An equilibrium mixture contains N2O4, (P= 0.30 atm ) and NO2 (P= 1.0 atm) at 350 K. The volume of the container is doubled at constant temperature. a) Calculate the equilibrium pressure of N2O4 when the system reaches a new equilibrium b) Calculate the equilibrium pressure of NO2 when the system reaches a new equilibrium.
An equilibrium mixture contains N2O4, (P= 0.30 atm ) and NO2 (P= 1.0 atm) at 350 K. The volume of the container is doubled at constant temperature. a) Calculate the equilibrium pressure of N2O4 when the system reaches a new equilibrium b) Calculate the equilibrium pressure of NO2 when the system reaches a new equilibrium.
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 12ALQ: In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What...
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An equilibrium mixture contains N2O4, (P= 0.30 atm ) and NO2 (P= 1.0 atm) at 350 K. The volume of the container is doubled at constant temperature.
a) Calculate the equilibrium pressure of N2O4 when the system reaches a new equilibrium
b) Calculate the equilibrium pressure of NO2 when the system reaches a new equilibrium.
Expert Solution
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Step 1
Le chatliers Principle:
As pressure decreases, equilibrium will shift to the side accompanied by an increase in the number of moles i.e. forward direction.
Boyle's Law: WIth an increase in pressure, the volume will decrease. There is an inverse relationship between pressure and volume.
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