A 2.90 mole quantity of NOCI was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 28.0 percent of the NOCI had dissociated: 2NOCI(g) 2NO(g) + Cl₂(g) Calculate the equilibrium constant K for the reaction. 0.0911 X
A 2.90 mole quantity of NOCI was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 28.0 percent of the NOCI had dissociated: 2NOCI(g) 2NO(g) + Cl₂(g) Calculate the equilibrium constant K for the reaction. 0.0911 X
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.56QE
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![A 2.90 mole quantity of NOCI was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 28.0 percent of the NOCI had dissociated:
2NOCI(g) → 2NO(g) + Cl₂(g)
Calculate the equilibrium constant K for the reaction.
0.0911
x](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86624ab7-da2a-4a5b-91b8-0bf4ad8ab366%2F966b63aa-252f-429d-aea2-ca2071fa0782%2Fswam8hi_processed.png&w=3840&q=75)
Transcribed Image Text:A 2.90 mole quantity of NOCI was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 28.0 percent of the NOCI had dissociated:
2NOCI(g) → 2NO(g) + Cl₂(g)
Calculate the equilibrium constant K for the reaction.
0.0911
x
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