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 58
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)?
Verified step by step guidance1
Identify the equilibrium expression for the reaction: \( K_p = \frac{(P_{NO})^2 (P_{Br_2})}{(P_{NOBr})^2} \).
Substitute the known values into the equilibrium expression: \( K_p = 0.416 \), \( P_{NOBr} = 0.100 \) atm, and \( P_{Br_2} = 0.100 \) atm.
Rearrange the equation to solve for \( (P_{NO})^2 \): \( (P_{NO})^2 = K_p \times (P_{NOBr})^2 / P_{Br_2} \).
Substitute the known values into the rearranged equation: \( (P_{NO})^2 = 0.416 \times (0.100)^2 / 0.100 \).
Calculate \( P_{NO} \) by taking the square root of \( (P_{NO})^2 \).
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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 partial pressures of NOBr, NO, and Br2 are crucial for calculating the equilibrium constant and determining the concentrations of each species at equilibrium. The total pressure of the gas mixture is the sum of the partial pressures of all components.
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Stoichiometry of the Reaction
Stoichiometry refers to the quantitative relationship between the reactants and products in a chemical reaction. In this equilibrium, the stoichiometric coefficients indicate that for every 2 moles of NOBr that dissociate, 2 moles of NO and 1 mole of Br2 are produced. This relationship is essential for calculating the equilibrium partial pressure of NO based on the known partial pressures of NOBr and Br2.
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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
Consider the following equilibrium, for which Ξπ»<0
2 SO2(π) + O2(π) β 2 SO3(π)
(e) the total pressure of the system is increased by adding a noble gas
Textbook Question
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?