At a particular temperature, Kp = 0.27ó for the reaction %3D N204(9) = 2NO2(g) A flask containing only N204(g) at an initial pressure of 3.60 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium. 4.060 atm You are correct. Previous Tries Your receipt no. is 159-9433 With no change in the amount of material in the flask, the volume of the container in question is decreased to 0.200 times the original volume. Assuming constant temperature, calculate the (new) total pressure, at equilibrium.
At a particular temperature, Kp = 0.27ó for the reaction %3D N204(9) = 2NO2(g) A flask containing only N204(g) at an initial pressure of 3.60 atm is allowed to reach equilibrium. Calculate the total pressure in this flask at equilibrium. 4.060 atm You are correct. Previous Tries Your receipt no. is 159-9433 With no change in the amount of material in the flask, the volume of the container in question is decreased to 0.200 times the original volume. Assuming constant temperature, calculate the (new) total pressure, at equilibrium.
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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Transcribed Image Text:At a particular temperature, Kp = 0.270 for the reaction
N204(g) = 2NO2(g)
A flask containing only N204(g) at an initial pressure of 3.60 atm is allowed to reach equilibrium. Calculate the
total pressure in this flask at equilibrium.
4.060 atm
You are correct.
Previous Tries
Your receipt no. is 159-9433
With no change in the amount of material in the flask, the volume of the container in question is decreased to
0.200 times the original volume. Assuming constant temperature, calculate the (new) total pressure, at
equilibrium.
20.3 atm
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