s2, fall 2017, Homework Problem Set 1 Name: following questions relate (loosely)

Question

s2, fall 2017, Homework Problem Set 1 Name: following questions relate (loosely) to Hill et al, Chapters 7-9 and our lab exercises. Using the data set below, 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. Notes: This is a very challenging problem, which you might choose to postpone until afer you have some practice with other quamtitative problems. To solive it, you can break it down into several parts; the instructors will help with hints and guidance n of a human male during ordinary daily activities: 25 h Average O2 consumptio Number of years after birth when Caesar was mortally stabbed in the Number of liters of O2 per mole: 22.4 Number of moles of O2 in Earth's atmosphere: 3.7 x 10" mol Number of molecules per mole: 6 x 10 molecules/mol Amount of O2 per liter of air at sea level (20°C): 195 mL/L Roman Forum: 56 years /mol Be prepared to be surprised! Of course, criticize the calculations if you feel they deserve it.

Explanation / Answer

1 mole of oxygen have 22.4 liters volume

Now calculate numbers of molecules in 1 Liter of oxygen by using following steps.

Therefore 22.4 liters = 1 mole oxygen

So, 1 liter = 1 / 22.4 moles

We know that 1 mole oxygen has 6× 1023 oxygen molecules.

So total numbers of molecules in 1-liter oxygen will be-

1 liter = (1 / 22.4) × 6× 1023

1 liter = 0.2678× 1023

1 liter = 26.78× 1021 molecules

Therefore, Julius Caeser used 26.78× 1021 molecules oxygen per liter for his aerobic catabolism.

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