1. The hemoglobin in blood establishes an equilibrium with oxygen gas very quickly. The equilibrium can be represented as heme + O2 heme-O2 where "heme" stands for hemoglobin and "heme-O;" stands for the hemoglobin-oxygen complex. The value for the equilibrium constant for this reaction is about 9.2 x 105. Carbon monoxide also binds with hemoglobin by the following reaction: heme + co = heme-co This reaction has an equilibrium constant of 2.3 x 103. Which reaction's equilibrium lies farther toward products? Does your answer justify the toxicity of CO?

1. The hemoglobin in blood establishes an equilibrium with oxygen gas very quickly. The equilibrium can be represented as heme + O2 heme-O2 where "heme" stands for hemoglobin and "heme-O;" stands for the hemoglobin-oxygen complex. The value for the equilibrium constant for this reaction is about 9.2 x 105. Carbon monoxide also binds with hemoglobin by the following reaction: heme + co = heme-co This reaction has an equilibrium constant of 2.3 x 103. Which reaction's equilibrium lies farther toward products? Does your answer justify the toxicity of CO?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

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