A flask is charged with 1.5 atm of N2O4 (g) and 1 atm NO2 (g) at 20°C and the following equilibrium is achieved: N204 (g) 2 NO2 (g). After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. a. What is the equilibrium partial pressure of N2O4 b. Calculate the value Kp for the reaction. c. Calculate Kc for the reaction.
A flask is charged with 1.5 atm of N2O4 (g) and 1 atm NO2 (g) at 20°C and the following equilibrium is achieved: N204 (g) 2 NO2 (g). After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. a. What is the equilibrium partial pressure of N2O4 b. Calculate the value Kp for the reaction. c. Calculate Kc for the reaction.
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 66QAP: Consider the equilibrium H2(g)+S(s)H2S(g)When this system is at equilibrium at 25C in a 2.00-L...
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A flask is charged with 1.5 atm of N2O4 (g) and 1 atm NO2 (g) at 20°C and the following equilibrium is achieved: N204 (g) 2 NO2 (g). After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.
a. What is the equilibrium partial pressure of N2O4
b. Calculate the value Kp for the reaction.
c. Calculate Kc for the reaction.
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