A student ran the following reaction in the laboratory at 226 K: 2 NOBR (g) = 2 NO (g) + Br2 (g) When she introduced 0.161 moles of NOBR (g) into a 1.00 liter container, she found the equilibrium concentration of Br, (g) to be 1.65x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. Kc =
A student ran the following reaction in the laboratory at 226 K: 2 NOBR (g) = 2 NO (g) + Br2 (g) When she introduced 0.161 moles of NOBR (g) into a 1.00 liter container, she found the equilibrium concentration of Br, (g) to be 1.65x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. Kc =
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter19: The Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 60QRT
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![A student ran the following reaction in the laboratory at 226 K:
2 NOBR (g) =2 NO (g) + Br, (g)
When she introduced 0.161 moles of NOB (g) into a 1.00 liter container, she found the equilibrium concentration of Br, (g) to be
1.65x10-2 M.
Calculate the equilibrium constant, Kc, she obtained for this reaction.
K. =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F631f387d-e56c-494e-b0c7-1d822ea6f684%2F759e95a2-12fc-4d60-ac86-4d7fc5bc9f36%2Fu774keq_processed.png&w=3840&q=75)
Transcribed Image Text:A student ran the following reaction in the laboratory at 226 K:
2 NOBR (g) =2 NO (g) + Br, (g)
When she introduced 0.161 moles of NOB (g) into a 1.00 liter container, she found the equilibrium concentration of Br, (g) to be
1.65x10-2 M.
Calculate the equilibrium constant, Kc, she obtained for this reaction.
K. =
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