N204 (g) = 2 NO2 (g) 11 N204 is placed into an empty container to an initial pressure of 1.292 atm at 219.0°C. After the reaction reaches equilibrium, the pressure of NO2 was 0.708. Assuming NO2 was only formed via the above reaction, calculate the value of Kp for the above reaction.

N204 (g) = 2 NO2 (g) 11 N204 is placed into an empty container to an initial pressure of 1.292 atm at 219.0°C. After the reaction reaches equilibrium, the pressure of NO2 was 0.708. Assuming NO2 was only formed via the above reaction, calculate the value of Kp for the above reaction.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

N204 (g) = 2 NO2 (g)
N204 is placed into an empty container to an initial pressure of 1.292 atm at 219.0°C.
After the reaction reaches equilibrium, the pressure of NO2 was 0.708. Assuming NO2
was only formed via the above reaction, calculate the value of Kp for the above
reaction.

Expert Solution

Step 1

The given equilibrium reaction is as follows:

$N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g)$

The initial pressure of N₂O₄ is = 1.292 atm

At the equilibrium, the pressure of NO₂ is = 0.708 atm

The value of the equilibrium constant, K_p is =?

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