The binding of oxygen to hemoglobin in the blood involves the equilibrium reaction: Carbon monoxide replaces...
4. (6 pts) Hemoglobin (Hb) binds to both oxygen and carbon monoxide. When the carbon monoxide replaces the oxygen in an organism, the following reaction occurs: HbO2 + CO → HbCO + O2) At 37°C. K is about 200. When equal concentrations of HbO2 and HbCO are present, the effect of CO inhalation is fatal. Assuming Poe = 0.21 atm, what is Poo when [HBO3) - [HbCO)?
Carbon monoxide (CO) is toxic because it binds more strongly to the iron in hemoglobin (Hb) than does oxygen (O2), as indicated by these approximate standard free-energy changes in blood: reaction A:reaction B:Hb+O2Hb+CO⟶⟶HbO2,HbCO, ΔG∘=−70 kJ/mol ΔG∘=−80 kJ/mol Part A Estimate the equilibrium constant K at 298 K for the equilibrium HbO2+CO⇌HbCO+O2
Carbon monoxide (CO) is toxic because it binds more strongly to the iron in hemoglobin (Hb) than does oxygen (O2), as indicated by these approximate standard free-energy changes in blood: Hb+O2=HbO2 Delta G= -70 kJ/mol Hb+CO=HbCO Delta G= -80 kJ/mol Part A Estimate the equilibrium constant K at 298 K for the equilibrium HbO2+CO==HbCO+O_2
1. Carbon monoxide poisoning can happen because carbon monoxide has a higher affinity for hemoglobin than oxygen does. This can be seen by comparing the equilibrium constants for the two reactions Hb(a)+02()Hb02(aq) Hb(a)C(e) HbCO(aq) K 1.9x1012 K 1.1x1014 where Hb is hemoglobin. The actual reactions are more complicated since each hemoglobin can accept up to four oxygen molecules, but we will simplify it for this problem A concentration of about 12,500 parts per million of CO is considered highly lethal....
< 19 of 20 > I DONT MONOXIDE (UU) IS IUXIC Decause I DITIUS MOTE rongly to the iron in hemoglobin (Hb) than does oxygen 2), as indicated by these approximate standard free- nergy changes in blood: reaction A: Hb + O2 + HBO2, AGⓇ = - 70 kJ/mol reaction B: Hb+ CO + HbCO, AGⓇ = -80 kJ/mol Part A Estimate the equilibrium constant K at 298 K for the equilibrium HbO2 + CO = HbCO + O2 Express...
For the following questions consider this equation for hemoglobin – oxygen equilibrium. Hb + 4O2⥤ Hb(O2)4 Carbon Monoxide (CO) bonds to hemoglobin approximately 230 times stronger than oxygen. How would you increase the bonding oxygen to a patient with carbon monoxide poisoning?
1. Blood chemistry (again). The chemical equation for the binding of oxygen in your blood can be written as follows: Hemoglobin(aq) + O2(aq) → Hemoglobin* O2(aq) The reaction was studied using initial rates and the following data was obtained: [Hemoglobin] [02] Initial Rate 0.0050 M 0.0100 M 2105 M/s 0.0050 M 0.0200 M 4201 M/s 0.0100 M 0.0100 M 4198 M/s a. Determine the rate law for binding of hemoglobin and oxygen b. What is the rate constant? c. What...
1. a) Predict the effect of the following changes on the reaction in which SO3 decomposes to form SO2 and O2. 2 SO3(g) → 2 SO2 (g) + O2 (g) delta Ho = 197.78 kJ (1) Increasing the temperature of the reaction. (2) Increasing the pressure on the reaction. (3) Adding more O2 when the reaction is at equilibrium. (4) Removing O2 from the system when the reaction is at equilibrium. b) A person exposed to high levels of carbon...
9. Carbon monoxide (CO) is toxic because it can displace oxygen (O2) from the iron in hemoglobin (Hgb) following the reaction: HgbO2 (s) + CO(g) + Hgbco (s) + O2 (g) AG®rx = -30. kl/mol A. Consider the following reactions involving hemoglobin, O2 and Co: Hgboz (s) + Hgb (s) + O2 (g) AG®rxn = 40. kJ/mol HgbCO (s) -- Hgb (s) + CO (6) AGºrx = ??? Using Hess's law, determine the free energy AG*rn (in kJ/mol) for the...
The reaction of carbon monoxide and oxygen has an equilibrium constant of 4.76: 2 CO(g) + O2(g) ⇌ 2 CO2(g) At equilibrium, the concentration of all species is 0.21 M. If 0.50 M oxygen gas is added to the system, the value of the equilibrium constant will be: Group of answer choices 23.8 1.19 4.76 47.6 2.38