Using the set of data that follows, calculate how many of the molecules of O_2 t

Question

Using the set of data that follows, calculate how many of the molecules of O_2 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 O_2 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 O_2 per mole: 22.4 L/mol. Number of molecules per mole: 6 x 10^23 molecules/mol. Amount of O_2 per liter of air at sea level (20 degree C): 195 mL/L. Be prepared to be surprised! Of course, criticize the calculations if you feel they deserve criticism.

Explanation / Answer

Amount of O2 per litre of air = 195 ml/L [or] 0.195 Litre O2 per 1 litre of air

Since aerobic catabolism is occurring at STP conditions, 22.4 litres = 1 mole

1 litre air * 0.195 L O2 * 1 mole * 6.022 * 10^23 molecules

1 1 litre air 22.4 litres 1 mole

= 5.24 * 1021 molecules of O2

So he consumes 5.24 * 1021 molecules of O2 in each litre of air that he takes in.

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