🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →

HomeTextbook Notes300,000US110,000

CHM 2046 Chapter Notes - Chapter 14: Inert Gas, Stoichiometry, Endothermic Process

50 views5 pages

emeraldkangaroo470

22 Mar 2018

School

Department

Course

Professor

For unlimited access to Textbook Notes, a Class+ subscription is required.

Document Summary

Chapter 14: equillibrium: hemoglobin is a protein found in red blood cells that reacts with o2. If there is a high concentration of o2 (reactant), the reaction shifts too the right to create more product. If there is a low concentration of o2 (reactant), the reaction shifts to the left to create more reactant (hbo2(product) dissociates, creating more oxygen) Law of mass action: k = ([c]c[d]d) / ([a]a[b]b) For the reaction 2n2o5 4no2 + o2. The equilibrium constant would be- k = [no2]4[o2]/[n2o5]2. Relationships between k and chemical equations: when the value of k is greater than one, when the reaction is at equilibrium, there will be more product molecules than reactant molecules. This reaction is product favored: when the value of k is less than one, when the reaction reaches equilibrium, there will be more reactant molecules than product molecules. C x pd d/pa partial pressure gas c.

Related Documents

CHM 2046 Chapter Notes - Chapter 13: Spectrophotometry, Polarimetry, Third Order

emeraldkangaroo470

CHM 111 Lecture Notes - Lecture 22: Equilibrium Constant, Spectrophotometry, Hemoglobin

PHYS 799 Lecture Notes - Lecture 1: Oxygen Saturation, Carbonic Anhydrase, Ph

ambermuskrat630

Related Questions

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(aq) + O_2(g) implies HbO_2(aq) K = 1.6 times 10^12 Hb(aq) + CO(g) implies HbCO(aq) K = 1.1 times 10^14 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. This corresponds to a partial pressure of about 10 torr of CO (5.1 times 10^-4 M). The concentration of hemoglobin in our blood (on average and roughly) is about 9.4 times 10^-3 M. Using reaction 2 and assuming the reaction goes to completion (limiting reactant, anyone?), determine the concentration of hemoglobin, CO and HbCO after the reaction Use your results from part (a) as your initial values in an ICE table and calculate the equilibrium concentration of carbon monoxide in your blood after exposure to a lethal dose of CO. You should get a very small number. Use wolfram alpha (http://www.wolframalpha.com) or another piece of software to solve your equations for you instead of using any approximate methods. If you breathe in pure oxygen, the partial pressure of oxygen is about the surrounding air pressure, or roughly 740 torr. However, by the time the oxygen mixes with your previous breath and the water in your lungs, the effective partial pressure of oxygen is lowered to about 500 torr which means a concentration of about 0.045M in your blood. Set up an ICE table using the initial concentrations of HbCO and CO from part (b), the initial concentration of O_2 of 0.045M and an initial concentration of HbO_2 of zero. Calculate the equilibrium concentration of HbO_2 when exposed to pure oxygen after carbon monoxide poisoning. Again, show the work to set up the equations and solve using Wolfram Alpha. In a healthy person, the concentration of HbO_2 in the arterial blood is about 8.9 times 10^-3M. If O_2 concentrations drop below about 80% of this a person will still have significant trouble breathing. Did this breathing treatment "cure" the patient?

Additional information:

Show transcribed image text

EXPERIMENT 5 Don't Get Stressed in the Lab "What a piece of work is a man! How noble in reason! How infinite in faculty! In form and moving how express and admirable! In action bow like an angel! -Hamlet 2.2 Hamlet's awe of humans is no wonder when one considers the amazingly complex intricacies of life. Chemical interactions are constantly taking place within us, regulating, maintaining, and adapting to change. We exist continually in a delicate state of balance between our internal components and the environment. For example, iron aids in the transport of oxygen to the body, which is essential for life. Red blood cells contain hemoglobin, which is a protein that is bound to iron. It is the iron that allows an oxygen molecule to attach to the hemoglobin in order to transport oxygen throughout the body. When the body experiences a deficiency in iron, the amount of oxygen being transported to the body is reduced. Therefore, the body is not able to function at full capacity, resulting in shortness of breath, dizziness, etc. This is called iron deficiency anemia. In order to increase the amount of iron in the body, doctors suggest eating foods high in iron, such as eggs and lean meats. However, people suffering with chis disease are also made aware chat the absorption of firon into the body is dependent on the extent to which iron remains soluble. Iron is easily absorbed when present in acidic conditions. Therefore, intake of iron with orange juice that contains ascorbic acid will increase the intake by the body. (The ascorbic acid also keeps iron in the +2 state which is more soluble.) Once enough iron has been taken in by the body an equilibrium is once again reached. The phenomena of chemical equilibrium is taking place all around us.Chemical equilibrium is never static; it is in constant motion. That motion is a balance between the rate of the forward reaction with the rate of the reverse process. This dynamic equilibrium is the result of the chemical reaction simultaneously producing products while also reverting back to reactants at an equal rate. The mol- ecules are constandy changing; therefore, being dynamic; however, being at equilbrium means the concentrations of the products and reactants have stopped changing.