Question

If you have ever hiked or climbed to high altitudes in the mountains, you surely have noticed how short of breath you get. This occurs because the air is thinner, so each breath contains fewer O2 molecules than at sea level. At the top o Mt. Everest, the pressure is only atm Air contains 21.0% O2 and 78.0% N2, and an average human breath is 0.450 L of air. For related problem-solving tips and strategies, you may want to view a Video Tutor Solution of Volume of a gas at STP revisited US

Answer 1

Top 3 Her R - universal n = thus Pressure at top of Mount Everest, p = 1 atm. volume of oxygen breathed = 21% of volume of air - 0. 21 0.45 Lt V = 0.0945 lt. Temperature at top of Mt. Everest is T = - 12°F = +248.70 kelvin. (a) o no. of moles of Oxygen (02) gas breathed in on breath is calculated art. PV=MRT gas constant 1 x 0.0945 R=0.082057 Latm Kines - 248.780.082057 (R = 0·082057 Laam K mot n = 1.5435x103 noles .. No. of molecules of Oxygen (O2) gas is No givences -- Not nXNA = 1.5435 * 6.023x10 23 N = g. 296 % 102 molecules Ans Ausbl since PV=nRT. At mean sea level, p= lahm, since temperature is constant . o Pvz Nosx 0:082057 x 248.7 6-0234 102 0.0945XNA 0.082057x248.07 Hence the required % = Nor x 100 = 1 x 100 = 33-33% - IX = 3 x 9.29 6810 molecules. Nos