Using the set of data that follows, calculate how many of the molecules of O2 th
ID: 3509246 • Letter: U
Question
Using the set of data that follows, calculate how many of the molecules of O2 that were used in aerobic catabolism by Julius Caesar are in each liter of atmospheric air today. All values given are expressed at Standard Conditions of Temperature and Pressure (see Appendix C) and therefore can be legitimately compared. Average rate of O2 consumption of a human male during ordinary daily activities: 25 L/h. Number of years after his birth when Caesar was mortally stabbed near the Roman Forum: 56 years. Number of liters of O2 per mole: 22.4 L/mol. Number of moles of O2 in Earth’s atmosphere: 3.7 x 1019 mol. Number of molecules per mole: 6 x 1023 molecules/mol. Amount of O2 per liter of air at sea level (20 degrees Celsius): 195 mL/L.
Explanation / Answer
Total litres of O2 consumed in the life time of Caesar =25 L O2/h X24 h/dayX365 day/yearX56 years = 12,264,000 L O2
the number of moles of O2 he used in his life time =1 2,264,000 L mol/22.4 L = 547,500 mol
Calculate the fraction atmospheric O2 he processes = 547,500 mol/3.7X1019mol = 1.5X1014
0.195 L O2 = 0.195/22.4 mol O2 = 0.00871 mol O2
The number of molecules present in this = 0.00871 x (6 x 1023) = 5.2 x 1021 molecules.
The number of molecules of O2 present in one liter = 5.2 x 1021
The number of molecules of O2 Caesar processed out of this = 1.5 x 10-14.
The number of molecules present in Caesar cells which participated in his metabolism=
(5.2 x 1021) x (1.5 x 10-14) = 7.8X107molecules
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