2 NO2CI (g) = 2 NO2 (g) + Cl2 (g) K = 7.81 x 10-5 NO2CI is placed into an evacuated container to an initial pressure of 1.984 M and allowed to reach equilibrium via the above reaction at 548 K. What is the molarity of NO2CI at equilibrium?
2 NO2CI (g) = 2 NO2 (g) + Cl2 (g) K = 7.81 x 10-5 NO2CI is placed into an evacuated container to an initial pressure of 1.984 M and allowed to reach equilibrium via the above reaction at 548 K. What is the molarity of NO2CI at equilibrium?
Chemistry
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Chapter1: Chemical Foundations
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![2 NO2CI (g) = 2 NO2 (g) + Cl2 (g)
K = 7.81 x 10-5
NO2CI is placed into an evacuated container to an initial pressure of 1.984 M and
allowed to reach equilibrium via the above reaction at 548 K. What is the molarity of
NO2CI at equilibrium?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1902aad2-21dc-465b-9a23-f1c58d314009%2F8e2ff6a8-bec0-4f71-b36a-59a4246da0e6%2Fgus8vf4_processed.jpeg&w=3840&q=75)
Transcribed Image Text:2 NO2CI (g) = 2 NO2 (g) + Cl2 (g)
K = 7.81 x 10-5
NO2CI is placed into an evacuated container to an initial pressure of 1.984 M and
allowed to reach equilibrium via the above reaction at 548 K. What is the molarity of
NO2CI at equilibrium?
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