MMED2931 Lecture Notes - Lecture 11: Carbonic Anhydrase, Porphyrin, Blood Plasma

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4 Jun 2018

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Week 6 lecture 11: respiratory lecture 3

Learning objectives:

- Gas laws – partial pressure

- Diffusion of gases

- Diffusion and transport of oxygen

o Dissolved / bound to Hb

o Oxygen-Hb Dissociation Curve

o Factors that affect release of O2

- Diffusion and transport of CO2

o Dissolved

o Bound to Hb

o Bicarbonate

- Release of CO2 in the lungs

Gas, pressure and units:

- Gas: a mixture of molecules in a continuous state of random motion

- Pressure: the F generated when the molecules collide with a surface

- Units: International Unit – Pascals 1 Torr = 1mmHg = 133.3 Pascals

Partial P of gases: individual P of each gas

- If 3 dry gases in a jar (1, 2, 3), each gas will fill jar and exert a pressure

o Ptotal = P1 + P2 + P3

- Dalto’s La: I a iture of gases, eah gas ats idepedetl of the others and the total

pressure is the sum of the independent pressures

Gases dissolve in liquids:

- Gas mixture will equilibrate with solution & dissolved gas will have same partial P as the gas

mixture

o Concentration (aq) = Partial P x Solubility  if diff gas, same P =/= same [ ]

- Just as gases dissolve in water, water molecules will escape from liquid and exert a partial P

(water vapour P)

o Water vapour P: the P at which water vapour is in equilibrium with its condensed

state. At 760mmHg, water vapour P at 100o C = 760mmHg  boils

o At 37o C, 47mmHg

Diffusio: gases oe aross a erae  diffusio. Affeted  fators…

- SA for diffusion P across membrane

- Diffusion constant (depends on solubility of gas) T (thickness) of membrane

Diffusion equation:

- where

- SolCO2 = 20x SolO2  20x more capable to diffuse

- Emphysema: chronic lung disease that causes breathlessness.  SA →  O2 supply to muscle

- Restrictive lung diseases: alveolar-capillary barrier T ↑  ↓ O2 transferred across into blood

Partial P of dry gasses O2 & CO2 at 760mmHg:

- PO2 = 160mmHg PCO2 = 0.23mmHg

Partial P of humidified 37oC (as in lungs) of O2, CO2: water vapour P must be considered

- PO2 = 150mmHg PCO2 = 0.21mmHg

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Document Summary

Diffusion and transport of oxygen: dissolved / bound to hb, oxygen-hb dissociation curve, factors that affect release of o2. Diffusion and transport of co2: dissolved, bound to hb, bicarbonate. Units: a mixture of molecules in a continuous state of random motion the f generated when the molecules collide with a surface. Partial p of gases: individual p of each gas. If 3 dry gases in a jar (1, 2, 3), each gas will fill jar and exert a pressure: ptotal = p1 + p2 + p3. Dalto(cid:374)"s la(cid:449): i(cid:374) a (cid:373)i(cid:454)ture of gases, ea(cid:272)h gas a(cid:272)ts i(cid:374)depe(cid:374)de(cid:374)tl(cid:455) of the others and the total pressure is the sum of the independent pressures. Gas mixture will equilibrate with solution & dissolved gas will have same partial p as the gas mixture: concentration (aq) = partial p x solubility. If diff gas, same p =/= same [ ]

Related Questions

Question 11 pts

Which general statement about gases is NOT correct?

The molecules of a pure gas are distributed evenly throughout the container.

Gases are much less dense than liquids or solids

Molecules in a gas mixture can form layers according to their densities

Gases can be compressed, even to the point of liquefaction

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Question 21 pts

Which example is the greatest pressure?

1.00 atm

101 kPa

760 mm Hg (= 760 torr)

All of the above pressures are equal.

Flag this Question

Question 31 pts

Which example is the greatest pressure?

850 mm Hg (= 850 torr)

1.5 atm

All of the above pressures are equal.

96 kPa

Flag this Question

Question 41 pts

Assuming all other variables are held constant, a graph of which of the following will NOT yield a straight line?

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Question 51 pts

A sealed vessel contains 0.250 mol of oxygen gas. Which of the following will result in a decrease in the pressure of the oxygen gas?

increasing the number of moles of oxygen

increasing the temperature of the vessel

increasing the volume of the vessel

adding some helium to the vessel

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Question 61 pts

According to Charlesâs law, which change will cause the pressure of a gas to double? Pressure and amount of gas are constant.

The temperature decreases from 650 K to 325 K.

The temperature of the sample decreases fromï¿½88 Â°C to 44 Â°C.

The temperature of the sample increases fromï¿½22 Â°C to 44 Â°C.

The temperature of the sample increases fromï¿½250 K to 500 K.

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Question 71 pts

Which set of units for P, V, and T can be used for combined gas law calculations?

torr, L, and Kelvins

tm, g/L, and Kelvins

atm, mL, and degrees Celsius

inches of mercury, g/mL, and degrees Celsius

Flag this Question

Question 81 pts

The vapor pressure of a gas is

the atmospheric pressure at which the boiling point is determined.

the pressure at a Kelvin temperature exactly two times the boiling point.

impossible to determine experimentally without knowing the temperature and volume.

the pressure above a gas sample when evaporation and condensation are balanced.

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Question 91 pts

In a chemistry experiment where CO2 is collected over water, the atmospheric pressure is 755 mm. The partial pressure of water at the temperature in the lab is 24.2 mm. What is the pressure of the CO2?

779 mm

731 mm

More information is needed to answer this question

755 mm

Flag this Question

Question 101 pts

Which statement is NOT true according to the kinetic molecular theory of gases?

Molecules undergo elastic collisions

Molecules move in straight-line paths.

Molecules of different gases have differentï¿½kinetic energies at the same temperature

Molecules occupy a negligible volume.

Flag this Question

Question 111 pts

Which statement is NOT true according to the ideal
gas law?

At constant P & T, V must increase when n increases.

At constant V & T, P must decrease when n decreases.

At constant V & n, P must increase when T increases.

At constant P & n, V must decrease when T increases

Need help with #7-9,11. Please show work and formulas, units, and constants you used. Thank you!

7. Air is a source of reactants for many chemical reactions. A sample of dry air of total mass 1.00g consists almost entirely of 0.76g of nitrogen gas and 0.24g of oxygen. Calculate the partial pressures of each of these gases when the total pressure is 0.87 atm.

8. The box below contains a visualized mixture of gas A (represented by the black circles) and gas B (represented by the white circles.) If the partial pressure of gas A is 422 Torr, determnie P in the box, in Torr. Hint: it will help to imagine each circle represents one mol of each species.

9. Answer the questions which follow using the Maxwell-Boltzmann distributions plotted below. a) assume we are dealing with two samples of argon gas. Which curved (dotted or dashed) represents the sample of Ar at the higher temperature? Briefly explain you choice. b) Assume we are dealing with a sample of fluorine and a sample of neion, each at the same temperature. Which curved (dotted or dashed) represetns the sample of fluorine? Briefly explain your choice.

11. Calculate the root mean square velocity of water molecules in the vapor above boiling water at 100.0 degrees celsius.

1. Match the word 1-39 above, with the descriptions labled k-t. Word 1-39 can be uses only one please!!

1. alveolar macrophages 2. alveoli 3. Bohr effect 4. bronchi 5. bronchiole 6. cerebral cortex 7. chloride shift 8. compliance 9. costal breathing 10. Daltonâs law 11. diaphragmatic breathing 12. epiglottis 13. eupnea 14. expiratory reserve volume 15. fauces 16. functional residual capacity 17. Haldane effect 18. Henryâs law 19. hilum 20. hypothalamus 21. inferior, middle, and superior nasal meatuses 22. inspiratory capacity 23. larynx 24. limbic system 25. medulla oblongata 26. nose 27. paranasal sinuses 28. pharynx 29. pleural membranes 30. pons 31. primary bronchus 32. secondary bronchus 33. surface tension 34. surfactant 35. terminal bronchiole 36. tertiary bronchus 37. total lung capacity 38. trachea 39. vital capacity

k) ----------------------- shallow breathing using just the external intercostal muscles

l) ------------------ amount of effort required to expand the lungs and chest wall

m) ------------------- tidal volume + inspiratory reserve volume, usually about 3600 mL in males

n) ----------------- tidal volume + inspiratory reserve volume + expiratory reserve volume; usually about 4800 mL in males

o) ------------------- residual volume + expiratory reserve volume; usually about 2400 mL in males

p) -------------------- states that the amount of gas that will dissolve in a liquid is proportional to the partial pressure of that gas and its solubility

q) ---------------- when pH decreases, O2 saturation of hemoglobin decreases

r) ------------------ each gas in a mixture of gases exerts its own partial pressure

s) ------------------- sets basic rhythm of breathing

t) ------------------------ includes the pontine respiratory group

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MMED2931 Lecture Notes - Lecture 11: Carbonic Anhydrase, Porphyrin, Blood Plasma

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