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Textbook Question
At 373 K, πΎπ = 0.416 for the equilibrium 2 NOBr(π) β 2 NO(π) + Br2(π) If the equilibrium partial pressures of NOBr(π) and Br2(π) are both 0.100 atm at 373 K, what is the equilibrium partial pressure of NO(π)?
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? (c) decrease [O2]
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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? (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? (e) add a catalyst
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