Open Question
For the reaction I2(g) + Br2(g) β 2 IBr(g), Kc = 280 at 150 _x001F_C. Suppose that 0.500 mol IBr in a 2.00-L flask is allowed to reach equilibrium at 150 _x001F_C. What are the equilibrium concentrations of IBr, I2, and Br2?
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.
Verified Solution
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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
At 25Β°C, the reaction CaCrO4(π ) β Ca2+(ππ) + CrO42β(ππ) has an equilibrium constant πΎπ = 7.1Γ10β4. What are the equilibrium concentrations of Ca2+ and CrO42β in a saturated solution of CaCrO4?
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Open Question
Methane, CH4, reacts with I2 according to the reaction CH4(g) + I2(g) β CH3I(g) + HI(g). At 630 K, Kp for this reaction is 2.26 Γ 10^-4. A reaction was set up at 630 K with initial partial pressures of methane at 105.1 torr and I2 at 7.96 torr. Calculate the pressures, in torr, of all reactants and products at equilibrium.
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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