part a,b and c please

Part 4: Simultaneous Equilibria Systems - Will complete on Mon, Feb 6 and Tues, Feb 7. In nature, equilibrium reactions will often affect one another. When two or more equilibrium reactions have an aqueous or gaseous substance in common. The change in concentration of the substance will affect more than one reaction. The hemoglobin (Hb) in our blood is an example of this. Blood Chemistry - It is a thought Experiment. (5 pts) Consider the hemoglobin (Hb) in the blood in equilibrium with four oxygenated hemoglobin: equilibrium rxn 1Hb+4O2(g)Hb(O2)4 In patients suffering from carbon monoxide poisoning, a relevant side reaction with an equilibrium occurring in the blood: equilibrium rxn2Hb+4CO(g)Hb(CO)4 Hemoglobin ( Hb ) is the common component in these two equilibria. Unfortunately, the equilibrium constant for rxn 2 is much greater than the equilibrium constant for rxn 1. Thus, in the presence of carbon monoxide, very little hemoglobin is available to bind with the oxygen in the blood and as a result oxygen deprivation occurs. In treating patients suffering from carbon monoxide poisoning, pure oxygen gas is administered to the patient. In the box below, a) Use Le Chatelier's Principle to indicate in which direction equilibrium reaction 2 shifts due to equilibrium reaction 1 shifting as indicated above. b) Explain why reaction 2 shifts in this direction. c) Due to this shift explain why the patient the remaining, CO(g) goes away when you breath out and the patient lives I (Do NOT add reaction 1 and reaction 2 in your explanation.)