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Lecture 1

BIOB34H3 Lecture 1: 12

3 Pages

Biological Sciences
Course Code
Blake Richards

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12202015 OneNote Online Gas Exchange Saturday, November 14, 2015 2:26 PM Transport: a general term referring to all movements. Respiratory gases: O C2 2 The respiratory gases move from place to place principally by two mechanisms: simple diffusion and convection (bulk flow). These in fact are the only mechanisms of O transpor2 because active transport of O is unknown. 2 the rate of diffusion of a solute from region to region is directly proportional to its difference in concentration between regions Chemical potential: the strength of the tendency of a chemical substance to undergo a physical or chemical change. Concentration, is not a useful surrogate for chemical potential when analyzing the diffusion of materials between gas mixtures and aqueous solutions When a gas dissolves in an aqueous solution, molecules of the gas become distributed among the H2O molecules in much the same way as glucose molecules or Na+ ions are incorporated among H2O molecules when solids dissolve. The molecules of a gas disappear when they go into solution. They do not appear as tiny bubbles any more than glucose in solution appears as tiny sugar grains; when we see bubbles of gas, they represent gas that is not in solution. Gas Phase: gas in gas mixtures Liquid phase: gas in aqueous solutions Partial Pressure: The individual pressure exerted by any particular gas in a gas mixture. An important property of partial pressure of each gas in a mixture is that it is independent of the other gases present. Mole fractional concentration of any particular gas in a mixture is the fraction of the total moles of gas present represented by the gas in question. To illustrate, in a volume of dry atmospheric air near sea level, the number of moles of O2 is 20.95 of the total number of moles of all gases taken together; therefore, the mole fractional concentration of O2 in dry air is 0.2095. The volume fractional concentration of a particular gas in a mixture is the fraction of the total volume represented by that particular gas. Equal molar quantities of different gases occupy essentially equal volumes. Thus the volume fractional concentration of a gas in a mixture is essentially the same as its mole fractional concentration. This means, for example, that if we remove the O2 from a volume of dry atmospheric air at a given temperature and pressure and we then restore the remaining gas to the same temperature and pressure, the final volume will be 20.95 less than the original volume. Henrys law is the fundamental law that relates partial pressure and concentration in aqueous https:adminmailutorontomy.sharepoint.compersonalhema_potluri_mail_utoronto_ca_layouts15WopiFrame.aspx?guestaccesstoken=0NXnTejTLtMMJI2 13
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