A flask is charged with 1.350 atm of N2O4(g) and 1.14 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below. N2O4(g) 2NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. (a) What is the equilibrium partial pressure of N2O4? _____ atm (b) Calculate the value of Kp for the reaction. (c) Is there sufficient information to calculate Kcfor the reaction? If Kc can be calculated, find the value of Kc.
A flask is charged with 1.350 atm of N2O4(g) and 1.14 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below. N2O4(g) 2NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. (a) What is the equilibrium partial pressure of N2O4? _____ atm (b) Calculate the value of Kp for the reaction. (c) Is there sufficient information to calculate Kcfor the reaction? If Kc can be calculated, find the value of Kc.
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 73QAP
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A flask is charged with 1.350 atm of N2O4(g) and 1.14 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below.
N2O4(g) 2NO2(g)
After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.
(a) What is the equilibrium partial pressure of N2O4?
_____ atm
(b) Calculate the value of Kp for the reaction.
(c) Is there sufficient information to calculate Kcfor the reaction?
If Kc can be calculated, find the value of Kc.
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