Open Question
At 800 K, the equilibrium constant for the reaction I2(g) β 2 I(g) is Kc = 3.1 * 10^-5. If an equilibrium mixture in a 10.0-L vessel contains 2.67 * 10^-2 g of I(g), how many grams of I2 are in the mixture?
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 53
At 373 K, πΎπ = 0.416 for the equilibrium 2 NOBr(π) β 2 NO(π) + Br2(π) If the pressures of NOBr(π) and NO(π) are equal, what is the equilibrium pressure of Br2(π)?
Verified step by step guidance1
Identify the balanced chemical equation: 2 NOBr(g) β 2 NO(g) + Br_2(g).
Write the expression for the equilibrium constant K_p: K_p = (P_NO^2 * P_Br2) / (P_NOBr^2).
Since the pressures of NOBr and NO are equal, let P_NOBr = P_NO = x.
Substitute the pressures into the K_p expression: 0.416 = (x^2 * P_Br2) / (x^2).
Solve for P_Br2: P_Br2 = 0.416.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Equilibrium Constant (Kp)
The equilibrium constant, Kp, is a ratio that expresses the relationship between the partial pressures of the products and reactants at equilibrium for a given reaction at a specific temperature. For the reaction 2 NOBr(g) β 2 NO(g) + Br2(g), Kp is calculated using the formula Kp = (P_NO^2 * P_Br2) / (P_NOBr^2), where P represents the partial pressures of the gases involved.
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Equilibrium Constant Expressions
Partial Pressure
Partial pressure is the pressure exerted by a single component of a gas mixture. In the context of the equilibrium reaction, the total pressure is the sum of the partial pressures of NOBr, NO, and Br2. Understanding how to calculate and relate these pressures is essential for determining the equilibrium state of the system.
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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 problem, if the pressures of NOBr and NO are equal, the system will shift to produce more Br2 to maintain the equilibrium constant, which is crucial for finding the equilibrium pressure of Br2.
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Related Practice
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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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 218Β°C, πΎπ = 1.2Γ10β4 for the equilibrium NH4SH(π ) β NH3(π) + H2S(π) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH4SH is placed in a closed vessel at 218Β°C and decomposes until equilibrium is reached.
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Open Question
Consider the reaction \( \text{CaSO}_4(\text{s}) \rightleftharpoons \text{Ca}^{2+}(\text{aq}) + \text{SO}_4^{2-}(\text{aq}) \) At 25 Β°C, the equilibrium constant is \( K_c = 2.4 \times 10^{-5} \) for this reaction. (a) If excess \( \text{CaSO}_4(\text{s}) \) is mixed with water at 25 Β°C to produce a saturated solution of \( \text{CaSO}_4 \), what are the equilibrium concentrations of \( \text{Ca}^{2+} \) and \( \text{SO}_4^{2-} \)? (b) If the resulting solution has a volume of 1.4 L, what is the minimum mass of \( \text{CaSO}_4(\text{s}) \) needed to achieve equilibrium?
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.
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