The equilibrium 2 NO1g2 + Cl21g2 ∆ 2 NOCl1g2 isestablished at 500 K. An equilibrium mixture of the threegases has partial pressures of 0.095 atm, 0.171 atm, and0.28 atm for NO, Cl2, and NOCl, respectively. (a) CalculateKp for this reaction at 500.0 K. (b) If the vessel has a volume of 5.00 L, calculate Kc at this temperature.
The equilibrium 2 NO1g2 + Cl21g2 ∆ 2 NOCl1g2 isestablished at 500 K. An equilibrium mixture of the threegases has partial pressures of 0.095 atm, 0.171 atm, and0.28 atm for NO, Cl2, and NOCl, respectively. (a) CalculateKp for this reaction at 500.0 K. (b) If the vessel has a volume of 5.00 L, calculate Kc at this temperature.
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 82QAP: A student studies the equilibrium I2(g)2I(g)at a high temperature. She finds that the total pressure...
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The equilibrium 2 NO1g2 + Cl21g2 ∆ 2 NOCl1g2 is
established at 500 K. An equilibrium mixture of the three
gases has partial pressures of 0.095 atm, 0.171 atm, and
0.28 atm for NO, Cl2, and NOCl, respectively. (a) Calculate
Kp for this reaction at 500.0 K. (b) If the vessel has a volume of 5.00 L, calculate Kc at this temperature.
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