Unfortunately, carbon monoxide was not a common molecule when hemoglobin evolved,and the binding site does not distinguish between Oz and Co. When carbon monoxide ispresent, it can bind to some of the available hemoglobin sites, which prevents thehemoglobin from carrying oxygen.Fo*Fe*Fe*B. CO binds at an absorption site with energy €co = -3.45 × 10-20 J. Suppose there is a 1to 100 ratio of CO to O2 present in the blood. For simplicity's sake, assume there are now100 Oz molecules available to bind.1. What are the possible states now, and what are their multiplicities?

The objective of this question is to explain the possible state and multipleties. It show 1:100…

Unfortunately, carbon monoxide was not a common molecule when hemoglobin evolved, and the binding site does not distinguish between O₂ and CO. When carbon monoxide is present, it can bind to some of the available hemoglobin sites, which prevents the hemoglobin from carrying oxygen. Fe² Fe² B. CO binds at an absorption site with energy co= -3.45 x 10-20 J. Suppose there is a 1 to 100 ratio of CO to O2 present in the blood. For simplicity's sake, assume there are now 100 0₂ molecules available to bind. 1. What are the possible states now, and what are their multiplicities?

Unfortunately, carbon monoxide was not a common molecule when hemoglobin evolved, and the binding site does not distinguish between O₂ and CO. When carbon monoxide is present, it can bind to some of the available hemoglobin sites, which prevents the hemoglobin from carrying oxygen. Fe² Fe² B. CO binds at an absorption site with energy co= -3.45 x 10-20 J. Suppose there is a 1 to 100 ratio of CO to O2 present in the blood. For simplicity's sake, assume there are now 100 0₂ molecules available to bind. 1. What are the possible states now, and what are their multiplicities?

Chemistry

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Chapter1: Chemical Foundations

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Spectroanalytical methods measure the wavelength and intensity of radiations that are either emitted or absorbed by a molecular or atomic species. These methods are useful for evaluating the electronic or atomic arrangement of the molecules of a given analyte.

Question

Unfortunately, carbon monoxide was not a common molecule when hemoglobin evolved,
and the binding site does not distinguish between Oz and Co. When carbon monoxide is
present, it can bind to some of the available hemoglobin sites, which prevents the
hemoglobin from carrying oxygen.
Fo*
Fe*
Fe*
B. CO binds at an absorption site with energy €co = -3.45 × 10-20 J. Suppose there is a 1
to 100 ratio of CO to O2 present in the blood. For simplicity's sake, assume there are now
100 Oz molecules available to bind.
1. What are the possible states now, and what are their multiplicities?

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