HBS204 Lecture Notes - Lecture 2: Venous Blood, Partial Pressure, Restrictive Lung Disease

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7 Apr 2020

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Hbs204 week 2 the respiratory system 2. Each individual gas in a mixture exerts its own pressure called partial pressure (pgas) Dalton"s law states that the total pressure of a mixture of gases is the sum of the partial pressures of each of the individual gases that the mixture contains. Air is a mixture of gases 78% nitrogen, 21% oxygen, 1% argon and very small amounts of other gases like carbon dioxide. Atmospheric pressure is the sum of the partial pressures of each of these gases, total atmospheric pressure at sea level - 760 mm of mercury is the sum of the partial pressure of nitrogen, oxygen, argon and other gases including carbon dioxide: we need to work out the partial pressures of each of the gases at different atmospheric pressures. At atmospheric pressure of 760 mm of mercury the partial pressure of oxygen in that mix equates to 160 mm of mercury.

Related Questions

Boyles Law

a) A10.0 L sample of a gas at 25oC and 1.5 atm iscompressed at constant temperature to a volume of 1.0 L. What isthe new pressure?

b) A3.5 L sample of a gas at 1.0 atm is expanded at constanttemperature until the pressure is 0.10atm. What is the volume of the gas?

Charless Law

a) A2.5 L sample of gas at 25oC is heated to50oC at constant pressure. What is the finalvolume?

b) Whattemperature would be required to increase the volume from 2.5 L to6.0 L?

Avogadros Law

a) Assumingno change in temperature and pressure, how many moles of methane(CH₄) need to be added to 0.50 moles of methane todouble the volume?

b) 50g of solid carbon dioxide evaporates to carbon dioxide gas atstandard temperature and pressure. What isthe volume of carbon dioxide gas?

Combined Gas Laws

Calculate the temperature when a 0.50 L sample of gas at 1.0 atmand 25oC is compressed to 0.05 L of gas at 5.0atm.

Ideal Gas Law

a) Whatis the volume of gas occupied by 10.0 g CH4 at37oC and 4 atm?

b) Whatis the mass of N2 required to occupy 5.0 L at80oC and 560 mmHg?

Molar Density of Gases

a) Whatis the density of He at STP?

b) Whatis the density of carbon dioxide at 120^oC and 1.5atm?

Application of Gas Laws:

a) How many grams ofNO₂, nitrogen dioxide, are contained in 0.500 L of thegas at STP?

b) Calculate thedensity of NO₂ gas, in grams per liter, at 110C and 12atm.

c) Calculate the molarmass of a gas if 0.125 g of the gas occupies 93.3 mL at STP.

d) On a spring morning(15C) you fill your tires to a pressure of 2.25 atmospheres. As youride along, the tire heats up to 45C from the friction on the road.What is the pressure in your tires now?

e) What volume ofH₂ is formed at STP when 6.0 g of Al is treated withexcess NaOH?

2NaOH+ 2Al + 6H₂O 2NaAl(OH)₄ +3H₂(g)

Application of Gas Law

a) Whatis the effect on the volume of an ideal gas when the temperature isdecreased from 700K to 350K at constant pressure?

b) Whatis the effect on the volume of an ideal gas when both the pressureand temperature are reduced by half?

c) Whatis the effect on the volume of an ideal gas when the pressure ischanged from 722 torr to 0.950 atm, and the temperature is changedfrom 5^oC to 273 K?

Stoichiometric Relationships

a) Howmany grams of phosphorus react with 35.5 L of O₂ at STPto form tetraphosphorus oxide, according to the following reactionequation?

P₄ (s) + 5 O₂ (g)P₄O₁₀ (s)

b) Ammonia decomposes to nitrogen and hydrogen when in thepresence of heated steel wool. What is thefinal volume of the gas when 45 g of ammonia decomposes at150^oC and 1 atm pressure. Writea balanced equation before you start your calculations!

Daltons Law of Partial Pressures

a) A sample of a natural gas contains 8.24 moles of methane(CH₄), 0.421 mole of ethane(C₂H₆), and 0.116 mole of propane(C₃H₈). If the totalpressure of the gases is 1.37 atm, what are the partial pressuresof the gases?

b) Earths atmosphere consist of 78% N₂and 20%O₂, and other gases. What is the partial pressure ofN₂ and O₂intorr, when the atmospheric pressure is 1 atm?

c) Ammonia is completely decomposed to nitrogen and hydrogen, asin question 9b). At the end of theexperiment the pressure of the gas mixture is 866mmHg. Calculate the partial pressures ofN₂ and H₂.

fill the blanks with the terms given

Terms: 0.21, 21, 78, 760, altitude, blood, Boyle's, Dalton's,decimal, decreased, diaphragm, directly, external intercostal,Henry's, into, inverse, lowers, out of, oxygen, parasternal,partial, percent concentration, pressure, solubility, temperature,total, volume

_________ law states that there is a/an ________ relationshipbetween [listed alphabetically] the _________ of a gas and the___________ of the gas. That is, an increase in one of the factorsis associated with a decrease in the other factor and vice versa.Thoracic cavity size determines the volume of the air in the lungs.Thus, this law is fundamental to explaining why an increase in thethoracic cavity size due to expansion of the rib cage in thehorizontal [front-to-back and side-to-side] directions viacontraction of the ___________ and _________ muscles, (listedalphabetically) and vertical [up-and-down] direction viacontraction of the ___________ causes a resultant decrease inintrapulmonary pressure, creating a pressure gradient that drivesair _____________ the lungs. Conversely, it explains why when thesize of the thoracic cavity is _________ by relaxing the musclesused during inspiration, the pressure of the gas in the lungsincreases, exceeding atmospheric pressure, creating a pressuregradient that then forces air _________ the lungs ________ lawstates that the _______ pressure of a mixed gas is equal to the sumof the ___________ pressures exerted by each of the individualgasses in the mix, which are exerted independent of one another.This law is important to pulmonary physiology because theatmospheric air we breath is a mixed gas that contains roughly__________% nitrogen and _______% oxygen. Moreover, according toHenry's law, it is the partial pressure of the oxygen in the air webreath that is the main determinant of how much of the air's oxygenwe can drive into our blood and make available to the body. A gas'spartial pressure can be calculated by multiplying the totalpressure of the mixed gas by the gas's ____________ in the mixedgas. Thus, the partial pressure of oxygen, at sea level isdetermined by multiplying total atmospheric pressure at sea level -which equals ___________ millimeters of mercury (denoted mm Hg) by________ - oxygen's percent concentration in atmospheric air,expressed as a ____________. ________ law actually states that theamount of gas we can drive into solution is _________ dependentupon 3 factors. These 3 factors are 1) the solubility of theparticular liquid for the particular gas you are considering, 2)the temperature (more gas can be driven into liquids at lowertemperatures than at higher temperatures) and 3) the partialpressure of the gas under consideration. In the body, theparticular gas we are interested in driving into a fluid is__________ and the particular fluid we are interested in drivingthe gas into is our ___________. Because blood has a particularsolubility for oxygen - and this is constant, and because thehomeostatic mechanisms in the body keep body temperature relativelyconstant, this means the single most important factor thatdetermines how much oxygen can be driven in to our blood is thepartial pressure of the oxygen in the air we breath. At sea level -the partial pressure of oxygen in atmospheric air = 760 x 0.21 =159 mm Hg. However, if one climbs to the peak of Mt. Everest, wherethe air is still a mixed gas that contains only ~21% oxygen, butthe air there is 'thinner' i.e. there is just less of it up there,the total pressure of the gas drops to about 250 mm Hg, whichsignificantly __________ the the partial pressure of oxygen and theamount of air that can be forced into the blood at that altitude.Thus this gas law explains why many individuals initiallyexperience ____________ sickness when they vacation in the Rockiesor the Swiss Alps but normally live at much lower elevations.

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HBS204 Lecture Notes - Lecture 2: Venous Blood, Partial Pressure, Restrictive Lung Disease

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Boyles Law

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