Hemoglobin and Carbon Monoxide

In today’s world there are much chemical equilibrium that tends to be abstract as foregoing section as equilibrium constant, and Le Chatelier’s principle. In addressing the subject of equilibrium, the result can be seen as a process that is involving human health as an importance and maintains the equilibrium in the reaction is between hemoglobin and carbon monoxide. When exposed or inhaled to a harmful gas such as carbon monoxide, “it takes the place of oxygen in hemoglobin, which the red blood pigment carries, oxygen to all parts of the body”.[2][3] Because carbon monoxide binds to hemoglobin which is much stronger than oxygen, this will affect the body causing oxygen starvation throughout the body.

The bonds between the carbon monoxide and the hemoglobin and the equilibrium expression thus becomes: “Hb (aq) + 4CO (g) ⇋ Hb (CO) 4 (aq)”[1] which is called carboxy-hemoglobin. The bonds between hemoglobin and carbon monoxide are approximately 300 times as stronger which indicates that the shift in equilibrium will move towards the right side of the equation of the carboxy-hemoglobin side. In this case K for the hemoglobin-carbon monoxide reaction has a much higher reaction. “The affinity of hemoglobin puts priority on carbon monoxide bonds, which the hemoglobin has bonded to carbon monoxide and is no longer able to carry out oxygen.”[1][2] Carbon monoxide can cause headaches and dizziness, which can be fatal. The reserve effect of carbon monoxide, oxygen has to introduce into the body. It will help with the carboxy- hemoglobin, which will produce oxygenated hemoglobin, along with carbon monoxide:”Hb (CO) 4 (aq) + 4O 2 (g) ⇋ Hb (O 2) 4 (aq) + 4CO (g)”.[1] Carbon monoxide thus produced is dissipated when the person exhales.

[1] http://www.ausetute.com.au/blood.html
[2] http://www.ncbi.nlm.nih.gov/pubmed/3976
[3] http://teachingcases.hematology.org/broudy/erythroprotein.cfm