Consider the following reaction N2 (g) + O2 (g) ↔ 2NO (g) If the equilibrium partial pressures of N2, O2 and NO are 0.15 atm, 0.33 atm and 0.05 atm, respectively, at 2200ºC. Calculate: a) The equilibrium constant Kc of the reaction. b) The equilibrium constant Kp of the reaction. C) What will be the new equilibrium compositions and the total pressure of the system if 0.5 moles of O2 are added to this initial equilibrium? Let V and T remain constant.
Consider the following reaction N2 (g) + O2 (g) ↔ 2NO (g) If the equilibrium partial pressures of N2, O2 and NO are 0.15 atm, 0.33 atm and 0.05 atm, respectively, at 2200ºC. Calculate: a) The equilibrium constant Kc of the reaction. b) The equilibrium constant Kp of the reaction. C) What will be the new equilibrium compositions and the total pressure of the system if 0.5 moles of O2 are added to this initial equilibrium? Let V and T remain constant.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter12: Gaseous Chemical Equilibrium
Section: Chapter Questions
Problem 20QAP: Consider the following hypothetical reactions and their equilibrium constants at 75C,...
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Consider the following reaction
N2 (g) + O2 (g) ↔ 2NO (g)
If the equilibrium partial pressures of N2, O2 and NO are 0.15 atm, 0.33 atm and 0.05 atm, respectively, at 2200ºC.
Calculate:
a) The equilibrium constant Kc of the reaction.
b) The equilibrium constant Kp of the reaction.
C) What will be the new equilibrium compositions and the total pressure of the system if 0.5 moles of O2 are added to this initial equilibrium? Let V and T remain constant.
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